__Hydrogen emission spectrum series:__

**\(\bar{\nu}=R_{H}(\frac{1}{2^{2}}-\frac{1}{n^{2}})\)**

_{H}is called the Rydberg constant for hydrogen. Rydberg constant is given by:

**\(R_{H}=\frac{me^{4}}{8 \varepsilon _{0}h^{3}c}\)**

Where, h = Planck’s constant and c = speed of light.

Using the known value of these constants we can compute the value of Rydberg constant, R_{H} = 109677.

The Balmer series is basically the part of hydrogen emission spectrum which is responsible for the excitation of electron from second shell to any other shell. Similarly, other transitions too have their own series names. Some of them are listed below,

- Transition from first shell to any other shell – Lyman series
- Transition from second shell to any other shell – Balmer series
- Transition from third shell to any other shell – Paschen series
- Transition from fourth shell to any other shell – Bracket series
- Transition from fifth shell to any other shell – Pfund series

**\(\bar{\nu }=109677(\frac{1}{n_{1}^{2}}-\frac{1}{n_{2}^{2}})\)**

Where,

n_{1} = 1,2,3,4 …

n_{2} = n_{1} + 1

= wave number of the electromagnetic radiation. The value 109,677 cm^{-1} is known as Rydberg constant for hydrogen.

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