## Explanation

The Rydberg constant is used to calculate the wavelengths in the hydrogen spectrum – energy which is absorbed or emitted in the form of photons as electrons move between shells in the hydrogen atom. The Rydberg constant expresses the photon that is released when the binding energy (Rydberg unit of energy) is transferred to transverse form, creating the photon. The photon is measured in frequency or wavelength. The Rydberg constant is expressed as a hybrid of both, as either frequency without wave speed (c) or as the inverse of wavelength.

See also: Rydberg Unit of Energy

## Derivation – Rydberg Constant

In classical format, the Rydberg constant is derived from the fine structure constant and electron radius. In wave format, it is derived from the Transverse Wavelength Equation. It is based on the electron at K=10 (ten wave centers). It is used with hydrogen calculations and the amplitude factor for a single electron-proton interaction is one (refer to the amplitude factor explanation in the Atoms section). A nucleus with two or more protons will have a different amplitude factor, which is why the Rydberg constant only works for hydrogen.

## Classical Constant Form |
## Wave Constant Form |

Using classical constants | Using energy wave constants |

**Calculated Value**: 1.0974E+07

**Difference from CODATA:** 0.000%

**Calculated Units**: m^{-1}

**G-Factor:**g_{λ}^{-1}

**Alternative Derivation**

An alternative derivation in classical form is shown with the Bohr radius, as further proof that the it occurs at the most probable location for the electron in orbit for hydrogen.

Its value was calculated and shown to match the known value in the Summary of Calculations table. *The derivation of this constant is available in the Fundamental Physical Constants paper.*