The Pyro Handbook
3.1 explosive classifications 4.0 Chemical equiv. lists
5.0 LISTS OF SUPPLIERS
AND MORE INFORMATION
6.0 Chemical
preparation and sources
6.40-8
hydrazine diperchlorate
6.40-22
titanium tetraperchlorate
7.2
Nitrogen Triiodide(touch explosives)
8.1
Simple Plastique Explosives
9.9 Firebombs(Molotov
cocktail)
9.11
Picallo bomb(bottle salute)
10.1 Pyrotechnic
compositions and formulas
10.1-2 Colored Flame formaulas and
torches
10.1-5
colored star compositions
10.1-6
smoke star compositions
10.2-3 Making tubes and end plugs
10.11 Meal Coated Corn Cob &
Rice Hulls
11.5-1
special effect fire balls
11.5-3
fire ball from hydrogen
12.0 fuses, delays, and timers
12.1-2
HOW TO MAKE BLACKMATCH FUSE
12.1-3 HOW TO MAKE AN ELECTRIC FUZE
12.1-6 The Nichrome/Fuse Igniter
12.1-7 HOW TO MAKE SULFURED WICK
12.1-8 Connecting fuses together
12.2-1
Blasting Cap Impact Igniter
12.3-1 ELECTRO-MECHANICAL IGNITION
12.3-3 Radio Control Detonators
1.0
Intro
It is assumed by the author that you would
not actually use this information as a guide for new activities. If you don’t know what you are doing, you
could make a mistake and DIE. Some of
the procedures are general ways of making a specific devise or chemical
composition, and lack the exact details that inexperienced people need to
safely make a desired material.
Also, there may be one or two references to terrorists and
procedures that they may use in a few sections; I HATE terrorists, and do not
in any way promote terrorism! (I
just didn’t feel like to go through the entire book and delete every sentence
containing the word “terrorist”.)
If you are wanting to carry out a death wish, and are going to
attempt some of these procedures, then READ THE SAFETY SECTION FIRST(if you
want a better chance of living)! Don’t
be a dumb-ass, and do it near people or houses, and hurt someone and/or
yourself! Don’t be a “Kewl”.
-The Author
2.0 SAFETY--HOW NOT TO GET KILLED (READ THIS!)
It is obvious that injury or death should be avoided at all
costs. While no safety device is 100% reliable, it is usually better to err on
the side of caution.
- Never
smoke anywhere near chemicals or
compositions.
- Be sure you are familiar with all the properties of the
compositions you work with. Thoroughly test new compositions for
sensitivity, stability, compatibility with other mixtures etc, until you
are absolutely sure that the mixture is ok to use in your application and
method of construction. Find out as much as you can about other peoples
experiences with a particular mixture.
- Use only non-sparking tools. Make your tools from
either: wood, paper, aluminum, lead or brass. Other metals and materials
may spark (especially steel).
- Paper bags or wooden containers are good to use for storing
mixed compositions. Store compositions dry and cool. Avoid plastics, glass
and metal. Avoid storing compositions in general. Make as much as you will
need in the near future and keep no more in stock than necessary.
- Never have large amounts of composition near you. If you must
use larger amounts of composition in multiple items, store the bulk of
composition in a safe place and bring only small amounts to your working
place. Finished items should also be brought to a safe place immediately.
- Prevent contamination of chemicals and mixtures. Have
separate tools for every type of mixture (i.e. black powder-like mixtures,
chlorates, perchlorates, etc) and clean them well with hot water and/or
alcohol after use. It is no luxury either to have different sets of
clothing for working with different mixtures. Wash them every time after
use (dust collects in the clothing). If you have the possibility, have
separate rooms or better yet: separate buildings for working with
different types of mixtures/chemicals.
- Keep a clean working place. Fine dust easily spreads all
over your working place. Keep chemicals in closed cabinets or in a
separate building. Mixtures should not be kept in the working place anyway
(see rules 4 and 5).
- Provide adequate ventilation. This is especially important
when working with volatile solvents or (poisonous, flammable) powdered
chemicals. Not only can you get yourself poisoned, vapor or dust may also
ignite.
- Be aware of static electricity buildup. Ground your working
table. Monitor humidity and keep it above 60% as a rule of thumb. This can
be especially important in winter when preparing for new years eve (on the
Northern Hemisphere at least). Touch a grounded surface before you place
things on it. Touch other people before handing over compositions or
finished items. Wear cotton clothing, avoid synthetics (do not be tempted
to wear fleece clothing if your working place is cold in winter). Simple
things such as unscrewing a (plastic) bottle, unwinding some tape or even
moving your arm may accumulate enough charge on your body to ignite a
sensitive composition. The risk of static electricity is often
underestimated or even completely ignored by beginning amateurs in pyro,
while it is actually one of the major causes of accidents in both
commercial/industrial and amateur pyro setups.
- Wear proper protective clothing. A face shield, dust mask,
heavy gloves and a leather apron are minimal. Wear cotton clothing.
Hearing protection can be good but it also makes it harder to hear other
people's warnings.
- Provide safety screens between you and compositions,
especially when pressing, ramming, sieving or in other ways causing
frictions/shocks/pressure etc.
- Be prepared for the worst. Have a plan for when something
should go wrong. Have a fire extinguisher and plenty of water ready. Think
beforehand of what might happen and how you could minimize the damage.
Know how to treat burns. Inform someone else so he/she can help in case of
an accident. Have a fast escape route from your working place.
- Test a device well before showing it to an audience. Inform
any audience well of what can happen.
2.1-Know What You're
Handling:
[This
is a publication of the Western New York Pyrotechnic Association. It may be
reproduced in whole or in part without permission or compensation providing:]
[Editors note: I have received several letters offering comments and/or
corrections on this document. Since I am not the author of the document, and do
not have the expertise to judge these comments, I have put them as received on another page]
- 1) credit is given to the Western New
York Pyrotechnic Association
- 2) it is distributed free. If you plan
to make a buck on it, we want a piece of it!!
We believe that the information contained herein is true and
correct, however it is offered only as a guide and not to be used as a
guarantee. We cannot assume responsibility nor liability for the use or misuse
of the information contained herein.
The following is a compilation of information gathered over the
years from various research and sources too numerous to remember.
Within these pages you will find
descriptions of almost 150 chemicals that are used in Fireworks, Explosives,
Rocket Fuels or are explosives in themselves. This list is not complete and is
not intended to be complete. All of the uses are not given and only the related
purposes of each are stated.
Whenever possible we explain
which grades are thought to be the best, the chemical formula, melting
temperature, decomposition temperature, form (liquid, powder, crystal, etc.),
if it will explode, if it is poisonous and its usage. Some of these chemicals
cannot be purchased and are offered as a guide for information purposes only.
CHEMICALS HAVE A CERTAIN PURPOSE TO PERFORM IN FIREWORKS AND CAN
BE CLASSIFIED INTO FOUR GROUPS:
GROUP I.
These
chemicals are the chemicals which produce the oxygen and are called oxidizers.
GROUP
II.
Those
which combine with the oxidizers are called reducers.
GROUP
III.
These are
the chemicals which regulate the rate of burning and help to produce the
desired effect.
GROUP IV.
This group of chemicals are those which impart color to the flame.
PLEASE
NOTE: ALL REFERENCES TO TEMPERATURE ARE IN DEGREES FARENHEIT.
SAFETY INCOMPATIBLE MATERIALS:
Certain combinations of chemicals are remarkable explosive,
poisonous or hazardous in some other way, and these are generally avoided as a
matter of course. There are many others that are perhaps equally dangerous but
do not come to mind as readily. The following list, although not complete, may
serve as a memory refresher. Stop and think for a moment before starting any
work, especially if one hazardous chemical is involved.
DO NOT CONTACT:
Alkali
metals, such as calcium, potassium and sodium with water, carbon dioxide, carbon tetrachloride,
and other chlorinated hydrocarbons.
Acetic Acid with chromic acid, nitric acid,
hydroxyl-containing compounds, ethylene glycol, perchloric acid, peroxides and
permanganates.
Acetone with concentrated sulfuric and
nitric acid mixtures.
Ammonia, Anhydrous with mercury,
halogens, calcium hypochlorite or hydrogen fluoride.
Ammonium Nitrate with acids,
metal powders, flammable fluids, chlorates, nitrates, sulphur and finely
divided organics or other combustibles.
Aniline with nitric acid, hydrogen
peroxide or other strong oxidizing agents.
Bromine with ammonia, acetylene,
butadiene, butane, hydrogen, sodium carbide, turpentine or finely divided
metals.
Chlorates with ammonium salts, acids,
metal powders, sulfur, carbon, finely divided organics or other combustibles.
Chromic Acid with acetic acid, naphthalene,
camphor, alcohol, glycerine, turpentine and other flammable liquids.
Chlorine with ammonia, acetylene,
butadiene, benzene and other petroleum fractions, hydrogen, sodium carbides,
turpentine and finely divided powdered metals.
Cyanides with acids.
Hydrogen Peroxide with copper,
chromium, iron, most metals or their respective salts, flammable fluids and
other combustible materials, aniline and nitromethane.
Hydrogen Sulfide with nitric
acid, oxidizing gases.
Hydrocarbons, generally, with
fluorine, chlorine, bromine, chromic acid or sodium peroxide.
Iodine with acetylene or ammonia
Mercury with acetylene, fulminic acid,
hydrogen.
Nitric acid with acetic, chromic and
hydrocyanic acids, aniline, carbon, hydrogen sulfide, flammable fluids or gases
and substances which are readily nitrated.
Oxygen with oils, grease, hydrogen,
flammable liquids, solids and gases.
Oxalic Acid with silver or mercury.
Perchloric Acid with acetic
anhydride, bismuth and its alloys, alcohol, paper, wood and other organic
materials.
Phosphorous Pentoxide with water
Sodium Peroxide with any
oxidizable substances, for instance: methanol, glacial acetic acid, acetic
anhydride, benzaldehyde, carbon disulfide, glycerine, ethylene glycol, ethyl
acetate, furfural, etc.
Sulfuric Acid with chlorates, perchlorates,
permanganates and water.
Some combinations of chemicals
lead to especially sensitive or unstable mixtures. There are many more of such
incompatible chemicals/mixtures than listed here but these are some of the more
commonly encountered types:
- Chlorates and sulfur. Mixtures containing both are not only
very sensitive to friction and shock but are also known to ignite
spontaneously. The sulfur reacts with water and air to form trace amounts
of sulfuric acid. This will react with chlorates to form chlorine dioxide,
a yellow explosive gas that will ignite most flammable materials upon
contact. Addition of small amounts of barium or strontium carbonate to
chlorate based compositions is sometimes done to prevent buildup of acid,
even in compositions without sulfur. Many older texts on pyrotechnics
describe the use of chlorate/sulfur based compositions. Today, many
alternative and much safer compositions are available and there is
therefore no excuse for the use of chlorate/sulfur mixtures. This also
means chlorate based compositions cannot be used in items that also
contain sulfur based mixtures. For example: chlorate based stars cannot be
primed with black powder. Nor can a H3 burst charge be used with black
powder primed stars (or stars containing sulfur).
- Chlorates and ammonium compounds. Mixing these will allow ammonium
chlorate to form in a double decomposition reaction that takes place in
solution (moisture speeds up the process). Ammonium chlorate is a highly instable
explosive compound. It decomposes over time producing chlorine dioxide gas
(see chlorates and sulfur). Mixtures are likely to spontaneously ignite
upon storage or may explode for no apparent reason. An exception seems to
be the use of ammonium chloride and potassium chlorate in some smoke
compositions. According to Shimizu this combination is safe due to the
lower solubility of potassium chlorate (compared to ammonium chlorate). I
personally would still use these mixtures with great caution (or avoid
them) since it seems inevitable that small amounts of ammonium chlorate
will still form. The lower solubility of potassium chlorate will make it
the -main- product in a double decomposition reaction but not the -only-
product.
- Chlorates with metals and nitrates. These mixtures show the same problems
as chlorate/ammonium compound mixtures. The reason is that nitrates can be
reduced by most metals used in pyrotechnics to ammonium. The reaction rate
of this reaction is increased by presence of water. Over time (for example
when drying) these mixtures may spontaneously ignite or become extremely
sensitive. The fact that ammonium forms in a relatively slow reaction is
treacherous. These mixtures are referred to as 'death mixes' by some.
- Aluminum and nitrates. Mixtures of these compounds sometimes
spontaneously ignite, especially when moist. The mechanism is assumed to
be as follows: the aluminum reduces some of the nitrate to ammonium,
simultaneously forming hydroxyl ions. The aluminum then reacts with the alkaline
products in a very exothermic reaction leading to spontaneous heating up
of the mixture. This can eventually lead to ignition. The reactions take
place in solution and therefore moisture speeds up the reaction. The
process is usually accompanied by the smell of ammonia. Some types of
aluminum are more problematic than others. Stearin coated aluminum is
generally safer to use. The whole process can be prevented in many cases
by the addition of 1 to 2 percent of boric acid. This will neutralise the
alkaline products. It is best to bind such compositions with non-aquaous
binder/solvent systems such as red gum/ethanol. Since aluminum/nitrate
mixtures are extensively used it is important to be aware of this problem
which is why the combination is listed here.
Flash Powder:
ALL
FLASH POWDERS ARE EXTREMELY HAZARDOUS. THEY WILL IGNITE FROM FRICTION, IMPACT,
OR FLAME.
While it is assumed that the individual who is dispensing these
materials is responsible and knowledgeable as to their use, the following pointers
will prove helpful:
- Always use electrical ignition, either a
commercial squib or Nichrome hot wire. The use of a squib is preferred
because it provides a more positive ignition.
- Always use an approved flash pot, made
from transite or other similar material.
- Always use the minimum amount of powder
required to achieve the desired effect. In general, one quarter of a
teaspoon will be sufficient.
