Which electron transition in a hydrogen atom | vedclass

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(A) The energy change for an electron transition in a hydrogen atom is given by $\Delta E = 13.6 \ 	ext{eV} 	imes Z^2 \left( \frac{1}{n_1^2} - \frac

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From $n = 1$ to $n = 2$

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(A) The energy change for an electron transition in a hydrogen atom is given by $\Delta E = 13.6 \ 	ext{eV} 	imes Z^2 \left( \frac{1}{n_1^2} - \frac{1}{n_2^2} ight)$.For a transition from $n_1$ to $n_2$,the energy required is proportional to $\left( \frac{1}{n_1^2} - \frac{1}{n_2^2} ight)$.Comparing the options:$A$: $n=1$ to $n=2$,$\Delta E \propto (1 - 0.25) = 0.75$.$B$: $n=2$ to $n=3$,$\Delta E \propto (0.25 - 0.111) = 0.139$.$C$: $n=\infty$ to $n=1$ represents an emission (energy release),not absorption.$D$: $n=3$ to $n=5$,$\Delta E \propto (0.111 - 0.04) = 0.071$.The transition from $n=1$ to $n=2$ requires the largest amount of energy among the given absorption transitions.

Which electron transition in a hydrogen atom requires the largest amount of energy?

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