1. Covalent Bonds

2. Objective Describe molecular bonds
Draw e- dot structures for covalent compounds

3. Molecular Compounds Covalent bond: when 2 non-metals share e-
Forms a covalent compound or molecular compound (also called a molecule)

4. Molecular Compounds Properties:
Low melting and boiling points due to weak bond (much weaker than ionic)
Mostly liquids, gases at room temp
Weak conductors of electricity
Diatomic molecule: 2 of same atom share e-
7 diatomic molecules: H2, Cl2, Br2, F2, I2, N2, O2

5. Octet Rule
Covalent bonds form when each non-metal atom shares e- in order to attain e- config. of a noble gas (8 electrons)
H: to act like He it only needs 2 e-

6. Now you try… Tell your neighbor 1 property of covalent compounds.
Tell you neighbor how electrons are involved in a covalent bond

7. Single Covalent Bonds Single bond: 1 pair of e- (2 e- ) shared
Ex 1: dot structure for H2

8. Single Covalent Bonds Ex 2: dot structure for Cl2
e- pairs that are not shared: unpaired or unshared e-

9. Single Covalent Bonds
Ex 3: dot structure for H2O

10. Single Covalent Bonds
Ex 4: dot structure for NH3

11. Now you try…
Use your periodic table to draw the dot structure for the following molecules in your notes.
A) SiH4
B) F2O
C) PCl3

12. Multiple Covalent Bonds
Double bond: 2 pairs of e- (4 total e-) shared
Triple bond: 3 pairs of e- (6 total e-) shared
Ex 1: dot structure for O2

13. Multiple Covalent Bonds
Ex 2: dot structure for N2

14. Now you try…
In your notes draw the dot structure for CO2.

15. Coordinate Covalent Bonds
Coordinate covalent bond: when 1 atom contributes both e- to a bond
Ex 1: CO

16. Coordinate Covalent Bonds
Ex 2: NH4+

17. Coordinate Covalent Bonds
Ex 3: SO3-2

18. Now You Try…
Draw the dot structure for SO2

19. Ticket Out the Door
Draw the dot structure for the following molecules:
1) F2
2) CH4