- Always have only one person who is
responsible for dispensing and storing the flash powders.
- Never pour the powder directly from the
bottle into the flash pot. Measure the correct amount using a non-sparking
metal, not plastic, spoon.
- Never confine or compact the powder in
any way. To do so may lead to a violent explosion.
- Never return unused powder to the original
bottle.
- Never mix two different colors of flash
powder. In many cases, the chemicals in the two materials are incompatible
with each other.
- Never pour flash powder from its plastic
bottle onto plastic film or into another plastic container. The material
is packed in plastic to reduce the danger of serious injury in case the
powder should ignite in the bottle.
- Be extra careful on dry or low humidity
days, when the chance of ignition by static electricity is high.
Chemical Notes:
Aluminum Al
An element
used for brilliancy in the fine powder form. It can be purchased as a fine
silvery or gray powder. All grades from technical to superpure (99.9%) can be
used. The danger is from inhaling the dust and explosive room condition if too
much dust goes into the air.
Aluminum
Chloride AlCl3
This
chemical must not come in contact with the skin as severe burns can result. The
yellowish-white crystals or powder have a strong attraction for water. Purchase
only in the anhydrous grade.
Amber
This is a
fossil resin of vegetable origin and is yellowish- brown in color. It is used
in fireworks to a small extent.
Ammonium
Bichromate and Dichromate (NH4)2Cr2O7
A mild
poison used in the manufacture of tabletop volcanoes (sometimes called Vesuvius
Fire). It is available as orange crystals in a technical grade. Also used in
smoke formulas.
Ammonium
Chloride NH4NO3
The
common name is Sal Ammoniac. Comes as colorless crystals or a white powder. The
technical grade is used to manufacture safety explosives and smokes.
Ammonium
Oxalate NH4C2O4
This
compound takes the form of colorless, poisonous, crystals. The technical grade
is suitable for the manufacture of safety explosives.
Ammonium
Perchlorate
(NH4ClO4)
This
chemical can be made to explode by either heat or shock. Besides exploding in
itself, it is used to manufacture other explosives.
Ammonium
Permanganate
NH4MnO4
A
moderate explosive which can be detonated by either heat or shock.
Ammonium
Picrate
(NH4C6H2N3O7)
These
bright orange crystals are used in armor piercing shells and fireworks. If
heated to 300 degrees it will explode or it can be set off by shock. If you do
any work with this chemical, it is advisable to keep it wet.
Aniline
Dyes
These are
used in smoke powder formulas. They are organic coal tar derivatives. Available
in many different colors.
Aniline
Green C23H25CIN2
Also
known as Malachite Green. One of the many Aniline dyes. The green crystals are
used in smoke formulas.
Anthracene
A coal
tar derivative used as a source of dyestuff and for colored smokes. Available
as colorless crystals which melt at 217 degrees.
Antimony Sb
Another
name for this metal element is Antimony Regulus. Purchase the black powder in
99% purity. Not the yellow variety. It is used in pyrotechnics.
Antimony
Fulminate
One of a
group of unstable, explosive compounds related to Mercury Fulminate.
Antimony
Potassium Tartrate
Also
known under the name of Tartar Emetic. These poisonous, transparent, odorless
crystals (or white powder) are used to make Antimony Fulminate. The moisture
that is present can be driven off by heating to 100 degrees. Do not exceed this
temperature or the chemical will decompose.
Antimony
Sulfide (Sb2S3)
This has
usefulness in sharpening the report of firecrackers, salutes, etc. or to add color
to a fire. The technical black powder is suitable. Avoid contact with the skin;
dermatitis or worse will be the result.
Aqua
Regia
A strong
acid containing 1 part concentrated Nitric Acid and 3 parts concentrated
Hydrochloric Acid. Store in a well closed glass bottle in a dark place. This
acid will attack all metals, including gold and platinum. It is used in making
some explosives.
Arsenic
Sulfide, Red
The
common name is Realgar and it is also known as Red Arsenic. Purchase the
technical grade, which is available as a poisonous orange-red powder. It is
used in fireworks to impart color to the flame.
Arsenic
Sulfide,Yellow
(As2S3)
This
Chemical is just as poisonous as its red brother and is also used in fireworks,
somewhat. The common name is Kings Gold.
Arsenious
Oxide (As2O)3
A white,
highly poisonous powder used in fireworks. It is also known as Arsenious
Trioxide, Arsenic Oxide and Arsenous Acid. Its uses are similar to Paris Green.
Asphaltum
A black
bituminous substance, best described as powdered tar.
Auramine
Hydrochloride
Also
known as Auramine. It is used in smoke formulas. Available as yellow flakes or
powder, which readily dissolves in alcohol.
Auramine
A
certified Biological stain used in smoke cartridges.
Barium
Carbonate BaCO3
This is a
poisonous salt of Barium, which decomposes at a fairly high temperature, 1300
degrees. It is available as a fine white powder in the technical grade. It is
used in fireworks as a color imparter.
Barium
Chlorate
Ba(ClO3)2H2O
Available
as a white powder. It is poisonous, as are all Barium salts. It is used in
fireworks, both as an oxidizer and color imparter. It is as powerful as
Potassium Chlorate and should be handled with the same care. Melting point is
414 degrees.
Barium
Nitrate Ba(NO3)2
The uses
and precautions are the same as above with a comparison equal to Potassium
Nitrate instead of the Chlorate. It melts at 500 degrees.
Bismuth
Fulminate
One of a
group of unstable, explosive compounds derived from Fulminic Acid.
Brass
This is
an alloy of Copper and Zinc. Some also contain a small percentage of Tin. The
commercial grade is suitable in powdered form. It is used in some fireworks
formulas.
Calcium
Carbide CaCO3
These
grayish, irregular lumps are normally packed in waterproof and airtight metal
containers. It is used in toy cannons. Mixed with water it forms Acetylene Gas
(EXPLOSIVE).
Calcium
Carbonate CaCO3
This
occurs as the mineral Calcite. It is used for Phosphorous Torpedoes, but does
not have any dangerous properties in itself. Also as an acid absorber in
fireworks.
Calcium
Fluoride CaF2
This
finds its use in a smokeless firework mixture and is not used elsewhere. It is
a white powder, also known as Fluorspar.
Calcium
Phosphide Ca3P2
This
compound, which comes as gray lumps, must be kept dry. Upon contact with water
it will form the flammable gas, Phosphine. It is used in signal fires.
Camphor OC10H16
A ketone
found in the wood of the Camphor tree, native to Taiwan and a few of our
states. For the best results, buy the granulated, technical grade. Used in
explosives and fireworks.
Castor
Oil
The
common drug store variety is used in some powders to reduce the sensitiveness
and to waterproof the mixture.
Charcoal C
A form of
the element, Carbon, it is used in fireworks and explosives as a reducing
agent. It can be purchased as a dust up to a coarse powder. The softwood
variety is best and it should be black, not brown.
Chrysoidine
An
organic dye available as a red-brown powder. It is used in smoke formulas.
Clay
This can
be purchased in the powdered form. It is used dry for chokes, nozzles and
sealing firework cases. You can mix it with water to form paste if so desired.
Confectioners
Sugar
Commonly
called powdered sugar, it can be purchased at your local food store. The
fineness is graded by the symbol XXXX. It is used in explosives.
Copper
Cu
As any
pure metal used in fireworks, this must also be in a powdered state. It is
reddish in color, in fact, it is the only element to be found in nature having
that color.
Copper
Acetoarsenite (Cu)3As2O3Cu(C2H3O2)2
The
popular name for this is Paris Green. It is also called Kings Green or Vienna
Green. It is readily available as an insecticide or as a technical grade,
poisonous, emerald green powder. It is used in fireworks to add color.
Copper
Arsenate CuHAsO3
A fine,
light green, poisonous powder. It is used in the technical grade for fireworks.
Copper
Carbonate
CuCO3.Cu(OH)2
Also
known as Cupric Carbonate or Artificial Malachite. It is a green powder used in
fireworks.
Copper
Chlorate
Cu(ClO3)2.6H2O
Or,
technically, Cupric Chlorate. A poison used in fireworks as an oxidizer and to
add color.
Copper
Chloride CuCl2
An
oxidizer and color imparter used in fireworks. Purchase the brownish-yellow
technical grade. This is a poisonous compound.
Copper
Nitrate
Cu(NO3)2.3H2O
Or Cupric
Nitrate. These blue crystals absorb water, as you can see from the formula. It
is used in fireworks.
Copper
Oxide CuO
When
ordering be sure to specify the black powder. It is also available in red. The
technical grade will serve the purpose for fireworks.
Copper
Oxychloride
A green
powder used to impart oxygen and color especially to blue star formulas. It is
a poison and the dust should not be inhaled.
Copper
Sulfate
CuSO4.5H2O
Known as Blue
Vitriol, this poisonous compound is available as blue crystals or blue powder.
It can be purchased in some drugstores. Used in fireworks for blue stars.
Copper
Sulfide CuS
As are
the other copper salts, this is also used in fireworks to add color. The
technical grade is suitable and is black in color. You can make your own by
passing Hydrogen Sulfide into a Copper salt.
Decaborane
B10H14
This
chemical is classed as a flammable solid and is used for rocket fuels. It will
remain stable indefinitely at room temperature.
Diazoacetic
Ester C4H6N2O2
A very
severe explosive in the form of a yellow oil. It will explode on contact with
Sulfuric acid or when heated. Very volatile and explosive.
Diazoaminobenzene C6H5N:N.NH.C6H5
These
golden yellow crystals will explode when heated to 150 degrees.
P-Diazobenzeneslfonic
Acid C6H4NSO3N
Another
severe explosive. It can be exploded by rubbing the white paste or powder, or
by heating.
Diazodimitrophenol HOC6H3(NO2)2N(:N)
An
organic explosive in the same group as the above compound. Also very sensitive
to shock or heat.
Diazomethane CH2N2
Also
known as Azimethylene. This yellow gas is also in the above group and can be
exploded by heat or shock.
Dinitrotoulene
Known as
DNT for short. These yellow crystals are used in the manufacture of other
explosives.
Ethyl
Alcohol
This
alcohol is the only one that is useful for fireworks. It should be about 95%
pure. It is poisonous because of the impurities. It is clear, like water, and
also a very flammable liquid.
Fluorine
Perchlorate
FClO4
A very
sensitive colorless gas which will explode on the slightest contact with a
rough surface. It can also be detonated by heating to 168 degrees. Avoid all
contact with this gas, as even a trace of it will attack the lungs.
Gallic
Acid C7H6O5.H2O
A white
or pale fawn colored powder used in fireworks to make whistles. When mixed with
some chlorates, Permanganates or Silver salts, it may explode.
Glycerol C3H8O3
Commonly
known as Glycerin. It is obtained from oils and fats as a by-product when
making soaps. It is a sweet warm tasting syrupy liquid which is used in several
explosives. Contact with Chromium Trionide or potassium Permanganate may cause
an explosion.
Gold
Explosive
A dark
brown powder which explodes when heated or rubbed. Upon exploding, it yields
Gold, Nitrogen and Ammonia. The exact composition is unknown because it is too
explosive to be dried.
Guanidine
Nitrate
CH5N3.HNO3
Guanidine
is found in turnip juice, rice hulls and earthworms. It is used in the preparation
of this chemical, or, it can be made from Ammonium Nitrate and Dicyanodiamide.
To be of any value, it should be 95% pure. Guanidine Nitrate is not explosive
itself, but is used in the manufacture of explosives. It is a white powder
which melts at 210 degrees.
Gum
Arabic
A dried,
gummy, exudate from tropical trees. It is available as flakes, fragments and
powder. It is used as a binder in firework formulas.
Hexachlorethane CCl3.CCl3
Also
known as Carbon Hexachloride, this chemical is used in smoke formulas It can be
obtained in either powder or crystals.
Indigo
A dark
blue crystalline powder which is a commercial dye. You can purchase either the
technical or pure grade for smokes.
Iodine
Heavy
grayish metallic looking crystals or flakes. Poisonous. Purchase the U.S.P.
grade. It is being used in making explosives.
Iron Fe
The
granular powder (at least 99% pure) is needed for several firework pieces. It
is not a dangerous element but will rust very easily, making it useless.
Iron Oxide FeO These black crystals are used in thermite mixtures. When
ordering, it may be listed as Ferrous Oxide. Black.
Kieselguhr
This is a
whitish powder used in dynamites. It is a siliceous earth, consisting mainly of
diatoms. A good grade will absorb about four times its own weight.
Lactose
Also
called milk sugar. This white powder has a sweet taste. The crude grade will
work for smoke formulas.
Lampblack
This is
another name for the element, carbon(pencil lead). It is a finely powdered
black dust, resulting from the burning of crude oils. It is used for special
effects in fireworks.
Lead
Azide PbN6
This is a
poisonous white powder which explodes by heating to 350 degrees or by
concussion. The main usage is in primers. It can be made from Sodium Azide and
Lead Nitrate.
Lead
Bromate
Pb(Bro3)2.H2O
Poisonous,
colorless crystals. Pure Lead Bromate is not explosive unless it is made from
precipitated Lead Acetate with an alkali bromate. Made in this manner, it can
be exploded by rubbing or striking.
Lead
Chloride PbCl2
It is
available as a white crystalline, poisonous powder which melts at 501 degrees.
It is used in fireworks.
Lead
Dioxide PbO2
Also
known as Brown Lead Oxide, this dark brown powder is used as an oxidizer in
matches and fireworks. Poisonous.
Lead
Nitrate Pb(NO3)2
Available
as white or colorless crystals in the technical grade. The uses include matches
and explosives. Poisonous.
Lead
Oxide Pb3O4
Also
known as Red Lead or Lead Tetroxide. A 95% purity is desired for matches. Also
poisonous.
