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Question

(A) The frequency of emitted radiation is directly proportional to the energy difference between the energy levels involved in the transition.Emission

Vedclass · Accepted Answer

$n = 2$ to $n = 1$

Vedclass · Answer

(A) The frequency of emitted radiation is directly proportional to the energy difference between the energy levels involved in the transition.Emission occurs when an electron jumps from a higher energy level $(n_2)$ to a lower energy level $(n_1)$.The frequency $
u$ is given by the Rydberg formula: $
u = R_{H} c z^2 \left[\frac{1}{n_1^2} - \frac{1}{n_2^2}ight]$.For option $A$ ($n = 2$ to $n = 1$): $\Delta E \propto \left[\frac{1}{1^2} - \frac{1}{2^2}ight] = 1 - 0.25 = 0.75$.For option $B$ ($n = 6$ to $n = 2$): $\Delta E \propto \left[\frac{1}{2^2} - \frac{1}{6^2}ight] = 0.25 - 0.027 = 0.223$.Comparing the values,the transition from $n = 2$ to $n = 1$ results in the largest energy difference and thus the maximum frequency of emission.

Maximum frequency of emission is obtained for the transition $:-$

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