Section 01
Ionic bonding
A metal donates one or more electrons to a nonmetal, forming a positive cation and a negative anion. Opposite charges attract, forming a crystalline lattice. NaCl (table salt) is the classic example.
Section 02
Covalent bonding
Two nonmetals share pairs of electrons to fill their outer shells. Single, double, and triple bonds involve one, two, and three shared pairs. Water (H₂O) has two O–H single covalent bonds.
Section 03
Metallic bonding
Metal atoms release valence electrons into a shared 'sea'. This explains why metals conduct electricity, are malleable, and shiny.