1. Covalent Bonding

2. Recall that in ionic bonds… Two atoms, one a metal and the other a nonmetal form due to an attraction between oppositely charged ions. It produces a very strong bond that takes much energy to break

3. Covalent bonds Form between two nonmetals Share electrons between the two atoms Form molecular compounds

4. Double and Triple Bonding This bonding pattern occurs frequently between atoms of the same element Two (double) or three (triple) pairs of electrons are shared between the atoms

5. Properties of molecular compounds Low boiling and melting points because it takes less energy to break the bonds between atoms Poor conductors of electricity (no charged particles) Good insulators

6. Polar covalent bonds Some atoms such as oxygen and fluorine are more electronegative meaning they pull more strongly on the shared covalent bonds Electrons tend to spend more time around the oxygen (or fluorine) atom causing them to have a slight negative electrical charge.

7. Water is a polar covalent molecule. The electrons from the hydrogen atoms are pulled closer to the oxygen atom giving the molecule a negative charge on one end and positive charges on the hydrogen ends.

8. Nonpolar covalent bonds Sharing of electrons is equally shared between the two atoms (pull with equal strength)

9. Just as a summary to what each bond looks like…

10. # of atomsPrefix OneNone, mono TwoDi- ThreeTri- FourTetra- FivePenta- SixHexa- SevenHepta- EightOcta- Naming covalent compounds Unlike ionic compounds, covalent compounds include prefixes These prefixes tell you the number of atoms of each element in the compound

11. Can you name the various compounds? CO 2 CCl 4 P 2 O 5 PBr 3 N 2 O Carbon dioxide Carbon tetrachloride Diphosphorus Pentaoxide Phosphorus tribromide Dinitrogen monoxide