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(B) The ultraviolet region corresponds to the Lyman series $(n_1 = 1)$.For $n_2$ to $n_1 = 1$ transitions,the number of spectral lines is given by $n_

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$6$

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(B) The ultraviolet region corresponds to the Lyman series $(n_1 = 1)$.For $n_2$ to $n_1 = 1$ transitions,the number of spectral lines is given by $n_2 - n_1 = 5$.Therefore,$n_2 - 1 = 5$,which gives $n_2 = 6$.Now,for transitions from $n_2 = 6$ to the infrared region (Paschen,Brackett,and Pfund series):$1$. Paschen series $(n_1 = 3)$: Transitions are $6 	o 3, 5 	o 3, 4 	o 3$ ($3$ lines).$2$. Brackett series $(n_1 = 4)$: Transitions are $6 	o 4, 5 	o 4$ ($2$ lines).$3$. Pfund series $(n_1 = 5)$: Transition is $6 	o 5$ ($1$ line).Total number of lines in the infrared region = $3 + 2 + 1 = 6$.

When a hydrogen atom in an excited state undergoes electronic transitions to the ground state,$5$ spectral lines are observed in the ultraviolet region. How many spectral lines will be observed in the infrared region due to transitions from the same excited state?

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