How are patterns produced by Hydrogen and Neon different from each other?

Patterns produced by hydrogen and neon are different due to the unique electronic structures of these elements, which determine their emission spectra. When an element is energized (for example, by applying an electric current), the electrons can absorb energy and transition to higher energy levels. As they return to lower energy levels, they emit photons of specific wavelengths, which translates to light of certain colors. The emitted wavelengths create a pattern known as the element's emission spectrum.

For hydrogen, its emission spectrum is characterized by the Lyman, Balmer, and Paschen series, among others, which correspond to electrons transitioning to and from specific energy levels in a hydrogen atom. Since hydrogen has only one electron, the patterns are simpler and consist of distinct spectral lines at certain wavelengths.

Neon, having ten electrons, exhibits a more complex arrangement of energy levels. The interactions between these electrons create many more possible transitions, hence a more complex pattern of emitted light. This is observable through neon signs that glow with a bright red-orange light, which is a mixture of various colors from the neon emission spectrum. The spectrum of neon consists of many more lines than that of hydrogen, and they are spread across a wider range of visible colors.