V =( E2 – E1)/ h
meVr = n( h / 2 * 3.14), n = 1,2,3 …
Bohr’ s model for hydrogen atom:
a. An electron in the hydrogen atom can move around the nucleus in a circular path of fixed radius and energy. These paths are called orbits or energy levels. These orbits are arranged concentrically around the nucleus.
b. As long as an electron remains in a particular orbit, it does not lose or gain energy and its energy remains constant.
c. When transition occurs between two stationary states that differ in energy, the frequency of the radiation absorbed or emitted can be calculated
V =( E2 – E1)/ h
d. An electron can move only in those orbits for which its angular momentum is an integral multiple of h / 2π
meVr = n( h / 2 * 3.14), n = 1,2,3 …
The radius of the nth orbit is given byrn = 52.9 pm x n 2 Z energy of electron in nth orbit is:
Limitations of Bohr’ s model of atom:
a. Bohr’ s model failed to account for the finer details of the hydrogen spectrum.
b. Bohr’ s model was also unable to explain spectrum of atoms containing more than one electron.