Covalent Bonding

• Covalent bonding is the sharing of electron pairs between two atoms.
• This type of bond usually occurs between non-metals.
• The atoms involved in covalent bonding achieve a stable electron configuration typically by reaching a full outer shell.
• Covalent bonding results in the formation of molecules or molecular compounds.
• The electron pair being shared in a covalent bond is often referred to as a “bonding pair.”
• In a single covalent bond, one pair of electrons is shared. In a double bond, two pairs are shared, and in a triple bond, three pairs are shared.
• In covalent bonding, the shared electron pair is often provided by each of the atoms participating, but there can be instances where both electrons come from one atom, which is referred to as a coordinate or dative covalent bond.
• Covalently bonded compounds can exist in several states including gases, liquids, and solids at room temperature.
• Simple molecular substances have low melting and boiling points due to the weak intermolecular forces which are present amongst the molecules.
• Covalent bonds can also form giant covalent structures, like diamonds or graphite, where each carbon atom is covalently bonded to four other carbons.
• Polarity in covalent bonding arises when there is a difference in electronegativity between the bonded atoms, causing a dipole moment. Water (H2O) is an example of a polar molecule.
• The shape of a covalent molecule is determined by the repulsion of the electron pairs around the central atom. This is often referred to as Valence Shell Electron Pair Repulsion Theory (VSEPR).
• The strength of covalent bonding impacts physical properties of substances like melting point, boiling point, hardness, and more.
• The theory of hybridization is used to explain the geometrical arrangement of atoms in molecules.