The energy level diagram of an element is given below. Identify, by doing necessary calculations , which transition corresponds of the emission of a spectral line of wavelength 102.7 nm.

The energy level diagram of an element is given below. Identify, by do

1.	The energy level diagram of an element is given below. Identify, by doing necessary calculations , which transition corresponds of the emission of a spectral line of wavelength 102.7 nm.
Answer» `lambda=102.7 nm = 102.7xx10^(-9)m` The energy of the emitted photons is, `E=(hc)/(lambda)=(6.626xx10^(-34)xx3xx10^(8))/(102.7xx10^(-9))=(19.878xx10^(-26))/(102.7xx10^(-9))=1.9355xx10^(-18)J` `:.` Energy corresponds `=(1.9355xx10^(-18))/(1.6xx10^(-19))` `eV=12.097 ev ~ 12.1 eV`.

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The energy level diagram of an element is given below. Identify, by doing necessary calculations , which transition corresponds of the emission of a spectral line of wavelength 102.7 nm.

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