Linseed
Oil
Available
in many forms: Brown, boiled, raw and refined. All are made from the seed of
the flax plant. The cheapest form is suitable for fireworks. Purchase from a
paint store.
Lithium
Chloride LiCl
The
technical grade is sometimes used to add color to fireworks compositions.
Available as a white powder.
Manganese
Dioxide MnO2
Used in
pyrotechnic mixtures, matches and match box friction surfaces. Available as a
technical grade, black powder. This oxidizer decomposes at 535 degrees.
Magnesium Mg
This
metal is used in a powdered state for brilliancy in flares and will even burn
vigorously underwater.
Mercuric
Chloride HgCl2
A white,
poisonous powder. Also known as Corrosive Sublimate. It can be made by
subliming Mercuric Sulfate with ordinary table salt and then purified by
recrystallization. The U.S.P. grade is used for some firework compositions.
Mercuric
Oxide HgO
Available
in two forms; red and yellow. Both forms give the same oxidizing effects in
fireworks. The technical grade is suitable.. All forms are poisonous.
Mercuric
Oxycyanide
HgO.Hg(CN)2
In the
pure state it is a violent poison which will explode when touched by flame or
friction.
Mercuric
Thiocyanate
Hg(SCN)2
A
poisonous, white odorless powder used in the making of Pharaoh"s Serpents.
Use the technical grade.
Mercurous
Chloride HgCl
Also
known as Calomel or Mercuric Monochloride. This white, non- poisonous powder
will brighten an otherwise dull colored mixture. Sometimes it is replaced by
PVC or Hexachlorobenzene and even Antimony Sulfide, for the same purpose. Note
that it is non poisonous only when it is 100% pure. Never confuse this chemical
with Mercuric Chloride, which is poisonous in any form.
Mercury
Fulminate
Hg(ONC)2.H2O
A
crystalline compound used in primers, percussion caps, blasting caps and other
detonators. Explodes very easily from heat or shock.
Methylene
Blue C16H18N3SCl
This dark
green powder is used for smokes in the technical grade. Also called
Methylthionine Chloride.
Mineral
Jelly
Also
known as Vaseline, Petrolatum or Petroleum Jelly. This acts as a stabilizer in
fireworks and explosives.
Naphthalene
This is a
tar product that you may know better as Moth Flakes or moth balls. Only the
100% pure form should be used in making smoke powders. The melting point is 100
degrees.
Nitric
Acid HNO3
Also
known as Aqua Fortis. It is a clear, colorless corrosive liquid, which fumes in
moist air. It can react violently with organic matter such as Charcoal, Alcohol
or Turpentine and consequently must be handled Very carefully. It is available
in three forms: White fuming, Red Fuming and Concentrated (70 to 71%). The
latter, with a specific gravity of 1.42, is the proper grade to buy. Whatever
grade, avoid contact with the fumes or the liquid. Contact with the skin will
cause it to burn and turn yellow. It is used to manufacture many explosives.
Nitroglycerin C3H5N3O9
A liquid
with a sweet burning taste, but do not taste it or it will produce a violent
headache or acute poisoning. It can be made to explode by rapid heating or
percussion. It is used as an explosive and also to make other explosives.
Nitroguanidine H2NC(NH)NHNO2
A yellow
solid made by dissolving Fuanidine in concentrated Sulfuric Acid and then
diluting with water. Dangerous Explosive.
Nitromethane CH3NO2
An oily,
poisonous liquid, which is used as rocket fuel.
Oil
of Spike
This is a
volatile oil obtained from the leaves of certain trees. Keep this colorless (or
pale yellow) liquid well closed and away from light. It is used in some
fireworks.
Paraffin
This is a
white or transparent wax. It is normally sold in a solid block. You can use it
to make the required powder.
Paranitroanaline
Red
(H2NC6H4)3COH
A dye
used in smoke formulas. It dissolves in alcohol and will melt at 139 degrees.
It is also known as P-Aminophenyl.
Pentaerythritol
Tetranitrate
C5H8N4O12
A high
explosive known as PRTN. Besides being an explosive itself it is used in a
detonating fuse called Primacord.
Perchloryl
Fluoride ClFO3
A gas
under normal air pressure. When brought in contact with alcohol, explosions
have resulted.
Phosphorus P
This
element comes in three forms, with three different ways of reacting. They
resemble each other in name only. Red Phosphorous is the only suitable form for
fireworks and matches. It is a non-poisonous violet-red powder. It will ignite
at 260 degrees. When making a formula containing Phosphorous, be sure to work
with it in a WET STATE. This is a most dangerous chemical to work with and
should be handled only by the most experienced. Oxidizers have been known to
detonate violently without warning when mixed with Red Phosphorous.
Phosphorous
Pentasulfide
Also
known as Phosphoric Sulfide. These light yellow crystals are used in matches.
Phosphorus
Trisulfide P2S3
This
chemical can catch fire from the moisture that is present in air, therefore the
container should be kept tightly capped. The technical grade, purchased as
grayish-yellow masses, is used in making matches.
Picric
Acid
This is
used to bring out and improve the tone of colors in various fireworks. It is
also used to make other chemicals that are used in fireworks and explosives.
Picric Acid can explode from heat or shock. It is interesting to note what it
is called in other countries: Britain - Lyddite; France - Melinite; Japan -
Shimose.
Plaster
of Paris
This is a
white powder, composed mostly of Calcium Sulfate. It is used, by mixing with
water, for end plugs in fireworks and also in some formulas.
Potassium K
A soft
silvery metal element. It will react vigorously with water and several acids.
It is not used directly except for some experiments.
Potassium
Chlorate KClO3
This,
perhaps, is the most widely used chemical in fireworks. Before it was known,
mixtures were never spectacular in performance. It opened the door to what
fireworks are today. It is a poisonous, white powder that is used as an
oxidizer. Never ram a mixture containing Potassium Chlorate. Do not store
mixtures which contain this chemical for any great length of time, as they may
explode spontaneously.
Potassium
Dichromate
K2CR2O7
Also
known as Potassium Bichromate. The commercial grade is used in fireworks and
matches. The bright orange crystals are poisonous. Also used in smokes.
Potassium
Ferrocyanide
K4Fe(CN)6.3H2O
Lemon
yellow crystals or powder which will decompose at high temperatures. It is used
in the manufacture of explosives.
Potassium
Nitrate KNO3
Commonly
called Saltpeter; this chemical is an oxidizer which decomposes at 400 degrees.
It is well known as a component in gunpowder and is also used in other firework
pieces. Available as a white powder.
Potassium
Perchlorate
KClO4
Much more
stable than its Chlorate brother, this chemical is a white or slightly pink
powder. It can often substitute for Potassium Chlorate to make the formula safer.
It will not yield its oxygen as easily, but to make up for this, it gives off
more oxygen. It is also poisonous.
Potassium
Picrate
C6H2KN3O7
A salt of
Picric Acid, this chemical comes in yellow, reddish or greenish crystals. It
will explode when struck or heated. It is used in fireworks.
Potassium
Thiocyanate KCNS
Colorless
or white crystals which are used to make the Pharaoh's Serpent. The commercial
grade or pure grade is suitable.
n-Propyl
Nitrate C3H7NC2
Prepared
from Silver Nitrate and n-Propyl Bromide and is used as a jet propellant.
Red
Gum
Rosin
similar to shellac and can often replace it in many firework formulas. Red gum
is obtained from the bark of trees.
Rhodamine
B
A basic
fluorescent organic pigment also known as Rhodamine Red. Available in green or
red crystals or powder. It is used in smoke formulas.
Shellac
An
organic rosin made from the secretion of insects which live in India. The exact
effect it produces in fireworks is not obtainable from other gums. The common
mixture of Shellac and Alcohol sold in hardware stores should be avoided.
Purchase the powdered variety, which is orange in color.
Silver
Fulminate AgONC
A
crystalline salt similar to Mercury Fulminate but more sensitive. In fact, too
sensitive for commercial blasting. It is used for toy torpedoes and poppers.
Silver
Oxide Ag2O
Dark
brown, odorless powder. It is potentially explosive and becomes increasingly
more so with time. Keep away from Ammonia and combustible solvents. The
technical grade, which is about 92% pure, is suitable.
Sodium
Aluminum Fluoride
Na3AlF6
Also
known as mineral, Cryolite. It is used in fireworks in the white powdered form.
Sodium
Bicarbonate
NaHCO3
When a
formula calls for this chemical, you can use Baking Soda (NOT Baking Powder).
It is a white, non-poisonous powder.
Sodium
Carbonate NaCO3
This
white powder is used in fireworks, but not to any great extent. The anhydrous
grade is best.
Sodium
Chlorate NaClO3
An
oxidizer similar to Potassium Chlorate, although not as powerful and also with
the disadvantage of absorbing water. Decomposes at 325 degrees.
Sodium
Chloride NaCl
This is
used in fireworks. You can use the common form, table salt (or rock salt if
made into a powder).
Sodium
Nitrate NaNO3
Also
known as Chile Saltpeter; very similar to Saltpeter, (Potassium Nitrate). It is
used where large amounts of powder are needed in fireworks and explosives. It
will absorb water as do other sodium salts.
Sodium
Oxalate Na2C2O4
This is
not a strong poison, but is poisonous, and you should not come in contact with
it or breathe the dust for any prolonged period. The technical grade is best
for making yellow fires.
Sodium
Perchlorate
NaClO4H2O
This
chemical is used in fireworks and explosives. It is very similar to Potassium
Perchlorate with the exception that it will absorb water.
Sodium
Peroxide Na2O2
A
yellowish-white powder. It can explode or ignite in contact with organic
substances.
Sodium
Picrate
Very
similar to Potassium Picrate and should be handled with the same precautions.
It is also known under the name of Sodium Trinitrophenolate.
Sodium
Silicate
Na2SlO3.9H2O
This
chemical, commonly called water glass, is used as a fireproof glue. It is
available in syrupy solution and can be thinned with water if necessary. When
dry it resembles glass, hence the name. It can, when desired, be thickened with
calcium carbonate, zinc oxide, powdered silica, or fiberglass (chopped) if
extra strength is desired.
Stearin
Colorless,
odorless, tasteless, soapy crystal or powder. Sometimes referred to as Stearic
Acid. Purchase the technical grade, powder. It can often take the place of
Sulphur and Charcoal in fireworks.
Strontium
Carbonate SrCO3
Known in
the natural state as Strontianite, this chemical is used for adding a red color
to fires. It comes as a white powder in a pure, technical or natural state.
Strontium
Chloride
SrCl2.6H2O
A
colorless or white granulated chemical used in pyrotechnics. It will absorb
water and is not used often.
Strontium
Nitrate Sr(NO3)2
By far
the most common chemical used to produce red in flares, stars and fires.
Available in the technical powder grade. An oxidizer with 45% oxygen and
absorbs water.
Strontium
Sulfate SrSO4
This does
not absorb water as quickly as nitrate and is used when storage is necessary.
In its natural state it is known as Celestine, which compares to grades used in
fireworks.
Sulphur
(Sulfur) S
For
example type II burns at 250 degrees giving off choking fumes. Purchase good
pyro grades low in acid. Used in many types of fireworks and explosives.
Sulfuric
Acid H2SO4
Also
called Oil of Vitriol, it is a clear liquid with the consistency of a thin
syrup. Bottles should be kept tightly closed as it is a very corrosive and
dangerous chemical. It has a great affinity for water and will absorb it from
any source. The effect can be a charred surface or fire. The grade used in
explosives is 93-98%.
Sulfur
Trioxide SO3
This
powder will combine with water with explosive violence to form Sulfuric Acid.
If brought in contact with wood flour and a drop of water is added, a fire will
start. It is used to make some explosives.
Trinitrotoluene (NO2)3C6H2CH3
Commonly
known as TNT. The poisonous crystals are colorless in the pure state. It is
more powerful and expensive than Dynamite. If not confined it will burn like
dynamite. Used as a high explosive and to make others.
Wood
Flour
This is
merely another name for sawdust or wood meal. It is used in fireworks and
explosives.
Zinc Zn
Of all
the forms, only the dust is suitable in the technical or high purity grade. It
is a gray powder used in star mixtures and for fuel in model rockets.
Zinc
Borate
3ZnO.2B2O3
A white
amorphous powder used in making smoke formulas. A relatively safe compound to
handle.
Zinc
Carbonate ZnCO3
Another
white Zinc compound used in some smoke formulas. Also a safe compound to
handle.
Zinc
Oxide ZnO
Sometimes called Flowers of Zinc. This is a white or yellowish
powder used in some firework formulas. It has also found use as a thickening
agent in water glass when a stronger pyro paste is desired.
The best way to mix two dry chemicals to form an explosive is to
do as the small-scale fireworks manufacturer's do:
Ingredients:
·
1
large sheet of smooth paper (for example a page from a newspaper that does not
use staples)
·
The
dry chemicals needed for the desired compound.
-Measure out the
appropriate amounts of the two chemicals, and pour them in two small heaps near
opposite corners of the sheet.
-Pick up the sheet
by the two corners near the powders, allowing the powders to roll towards the middle of the sheet.
-By raising one corner and
then the other, roll the powders back and forth in the middle of the open
sheet, taking care not to let the mixture spill from either of the loose ends.
-Pour the powder
off from the middle of the sheet, and use immediately. If it must be stored use
airtight containers (35mm film canisters work nicely) and store away from
people, houses, and valuable items.
As with many hobbies, pyrotechnics requires some tools. For what I
do, it's usually all pretty simple stuff. When you get into real pyrotechnics,
you need things like ball mills, presses, and star rollers. For some info on
those things, click here and here.
Scales:
A good scale is an absolute must for real pyrotechnics. When
measuring compositions, all measurements are done by weight, so you need an
accurate scale. Postal scales that use a spring are crap and are not suitable
for accurate measurements. You need either a digital scale or a tripe beam
balance.
