Bohr's Hydrogen model is a simplified model of the atom proposed by Niels Bohr in 1913. It states that electrons orbit the nucleus in specific energy levels, and can only transition between these levels by absorbing or emitting specific amounts of energy. This model can be applied to a He ion, which contains only two electrons, by using the same principles to determine the energy levels and transitions of the electrons.
The energy of a He ion's electron can be determined by using the equation E = -13.6/n^2, where n is the energy level. This equation is derived from Bohr's model and shows that the energy of an electron is inversely proportional to the square of its energy level. So, the higher the energy level, the lower the energy of the electron.
Bohr's model is a simplified model and does not account for the more complex behavior of electrons in atoms with multiple electrons. However, it can still provide a general understanding of the behavior of electrons in a He ion. More accurate models, such as the quantum mechanical model, are necessary for more precise predictions.
Bohr's model explains the emission spectrum of a He ion by showing that when an electron transitions from a higher to a lower energy level, it emits a photon of specific energy. This energy corresponds to a specific wavelength of light, creating the characteristic emission spectrum of a He ion.
Bohr's model can be applied to other ions or atoms, but it may not accurately predict their behavior. This is because it was developed specifically for the hydrogen atom and does not account for the complexity of other atoms and ions. However, it can still provide a basic understanding of their energy levels and transitions.