What bond is formed between a metal and a non-metal through electron transfer?

The bond formed between a metal and a non-metal through electron transfer is known as an ionic bond. In this type of bonding, the metal atom donates one or more electrons to become a positively charged cation, while the non-metal atom accepts the electrons to become a negatively charged anion. This transfer of electrons results in an electrostatic attraction between the oppositely charged ions, leading to the formation of a stable ionic compound.

Ionic bonding typically occurs between elements that have significantly different electronegativities, which is common for metals and non-metals. For instance, sodium (a metal) tends to lose one electron, while chlorine (a non-metal) tends to gain one electron, resulting in the formation of sodium chloride (table salt).

In contrast, metallic bonds involve the pooling of electrons among a lattice of metal atoms, hydrogen bonds are weak attractions between hydrogen and electronegative atoms, and covalent bonds involve the sharing of electrons between atoms, usually between non-metals. Each of these other bonding types has distinct characteristics and is not formed through the same electron transfer process that defines ionic bonds.