The Bohr model of the Helium atom is a simplified representation of the Helium atom proposed by Niels Bohr in 1913. It describes the Helium atom as having a nucleus containing two protons and two neutrons, orbited by two electrons in specific energy levels or shells.
The Bohr model explains the stability of the Helium atom by proposing that the two electrons in the atom's outermost shell have a stable configuration, known as the duplet, with two electrons in the s orbital. This configuration satisfies the octet rule and makes the Helium atom less reactive.
The energy levels in the Bohr model of the Helium atom represent the different allowed energy states of the electrons in the atom. These levels are quantized, meaning that the electrons can only exist in specific energy levels and cannot exist in between them. The energy levels determine the electron's energy and its distance from the nucleus.
The Bohr model explains the emission spectrum of Helium by proposing that the electron can jump from one energy level to another by absorbing or emitting a precise amount of energy. When the electron jumps from a higher energy level to a lower one, it emits energy in the form of light, creating a unique emission spectrum for each element.
The Bohr model has several limitations, including its inability to explain the fine details of atomic structure and the behavior of atoms with more than one electron. It also does not account for the wave-like behavior of electrons, and it does not accurately predict the energy levels of heavier elements. These limitations were addressed by the development of quantum mechanics, which provides a more comprehensive understanding of atomic structure.