The energy levels of an electron in an atom a | vedclass

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(C) The transition $I$ represents the absorption of a photon because the electron moves from a lower energy level to a higher energy level.Among the r

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$III$

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(C) The transition $I$ represents the absorption of a photon because the electron moves from a lower energy level to a higher energy level.Among the remaining transitions $(II, III, IV)$,all represent the emission of a photon as the electron moves from a higher energy level to a lower energy level.The energy of the emitted photon is given by $\Delta E = E_{initial} - E_{final} = 13.6 	ext{ eV} 	imes Z^2 \left( \frac{1}{n_{final}^2} - \frac{1}{n_{initial}^2} ight)$.Comparing the transitions:Transition $II$: $n=4$ to $n=3$,$\Delta E \propto (1/9 - 1/16) = 7/144 \approx 0.048$Transition $III$: $n=2$ to $n=1$,$\Delta E \propto (1/1 - 1/4) = 3/4 = 0.75$Transition $IV$: $n=4$ to $n=2$,$\Delta E \propto (1/4 - 1/16) = 3/16 = 0.1875$Comparing the values,transition $III$ corresponds to the largest energy difference,thus representing the emission of a photon with the highest energy.

The energy levels of an electron in an atom are shown. Which transition of the electron represents the emission of a photon with the highest energy?

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