Covalent Bonds

We Will:

1. Overview Covalent Bonds

2. Lewis Structural Formulas for Molecular Bonding

3. Single, Double, and Triple Covalent Bonding

   
   

Sharing electrons to fill the octet

• Polar Covalent bond (nonmetal-nonmetal)

  • unequal sharing of electrons

    • stronger electronegative atom

• Nonpolar Covalent Bond (nonmetal-nonmetal)

  • equal sharing of electrons

Physical Properties

• Low melting point

• Usually, they are gasses, liquids, or waxy.

• Do not conduct electricity.

​Electron pair bonds (atoms share one or more valence electrons)

*Octet Rule (stable atoms desire a filled shell of 8)

• A dash or line represents shared electrons.

• Dots represent lone pairs (non-bonded) electrons.
  

Atoms can share one or more pairs of electrons

• Single Bonds

  • Share a single pair of electrons and have a single dash/line representing the paired electrons

• Double Bonds

  • Share two sets (pairs) of electrons and have a double dash/line representing the paired electrons.

• Triple Bonds

  • Share three sets (pairs) ...

• Triple Bonds

  • are the strongest and shortest

• Double Bonds

  • are in the middle

• Triple Bonds

  • are weaker than the triple and double bonds

​Energy is needed to break bonds—the more bonds, the more energy is required to separate atoms.

A chemical compound with a central atom surrounded by other atoms.

• Central atom often has the lowest electronegativity.

• The central atom has the least number of electrons