Bohr’s theory was a start but it only explained the hydrogen atom (one electron as a particle orbiting around a nucleus). The Quantum-Mechanical (QM) model, first developed by Erwin Schrodinger in 1926 describes electrons mathematically…

The simplest spectra to study are those of H, as it only has one electron. These contain sets of lines which can be related to the energy levels. The Lyman series (in the ultra-violet) correspond…

Moving an electron between a lower and higher energy level can only be achieved if it absorbs energy of a particular amount; this could be from a particular wavelength of light. Conversely if an electron…

Emission and absorption spectra are evidence that the electrons within an atom have quantised energies i.e. an electron cannot possess a continuous range of values for energy but must have specific values called energy levels.…

An element can also absorb light at specific wavelengths. An absorption spectrum can be obtained by passing a continuous radiation spectrum (white light) through a vapour of the gas. The absorption spectrum consists of a…