An atom has x energy levels,then the total nu | vedclass

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(C) When an electron transitions from an excited state $x$ to lower energy levels,the total number of spectral lines is calculated by summing the poss

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$1 + 2 + 3 + \dots + (x - 1)$

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(C) When an electron transitions from an excited state $x$ to lower energy levels,the total number of spectral lines is calculated by summing the possible transitions from each level.For an atom with $x$ energy levels,the transitions are from level $x$ to $(x-1), (x-2), \dots, 1$.The number of lines is given by the sum: $(x-1) + (x-2) + (x-3) + \dots + 2 + 1$.This is equivalent to the sum of the first $(x-1)$ natural numbers,which is $1 + 2 + 3 + \dots + (x - 1)$.

An atom has $x$ energy levels,then the total number of spectral lines in its emission spectrum is given by:

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