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.

The central atom may have an incomplete octet, especially common with Beryllium and Boron.

Form double or triple bonds by erasing lone pairs on surrounding atoms.

It is impossible to pair all electrons, resulting in a molecule with unpaired electrons.

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.