Question

The emission spectrum of hydrogen is found to satisfy the expression for the energy change $\Delta E$ (in joules) such that $\Delta E=2.18\times 10^{-18}\left(\frac{1}{n_1^2}-\frac{1}{n_2^2}\right)J$ where $n_1=1$, $2$, $3$, $.....$ and $n_2=2$, $3$, $4$. The spectral lines corresponds to Paschen series if

• A. $n_1=1$ and $n_2=2$, $3$, $4$
• B. $n_1=3$ and $n_2=4$, $5$, $6$
• C. $n_1=1$ and $n_2=3$, $4$, $5$
• D. $n_1=2$ and $n_2=3$, $4$, $5$

Answer 1

Answer: (B)

In the emission spectra of hydrogen atom, Paschen series is the one where the transition from higher energy states to third energy state takes place.
i.e. $n_f=n_1=3$ and $n_i=n_2>3$