Which of the following electronic transitions | vedclass

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(C) The energy difference for an electronic transition in a hydrogen atom is given by $\Delta E = 13.6 	imes Z^2 	imes (\frac{1}{n_1^2} - \frac{1}{n

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from $n=1$ to $n=\infty$

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(C) The energy difference for an electronic transition in a hydrogen atom is given by $\Delta E = 13.6 	imes Z^2 	imes (\frac{1}{n_1^2} - \frac{1}{n_2^2}) 	ext{ eV}$.For a hydrogen atom,$Z=1$,so $\Delta E = 13.6 	imes (\frac{1}{n_1^2} - \frac{1}{n_2^2}) 	ext{ eV}$.Calculating the energy for each transition:$A$: $n=1$ to $n=2$,$\Delta E = 13.6 	imes (1 - 1/4) = 13.6 	imes 0.75 = 10.2 	ext{ eV}$.$B$: $n=2$ to $n=3$,$\Delta E = 13.6 	imes (1/4 - 1/9) = 13.6 	imes 0.138 = 1.89 	ext{ eV}$.$C$: $n=1$ to $n=\infty$,$\Delta E = 13.6 	imes (1 - 0) = 13.6 	ext{ eV}$.$D$: $n=3$ to $n=5$,$\Delta E = 13.6 	imes (1/9 - 1/25) = 13.6 	imes 0.071 = 0.97 	ext{ eV}$.Comparing the values,the transition from $n=1$ to $n=\infty$ requires the largest amount of energy.

Which of the following electronic transitions in a hydrogen atom will require the largest amount of energy?

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