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  • What is the wavelength of light emitted when the electron in a hydrogen atom undergoes transition from an energy level with n = 4 to an energy level with n = 2?

2.13    What is the wavelength of light emitted when the electron in a hydrogen atom undergoes transition from an energy level with n = 4 to an energy level with n = 2?

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When an electron in a hydrogen atom undergoes a transition from an energy level with n=4 to an energy level n=2, there will be an emission of energy whose wavelength can be found by:

\vartheta =R\left ( \frac{1}{n_{1}^2}-\frac{1}{n_{2}^2} \right )

=109677\left ( \frac{1}{2^2}-\frac{1}{4^2} \right )cm^{-1} = 20564.4cm^{-1}

and wavelength will be equal to:

\lambda =\frac{1}{\vartheta } = \frac{1}{20564.4} = 486\times10^{-7}cm = 486\times10^{-9}m = 486 nm

 

Posted by

Divya Prakash Singh

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