Which arrow in the energy diagram for an atom represents the absorption of light with the shortest wavelength? (LO 5.7)

Atoms have quantized energy levels, represented by principal quantum numbers (n). Electrons can occupy these levels, and transitions between them involve the absorption or emission of energy, typically in the form of light. The greater the difference in energy between levels, the higher the energy (and shorter the wavelength) of the absorbed or emitted light.

The energy of a photon is inversely related to its wavelength, described by the equation E = hc/λ, where E is energy, h is Planck's constant, c is the speed of light, and λ is the wavelength. Therefore, shorter wavelengths correspond to higher energy photons. This relationship is crucial for understanding which transitions in an energy diagram correspond to the absorption of light with the shortest wavelength.

The Bohr model describes the behavior of electrons in hydrogen-like atoms, where electrons orbit the nucleus in defined energy levels. When an electron absorbs energy, it can move to a higher energy level, which is depicted in energy diagrams with arrows indicating the direction of the transition. The arrows' lengths and positions reflect the energy differences between levels, helping to identify which transition corresponds to the absorption of light with the shortest wavelength.