S C Kheterpal, S N Dhawan and, P N Kapil Solutions for Chapter: Structure of Atom, Exercise 5: PROBLEMS FOR PRACTICE

If the energy difference between two electronic states is $214.68 \mathrm{k}\mathrm{J} \mathrm{m}\mathrm{o}{\mathrm{l}}^{-1},$ calculate the frequency of light emitted when an electron drops from the higher to the lower state. Planck’s constant, $\mathrm{h}=39.79\times {10}^{-14} \mathrm{k}\mathrm{J} \sec \mathrm{m}\mathrm{o}{\mathrm{l}}^{-1}.$

In hydrogen atom, an electron jumps from $3^{\mathrm{r}\mathrm{d}}$ orbit to the $2^{\mathrm{n}\mathrm{d}}$ orbit. Calculate the wavelength of the radiation emitted. $\left(\mathrm{h}=6.63\times {10}^{-34}\mathrm{J} \mathrm{s}\mathrm{e}\mathrm{c}\right).$

Calculate the wave number for the longest wavelength transition in the Balmer series of atomic hydrogen.

Applying Bohr’s model when electron in $\mathrm{H}$ atom comes from $\mathrm{n}=4$ to $\mathrm{n}=2,$ calculate the wavelength of the line. In this process, write whether energy is released or absorbed. Also write the range of radiation $\left({\mathrm{R}}_{\mathrm{H}}=2.18\times {10}^{-18}\mathrm{J},\mathrm{}\mathrm{h}=6.63\times {10}^{-34}\mathrm{J}\right)$