Covalent Bonds Overview

• Involves non-metals sharing electrons to achieve a full stable valence shell (no gain or loss of electrons).

Drawing Covalent Lewis Dots

1. Calculate total number of valence electrons across all atoms.

2. Identify the central atom based on electronegativity (usually C or the least electronegative element).

3. Positioning:

   • Evenly space other atoms around the central atom.

4. Draw in the valence electrons for each atom.

5. Forming Bonds:

   • Look for unpaired electrons and connect using single dots to form bonds.

   • Pair and bond until all atoms have 8 valence electrons (or 2 for H).

6. Replace dots with dashes to represent bonds.

Types of Covalent Bonds

• Single Bond: Sharing of two electrons.

• Double Bond: Sharing of four electrons.

• Triple Bond: Sharing of six electrons.

• Example diagrams include water (H₂O) and carbon dioxide (CO₂).

• Single Bond: Determine central element for H₂O.

• Double/Triple Bonds: Practice with CO₂ and N₂.

• Review ionic and covalent compounds.

• Box the first element to determine the bond type.

• Show electron transfer for ionic compounds and sharing for covalent in dot diagrams.