Electrons orbiting around atoms do not follow a classical planetary motion, where they orbit the nucleus in a manner similar to planets orbiting the Sun. Instead, the behavior of electrons in atoms is described by quantum mechanics, which introduces a different concept called electron orbitals or electron clouds.
According to quantum mechanics, electrons are not thought of as particles moving in well-defined paths or orbits. Instead, they exist in a state of wave-particle duality, where they exhibit both particle-like and wave-like properties. Electron orbitals describe the probability distribution of finding an electron at a particular location around the nucleus.
The reason electrons do not "spin" around the nucleus like a macroscopic object is due to the wave nature of matter and the Heisenberg uncertainty principle. The uncertainty principle states that it is impossible to simultaneously know the exact position and momentum of a particle with absolute certainty. This principle applies at the microscopic level, such as with electrons.
The electron orbitals represent regions of space where electrons are likely to be found with a high probability. These orbitals have different shapes and energy levels, and each orbital can accommodate a specific number of electrons based on their quantum numbers.
The behavior of electrons in atoms is governed by the principles of quantum mechanics, including the quantization of energy levels and the wave-like nature of particles. Electrons occupy specific energy levels and transition between them by absorbing or emitting discrete amounts of energy.
In summary, the concept of electron orbitals in quantum mechanics provides a more accurate description of electron behavior in atoms compared to classical planetary motion. The wave-particle duality of electrons and the uncertainty principle play a fundamental role in understanding the behavior and distribution of electrons in atoms.