My digital scale:
I didn't shop around when I bought my scale, so I got ripped off!
I bought the "MX-200 Pyro Scale" for $90 and later found it on eBay for much less. There are many
different places that sell scales, and you should get one with 0.1g accuracy.
A few sites that sell scales (there are many more):
Cyberscale
eBay is definitely worth a look, you can get great deals sometimes!
eXactaDigital
Balances.com
Pyrotek has scales, along with a lot of other stuff.
Ball mills:
Ball mills are very important to the serious pyrotechnician
because they are needed to make good blackpowder at home and to mill powders
finely. You can either buy one or make one and rock tumblers often work just as
well (some ball mills are just rock tumblers with a different name).
Lortone rock tumbler sold by United Nuclear as a ball mill:
UN ball mills and
milling media.
The "ball mills" UN sells are Lortone rock/jewelry tumblers, but from what I've heard, they work very
well. The Lortone website has them listed much cheaper than UN sells them, so you should check it out. eBay is also a
place to find them, but after shipping it might not be any cheaper.
Making a bal mill can be a good project if you like building
things, and it will be a lot cheaper than buying one. A few pages on making
your own:
Dan
Williams ball mill
Wouter Visser's ball
mill
Mortar & Pestle:
A mortar and pestle are very useful for grinding up chemicals into
powder. For larger amounts or for making black powder you will obviously want a
ball mill, but for small amounts a mortar and pestle can be very useful. They
can be purchased at cooking stores and chemistry supply stores/websites.
Mortar and Pestle:
Coffee Grinder:
Coffee grinders are somewhere between a mortal and pestle and a
ball mill. I find some of the best things to use them for is to grind prilled
KNO3 and NH4NO3. Some people also use them to grind Al foil before they ball
mill it to make rather large flake Al powder. I got mine for $11.
Coffee grinder:
Glassware:
Glassware is used more often to make HE's than to be used for
LE's. The basics are shown here, flasks, graduated cylinders and thermometers.
Assorted glassware:
Electric Hotplate:
Hotplates can be used for a number of things related to pyrotechnics/explosives.
You could use it for melting KNO3/sucrose, boiling 3% H2O2 to concentrate, or
any other procedure like TNP that requires heating. You could get a fancy one
specifically for lab use that will get hotter and do it faster, or you can buy one
intended for home use. I bought a "Toastmaster" hotplate for $20 at a
large hardware/appliance store.
Hotplate:
There are plenty of basic tools that will often come in handy,
that are a lot cheaper also!
Ignition supplies:
You will definitely need something to light your devices (unless
you are using electrical ignition) so these are some of the most basic things.
A lighter and matches are both good, but are not ideal for directly lighting
fuses. A better choice is a punk. Punks are pretty much just a stick with
sawdust or something on them. They look and burn like incense, but without the
smell. Because you have a constant coal, they work very well for lighting
fuses. Just be sure not to light your device and then toss your lit punk into a
pile of dry grass! There are two general sizes, incense size and much larger
ones that I like better.
Protection:
Safety is a very important part of pyro, as it can be a fairly
dangerous hobby. Your eyes are very vulnerable, so you should were eye
protection while working with devices and setting them off. There are several different
choices of protection, either eye or full face. Choose what to wear depending
on what you are doing. It would of course be best to have full face protection
at all times, but it isn't always essential.
Hand protection should be used whenever you are working with
something that has the potential to ignite. Leather gloves should be worn for
best protection. While working with powders, you should were a dust mask to
keep particles out of your nose, mouth, throat and lungs. Check MSDS sheets for
specific precautions for different chemicals. A respirator is a good thing to
have sometimes, IÌll probably buy one myself before too long.
Knives:
Knives have all kinds of uses, and can often be used for things
such as cutting open firework casings. There are millions of things to do with
a knife, not just pyro related. Buy a good one and it should last you a long
time.
Light:
You will probably set off some of your devices at night, and it's
a good idea to be able to see where you are going! This is very basic, so it
can sometimes be forgotten. Maglites are good, but I really like a lightweight
LED headlamp because you don't need your hands and it is very bright.
Pliers/cutters:
Pliers can both be useful for things like peeling casings or
crushing powder. I use wire cutters for things like cutting the sticks off
bottle rockets for making a Can o Rockets.
If you think of any other tools I forgot, feel free to email me
and I'll add them.
[Information
copied from http://krimzonpyro.com/ep/infodir/tools.html]
3.0 EXPLOSIVE THEORY
An explosive is any material that, when ignited by
heat or shock, undergoes rapid decomposition or oxidation. This process
releases energy that is stored in the material in the form of heat and light,
or by breaking down into gaseous compounds that occupy a much larger volume
that the original piece of material. Because this expansion is very
rapid, large volumes of air are displaced by the expanding gases. This
expansion occurs at a speed greater than the speed of sound, and so a sonic
boom occurs. This explains the mechanics behind an explosion.
Explosives occur in several forms: high-order explosives which detonate, low
order explosives, which burn, and primers, which may do both.
High order explosives detonate. A detonation
occurs only in a high order explosive. Detonations are usually incurred
by a shockwave that passes through a block of the high explosive
material. The shockwave breaks apart the molecular bonds between the
atoms of the substance, at a rate approximately equal to the speed of sound
traveling through that material. In a high explosive, the fuel and
oxidizer are chemically bonded, and the shockwave breaks apart these bonds, and
re-combines the two materials to produce mostly gasses. T.N.T., ammonium
nitrate, and R.D.X. are examples of high order explosives.
Low order explosives do not detonate; they burn, or
undergo oxidation. when heated, the fuel(s) and oxidizer(s) combine to produce
heat, light, and gaseous products. Some low order materials burn at about
the same speed under pressure as they do in the open, such as black powder.
Others, such as gunpowder, which is correctly called nitrocellulose, burn much
faster and hotter when they are in a confined space, such as the barrel of a
firearm; they usually burn much slower than black powder when they are ignited
in unpressurized conditions.
Black powder, nitrocellulose, and flash powder are good examples of low order
explosives.
Primers are peculiarities to the explosive
field. Some of them, such as mercury fulminate, will function as a low or
high order explosive. They are usually more sensitive to friction, heat,
or shock, than the high or low explosives. Most primers perform like a
high order explosive, except that they are much more sensitive. Still
others merely burn, but when they are confined, they burn at a great rate and
with a large expansion of gasses and a shockwave. Primers are usually used in a
small amount to initiate, or cause to decompose, a high order explosive, as in
an artillery shell. But, they are also frequently used to ignite a low
order explosive; the gunpowder in a bullet is ignited by the detonation of
its primer.
4.0 Chemical Equivalency list:
Acacia................................................................Gum
Arabic
Acetic
Acid..............................................................Vinegar
Aluminum
Oxide............................................................Alumia
Aluminum Potassium
Sulphate.................................................Alum
Aluminum
Sulfate............................................................Alum
Ammonium
Carbonate.....................................................Hartshorn
Ammonium
Hydroxide.......................................................Ammonia
Ammonium
Oleate.....................................................Ammonia Soap
Amylacetate...........................................................Banana
Oil
Barium Sulfide.........................................................Black
Ash
Carbon
Carbinate...........................................................Chalk
Carbontetrachloride...............................................Cleaning
Fluid
Calcium Hypochloride............................................Bleaching
Powder
Calcium
Oxide...............................................................Lime
Calcium
Sulfate.................................................Plaster of Paris
Carbonic Acid............................................................Seltzer
Cetyltrimethylammoniumbromide......................................Ammonium
Salt
Ethylinedichloride...................................................Dutch
Fluid
Furfuraldehyde..........................................................Bran
Oil
Glucose...............................................................Corn
Syrup
Graphite.............................................................Pencil
Lead
Hydrochloric
Acid..................................................Muriatic Acid
Hydrogen
Peroxide.......................................................Peroxide
Lead
Acetate.......................................................Sugar of Lead
Lead
Tero-oxide.........................................................Red Lead
Magnesium
Silicate..........................................................Talc
Magnesium
Sulfate.....................................................Epsom Salt
Methylsalicylate................................................Winter
Green Oil
Naphthalene............................................................Mothballs
Phenol.............................................................Carbolic
Acid
Potassium
Bicarbonate............................................Cream of Tarter
Potassium Chromium Sulfate............................................Chromealum
Potassium
Nitrate.....................................................Salt Peter
Sodium
Oxide................................................................Sand
Sodium Bicarbonate...................................................Baking
Soda
Sodium
Borate..............................................................Borax
Sodium
Carbonate....................................................Washing Soda
Sodium Chloride.............................................................Salt
Sodium
Hydroxide.............................................................Lye
Sodium
Silicate............................................................Glass
Sodium Sulfate....................................................Glauber's
Salt
Sodium
Thiosulfate...........................................Photographer's Hypo
Sulfuric
Acid.......................................................Battery Acid
Sucrose...............................................................Cane
Sugar
Zinc
Chloride.....................................................Tinner's Fluid
Zinc
Sulfate.......................................................White Vitriol
5.0 LISTS OF SUPPLIERS AND MORE
INFORMATION
Most, if not all, of the information in this
publication can be obtained through a public or university library. There
are also many publications that are put out by people who want to make money by
telling other people how to make explosives at home. Adds for such appear
frequently in paramilitary magazines and newspapers. This list is
presented to show the large number of places that information and materials can
be purchased from. It also includes
fireworks companies and the like.
COMPANY NAME AND
ADDRESS
WHAT COMPANY SELLS
________________________
__________________
FULL AUTO CO.
INC.
EXPLOSIVE RECIPES,
P.O. BOX
1881
PAPER TUBING
MURFREESBORO, TN
37133
_______________________________________________________________________________
UNLIMITED
CHEMICALS AND FUSE
BOX 1378-SN
HERMISTON, OREGON
97838
_______________________________________________________________________________
AMERICAN FIREWORKS
NEWS
FIREWORKS NEWS MAGAZINE WITH
SR BOX
30
SOURCES AND TECHNIQUES
DINGMAN'S FERRY, PENNSYLVANIA
18328
_______________________________________________________________________________
BARNETT INTERNATIONAL
INC.
BOWS, CROSSBOWS, ARCHERY MATERIALS,
125 RUNNELS
STREET
AIR RIFLES
P.O. BOX 226
PORT HURON, MICHIGAN
48060
_______________________________________________________________________________
CROSSMAN AIR
GUNS
AIR GUNS
P.O. BOX 22927
ROCHESTER, NEW YORK
14692
_______________________________________________________________________________
EXECUTIVE PROTECTION PRODUCTS INC. TEAR GAS GRENADES,
316 CALIFORNIA
AVE.
PROTECTION DEVICES
RENO, NEVADA
89509
_______________________________________________________________________________
BADGER FIREWORKS CO.
INC.
CLASS "B" AND "C" FIREWORKS
BOX 1451
JANESVILLE, WISCONSIN
53547
_______________________________________________________________________________
NEW ENGLAND FIREWORKS CO. INC.
CLASS "C" FIREWORKS
P.O. BOX 3504
STAMFORD, CONNECTICUTT
06095
_______________________________________________________________________________
RAINBOW
TRAIL
CLASS "C" FIREWORKS
BOX 581
EDGEMONT, PENNSYLVANIA
19028
_______________________________________________________________________________
STONINGTON FIREWORKS
INC.
CLASS "C" AND "B" FIREWORKS
4010 NEW WILSEY BAY U.25 ROAD
RAPID RIVER, MICHIGAN
49878
_______________________________________________________________________________
WINDY CITY FIREWORKS
INC.
CLASS "C" AND "B" FIREWORKS
P.O. BOX
11
{GOOD PRICES!}
ROCHESTER, INDIANNA
46975
_______________________________________________________________________________
*Any high school or college science or MST classroom has a buch of good
chemicals that are very useful in making many things in this book. Obviously you’l have to steal what you need,
so be careful; if you are caught, you problley be arrested and/or expelled.
_______________________________________________________________________________
Skylighter-http://www.skylighter.com/- Probably the biggest and best
online supplier. They have a massive product selection and good prices.
They have many books and videos on pyrotechnics, as well as high quality pyro
tools. You must be on file with them to order, which means sending a copy of
your drivers license or other ID.
Firefox-http://www.firefox-fx.com/- Similar selection to Skylighter.
They have some products Skylighter does not and vice versa. You must be on file
with them to order.
Iowa Pyro Supply-http://www.iowapyrosupply.com/-I don't really know much about
this place, but they seem to have a good reputation on rec.pyrotechnics. Good
selection and prices, you must be on file to order.
Pyrotek-http://www.pyrotek.org/cgi-bin/newCataloger.cgi- Pyrotek sells a wide variety of
pyro, rocketry and chemistry supplies. They have a large selection and decent
prices. Warning! I have heard some bad things about this place. For example, I
got an email from somebody saying they ordered fuse here, never got it, and did
not get their money back. I have also heard from numerous people who report
having no problems at all. I have ordered from them with no problems.
Dawntreader Pyrotechnics-http://www.dawntreader.net/info.html
- Haven't heard
much about them, but they have quite a few chemicals and decent prices.
Wolter Pyro Tools-http://www.wolterpyrotools.com/index.html
- Nice tools for
rockets, comets etc.
Pyrosupplies.com-http://www.pyrosupplies.com/ - "High quality and hard to
find pyrotechnic supplies"
Precocious Pyrotechnics-http://www.pyro-pro.com/ - Non-chemical supplies like mortar tubes and other cardboard
products.
LORTONE, inc.-http://www.lortone.com/ - Rock tumblers often used as ball mills. Lists local
distributors.
United Nuclear-http://www.unitednuclear.com/-No ID required, they have a lot
of good products, but prices are very high for many things. Shop around before
buying here. The no longer carry things like KClO4 and dark flake Al because
too many losers ordered them and got in trouble.
Stanford Systems Aerospace-http://www.ssaerospace.com/-A rocketry supplier. Warning!
