(A) The wave number $\bar{\nu}$ is given by the Rydberg formula: $\bar{\nu} = R_{H} [\frac{1}{n_1^2} - \frac{1}{n_2^2}]$ Given $n_1 = 2$,$n_2 = 4$,and

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(A) The wave number $\bar{\nu}$ is given by the Rydberg formula: $\bar{\nu} = R_{H} [\frac{1}{n_1^2} - \frac{1}{n_2^2}]$ Given $n_1 = 2$,$n_2 = 4$,and $R_{H} = 109677 \ cm^{-1}$. Substituting the values: $\bar{\nu} = 109677 [\frac{1}{2^2} - \frac{1}{4^2}] \ cm^{-1}$ $= 109677 [\frac{1}{4} - \frac{1}{16}] \ cm^{-1}$ $= 109677 [\frac{4-1}{16}] \ cm^{-1}$ $= 109677 [\frac{3}{16}] \ cm^{-1}$ $= 20564.44 \ cm^{-1}$

Class 11 Chemistry Structure of Atom Atomic models and Planck's quantum theory

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What is the wave number of a photon emitted during the transition from orbit $n=4$ to $n=2$ in a hydrogen atom (in $cm^{-1}$)? $[R_{H}=109677 \ cm^{-1}]$

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A
$20564.44$
B
$23032.17$
C
$15354.78$
D
$25225.7$

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What is the wave number of a photon emitted during the transition from orbit $n=4$ to $n=2$ in a hydrogen atom (in $cm^{-1}$)? $[R_{H}=109677 \ cm^{-1}]$

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