Question

each hydrogen atom is excited by giving 10.2 ev . The maximum number of spectral lines in the emission is equal to
a. 1
b. 2
c. 3
d. 4

Answer 1

Answer:

   E µ 1/n2

 For n=1, E = 13.6 eV

Thus energy absorbed =13.6 (1 - (1 / n2) eV., where n =1 to ¥

For n=2, E = 13.6(1 - (1 / 22) = 10.2

This is the lowest energy state possible for emission of spectral lines.

Thus the energy absorbed should always be between 10.2 and 13.6 eV

Hence , no emission takes place when  hydrogen atom is excited by giving 8.4eV.

Answer 2

Answer:

Explanation:  E2-E1=10.2eV , so electron is excited to econd orbit, therefore no.of spectral lines= n(n-1)/2