Many people (including myself) have ordered from here and had serious delays or
have not received orders. DO NOT ORDER FROM HERE!
EBay-http://www.ebay.com/ - You can sometimes find chemicals like kno3, sulfur, and
potassium perchlorate here, but prices will most likely not be very good.
Cannonfuse.com-http://www.cannonfuse.com/- They sell fuse and one size of
tubes, along with a few books and plans. You do not have to be on file and can
pay with cash. I have ordered from here with quick service, the price for fuse
is far better than United Nuclear.
Discount Pyro-http://www.discountpyro.com/index.htm- Small selection, but very
cheap. Requires ID. I have ordered here with no problems.
Pyro Plastics-http://www.pyroplastics.net/- Plastic aerial shell casings,
class B shells listed and a mention of expanding to Class C sales.
Pyrohobby-http://www.pyrohobby.com/ - A new supplier, sells a few chemicals and doesnít require ID.
Pyrostuff-http://www.pyrostuff.com
http://www.hummelcroton.com-good source
for ordering chemicals!
http://roguesci.org/megalomania/explosives.html-Really good source of
information on explosives(which is where I got many of the procedures that are
in this book…), any kind of chemicals, and other cool scientific info.
-www.totse.com-Website with info on guns,
explosives, drugs, and other stuff people have sent in(although much information is questionable).
-http://www.armory.com/~spcecdt/pyrotech/pyrotest.html-a cool “pyro purity test”.
http://www.bombshock.com/cgi-bin/ib/ikonboard.cgi-kick-ass
forum, good info. (check it out!)
5.3-BOOKS:
_____
-THE IMPROVISED MUNITIONS MANUAL
-MILITARY
EXPLOSIVES
-FIRES AND EXPLOSIONS
-Modern
Chemical Magic
-Making Reliable Ignition Products
at Home
6.0 Chemical preparation and sources:
6.1 Ammonium chloride:
Formula: NH4Cl
Description: Ammonium chloride is used in
smoke compositions. When heated ammonium chloride decomposes to HCl and NH3,
both gasses. These recombine in the air to give a smoke consisting of fine
particles of ammonium chloride.
Hazards: Ammonium chloride based smoke is
irritating to the eyes and lungs as it contains some remaining HCl and NH3.
Ammonium chloride itself is not poisonous and is even used in some type of
candy. According to Shimizu ammonium chloride forms an exception to the rule
that ammonium compounds should not be mixed with chlorates. Due to the lower
solubility of potassium chlorate (compared to ammonium chlorate) no ammonium
chlorate . I personally would still use these mixtures with great caution (or
avoid them) since it seems inevitable that small amounts of ammonium chlorate
will still form. The lower solubility of potassium chlorate will make it the
-main- product in a double decomposition reaction but not the -only- product.
Sources: Ammonium chloride solution is
easily prepared by neutralising ammonia solution with hydrochloric acid. It is
advised to use a slight excess of ammonia. That is to make sure no remaining
acid will be present in the ammonium chloride obtained on evaporation and
crystallisation. Otherwise traces of the acid solution may be enclosed in the
crystals, possibly leading to spontaneous ignition of mixtures made with it.
6.2 Ammonium nitrate:
Formula: NH4 NO3
Description: Ammonium nitrate is an oxidiser.
It is very hygroscopic and therefore not used very often in fireworks. It finds
some use in composite propellants, but performance is not as good as
perchlorate based propellants.
Hazards: Large masses of ammonium nitrate
have been known to explode on some occasions although it is very unsensitive.
Smaller quantities are less likely to detonate. The risk of detonation
increases when ammonium nitrate is molten or mixed with fuels such as metal
powders or organic substances. Ammonium nitrate should never be mixed with
chlorates as this may result in ammonium chlorate formation, possibly leading
to spontaneous ignition. Mixtures of metal powders and ammonium nitrate are
likely to heat up spontaneously and may ignite, especially when moist. This can
sometimes be prevented by the addition of small amounts of boric acid (1 to
2%), but in general it is better to avoid these mixtures at all. The
hygroscopic nature of ammonium nitrates makes this problem worse.
Sources: Ammonium nitrate solution can be
prepared by neutralising ammonia solution with nitric acid. It is advised to
use a slight excess of ammonia. That is to make sure no remaining acid will be
present in the ammonium nitrate obtained on evaporation and crystallisation.
Otherwise traces of the acid solution may be enclosed in the crystals, possibly
leading to spontaneous ignition of mixtures made with it. Large quantities of
ammonium nitrate can also be cheaply bought as fertilizer. In the Netherlands a
fertilizer called 'kalkammonsalpeter' is sold. This consists of ammonium
nitrate mixed with 'mergel', a mineral consisting mainly of calcium carbonate.
The ammonium nitrate can be extracted with water.
6.3 Ammonium perchlorate:
Formula: NH4ClO4
Description: Ammonium perchlorate is an
oxidiser used in a large number of compositions. Very impressive color
compositions can be made with it, but their burn rate is often too low for use
in star compositions. For lancework and torches slow burning is an advantage
and it is therefore commonly used in these items. Ammonium perchlorate is also
used in composite rocket propellants, including the propellants used in the
solid propellant boosters used for the space shuttle. The decomposition
products of ammonium perchlorate are all gasses which is very beneficial for
rocket propellants.
Hazards: Ammonium perchlorate can
detonate by itself, although it is not very sensitive. Larger amounts and
mixtures of ammonium perchlorate with metal powders or organic substances are
more likely to detonate.
Sources: Ammonium perchlorate is usually
bought from chemical suppliers or from dedicated pyro suppliers. Fine ammonium
perchlorate powder is a regulated substance in most countries and cannot easily
be bought or transported. Since it is such a usefull chemical in pyrotechnics
it can be worth the time and effort to try to prepare it at home. This can be
done by first making sodium perchlorate followed by double decomposition with
ammonium chloride (other ammonium compounds can be used). The preparation of
sodium perchlorate is most easily accomplished by electrolysis, the procedure
for which is described elsewhere on this page.
6.4 Barium carbonate:
Formula: BaCO3
Description: Barium carbonate is used both in
white and green color compositions. When chlorine donors are present in a
composition a green color will result from the formation of BaCl+ in
the flame. Without chlorine donors BaO will be formed which emits white light.
Barium carbonate is convenient to use in chlorate based color compositions
since it will neutralize residual acid which reduces the risk of spontaneous
ignition.
Hazards: Most barium compounds are very
poisonous, especially the more soluble barium compounds such as the chlorate
and nitrate. A dust mask should be worn at all times when working with barium
carbonate.
Sources: Barium carbonate is cheaply
available in kilogram quantities from ceramic supply shops. However, this
material is often contaminated with small amounts of barium sulfide which are
left over from the production process. Therefore, ceramics grade barium
carbonate should never be used in mixtures incompatible with sulfides such as
chlorate based mixtures. Barium carbonate is not easily made at home.
6.5 Barium chlorate:
Formula: BaClO3
Description: Barium chlorate is used as an
oxidiser in green color compositions. Fierce burning and high color purity
compositions can be made with it.
Hazards: Barium chlorate is poisonous and
a dust mask should be worn at all times when handling it. Barium chlorate
should never be mixed with sulfur or sulfides or allowed to come in contact
with mixtures containg sulfur or sulfides since this could result in
spontaneous ignition. (Sulfur reacts with water and air to form small amounts
of sulfuric acid. Sulfuric acid and chlorates react producing ClO2, an
explosive gas which will ignite many organic materials on contact). Mixtures
made with barium chlorate are often especially sensitive to friction and shock
(even more so than potassium chlorate based mixtures) and should be handled
with extra care.
Sources: Barium chlorate is usually
purchased from chemical suppliers or from dedicated pyro suppliers. It can be
made at home from sodium chlorate and barium chloride by double decomposition.
Barium chlorate can also be prepared from barium chloride by electrolysis in a
process analogous to that used for preparing sodium chlorate.
6.6 Barium nitrate:
Formula: BaNO3
Description: Barium nitrate is used as an
oxidiser in both white and green color compositions. When chlorine donors are
present in a composition a green color will result from the formation of BaCl+
in the flame. Without chlorine donors BaO will be formed which emits bright
white light. Barium nitrate is seldom used as the sole oxidiser in green color
compositions. It is usually combined with perchlorates to improve the color and
increase the burning rate.
Hazards: Barium nitrate is poisonous and
a dust mask should be worn at all times when handling it. Mixtures of metal
powders and barium nitrate sometimes heat up spontaneously and may ignite,
especially when moist. This can usually be prevented by the addition of small
amounts of boric acid (1 to 2%). It is advisable to avoid using water to bind
such compositions. Red gum or shellac with alcohol or nitrocellulose lacquer
are preffered binder and solvents.
Sources: Barium nitrate may be prepared
from nitric acid or ammonium nitrate and barium carbonate, which is available
from ceramic supply stores.
6.7 Barium sulfate:
Formula: BaSO4
Description: Barium sulfate is used as a
high-temperature oxidiser in some metal based green color compositions.
Hazards: Unlike many other barium
compounds, barium sulfate is not very poisonous due to its low solubility in
water.
Sources: Barium sulfate may be
precipitated from a solution of a soluble barium salt, such as barium nitrate
or chloride, and a sulfate. Magnesium and potassium sulfate are both cheaply
available as fertilizer and are convenient to use. The precipitated barium
sulfate is a very fine powder which may be rinsed by repeated washings with hot
water, settling and decanting. A final washing in the filter with acetone or
ethanol will allow it to dry quickly. Do not use sulfuric acid to precipitate
barium sulfate as this may result in the inclusion of acid droplets in the
precipitated particles which can lead to spontaneous ignition of some mixtures.
6.8 Boric acid:
Formula: H3BO3
Description: Boric acid is a white powder
which is used as an additive to compositions containing aluminum or magnesium
and a nitrate. The metal powder can reduce the nitrate to an amide which will
react with the metal powder in a very exothermic reaction that can lead to
spontaneous ignition of the composition. This process is often accompanied by a
smell of ammonia and is most likely to occur with wet compositions. Addition of
a few percent boric acid can often prevent this reaction from taking place
since it neutralizes the very basic amides forming ammonia and a borate. It is
also advisable to avoid using a water soluble binder for these composition.
Using red gum or shellac with alcohol or nitrocellulose lacquer is safer.
Hazards: Boric acid is not particularly
toxic or dangerous.
Sources: Boric acid is cheaply and in
kilogram quantities available from ceramic supply shops. It is also sold in
many drug stores at a somewhat higher price, but since only small quantities
are needed the price is not really important.
6.9 Calcium sulphate:
Formula: CaSO4.x H2O
where x= 0, 2, 3 or 5
Description: The trihydrate is commonly known
as plaster of paris. The dihydrate occurs as a mineral known as gypsum . Calcium
sulphate can be used as a high temperature oxidiser in orange color
compositions. Excellent strobe compositions can be made with it.
Hazards: Calcium sulphate is not
particularly toxic or dangerous.
Sources: Plaster can be used as is in
strobe compositions, but is better to remove the water which is easily
accomplished by heating.
6.10 Dextrin:
Formula: mixture of polysacharides
Description: Dextrine is one of the most
commonly used binders in pyrotechincs as it is very cheap and readily
available. It is water soluble and can produce rock hard stars.
Hazards: Colophonium is not particularly
toxic or dangerous.
Sources: Dextrine is easily prepared from
starch. Potato and corn starch will both work fine. The starch is spread out on
a sheet in a layer about 1 cm thick and placed in the oven. The oven is then
heated to 220°C for several hours. The dextrine will turn slightly yellowish
brown. One way to check if all the starch has been converted is to dissolve a
small sample in boiling hot water and add a drop of KI3 solution. A
blue color indicates presence of starch, which means the conversion hasn't
completed yet. KI3 solution is conveniently prepared by dissolving a
crystal of elemental iodine in a potassium iodide solution.
6.11 Ethanol:
Formula: CH3CH2OH
Description: Ethanol is used as a solvent.
Red gum and shellac, two common binders both dissolve in ethanol well.
Ethanol/water mixtures are also often used since the ethanol increases the
'wetness' of the water (it reduces the surface tension of the water) and
reduces the solubility of common oxidisers.
Hazards: Ethanol is flammable and
volatile. Ethanol vapour is heavier than air and spreads over the ground.
Provide adequate ventilation when working with ethanol.
Sources: Chemically pure ethanol can be
quite expensive due to increased tax, unless it is used for laboratory
purposes. Denaturated alcohol (usually a mixture of ethanol and methanol) has
been made undrinkable and therefore a lot cheaper. It can be used for pyro
purposes. Some types of denaturated alcohol exist with other chemicals mixed in
besides methanol to make it undrinkable and recognisable as such (colorants
etc). I have no idea what these extra additives are and wheter they can cause
problems in compositions. I have been using 'spiritus' (a well known type of
denaturated alcohol in the Netherlands) for several years without problems.
6.12 Iron:
Formula: Fe
Description: Iron powder is used for spark
effects, mainly in fountains and sparklers. It produces golden yellow branching
sparks. Not every iron alloy will work equally well. Iron alloys with a high
carbon content generally work best. Stainless steel will produce hardly any
sparks.
Hazards: Iron needs to be protected
before use in pyrotechnic compositions. Otherwise it will corrode and render
the composition useless or even dangerous. Iron containing compositions are
generally best kept dry and not bound with water soluble binders. Iron can be
coated with linseed or tung oil. The latter was used in ancient China (and may
still be used today). Linseed is very convenient to use and easy to obtain.
Blackpowder-like compositions (ie Charcoal/sulfur/saltpeter based) with added
metal, such as they are often used in fountains, are more sensitive than the
composition without added metal. Extra caution, especially when pressing or
ramming, should be excersised.
