Question

The quantized energy of electron in hydrogen atom for the nth energy level is
given by En = -1.312/n2 x 106 J/mol. Calculate the minimum energy required to
remove the electron completely from hydrogen atom when its quantized energy level
n equals 2. What should be the wavelength of light that can be used to cause this
transition?

Answer 1

Answer:

In general, according to Bohr's model, energy of an electron of hydrogen Atom, in n= n is En=-13.6/n^2 eV/electron………….(1)

But 1 eV=1.6x10^-19J.=1.6x10^-19 (J/mol)mol……….(2)

But, mol=6.023x10^23 electron………(3)

Using (2) and (3) in equation (1),

En=-(13.6/n^2)x10^5 J/mole

E1=-13.6 x10^5 J/mol and taking n=2,

E2=-(13.6/4) x10^5 J/mol

Then, energy required to excite electron from n=1 state to n= state is

E2-E1=(3/4)(13.6) x10^5 J/molt=10.2 x10^5 J/mol=10.2 eV / electron.

Explanation: