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(A) The ultraviolet $(UV)$ region corresponds to the Lyman series,where transitions occur to the $n = 1$ energy level. Since there are $3$ lines in th

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$1$

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(A) The ultraviolet $(UV)$ region corresponds to the Lyman series,where transitions occur to the $n = 1$ energy level. Since there are $3$ lines in the $UV$ region,the electron must have transitioned from $n = 4$ to $n = 1$ $(4$ $\rightarrow 1, 3$ $\rightarrow 1, 2$ $\rightarrow 1)$. Thus,the excited state is $n = 4$. For the infrared $(IR)$ region,we look for transitions ending at $n = 3$ (Paschen series). From $n = 4$,the possible transition to the $n = 3$ level is $4 \rightarrow 3$. Therefore,the number of lines produced in the infrared region is $1$.

$A$ certain electronic transition from an excited state to the ground state of the $H$ atom in one or more steps gives rise to three lines in the ultraviolet region of the spectrum. How many lines does this transition produce in the infrared region of the spectrum?

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