Sources: Iron turnings can often be had
for free from places were iron is used for construction. Drilling, sawing etc
produces a powder with wide range of particles. This powder is treated with
mineral oil to remove oil and grease, sieved, and then coated with linseed oil.
6.13 Iron oxide (red):
Formula: Fe2O3
Description: Red iron oxide is used as a
catalyst in composite and whistling rocket propellant formulations. It is also
added to some glitter formulations and used for 'thermite', a mixture that
produces enormous amounts of heat, forming molten iron.
Hazards: Red iron oxide is not
particularly toxic or dangerous.
Sources: Common rust is not iron oxide.
It is a mixture of oxides and hydroxides. A cheap source for red iron oxide is
the ceramics supply shop.
6.14 Lead tetraoxide:
Formula: Pb3O4
Description: Lead tetraoxide, sometimes
called 'lead minium', is used to make crackling microstars. The composition is
very sensitive, explosive and poisonous. It is in fact one of the most
dangerous mixtures used commonly in modern pyrotechnics. An alternative mixture
based on bismuth trioxide exists (which is less poisonous), but the high price
of bismuth trioxide restricts its use.
Hazards: Lead tetraoxide, like most lead
compounds, is extremely poisonous. Lead is an accumulative neurotoxin and
extreme care should be taken to prevent direct contact. Lead tetraoxide may be
absorbed by inhalation and ingestion. Wear a respirator, gloves, and protective
clothing.
Sources: Lead tetraoxide may be prepared
from a solution of lead nitrate and sodium hydroxide. Note that the procedure
involves extremely corrosive and poisonous chemicals and should only be
attempted by those who have access to (and know how to use) the right equipment
and can handle the waste properly. Prepare a concentrated solution of sodium
hydroxide by dissolving 300 grams of sodium hydroxide in water. The solution
will heat up during this. To prevent it from boiling suddenly add only small
portions at a time. When all has dissolved, allow it to cool down to room
temperature. Dissolve 50 grams of lead nitrate in 200 ml of water, and slowly
add the sodium hydroxide solution to this solution while stirring continuesly.
A white precipitate will form first, which will turn orange when all sodium
hydroxide solution has been added. Stir this solution well for another hour,
and then allow the lead tetraoxide to settle. Carefully decant the supernatant,
add boiling hot water to the residue, stir, allow to settle and decant again.
Repeat this 5 more times. Then filter and rinse the lead tetraoxide in the
filter several times with hot water.
6.15 Manganese dioxide:
Formula: MnO2
Description: Manganese dioxide can be used as
a catalyst in composite and whistling rocket propellant formulations. A
thermite-like mixture can also be made with it. The manganese dioxide thermite
burns more slowly than the iron oxide based mixture with a bright white glow.
Hazards: Mangese dioxide is poisonous and
leaves brown stains on glassware etc. The stains can be removed with dilute
hydrochloric acid (of course, only when the stained object is not attacked by
it).
Sources: Mangese dioxide can be obtained
from old batteries or from the ceramics supply store. The mangese dioxide in
batteries is mixed with several other compounds from which it must be
separated. An easy, though messy way to do this is as follows: Find a couple of
depleted carbon-zinc batteries. Only carbon-zinc type batteries will do. Do not
use other types such as rechargable or lithium based batteries. These,
especially the rechargable ones, contain extremely dangerous and/or poisonous
compounds such as cadmium, mercury and metallic lithium. Carbon-zinc batteries
may contain small amounts of mercury as well, especially the older types, so
precautions should be taken to prevent skin and eye contact and to prevent
breathing or swallowing of dust. So: wear your dust mask, glasses, gloves and
old clothing. Then carefully take the battery apart. You'll find a greyish
white (zinc oxide) or metallic coating (zinc metal) inside, depending on wheter
the battery is empty or not. This surrounds a black, sometimes wet, mass. This
black stuff contains among other things the mangese dioxide. Peel the coating
off and save the black mass. There is also a black rod inside attached to the
anode. This is a graphite rod and can be safed for chlorate (and maybe
perchlorate) preparations. We'll assume you use 2 batteries from here on. (if
not, adjust amounts accordingly). Place the black mass in 200 ml of 30%
hydrochloric acid. The manganese dioxide will slowly dissolve, giving off
chlorine gas. Chlorine gas is dangerous: it attacks the lungs and is poisonous.
Do this outside or better yet: in a fume hood if you have one. Allow the
manganese dioxide several days to dissolve. The solution is then filtered which
should yield a clear solution of manganese(III)chloride. In a separate
container dissolve 200 grams of sodium hydroxide in a liter of bleach. Add the
manganese(III)chloride solution slowly to the bleach/sodium hydroxide solution.
This results in a brown precipitate of manganese dioxide which is filtered,
rinsed several times with boiling hot water and dried.
6.16 Magnalium:
Formula: Alloy of magnesium and aluminum,
usually 50:50. Sometimes written: MgAl
Description: Magnalium is a very brittle
alloy of magnesium and aluminum. Some common uses are in for spark effects, in
strobing compositions and in crackling stars. It is commonly alloyed in
Hazards: Magnalium dust is harmfull and a
dust mask should be worn when handling fine dust. Mixtures containing nitrates
and mangalium sometimes heat up and may ignite spontaneously, especially when
moist. This can usually be prevented by treating the magnalium with potassium
dichromate. This is done by boiling the magnalium in a 5% potassium dichromate
solution. Adding fine potassium dichromate powder to such compositions may also
help.
Sources: Magnalium can be made at home.
Plan well and prepare yourself for working with molten metals that may ignite
if you plan to make it at home. If the metal ignites expect it to burn very
brightly and hot. Explosions are not common but may occur if the hot melt is
allowed to contact water or oxidisers. Do it outside and away from anything
flammable. If it ignites don't try to extuingish it but get away from the
burning mass and let it burn out and cool before approaching it. Don't look
directly into the burning metal as it may damage your eyes. Start by melting
aluminum in a stainless steel container. The molten metal should be covered
with a blanked of inert gas. In this case neither nitrogen nor carbon dioxide
will function as an inert gas. It is best to get a cylinder of argon gas at a
welding supply store. Using an electric furnace for the melting is very
convenient and allows good control over the temperature. To the molten aluminum
magnesium is added in solid form. The melt should be stirred from time to time.
When all the magnesium has melted, the melt is allowed to solidify. It is then
easily crushed up in smaller chunks with an heavy hammer. These chunks are
crushed further and sieved. It can also be ball milled into a fine powder using
steel media but this can be dangerous since the metal powder can become
pyrophoric.
6.17 Magnesium:
Formula: Mg
Description: Magnesium powder is used in a
wide variety of compositions, both for spark effects and 'normal' fuel
purposes. Relatively coarse magnalium is used for spark effects. In flares and
some bright colored star compositions it functions as a normal fuel. It is
superior to aluminum in color compositions since MgCl2 and MgO are more easily
vaporised than the corresponding aluminum compounds. This reduces the amount of
black-body radiation and improves the color purity.
Hazards: Magnesium dust is harmfull and a
dust mask should be worn when handling fine dust. Mixtures containing nitrates
and magnesium sometimes heat up and may ignite spontaneously, especially when
moist. This can usually be prevented by treating the magnesium with potassium
dichromate. This is done by boiling the magnalium in a 5% potassium dichromate
solution. The magnesium will turn brown when this is done. Adding fine
potassium dichromate powder to such compositions may also help.
Sources: Making magnesium at home is very
difficult. Magnesium can be bought in boating supply stores. It is used to
prevent corrosion of a ships hull. For that purpose it is welded to the hull.
The lower position of magnesium in the electrochemical series will make the
magnesium corrode before the steel will. Making such a block of magnesium into
a fine powder will not be easy. Filing or cutting and ball milling may be
tried. Ball milling of metals can be dangerous however since the metal can
become pyrophoric.
6.18 Methanol:
Formula: CH3OH
Description: Methanol is used as a solvent,
much in the same way ethanol is used. Red gum and shellac, two common binders
both dissolve in methanol. Methanol/water mixtures are also often used since
the methanol increases the 'wetness' of the water (it reduces the surface
tension of the water) and reduces the solubility of common oxidisers.
Hazards: Methanol is flammable, volatile
and toxic. Methanol vapour is heavier than air and spreads over the ground.
Provide adequate ventilation when working with methanol
Sources: Methanol is often more cheaply
and easily availble than ethanol because it is toxic and no extra taxes are
charged for it. It finds use in a certain type of camping stove and can often
be bought in camping supply stores.
6.19 Parlon:
Formula: (C4H6Cl2)n
Description: Parlon is a acetone-soluble
polymere that is used as a chlorine donor and binder. It is a good example of
one of the new chemicals that has become available in the past few decades for
use in compositions.
Hazards: Parlon is not particularly dangerous.
Sources: Parlon seems to be available
from dedicated pyro suppliers only.
6.20 Potassium benzoate:
Formula: KC7H5O2
Description: Potassium benzoate is commonly
used in whistle compositions. It is a white powder
Hazards: Potassium benzoate is not particularly
dangerous.
Sources: Potassium benzoate can be
prepared from benzoic acid and potassium carbonate or hydroxide. Benzoic acid
is not very soluble, but both potassium carbonate and hydroxide are. Dissolve
140.2g potassium carbonate or 56.1g potassium carbonate in 250 ml water, and
add 146g benzoic acid. Bring the mixture to a boil. If potassium carbonate is
used, CO2 gas will evolve. Continue boiling untill all benzoic acid
has dissolved, occasionally adding some water to make up for what has evaporated.
When all benzoic acid has dissolved, continue boiling untill the first crystals
of potassium benzoate are observed (ie the saturation point has been reached).
Then allow the solution to cool to room temperature. Potassium benzoate will
crystalise in needle shaped crystals. Filter, and rinse the crystals twice with
ice-cold water. The crystals may be dried in an oven at 100 deg C.
6.21 Potassium chlorate:
Formula: KClO3
Description: Potassium chlorate is a very
common oxidiser in pyrotechnics, even though it has some treacherous properties
and other oxidisers would sometimes be safer to use. Part of the reason of its
popularity in commercial pyrotechnics is that it is cheap and easily available.
The large scale production of this compound made the first quality colored
fireworks possible, about a century ago.
Hazards: Potassium chlorate is toxic, and
breathing protection should be worn when handling fine powder. Compositions
made with potassium chlorate tend to be more sensitive than those based on nitrates
and perchlorates and should therefore be handled accordingly. Potassium
chlorate, or any chlorate for that matter, should never be used in combination
with sulfur and sulfides. Mixtures containing both are very sensitive and may
spontaneously ignite. In general, when using chlorates great care should be
taken to avoid contamination of other compositions or tools. Also read the safety
section for more information on this problem.
Sources:
Potassium
chlorate can be prepared at home. For this purpose, sodium chlorate is prepared
first by electrolysis. It may also be obtained as a herbicide in some countries
(France, for example) Then, by double decomposition with potassium chloride,
potassium chlorate is prepared from this solution. The product is recrystallised,
dried and powdered.
This chemicals is used in many explosives. Potassium chlorate can also be made into
plastique explosives(*See Chapter 8-High Order Explosives). Common household bleach contains a small
amount of potassium chlorate, which can be extracted in the procedure that
follows.
Materials:
-A heat source (hot
plate, stove, etc.)
-A hydrometer, or
battery hydrometer
-A large Pyrex, or
enameled steel container (to weigh chemicals)
-Potassium
chloride(sold as a salt substitute at health and nutrition stores)
Procedure:
Take one gallon of bleach, place it in the container, and begin
heating it. While this solution heats, weigh out 63 grams of potassium chloride
and add this to the bleach being heated. Constantly check the solution being
heated with the hydrometer, and boil until you get a reading of 1.3. If using a
battery hydrometer, boil until you read a FULL charge.
Take the solution and allow it to cool in a refrigerator until it
is between room temperature and 0øC. Filter out the crystals that have formed
and save them. Boil this solution again and cool as before. Filter and save the
crystals.
Take the crystals that have been saved, and mix them with
distilled water in the following proportions: 56 grams per 100 milliliters distilled
water. Heat this solution until it boils and allow to cool. Filter the solution
and save the crystals that form upon cooling. This process of purification is
called "fractional crystallization". These crystals should be
relatively pure potassium chlorate.
*Powder these to the consistency of face powder, and heat gently
to drive off all moisture.
6.22 Potassium dichromate:
Formula: K2Cr2O7
Description: Potassium dichromate is a bright
orange crystalline subststance that is used to treat magnesium powder. The
treatment makes magnesium more resistant to spontaneous reactions that could
result in lower reliability of the mixture or spontaneous ignition.
Hazards: Potassium dichromate is toxic
and a carcinogen. It should be handled with extreme care and proper protective
clothing.
Sources: Potassium dichromate seems to be
available from chemical suppliers and dedicated pyro suppliers only.
6.23 Potassium perchlorate:
Formula: KClO4
Description: Potassium perchlorate is a very
common oxidiser in pyrotechnics. Composition based on perchlorates tend to be
less sensitive than those based on chlorates, and perchlorates can be used with
sulfur and sulfides. For these reasons potassium perchlorate is much preferred
above chlorates. Drawback is its slightly higher price.
Hazards: Potassium perchlorate is toxic,
and breathing protection should be worn when handling fine powder.
Sources:Potassium perchlorate can be
prepared at home. For this purpose, sodium perchlorate is prepared first by
electrolysis. Then, by double decomposition with potassium chloride, potassium
perchlorate is prepared from this solution. The product is recrystallised,
dried and powdered.
6.24 Potassium Picrate:
Description: Potassium picrate was first
prepared back in the mid 17th century by J.R. Glauber. The first use for
potassium picrate came in 1869, it found its way into explosives, propellents,
primers, and pyrotechnics. This explosive is stable and resists shock,
friction, etc. It will deflagrate if subjected to flame, and in mixtures with
oxidizing agents, it will only burn if ignited, but it has lower sensitivity.
