What type of bond is formed when atoms have different electronegativities and transfer electrons?

The formation of an ionic bond occurs when atoms with significantly different electronegativities transfer electrons from one atom to another. In this type of bond, one atom, typically a metal, loses one or more electrons and becomes positively charged, while the other atom, usually a nonmetal, gains those electrons and becomes negatively charged. This transfer of electrons results in the formation of charged ions, which are held together by the electrostatic attraction between the positive and negative charges.

The strength of ionic bonds comes from this attraction, and the resulting ionic compounds often have high melting and boiling points due to the strong forces holding the ions together. These compounds also tend to be soluble in water and conduct electricity when dissolved or molten, further indicating the presence of freely moving ions.

The other bond types have different characteristics: metallic bonds involve the sharing of free electrons among a lattice of metal atoms, covalent bonds involve the sharing of electrons between atoms with similar electronegativities, and coordinate covalent bonds involve one atom donating both electrons for a shared pair. Understanding these distinctions clarifies why the transfer of electrons specifically leads to ionic bonds.