Explain How Chemical Bonding Forms Compounds With Examples

A compound is formed when atoms of different elements join together via chemical bonds. This bonding process is driven by the atoms' tendency to achieve a more stable electron configuration, typically a full outer shell (the octet rule). Atoms will transfer or share electrons to reach this stable state.

1. Ionic Bonding (Transfer of Electrons)

This type of bond typically forms between a metal and a non-metal. The metal atom loses one or more electrons (becoming a positive ion, or cation) and the non-metal atom gains those electrons (becoming a negative ion, or anion). The compound is held together by the strong electrostatic attraction between these opposite charges.

• Example: Sodium Chloride ($NaCl$)
  Sodium (Na), a metal, has one valence electron. Chlorine (Cl), a non-metal, has seven. Sodium transfers its one electron to chlorine. This gives Na a full inner shell ( and Cl a full outer shell . The resulting ions  attract each other strongly, forming the compound table salt.

2. Covalent Bonding (Sharing of Electrons)

This type of bond typically forms between two non-metals. The atoms share one or more pairs of valence electrons to achieve stable outer shells. This shared pair of electrons forms the bond that holds the atoms together, creating a molecule.

• Example: Water 
  Oxygen (O) needs two electrons to complete its outer shell. Hydrogen (H) needs one. The oxygen atom shares one electron pair with one hydrogen atom, and a second electron pair with another hydrogen atom. This sharing allows the oxygen to "count" 8 electrons in its outer shell and each hydrogen to "count" 2, making all atoms stable.