Every bit of matter around you is held together by chemical bonds. Sometimes, chemical bonds are broken, such as during a chemical reaction, only for atoms to bond again to form different molecules. Energy is always released to generate bonds and, likewise, energy is always required to break bonds.

There are two main types of chemical bonds: ionic and covalent.

What are ionic and covalent bonds?

Atoms bond together to form compounds because in doing so they attain lower energies than they possess as individual atoms, becoming more stable in the process. By the Law of Conservation of Energy, when a new chemical bond is formed, the chemical reaction releases an amount of energy (usually as heat) almost equal to the difference in the amounts of stored chemical energy between the products and the reactants. This stored chemical energy of the system, or heat content, is known as its enthalpy.

An ionic bond forms when two ions of opposite charges exchange electrons between them, where an ion is an atom that has either lost or gained an electron. Ions that loss one or more electrons have more protons than electrons, which means they have a positive charge. Such ions are called cations (metals). On the other hand, gaining electrons grants the ion a negative charge. Chemists refer to such ions as anions (non-metals).

Ionic compounds are typically neutral. Therefore, ions combine in ways that neutralize their charges.

A textbook example of an ionic compound is sodium chloride, also known as table salt. A single sodium atom has 11 protons and 11 electrons, but only a single electron in its outer shell (or valence shell). Chlorine is made up of 17 protons and 17 electrons, and has 7 electrons in its outer shell. When the two atoms react, sodium (electropositive) loses its valence electron to chlorine (electronegative). Now, in the resulting crystal structure, each sodium ion is surrounded by six chloride ions and each chloride ion is surrounded by six sodium ions. What’s more, each ion has a complete electron shell that corresponds to the nearest inert gas; neon for a sodium ion, argon for a chloride ion

Covalent bonds form when atoms or ions share electrons such that their outer shells become occupied. Covalent bonds, also called molecular bonds, only form between nonmetal atoms with identical or relatively close electronegativity value.  Electronegativity, denoted by the symbol χ, is a chemical property that describes the tendency of an atom to attract a shared pair of electrons (or electron density) towards itself.

The number of covalent bonds an atom can form is called the valence of the atom. This property represents the electrons of an atom that can participate in the formation of chemical bonds with other atoms. They are the furthest electrons from the nucleus.

A prime example of a covalent bond is the hydrogen molecule, which forms from two hydrogen atoms, each with one electron in their outer shell. Bond formation releases heat; therefore, it is exothermic. For the hydrogen molecule, the heat released during its formation, also known as the standard enthalpy change (ΔH°),  is −435 kJ per mole. The reverse process, breaking the H—H bond, requires 435 kJ per mole, a quantity called the bond strength.

Another classic example of a covalent bond is hydrogen chloride (HCl), which is a hydrogen halide. The chlorine atom has 7 atoms in its outer shell while hydrogen has 1 electron in its outer shell. Both combine perfectly so each atom fills their valence shells, forming a highly stable molecule. Now, the HCl molecule will not react further with other chlorine or hydrogen atoms.

 

Differences between ionic and covalent bonds

  • Covalent bonds are much more common in organic chemistry than ionic bonds.
  • In covalent bonds, atoms share electrons, whereas in ionic bonds atoms transfer electrons.
  • The reaction components of covalent bonds are electrically neutral, whereas for ionic bonds they are both charged. This explains why sodium chloride (salt) conducts electricity when dissolved — its components are charged.
  • Covalent bonds are easier to break than ionic bonds.
  • Covalent bonds are far more common in nature than ionic bonds. Most molecules in living things are covalently bonded, for instance.
  • Covalent bonds can form between atoms of the same elements (i.e. H2). However, ionic bonds cannot do this.
  • Covalent bonds are formed between two non-metals, whereas ionic bonds are formed between a metal and non-metal.
  • Molecules formed by covalent bonds have a low melting point, whereas those with ionic bonds have a high melting point. The same relationship exists for boiling point.
  • At room temperature, covalently bonded molecules are in the vast majority of cases liquids or gases, whereas ionic compounds are solid.

Similarities between ionic and covalent bonds

  • Both types of bonds lead to the formation of stable chemical compounds.
  • It takes exothermic reactions (i.e. that release heat) in order to create ionic and covalent bonds.
  • Valence electrons are involved in both bonding processes.
  • It doesn’t matter whether a molecule is formed through ionic or covalent bonding as far as its electrical charge is concerned: the result is always electrically neutral.