What type of bond results from the transfer of electrons?

An ionic bond is formed through the transfer of electrons from one atom to another, resulting in the creation of charged ions. When an electron is transferred, one atom becomes positively charged (the cation) and the other becomes negatively charged (the anion). This electrostatic attraction between the oppositely charged ions constitutes the ionic bond.

For instance, in the formation of sodium chloride (table salt), sodium donates an electron to chlorine, resulting in a sodium ion (Na⁺) and a chloride ion (Cl⁻). The resulting attraction between these two oppositely charged ions is a classic example of an ionic bond. This kind of bonding is typically seen between metals and nonmetals and is characterized by high melting and boiling points due to the strength of the ionic interactions.

Other types of bonds, such as hydrogen, covalent, and polar bonds differ fundamentally in their formation. Hydrogen bonds are weak attractions between a hydrogen atom covalently bonded to an electronegative atom and another electronegative atom. Covalent bonds involve the sharing of electrons rather than their transfer. Polar bonds occur when electrons are shared unequally between atoms, leading to a distribution of electrical charge. Each of these bonds employs different mechanisms for their formation,