Chapter 9, Problem 9.50E

Interpretation Introduction

(a)

Interpretation:

A diagram that illustrates the electronic transitions from the Lyman series is to be drawn.

Concept introduction:

Rydberg equation is used to represent the wavenumber or wavelength of the lines present in the atomic spectrum of an element. The Rydberg equation for the hydrogen atom is represented as,

$\overline{\nu }=R_{\text{H}}\left(\frac{1}{n_{\text{f}}^2}-\frac{1}{n_{\text{i}}^2}\right)$

Where,

• $R_{\text{H}}$ represents Rydberg constant with a value for hydrogen $1.09737\times {10}^7{\text{m}}^{-1}$.

• $n_{\text{i}}$ represents the initial energy level.

• $n_{\text{f}}$ represents the final energy level.

Interpretation Introduction

(b)

Interpretation:

A diagram that illustrates the electronic transitions from the Brackett series is to be drawn.

Concept introduction:

Rydberg equation is used to represent the wavenumber or wavelength of the lines present in the atomic spectrum of an element. The Rydberg equation for the hydrogen atom is represented as,

$\overline{\nu }=R_{\text{H}}\left(\frac{1}{n_{\text{f}}^2}-\frac{1}{n_{\text{i}}^2}\right)$

Where,

• $R_{\text{H}}$ represents Rydberg constant with a value for hydrogen $1.09737\times {10}^7{\text{m}}^{-1}$.

• $n_{\text{i}}$ represents the initial energy level.

• $n_{\text{f}}$ represents the final energy level.