What type of bond occurs when electrons are transferred from one atom to another?

An ionic bond occurs when electrons are transferred from one atom to another, resulting in the formation of charged ions. This process typically happens between atoms with significantly different electronegativities, such as metals and nonmetals. The atom that loses one or more electrons becomes positively charged (a cation), while the atom that gains those electrons becomes negatively charged (an anion). The electrostatic attraction between these oppositely charged ions creates the ionic bond.

In contrast, a covalent bond involves the sharing of electrons between two atoms, which typically occurs between nonmetals. A hydrogen bond is a weaker interaction that arises when a hydrogen atom, covalently bonded to a highly electronegative atom, interacts with another electronegative atom. Metallic bonds occur between metal atoms and involve a 'sea of electrons' that are shared among many atoms, allowing for electrical conductivity and malleability in metals. Understanding these different types of bonds is crucial for grasping how atoms interact to form compounds.