In which type of bond do electrons get transferred between atoms?

In ionic bonds, electrons are transferred from one atom to another, resulting in the formation of charged ions. This process typically occurs between atoms with significantly different electronegativities, such as alkali metals and halogens. When an electron is transferred from a metal atom (which tends to lose electrons easily) to a non-metal atom (which tends to gain electrons), the metal becomes positively charged (cation), and the non-metal becomes negatively charged (anion). The resultant opposite charges create an electrostatic attraction that holds the ions together in an ionic compound.

Covalent bonds involve the sharing of electrons between atoms rather than transferring them, which distinguishes them from ionic bonds. Metallic bonds, on the other hand, involve a "sea of electrons" where electrons are delocalized across a lattice of metal atoms, allowing for conductivity and malleability. Hydrogen bonds are a type of intermolecular force that occurs between molecules and do not involve the transfer of electrons. Therefore, the correct identification of ionic bonds as the type where electrons are transferred highlights the fundamental nature of how these bonds form and the resulting impact on the properties of the compounds formed.