Electrons do indeed repel each other due to their mutual electric charges. The repulsion between electrons is a fundamental aspect of electromagnetism. However, within the framework of quantum theory, there are additional factors that come into play, leading to the stability of atoms and matter. Let's explore these factors:
Quantum Mechanical Wavefunction: According to quantum mechanics, electrons are described by wavefunctions, which represent the probability amplitudes of finding an electron at a particular location. The wavefunction accounts for the wavelike behavior of particles and determines the electron's distribution in space.
Pauli Exclusion Principle: The Pauli exclusion principle, a fundamental principle in quantum mechanics, states that no two identical fermions (such as electrons) can occupy the same quantum state simultaneously. In other words, within a given system, each electron must have a unique set of quantum numbers, including spin, orbital angular momentum, and energy level. This principle ensures that electrons in an atom cannot crowd into the same state and provides a mechanism to distribute them in different energy levels and orbitals.
Electron Orbital Structure: Electrons in atoms occupy discrete energy levels and specific spatial regions called orbitals. Each orbital can accommodate a maximum number of electrons, following a specific pattern determined by quantum numbers. These orbitals act as "containers" for electrons and help distribute them within the atom in a way that minimizes their repulsion. The shape and orientation of the orbitals influence the electron distribution and determine the overall stability of the atom.
Shielding and Screening: Electrons in an atom are subject to the electric field created by the positively charged nucleus. However, the outer electrons experience a reduced net electrostatic attraction due to the shielding effect of inner electrons. Inner electrons partially shield the outer electrons from the full nuclear charge, reducing their repulsion and stabilizing the atom.
It is important to note that while electrons repel each other, the quantum mechanical effects described above play a crucial role in determining their distribution, stability, and behavior within atoms. The interplay between the repulsion of electrons and the quantum-mechanical principles allows for the formation of stable atomic structures and the diverse chemical properties observed in matter.