Introduction
Bohr's atomic model, proposed by Niels Bohr in 1913, was a significant leap in understanding atomic structure, particularly for hydrogen and hydrogen-like species. It successfully addressed the limitations of Rutherford's model, which failed to explain the stability of atoms and the line spectrum of hydrogen. Bohr's model introduced the revolutionary concept of quantized energy levels, fundamentally changing our perception of electron behavior within an atom. This concept is crucial for NEET Chemistry, as it forms the basis for understanding atomic spectra, electronic configurations, and various chemical phenomena.
Bohr's model postulates that electrons revolve around the nucleus in specific, stable orbits, also known as stationary states, without radiating energy. These orbits are associated with definite amounts of energy, meaning that the electron can only exist in certain discrete energy states. The electron's energy is said to be "quantized." When an electron jumps from one energy level to another, it either absorbs or emits energy in the form of a photon, corresponding to the energy difference between the levels. Mastering these energy levels and their associated calculations is key to scoring well in NEET.