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cbram
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Why is electron rotating in h/2pi orbit does not radiate energy
The value of h/2π, also known as the reduced Planck's constant, is a fundamental constant in quantum mechanics. It represents the minimum amount of angular momentum that can be possessed by a particle, such as an electron, in a given quantum state.
Electrons in h/2π orbits do not radiate because they are in a state of constant motion and do not experience any acceleration. According to classical electromagnetic theory, accelerated charges emit electromagnetic radiation, but this does not apply to the quantum realm where electrons are confined to discrete energy levels.
Electrons can transition between h/2π orbits without radiating by absorbing or emitting a photon. When an electron absorbs a photon, it gains energy and jumps to a higher energy level, and when it emits a photon, it loses energy and drops to a lower energy level. These transitions do not involve acceleration and therefore do not result in radiation.
Yes, electrons can emit radiation in other types of orbits, such as circular orbits. These orbits are not quantized like h/2π orbits and allow for continuous changes in velocity, resulting in acceleration and radiation. However, in the quantum realm, electrons are typically found in discrete energy levels rather than continuous orbits.
The concept of h/2π orbits is a key component of the Bohr model of the atom, which describes electrons as orbiting the nucleus in specific energy levels. The allowed energy levels in the Bohr model correspond to the h/2π orbits of the electron, with each level representing a different energy state. This model was later refined and expanded upon by quantum mechanics, which introduced the concept of orbitals and the uncertainty principle.