A certain electronic transition from an excit | vedclass

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Question

(C) The ultraviolet region of the hydrogen spectrum corresponds to the Lyman series,where transitions occur to the ground state $(n_1 = 1)$.Four lines

Vedclass · Accepted Answer

$3$

Vedclass · Answer

(C) The ultraviolet region of the hydrogen spectrum corresponds to the Lyman series,where transitions occur to the ground state $(n_1 = 1)$.Four lines in the ultraviolet region imply transitions from $n_2 = 2, 3, 4, 5$ to $n_1 = 1$.This indicates the electron is initially in the $n = 5$ excited state.The possible transitions from $n = 5$ to lower energy levels are given by the formula $\frac{n(n-1)}{2} = \frac{5(5-1)}{2} = 10$ total lines.The lines in the infrared region correspond to the Paschen series $(n_1 = 3)$ and Brackett series $(n_1 = 4)$.For $n = 5$,the possible transitions are:$5 \rightarrow 4$ (Brackett series,$IR$),$5 \rightarrow 3$ (Paschen series,$IR$),$4 \rightarrow 3$ (Paschen series,$IR$).Thus,there are $3$ lines in the infrared region.Therefore,the correct option is $C$.

Column $I$	Column $II$
$A$. $V_{n} / K_{n} = ?$	$P$. $0$
$B$. If radius of $n^{\text{th}}$ orbit $\propto E_{n}^{x}, x = ?$	$Q$. $-1$
$C$. Angular momentum in lowest orbital	$R$. $-2$
$D$. $1/r_{n} \propto Z^{y}, y = ?$	$S$. $1$

$A$ certain electronic transition from an excited state to the ground state of the $H$ atom in one or more steps gives rise to four 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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