Question

Energy levels $$A,B,C$$   of a certain atom correspond to increasing values of energy i.e. $${E_A} < {E_B} < {E_C}.$$    If $${\lambda _1},{\lambda _2},{\lambda _3}$$   are the wavelengths of radiation corresponding to the transitions $$C$$ to $$B,B$$  to $$A$$ and $$C$$ to $$A$$ respectively, which of the following relation is correct ?

A. $${\lambda _3} = {\lambda _1} + {\lambda _2}$$
B. $${\lambda _3} = \frac{{{\lambda _1}{\lambda _2}}}{{{\lambda _1} + {\lambda _2}}}$$  
C. $${\lambda _1} + {\lambda _2} + {\lambda _3} = 0$$
D. $$\lambda _3^2 = \lambda _1^2 + \lambda _2^2$$
Answer :   $${\lambda _3} = \frac{{{\lambda _1}{\lambda _2}}}{{{\lambda _1} + {\lambda _2}}}$$
Solution :
Atoms And Nuclei mcq solution image
Using Bohr's postulate for radiation of spectral line, we have
Radiation of wavelength from $$C$$ to $$B$$
$${E_C} - {E_B} = \frac{{hc}}{{{\lambda _1}}}\,.......\left( {\text{i}} \right)$$
Radiation of wavelength from $$B$$ to $$A$$
$${E_B} - {E_A} = \frac{{hc}}{{{\lambda _2}}}\,.......\left( {{\text{ii}}} \right)$$
Radiation of wavelength from $$C$$ to $$A$$
$${E_C} - {E_A} = \frac{{hc}}{{{\lambda _3}}}\,.......\left( {{\text{iii}}} \right)$$
Also, $$\left( {{E_C} - {E_A}} \right) = \left( {{E_C} - {E_B}} \right) + \left( {{E_B} - {E_A}} \right)$$
$$\eqalign{ & \therefore \frac{{hc}}{{{\lambda _3}}} = \frac{{hc}}{{{\lambda _1}}} + \frac{{hc}}{{{\lambda _2}}}\, \cr & {\text{or}}\,\,\frac{1}{{{\lambda _3}}} = \frac{1}{{{\lambda _1}}} + \frac{1}{{{\lambda _2}}} \cr & \Rightarrow {\lambda _3} = \frac{{{\lambda _1}{\lambda _2}}}{{{\lambda _1} + {\lambda _2}}} \cr} $$

Releted MCQ Question on
Modern Physics >> Atoms And Nuclei

Releted Question 1

If elements with principal quantum number $$n > 4$$  were not allowed in nature, the number of possible elements would be

A. 60
B. 32
C. 4
D. 64
Releted Question 2

Consider the spectral line resulting from the transition $$n = 2 \to n = 1$$    in the atoms and ions given below. The shortest wavelength is produced by

A. Hydrogen atom
B. Deuterium atom
C. Singly ionized Helium
D. Doubly ionised Lithium
Releted Question 3

An energy of $$24.6\,eV$$  is required to remove one of the electrons from a neutral helium atom. The energy in $$\left( {eV} \right)$$  required to remove both the electrons from a neutral helium atom is

A. 38.2
B. 49.2
C. 51.8
D. 79.0
Releted Question 4

As per Bohr model, the minimum energy (in $$eV$$ ) required to remove an electron from the ground state of doubly ionized $$Li$$ atom $$\left( {Z = 3} \right)$$  is

A. 1.51
B. 13.6
C. 40.8
D. 122.4

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