Textbook Problem

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A line in the Balmer series of emission lines of excited H atoms has a wavelength of 410.2 nm (Figure 6.10). What color is the light emitted in this transition? What quantum levels are involved in this emission line? That is, what are the values of n_initial and n_final?

Interpretation Introduction

Interpretation: The colour emitted during the transition and also the initial and the final electronic state for the line in $410.2\text{nm}$ of the $\text{H}$ atom in the Balmer series has to be identified.

Concept introduction:

• Electronic transitions that take place in excited $\text{H}$ atom is,

1. 1. Lyman series: electronic transitions take place to the $\text{n}\text{=}\text{1}$ level and it is in ultraviolet region.
2. 2. Balmer series: electronic transitions take place from $\text{n}\text{>}\text{2}$ to the $\text{n}\text{=}2$ level and it is in visible region.
3. 3. Ritz-Paschen series: electronic transitions take place from $\text{n}\text{>}3$ to the $\text{n}\text{=}3$ level and it is in infrared region.
4. 4. Brackett series: electronic transitions take place from $\text{n}\text{>}4$ to the $\text{n}\text{=}4$ level.
5. 5. Pfund series: electronic transitions take place from $\text{n}\text{>}5$ to the $\text{n}\text{=}5$ level

• Electromagnetic radiations are a type of energy surrounding us. They are of different types like radio waves, IR, UV, X-ray etc.
• Visible radiation in the wavelength of $\text{400}\text{nm}$ to $\text{700}\text{nm}$. The wavelength region of violet color is $450nm–400 nm$

Explanation of Solution

In Balmer series, the electronic transitions take place from $\text{n}\text{>}\text{2}$ to the $\text{n}\text{=}2$ level and it is in visible region. The wavelength of line is $410.2\text{nm}$.

The line having wavelength of $410.2\text{nm}$ emits violet colour during the transition.

The line with wavelength $410$