Electrons in covalent bonds do not revolve around nuclei in the classical sense, as suggested by the planetary model. Instead, they exhibit wave-like behavior and are described as probability clouds rather than point particles. In a covalent bond, an electron is shared between two nuclei, spending time around both, but it does not move in a traditional manner. The concept of delocalization allows an electron to exist in multiple locations simultaneously, influenced by quantum mechanics. The energy of a chemical bond involves not only the electrostatic attraction between the nucleus and the electron cloud but also an "exchange energy" due to quantum effects. Additionally, the shape of orbitals can extend beyond the bond center, affecting bond strength through anti-bonding interactions. Understanding these principles is crucial for grasping the nature of covalent bonding and electron behavior in molecules.