This is not a very powerful explosive, it is more suited to pyrotechnics and
bullet primers.
CHEMICALS
APPARATUS
nitric
acid beaker
picric
acid
potassium
carbonate
Potassium picrate can
be prepared by Glaubers original method of dissolving wood in nitric acid then
neutralizing the resulting mixture with potassium carbonate. For the modern
method, neutralize a hot aqueous solution of potassium carbonate with a hot
picric acid solution in a beaker of suitable size, test the solution with
litmus paper until neutral. Filter the crystals that separate when the solution
cools to collect them and allow to dry.
6.25 Polyvinyl chloride:
Formula: [C2H3Cl]n
Description: Like parlon and saran, PVC is a
polymeric chlorine donor and fuel. It can be used in the form of a fine powder
or as a solution in tetrahydrofuran (THF). It is sometimes used as a binder,
but it is very brittle. Small amounts of plasticiser (dioctyl phtalate is
common) may be added to improve the mechanical properties.
Hazards: PVC itself is not particularly
dangerous or toxic. Dioctyl phtalate is a suspected carcinogen however and THF
is a very flamable and volatile liquid.
Sources: As an alternative to the PVC
powder available from chemical suppliers and dedicated pyro suppliers, PVC glue
may also be used. It is usually sold in hardware stores and comes in two
varieties: gelling or gap-filling and normal. Both are essentially a
concentrated solution of PVC. I have no experience with the gelling variety,
but the normal variety can succesfully be used in compositions. The gelling
variety may be better suited for pyro purposes since it seems it contains more
PVC. Another possibility is to use 'Sculpy' or 'Fimo' clay. These modelling
clays consist of PVC with a large amount of plasticiser. The plasticiser may
affect the color of a composition negatively, but reasonable results can still
be obtained with it. It can simply be kneaded into a composition with some
effort. This type of clay is usually hardened by heating it in an oven, but do
not be tempted to do this with pyrotechnic mixtures as they may ignite.
6.26 PICRIC ACID:
Picric acid, also known as Tri-Nitro-Phenol, or T.N.P., is a military explosive that is most often used as a booster charge to set off another less sensitive explosive, such as T.N.T. It another explosive that is fairly simple to make, assuming that one can acquire the concentrated sulfuric and nitric acids. Its procedure for manufacture is given in many college chemistry lab manuals, and is easy to follow. The main problem with picric acid is its tendency to form dangerously sensitive and unstable picrate salts, such as potassium picrate. For this reason, it is usually made into a safer form, such
as ammonium picrate, also called explosive D. A social deviant would probably use a formula similar to the one presented here to make picric acid.
MATERIALS EQUIPMENT
_________ _________
phenol (9.5 g) 500 ml flask
concentrated adjustable heat source
sulfuric acid (12.5 ml)
1000 ml beaker
concentrated nitric or other container
acid (38 ml) suitable for boiling in
distilled water filter paper
and funnel
glass stirring rod
1) Place 9.5 grams of phenol into the 500 ml flask, and carefully add 12.5
ml of concentrated sulfuric acid and stir the mixture.
2) Put 400 ml of tap water into the 1000 ml beaker or boiling container and
bring the water to a gentle boil.
3) After warming the 500 ml flask under hot tap water, place it in the boiling
water, and continue to stir the mixture of phenol and acid for about thirty
minutes. After thirty minutes, take the flask out, and allow it to cool for
about five minutes.
4) Pour out the boiling water used above, and after allowing the container to
cool, use it to create an ice bath, similar to the one used in section 3.13,
steps 3-4. Place the 500 ml flask with the mixed acid an phenol in the ice
bath. Add 38 ml of concentrated nitric acid in small amounts, stirring the
mixture constantly. A vigorous but "harmless" reaction should occur. When
the mixture stops reacting vigorously, take the flask out of the ice bath.
5) Warm the ice bath container, if it is glass, and then begin boiling more tap
water. Place the flask containing the mixture in the boiling water, and heat
it in the boiling water for 1.5 to 2 hours.
6) Add 100 ml of cold distilled water to the solution, and chill it in an ice
bath until it is cold.
7) Filter out the yellowish-white picric acid crystals by pouring the solution
through the filter paper in the funnel. Collect the liquid and dispose of it
in a safe place, since it is corrosive.
8) Wash out the 500 ml flask with distilled water, and put the contents of the
filter paper in the flask. Add 300 ml of water, and shake vigorously.
9) Re-filter the crystals, and allow them to dry.
10) Store the crystals in a safe place in a glass container, since they will
react with metal containers to produce picrates that could explode
spontaneously.
6.27 Red gum:
Formula: Mixture of compounds.
Description: Red gum, or accaroid resin, is
one of the most commonly used binders. It is made from the excretions of a
certain tree native to Australia. Red gum is soluble in ethanol and acetone.
Hazards: Red gum is not particularly
dangerous or toxic.
Sources: Red gum may be bought in
artistic painting supply stores.
6.28 Sodium benzoate:
Formula: NaC7O2H5
Description: Sodium benzoate is a white solid
that is used as a fuel. It's most common use is in 'whistle mix', a mixture of
potassium perchlorate and either sodium or potassium benzoate.
Hazards: Sodium benzoate is not
particularly dangerous or toxic.
Sources: Sodium benzoate can be made from
sodium carbonate (soda) or sodium hydroxide and benzoic acid which is often
more easily available than it's salts. Benzoic acid is only sparingly soluble
in water. Dissolve either 425 g hydrated sodium carbonate (common household
soda) or 30 g sodium hydroxide in water. Add 100 g of benzoic acid and boil the
solution. The benzoic acid will slowly dissolve. During boiling, occasionally
add water to make up for what has evaporated. If sodium carbonate was used,
carbon dioxide gas will evolve. After all the benzoic acid has dissolved,
continue boiling allowing the water to evaporate untill crystallisation begins.
Then stop heating and allow the solution to cool slowly to room temperature.
Needle-shaped crystals of sodium benzoate will form upon cooling. Cool the
solution further to 0 deg C, filtrate and rinse the crystals with ice-cold
water. Purify the product by recrystallisation from water.
6.29 Sodium chlorate:
Formula: NaClO3
Description: Sodium chlorate is hardly ever
used in pyrotechnics, since it is very hygroscopic. It finds occasional use in
composite rocket propellants. It is however very usefull as a starting point in
the preparation of several other (less hygroscopic) chlorates for which reason
it is included here.
Hazards: Sodium chlorate is toxic, and
breathing protection should be worn when handling fine powder. Compositions
made with sodium chlorate tend to be more sensitive than those based on
nitrates and perchlorates and should therefore be handled accordingly. Sodium
chlorate, or any chlorate for that matter, should never be used in combination
with sulfur and sulfides. Mixtures containing both are very sensitive and may
spontaneously ignite. In general, when using chlorates great care should be
taken to avoid contamination of other compositions or tools. Also read the
safety section for more information on this problem. Acidic solutions
containing chlorates generate a very poisonous and explosive gas, ClO2.
Sources:Sodium chlorate can be prepared
at home. It involves electrolysing a sodium chloride solution under certain
circumstances. A description of the process, cell and anode design, etc. for
home produciton may be found in the chlorate and perchlorate section of this
page. In some countries, France for example, sodium chlorate may be obtained as
a herbicide.
6.30 Sodium nitrate:
Formula: NaNO3
Description: Sodium nitrate finds occasional
use as an oxidiser in flare and tracer compositions because of the high
efficiency of light emmision that can be obtained with it, but its high hygroscopic
nature limits its use. Sodium nitrate can be used to prepare potassium nitrate,
a much less hygroscopic and more often used oxidiser.
Hazards: Sodium nitrate is not
particularly dangerous or toxic.
Sources: 95% pure sodium nitrate is
available as a fertilizer. In the Netherlands this fertilizer is sold under the
name 'chilisalpeter'. If required, it can be easily purified by
recrystallisation.
6.31 Sodium perchlorate:
Formula: NaClO4
Description: Sodium perchlorate is hardly
ever used in pyrotechnics, since it is very hygroscopic. It finds occasional
use in composite rocket propellants. It is however very usefull as a starting
point in the preparation of several other (less hygroscopic) perchlorates for
which reason it is included here.
Hazards: Sodium perchlorate is toxic, and
breathing protection should be worn when handling fine powder.
Sources:Sodium perchlorate can be
prepared at home. It involves electrolysing a sodium chlorate solution under
certain circumstances. A description of the process, cell and anode design,
etc. for home produciton may be found in the chlorate and perchlorate section
of this page.
6.32 Strontium carbonate:
Formula: SrCO3
Description: Strontium carbonate is used in
combination with chlorine donors to produce red colors. It also acts as an acid
neutraliser, for which reason it is prefered in chlorate based compositions
(which may spontaneously ignite when traces of acid are present).
Hazards: Strontium carbonate is not
particularly dangerous or toxic.
Sources: Strontium carbonate is cheaply
available in kilogram quantities from ceramic supply shops. However, this
material is often contaminated with small amounts of strontium sulfide which
are left over from the production process. Therefore, ceramics grade strontium
carbonate should never be used in mixtures incompatible with sulfides such as
chlorate based mixtures. Strontium carbonate is not easily made at home.
6.33 Strontium nitrate:
Formula: Sr(NO3)2
Description: Strontium nitrate is an oxidiser
commonly employed in red color compositions in combination with chlorine
donors.
Hazards: Strontium nitrate is not
particularly dangerous or toxic.
Sources: Strontium nitrate may be
prepared from nitric acid or ammonium nitrate and strontium carbonate, which is
available from ceramic supply stores. Use an excess of strontium carbonate to
ensure complete neutralisation of acid and recrystallise the product from a
slightly alkaline solution to prevent the inclusion of acid solvent droplets in
the crystals.
6.34 Strontium sulfate:
Formula: SrSO4
Description: Strontium sulfate is used as a
high-temperature oxidiser in some metal based red color compositions.
Hazards: Strontium sulfate is not
particularly dangerous or toxic.
Sources: Strontium sulfate may be
precipitated from a solution of a soluble strontium salt, such as strontium
nitrate or chloride, and a sulfate. Magnesium and potassium sulfate are both
cheaply available as fertilizer and are convenient to use. The precipitated
strontium sulfate is a very fine powder which may be rinsed by repeated
washings with hot water, settling and decanting. A final washing in the filter
with acetone or ethanol will allow it to dry quickly. Do not use sulfuric acid
to precipitate strontium sulfate as this may result in the inclusion of acid
droplets in the precipitated particles which can lead to spontaneous ignition
of some mixtures.
6.35 Sulfuric acid:
Formula: H2SO4
Description: Sulfuric acid itself finds no
use in pyrotechnics, but it can be used in the preparation of an number of usefull
compounds for which reason it is included here.
Hazards: Sulfuric acid and its fumes are
extremely corrosive. Wear proper protective clothing (gloves, apron and a face
shield are minimal) and provide adequate ventilation when working with it.
Reactions with metals often produce flammable hydrogen gas (hydrogen). The
presence of acid can cause spontaneous reactions in many pyrotechnic mixtures
and should at all times be avoided. When working with sulfuric acid, have no
chemicals or compositions nearby to prevent contamination. Make sure all traces
of acid in chemicals produced with sulfuric acid are removed if they are to be
used in pyrotechnics compositions.
Sources: Sulfur is available from
agricultural supply stores where it is sold as a fungicide under the name
'dusting sulfur'. It is a fine powder mixed with a few percent of calcium
carbonate. The calcium carbonate may disturb delicate color compositions, but
for most purposes dusting sulfur works well. If a purer form of sulfur is
required, sulfur may also be obtained from drug stores sometimes. However,
these often sell 'flowers of sulfur', which has been purified by sublimation
and which contains some acid. This needs to be neutralised before use as it
could cause spontaneous ignition. To do this, allow 100g of this sulfur to soak
in a liter of water/household ammonia (1:5). Stir well occasionally and measure
the pH. It should still be alkaline after two days, after which time the sulfur
may be filtered and washed with hot water to remove the ammonia. Check the pH
of the washing water while filtering. After it has become neutral, flush the
water away with ethanol and allow the sulfur to dry. Mix the dry powder with 2%
magnesium carbonate to neutralise any acid that may be formed in reactions with
the atmosphere.
6.36 Zinc:
Formula: Zn
Description: Metallic zinc is used in rocket
propellants, for spark effects and in white smoke compositions. Zinc powder is
quite heavy and zinc-based stars often require heavier lift or burst charges to
propell them.
Hazards: Zinc powder can spontanesouly
heat up when wet.
Sources: Zinc powder is used in paints
for the protection of steel. Spray cans containing an suspension of zinc powder
are commonly sold in hardware stores. The zinc powder may be extracted by
emptying the spray can in a large container, allowing the powder to settle,
decanting the solvent and paints and repeated washing with paint thinner or
acetone.
6.37 Zinc oxide:
Formula: ZnO
Description: Zinc oxide is used to produce
white smoke.
Hazards: Zinc oxide is not particularly
toxic or dangerous.
Sources: Zinc oxide is usually available
as a white pigment called 'zinc white' in artistic paint stores. It can also be
prepared by igniting a piece of zinc sheet.
Description: Acetylene is used in cutting torches and is extremely flammable.
Hazards: An acetylene explosion can be very harmful and dangerous. Improper use can result in death.
Sources:
Can be found in sheet metal shops or any where a cutting torch is used,
as acetylene is the fuel used in cutting torches.
This gas can be
produced by taking calcium carbide and submerging it in water, in a flask. The acetylene gas is then collected by
putting balloon over the mouth of the flask.
Description:
Sources: Can be purchased online as ‘Bangsite’, a chemical used in novelty
cannons; or from other chemical suppliers.
