The maximum number of emission lines for atom | vedclass

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(B) The spectral lines of the Balmer series lie in the visible range.These lines are obtained due to the transition of an electron from any higher ene

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(B) The spectral lines of the Balmer series lie in the visible range.These lines are obtained due to the transition of an electron from any higher energy state $(n > 2)$ to the $n = 2$ state.According to the provided figure,the energy levels involved are from $n = 1$ to $n = 7$.Therefore,the possible transitions to the $n = 2$ state are from $n = 3, 4, 5, 6, 	ext{ and } 7$.This gives a total of $5$ possible emission lines in the visible range $(3$ $ightarrow 2, 4$ $ightarrow 2, 5$ $ightarrow 2, 6$ $ightarrow 2, 7$ $ightarrow 2)$.

The maximum number of emission lines for atomic hydrogen that you would expect to see with the naked eye if the only electronic levels involved are those shown in the figure,is

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