Which type of bonding involves the transfer of electrons?

Ionic bonding involves the transfer of electrons between atoms. This occurs typically between metals and non-metals. In this type of bond, one atom donates one or more of its electrons to another atom, leading to the formation of charged ions. The metal atom, having a tendency to lose electrons, becomes a positively charged ion (cation), while the non-metal atom, which gains electrons, becomes a negatively charged ion (anion). The resulting electrostatic attraction between these oppositely charged ions creates the ionic bond. This process results in stable compounds with distinct properties, such as higher melting and boiling points compared to covalent compounds.

Covalent bonding, on the other hand, does not involve the transfer of electrons but rather the sharing of electron pairs between atoms. Metallic bonding is characterized by a 'sea of electrons' that are free to move around, which gives metals their conductivity and malleability. Hydrogen bonding is a specific type of dipole-dipole attraction between molecules, particularly involving hydrogen atoms, and does not involve electron transfer either. This understanding highlights why ionic bonding is the only type of bonding among the options that specifically involves electron transfer.