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 .