Co-valent bond

Covalent Bond

A covalent bond is a type of chemical bond that involves the sharing of electron pairs between atoms. These shared electrons allow each atom to achieve a stable electronic configuration, typically resembling that of a noble gas. Covalent bonding commonly occurs between non-metal atoms that have similar electronegativities.

Characteristics of Covalent Bonds

• Formed by the mutual sharing of one or more pairs of electrons between two atoms.
• Typically occurs between non-metallic elements.
• The resulting compounds are called covalent or molecular compounds.
• Covalent bonds can be single (sharing one pair of electrons), double (two pairs), or triple (three pairs).
• Usually result in molecules with low melting and boiling points compared to ionic compounds.
• Do not conduct electricity in solid or liquid state as there are no free ions.

Types of Covalent Bonds

• Single Covalent Bond: One pair of electrons is shared between two atoms (e.g., H₂, Cl₂, CH₄).
• Double Covalent Bond: Two pairs of electrons are shared (e.g., O₂, CO₂).
• Triple Covalent Bond: Three pairs of electrons are shared (e.g., N₂, C₂H₂).

Examples of Covalent Bonds

• Hydrogen Molecule (H₂): Each hydrogen atom shares one electron to form a stable H–H bond.
• Water (H₂O): Oxygen shares two of its electrons with two hydrogen atoms, forming two single covalent bonds.
• Methane (CH₄): Carbon forms four single covalent bonds with four hydrogen atoms.

Polar and Non-Polar Covalent Bonds

• Non-Polar Covalent Bond: Electrons are shared equally between atoms (e.g., H₂, N₂).
• Polar Covalent Bond: Electrons are shared unequally due to differences in electronegativity (e.g., H₂O, HCl).

Covalent bonding is fundamental in the formation of countless substances around us. These bonds determine the structure, reactivity, and properties of molecules and are central to both organic and inorganic chemistry.