What type of bond is formed when electrons are shared between atoms?

When electrons are shared between atoms, a covalent bond is formed. This type of bonding occurs when two nonmetal atoms come together and share their valence electrons in order to achieve a full outer shell, which is often a stable electronic configuration.

In covalent bonding, the shared electrons allow each atom to attain a more stable electron configuration, typically resembling that of the nearest noble gas. This is crucial in many compounds, as it not only stabilizes the individual atoms involved but also contributes to the characteristics of the resulting molecules, such as their shape, polarity, and reactivity.

In contrast, ionic bonds involve the transfer of electrons from one atom to another, leading to the formation of charged ions that attract each other. Metallic bonds consist of a "sea of electrons" that are shared more free-form among metal atoms, contributing to properties like conductivity and malleability. Hydrogen bonds are a type of intermolecular force rather than a true bond between atoms; they arise from the attraction between a hydrogen atom covalently bonded to a more electronegative atom and another electronegative atom.

Therefore, the sharing of electrons specifically defines a covalent bond, highlighting the unique nature of molecular interactions in chemistry.