Chemical Bonding and its type ?

Chemical bonds are forces that hold atoms together in molecules and compounds. Atoms bond to achieve a stable electron configuration (usually 8 electrons in the outer shell — the octet rule).

1. Ionic Bond:
An ionic bond forms when one atom transfers one or more electrons to another atom. This usually occurs between a metal and a non-metal. The atom that loses electrons becomes a positively charged ion (cation). The atom that gains electrons becomes a negatively charged ion (anion). The opposite charges attract each other, forming an ionic bond.

Example: Sodium chloride (NaCl — table salt). Sodium (Na) gives one electron to Chlorine (Cl). Na becomes Na⁺ and Cl becomes Cl⁻. The attraction between Na⁺ and Cl⁻ is the ionic bond.

Properties of ionic compounds: High melting points, conduct electricity when dissolved in water, form crystalline structures.

2. Covalent Bond:
A covalent bond forms when two atoms share one or more pairs of electrons. This usually occurs between two non-metals. Neither atom completely takes the electrons — they share them.

Single covalent bond: One pair of electrons shared. Example: H₂ (H—H)
Double covalent bond: Two pairs of electrons shared. Example: O₂ (O=O)
Triple covalent bond: Three pairs of electrons shared. Example: N₂ (N≡N)

Example: Water (H₂O). Each hydrogen atom shares one electron with oxygen. This sharing satisfies the needs of all atoms.

3. Coordinate Covalent Bond (Dative Bond):
A coordinate covalent bond is a special type of covalent bond where both electrons in the shared pair are contributed by the same atom (called the donor). The other atom (called the acceptor) provides an empty orbital to accept the pair.

Example: The formation of the ammonium ion (NH₄⁺). Nitrogen in ammonia (NH₃) has a lone pair of electrons that it donates to a hydrogen ion (H⁺), which has an empty orbital. The resulting bond is a coordinate covalent bond.