1. Write the empirical formula. 2. Draw each atom with valence electrons. 3. Transfer electrons from metal to nonmetal to achieve full octets. 4. Use brackets around each ion with charges outside.

1. Count total valence electrons. 2. Draw the central atom. 3. Connect atoms with single bonds. 4. Add lone pairs to outer atoms to complete octets. 5. Count electrons used. 6. Form double/triple bonds if too many electrons. 7. Add to central atom if too few.

A double bond

A triple bond

Ionic bond

Visual tool showing how atoms bond, displaying valence electrons and bonds to understand molecular shapes and reactivity.

Atoms 'want' a full valence shell, usually 8 electrons, to achieve stability.

Electrons around a single atom, not shared with other atoms in a bond.

Electrons shared between atoms, forming a chemical bond (represented by a dash in Lewis diagrams).

A model stating that electrons are localized and stay put, not freely roaming around the molecule.

Central atoms with atomic number ≥ 14 can have more than 8 electrons in their valence shell.