Microwave (Bohr's Theory)
BOHR’S THEORY OF THE HYDROGEN MODEL
EMISSION SPECTRA
Emission Spectra are continuous or line spectra that are emitted by substances. It can be sensed by energizing a substance by some form of energy most commonly thermal energy for solids and electrical energy for gases. The colors emitted are part of the visible light while the heat emitted is part of the infrared region of the spectra.
The emission spectra of the gas phase emit line spectra. Line spectra are the light emissions at specific wavelengths unlike the continuous spectra which include a range of wavelengths.
Every substance has a unique emission spectrum. The uniqueness of it helps in identifying an unknown element or substance.
THE HYDROGEN ATOM’S EMISSION SPECTRA
In 1913, Niels Bohr provided an explanation for the cause of the emission spectra. Although some of his findings have been proven to be incorrect many of his ideas are infallible. Bohr stated:
* Electrons move in circular orbits around the nucleus, but the single electron around the hydrogen atom can only be located around certain orbits.
* The electron motion in each orbit must be of a fixed value, or quantized.
* The emission spectrum is the result of the energized electron moving to an excited state then dropping to the ground state because this process releases photons.
The ground state or ground level refers to the lowest energy state of a system or the first energy level.
The excited state refers to any energy level higher than the ground state.
As an electron makes its way to a higher energy level it needs more and more energy to reach the next state by an average of n2 . Bohr’s theory allows the explanation of the line spectrum of the hydrogen atom. Here’s how.
Radiant energy is absorbed by the electron enabling it to move out into higher energy levels or the excited state. As the electron loses energy and descends back to the ground state, it releases photons emitting the radiant energy.
