Define and describe ionic and covalent bonds. An ionic bond is a type of chemical bond formed through an electrostatic attraction between two oppositely charged ions. A covalent bond is the chemical bond that involves the sharing of pairs of electrons between atoms. A compound is made when two or more atoms form a chemical bond, linking them together. The two types of bonds are ionic bonds and covalent bonds. In an ionic bond, the atoms are bound together by the attraction between oppositely charged ions. If the electron is shared equally between the atoms forming a covalent bond, then the bond is said to be nonpolar.
An electron is more attracted to one atom than to another which forming a polar covalent bond. Ionic bonds are formed between a cation and an anion. Pure ionic bonding cannot exist: all ionic compounds have some degree of covalent bonding. An ionic bond is considered a bond where the ionic character is greater than the covalent character. The larger the difference in electronegativity between the two atoms involved in the bond, the more ionic the bond is. Bonds with partially ionic and partially covalent character are called polar covalent bonds. Ionic bonding is a form of no covalent bonding.
Ionic compounds conduct electricity when molten or in solution, but not as a solid. They generally have a high melting point and tend to be soluble in water. The stable balance of attractive and repulsive forces between atoms when they share electrons is known as covalent bonding. For many molecules, the sharing of electrons allows each atom to attain the equivalent of a full outer shell, corresponding to a stable electronic configuration. Covalent bonding includes many kinds of interaction, including ? -bonding, ? -bonding, metal-to-metal bonding, agnostic interactions, and three-center two-electron bonds.