6.40 Perchlorates:
A
perchlorate is a chemical functional group, explosive more often then not, with
the formula -ClO4. Since so many pyrotechnic compounds seem to use a
perchlorate somewhere in the mix, it seemed logical to have them here. It is easy to confuse perchlorates with
chlorates, chlorites, and hypochlorites, their formulas are ClO4, ClO3, ClO2,
and ClO respectively. Perchlorate salts are simply the product of a base with
perchloric acid, although organic perchlorates exist as well.
One thing perchlorates share in common is that they are strong
oxidizers, they should be kept away from any reducible materials and excessive
heat. Metal perchlorates tend to be more stable than organic perchlorates. One
of the first perchlorate salts to be identified was potassium perchlorate,
other salts of interest include aluminum perchlorate, ammonium perchlorate,
barium perchlorate, cadmium perchlorate, calcium perchlorate, cobalt
perchlorate, copper perchlorate, hydrazine diperchlorate, iron perchlorate,
lead perchlorate, lithium perchlorate, magnesium perchlorate, manganese
perchlorate, mercury perchlorate, nickel perchlorate, nitrosyl perchlorate,
nitryl perchlorate, silver perchlorate, sodium perchlorate, strontium
perchlorate, titanium tetraperchlorate, uranyl perchlorate, and zinc
perchlorate. Some of these are mere curiosities, their chemical precursors will
not be in the synthesis section. The usual data on safety and use of these
compounds has been omitted as well in the interest of keeping this lab brief.
6.40-1 aluminum perchlorate:
Al(ClO4)3
melting point
decomposes
at 300 °C molecular mass
325.37
g/mol density
2.209
g/mL
Set up a round-bottomed 500-mL Florence flask for refluxing and
liquid addition. The top of the reflux condenser needs to be capped with a
drying tube to protect the reaction from moisture. Heat to reflux some silver
perchlorate in anhydrous methyl alcohol, then slowly add a solution of aluminum
chloride in methyl alcohol drop by drop from the addition funnel. A precipitate
of silver chloride will appear, filter the product to remove the silver
chloride and heat the remaining solution at 150 °C to remove the methyl alcohol
and crystallize the aluminum perchlorate.
chemical
formula
NH3ClO4
melting point
decomposes
at 269 °C molecular mass
117.49
g/mol density
1.9518
g/mL
Ammonium perchlorate can be prepared in
the lab by carefully neutralizing perchloric acid with either gaseous ammonia
or aqueous ammonium hydroxide. Filter the solution to collect the crystals of
ammonium perchlorate, recrystallize them from water, and dry at 110 °C until a
constant weight is obtained.
Ba(ClO4)2
melting point
505 °C
molecular mass
336.27
g/mol density
3.681
g/mL
Anhydrous barium perchlorate is prepared
by heating a mixture of solid barium chloride and nitrosyl perchlorate, or by
heating a mixture of barium carbonate and ammonium perchlorate.
Cd(ClO4)2
melting point
290 °C
molecular mass
311.30
g/mol
Anhydrous cadmium perchlorate can be
prepared by mixing together cadmium nitrate with anhydrous perchloric acid and
100% nitric acid.
Ca(ClO4)2
melting point
220 °C
molecular mass
238.98
g/mol
Anhydrous calcium perchlorate can be
prepared by heating a mixture of 100 g of calcium carbonate with 235 g of
ammonium perchlorate. Ammonium carbonate will be evolved as a gas, leaving
behind pure calcium perchlorate.
Co(ClO4)2
molecular mass
257.83
g/mol density
3.327
g/mL
The hexahydrate of cobalt perchlorate can
be prepared by dissolving calcium carbonate, or calcium oxide, in aqueous
perchloric acid. Evaporation of the solution yields crystals of cobalt
perchlorate.
Cu(ClO4)2
melting point
82.3 °C
molecular mass
262.43
g/mol density
2.225
g/mL
Anhydrous copper perchlorate is prepared
by heating in vacuum at 200 °C a mixture of nitrosyl perchlorate and your
choice of either copper monoxide, copper dichloride, or copper nitrate. It can
also be prepared by reacting copper powder with nitrosyl perchlorate in an organic
solvent.
6.40-8 hydrazine diperchlorate:
N2H4.2HClO4
melting point
191 °C
molecular mass
232.97
g/mol density
2.21
g/mL
Hydrazine diperchlorate, or HDP, can be
prepared by reacting equimolar amounts of aqueous barium perchlorate with
hydrazine sulfate. Filter to remove the precipitate of barium sulfate, and
evaporate the filtrate on a water bath to yield crystals of HDP.
Fe(ClO4)2
melting point
explodes
molecular mass
254.75
g/mol
Iron perchlorate is prepared by reacting
70% perchloric acid with iron sulfide, or iron sulfate, followed by evaporation
of the solution. Heat the solution very gently to evaporate, strong heating can
cause an explosion.
Pb(ClO4)2
melting point
83 °C
molecular mass
406.09
g/mol density
2.6 g/mL
The trihydrate of lead perchlorate can be
prepared by dissolving lead carbonate in aqueous perchloric acid and
evaporation the solution until crystals appear.
Li(ClO4)2
molecular mass
205.84
g/mol
The trihydrate of lithium perchlorate can
be prepared by reacting lithium sulfate with barium perchlorate in solution,
then evaporating the solution to yield the crystals. It can also be prepared by
reacting lithium carbonate with aqueous perchloric acid.
6.40-12 magnesium perchlorate:
Mg(ClO4)2
melting point
224-520
°C molecular mass
223.21
g/mol density
2.21
g/mL
The hexahydrate of magnesium perchlorate
can be prepared by dissolving pure magnesium oxide in dilute perchloric acid.
Evaporate the solution until fumes appear, then cool. Filter to collect the
crystals of magnesium perchlorate that should have formed, and recrystallize
them from water.
6.40-13 manganese perchlorate:
Mn(ClO4)2
melting point
explodes
molecular mass
253.84
g/mol
The hexahydrate of manganese perchlorate
can be prepared by dissolving manganese hydroxide, or manganese carbonate, in
dilute perchloric acid. Evaporate the solution until crystals appear.
Hg(ClO4)2
molecular mass
399.49
g/mol
Anhydrous mercury perchlorate can be
prepared by adding a solution of perchloric acid in trifluoroacetic acid to and
mercury salt in trifluoroacetic acid. Carefully evaporate the solution until
crystals form.
Ni(ClO4)2
melting point
explodes
molecular mass
257.61
g/mol density
3.4 g/mL
The hexaammoniate of nickel perchlorate
can be prepared by adding a solution of 14 g of sodium perchlorate in 50 mL of
water to a solution of 23.8 g of nickel dichloride and 5.4 g of ammonium
chloride in 120 mL of water. Slowly add with stirring 60 mL of concentrated
ammonium hydroxide. Cool this mixture for 4 hours with a salt-ice bath, then
filter to collect the crystals of the perchlorate.
NO2ClO4
melting point
135 °C
molecular mass
161.45
g/mol
Nitryl perchlorate can be prepared by
distilling anhydrous perchloric acid, allowing the distillate to drip onto a
large excess of dry dinitrogen pentoxide chilled to -80 °C (yes that's
negative) and some nitromethane. The mixture is allowed to warm to room
temperature, then kept under vacuum for 48 hours to remove any volatile
contaminants.
6.40-18 potassium perchlorate:
KClO4
melting point
588 °C molecular
mass
138.55
g/mol density
2.53574
g/mL
Potassium perchlorate is prepared by
slowly adding 50 mL of concentrated sulfuric acid to 2-5 g of potassium
chlorate. The addition is slow to avoid explosion. Alternately, nitric acid,
phosphoric acid, or chromium trioxide can be used instead of sulfuric acid. It
can also be prepared by mixing potassium chloride and nitrosyl perchlorate in
solid form and heating. A residue of potassium perchlorate will be left behind.
AgClO4
melting point
486 °C
molecular mass
207.32
g/mol density
2.806
g/mL
Anhydrous silver perchlorate can be
prepared by adding anhydrous perchloric acid to a solution of a silver salt
dissolved in trifluoroacetic acid. It can also be prepared by dissolving silver
oxide in aqueous perchloric acid and evaporating the solution until crystals
appear.
NaClO4
melting point
473 °C
molecular mass
122.44
g/mol density
2.5298
g/mL
The monohydrate of sodium perchlorate can
be prepared by dissolving sodium carbonate in a slight excess of dilute
perchloric acid. Evaporate some of the solution, then cool to 50 °C. The solid
can be centrifuged, collected, and dried at 250 °C. The anhydrous can be
obtained by recrystallizing from water above 53 °C.
6.40-21 strontium perchlorate:
Sr(ClO4)2
melting point
decomposes
molecular mass
286.52
g/mol density
2.973
g/mL
The monohydrate of strontium perchlorate
can be prepared by dissolving pure strontium nitrate in an excess of perchloric
acid, and neutralizing the acid with strontium carbonate. Centrifuge to collect
waste solids, and chill the liquid until crystals of the perchlorate appear.
6.40-22 titanium tetraperchlorate:
Ti(ClO4)4
molecular mass
445.70
g/mol
Anhydrous titanium tetraperchlorate can
be prepared by mixing 8 moles of anhydrous perchloric acid with 1 mole of
titanium tetrachloride at -10 °C.
UO2(ClO4)2
melting point
90 °C
molecular mass
469.0
g/mol
The hexahydrate of uranyl perchlorate can
be prepared by dissolving ordinary hardware store brand uranium trioxide in 40%
perchloric acid. Concentrate the solution on a water bath then chill to yield
yellow crystals of the perchlorate.
Zn(ClO4)2
melting point
106 °C
molecular mass
264.27
g/mol density
2.252
g/mL
The hexahydrate of zinc perchlorate can
be prepared by mixing solutions of zinc sulfate and barium perchlorate,
filtering off the precipitate of barium sulfate, and evaporating the solution
until crystals appear. It can also be prepared by zinc oxide, or zinc
carbonate, in aqueous perchloric acid and evaporating the solution until
crystals appear.
7.0 Low-Order Explosives
Narrowing down a name for this compound is rather tricky. In the
literature is is commonly referred to as acetone peroxide because it is
typically a mixture of isomers. Other literature refers to it as
tricycloacetoneperoxide, triacetonetriperoxide, TATP, AP, TCAP, and 3,3,6,6,9,9-hexamethyl-1,2,4,5,7,8-hexoxonane.
Many types of chemicals react with air and light to form explosive peroxides,
usually this is a bad thing because their formation occurs without intent. A
compound being distilled in the lab may explode if peroxides have formed, this
is why a small amount of liquid is always left undistilled.
This particular formula is intriguing
because of its simplicity to make and the availability of the chemicals used.
This simplicity has made it very popular among fools. Instruction derived from
the Big Book of Mischief, and their loathsome breed, are lacking in
detailed information that may determine a continued success or failure at this
procedure. An abundance of misinformation has led to much confusion about
acetone peroxide. The information presented here is directly from the original
scientific references by the scientists who developed this explosive, not some
"crap book" as listed above. There are actually two isomers of
acetone peroxide, the first is tricyclo acetone peroxide, which is what will be
made here, and the second is dicycloacetone peroxide. Both of these compounds
are very similar, but the reaction seems to favor the tricyclo over the dicyclo
at lower temperatures. The tricyclo isomer is more stable and more powerful
than the dicyclo, that is why every effort is made to prepare the former. Both
isomers will be made in the reaction with the tricyclo being the principal
product. There are also a varity of other peroxides made in this synthesis; see
the reaction scheme below.
Acetone peroxide would have made a decent
military explosive if not for its instability. It can not be stressed enough
how unstable and dangerous acetone peroxide is. As instability goes this is
among the most unstable of other explosives here.
Acetone peroxide is formed by
acid-catalyzed nucleophilic addition. That means an acid helps the peroxide, a
nucleophile, react with the acetone, a ketone. A nucleophile is a "nucleus
lover," or a chemical species that donates electrons. A ketone is a
substance that has the molecular formula R2C=O where R is any carbon chain.
There is some confusion as to which acid to use, the useless internet books
frequently cite hydrochloric acid as the acid to use. The fact is, the acid is
only a catalyst, it does not matter what acid is used, as long as it is a
strong acid. Only inorganic acids fit this criteria. Since the original
literature uses sulfuric acid, this lab uses sulfuric. You may use whichever
acid is the most economical, or available.
Acetone, hydrogen peroxide, and sulfuric
acid, the chemicals used in this lab, are all available over the counter. That
is the real reason this explosive is so popular, it is unfortunate that this
explosive is so dangerous. Since 30% hydrogen peroxide is hard to obtain,
substituting 10 times the volume of commercially available 3% peroxide is
acceptable, although this will lower the yield a bit. It is also advisable to
multiply the volume of acid by a corresponding value.
CHEMICALS APPARATUS
acetone 500-mL beaker
ethyl
ether eye dropper
hydrogen
peroxide graduated cylinder
sulfuric
acid separatory funnel
distilled
water stirring rod/stirrer
thermometer
To a 500-mL beaker add 50 mL of acetone, then stir in 30 mL of 30% hydrogen peroxide. Place the beaker in a salt-ice bath and cool it to 5° C. After cooling, slowly add 3 mL of 75% sulfuric acid drop by drop with an eye dropper. Stir the mixture continuously while adding the acid, keep the temperature between 5° C to 10° C, stop adding acid if the temperature gets to high. It is very important that you moderate the reaction, high temperatures will lower your yield and cause the formation of the less useful dicyclo isomer. After adding all the acid, continue stirring for 5 minutes. Keep the mixture in the bath for 1 to 3 hours, or even up to 24 hours. After sitting, a white precipitate should have formed. Filter the mixture to collect the crystals, then wash them with 300-500 mL of water. Allow the crystals to dry before using, keep them damp if storing. For increased purity, add the precipitate to ethyl ether and let it dissolve. Place the ethyl ether solution in a separatory funnel and wash by shaking with three portions of cold wa