The Balmer series in a hydrogen atom relates the possible electron transitions down to the *n* = 2 position to the wavelength of the emission that scientists observe. In quantum physics, when electrons transition between different energy levels around the atom (described by the principal quantum number, *n*) they either release or absorb a photon. The Balmer series describes the transitions from higher energy levels to the second energy level and the wavelengths of the emitted photons. You can calculate this using the Rydberg formula.

#### TL;DR (Too Long; Didn't Read)

Calculate the wavelength of the hydrogen Balmer series transitions based on:

1/*λ* = *R _{H}* ((1/2

^{2}) − (1 /

*n*

_{2}

^{2}))

Where *λ* is the wavelength, *R _{H}* = 1.0968 × 10

^{7}m

^{−}

^{1}and

*n*

_{2}is the principle quantum number of the state the electron transitions from.

## The Rydberg Formula and Balmer’s Formula

The Rydberg formula relates the wavelength of the observed emissions to the principle quantum numbers involved in the transition:

1/*λ* = *R _{H}* ((1/

*n*

_{1}

^{2}) − (1 /

*n*

_{2}

^{2}))

## Sciencing Video Vault

The *λ* symbol represents the wavelength, and *R _{H}* is the Rydberg constant for hydrogen, with

*R*= 1.0968 × 10

_{H}^{7}m

^{−}

^{1}. You can use this formula for any transitions, not just the ones involving the second energy level.

The Balmer series just sets *n*_{1} = 2, which means the value of the principal quantum number (*n*) is two for the transitions being considered. Balmer’s formula can therefore be written:

1/*λ* = *R _{H}* ((1/2

^{2}) − (1 /

*n*

_{2}

^{2}))

## Calculating a Balmer Series Wavelength

The first step in the calculation is to find the principle quantum number for the transition you’re considering. This simply means putting a numerical value on the “energy level” you’re considering. So the third energy level has *n* = 3, the fourth has *n* = 4 and so on. These go in the spot for *n*_{2} in the equations above.

Start by calculating the part of the equation in brackets:

(1/2^{2}) − (1 / *n*_{2}^{2})

All you need is the value for *n*_{2} you found in the previous section. For *n*_{2} = 4, you get:

(1/2^{2}) − (1 / *n*_{2}^{2}) = (1/2^{2}) − (1 / 4^{2})

= (1/4) − (1/16)

= 3/16

Multiply the result from the previous section by the Rydberg constant, *R _{H}* = 1.0968 × 10

^{7}m

^{−}

^{1}, to find a value for 1/

*λ*. The formula and the example calculation gives:

1/*λ* = *R _{H}* ((1/2

^{2}) − (1 /

*n*

_{2}

^{2}))

= 1.0968 × 10^{7} m^{−}^{1} × 3/16

= 2,056,500 m^{−}^{1}

Find the wavelength for the transition by dividing 1 by the result from the previous section. Because the Rydberg formula gives the reciprocal wavelength, you need to take the reciprocal of the result to find the wavelength.

So, continuing the example:

* λ* = 1 / 2,056,500 m

^{−}

^{1}

= 4.86 × 10^{−}^{7} m

= 486 nanometers

This matches the established wavelength emitted in this transition based on experiments.