Bohr’s hypothesis explained only spherical orbits. This concept was only relevant to atoms with one electron. The Bohr model could not explain atoms with more than one electron, such as lithium and helium. It may be defined as a function of electron mass, velocity, and the radius of the orbit where the electron is travelling in a particular stationary condition. An electron’s angular momentum is quantised.The frequency of radiation received or released when a transition occurs between two stationary states with ΔE energy differences.The shift in energy does not occur continuously. However, when the electron or energy absorbs the requisite quantity of energy is released when the electron goes from a higher stationary state to a lower stationary state, the electron will move from a lower stationary state to a higher stationary state.

The energy of an electron in orbit remains constant over time.

These orbits are arranged in a concentric circle around the nucleus. Orbits, stationary states, and permitted energy states are all names for these routes.

The electron in a hydrogen atom can travel in a circular route with a set radius and energy around the nucleus.

The following postulates underpin Bohr’s model of the hydrogen atom: We may use the model to justify much atomic structure and spectra points, though not current quantum mechanics. He applied Planck’s notion of energy quantification. Neils Bohr (1913) was the first to statistically explain the general properties of the structure and spectrum of the hydrogen atom. As a result, it was proposed that an electron might travel between these orbits by absorbing or emitting photons (energy). As a result, an atom in the smallest orbit will be stable since the electron will not hop to a lower orbit. In addition, atoms are unstable because electrons shift to lower orbits, causing radiation to be produced. Electrons in smaller orbits will have less energy as a result. To summarise Bohr’s atomic model, electron energy levels are focussed on the size of the orbits. In Niels Bohr’s atomic theory, electrons with fixed sizes and energies travel in orbits around a positively charged nucleus, similar to how planets orbit the sun.

Electrons do not emit energy when rotating in distinct orbits.

Only specific unique orbits known as discrete orbits of electrons are permitted inside the atom.

To address the criticisms levelled about Rutherford’s atomic model, Neils Bohr proposed the following postulates concerning the atomic model: These were: electromagnetic radiation’s dual nature suggests that it has both wave-like and particle-like properties and only by assuming quantised electronic energy levels in atoms could experimental data about atomic spectra be described. Two breakthroughs were crucial in the development of Bohr’s atomic model. Niels Bohr utilised these observations to elaborate on Rutherford’s concept.

Previously, studies from radiation interactions with matter offered a plethora of information on the structure of atoms and molecules. On the majority of topics, he agrees with him, such as the notions of nucleus and electrons surrounding it. It was essentially an upgraded version of Rutherford’s atomic model that overcame its shortcomings. Niels Bohr suggested an atomic structure model, commonly known as Bohr’s atomic model, explaining an atom as a tiny, positively charged nucleus surrounded by electrons which move in circular orbits all around positively charged nucleus such as planets around the sun in our solar system, with attraction supplied by electrostatic forces. Thomson’s and Rutherford’s atomic models failed to answer any atom’s energy and stability problems.

Bohr model of helium atom