1. “Dancer”, Fernando Botero Colombian, 1982
Covalent Bonding
Vocabulary
covalent bond
single bond
double bond
triple bond
molecule
structural formula
“Dancer”, Fernando Botero Colombian, 1982

2. Review
What is an ionic bond?

3. What if?
If an ionic bond requires one atom to lose electrons and one atom to gain electrons, how could two atoms bond if both atoms do not want to lose electrons but still must follow the octet rule?

4. What if?
Let’s look at an example: chlorine gas, Cl2 How many electrons does each chlorine atom need to gain to have a full octet? Cl Cl

5. What if?
Because neither chlorine atom is willing to to give up an electron, they can not form an ionic bond. Instead each atom can SHARE one electron with the other atom to fulfill the octet rule for each. Cl Cl

6. What if?
Because neither chlorine atom is willing to to give up an electron, they can not form an ionic bond. Instead each atom can SHARE one electron with the other atom to fulfill the octet rule for each. Cl Cl

7. What if?
Because neither chlorine atom is willing to to give up an electron, they can not form an ionic bond. Instead each atom can SHARE one electron with the other atom to fulfill the octet rule for each. Cl Cl

8. What if?
Notice that by sharing, each atom now has 8 valence electrons around it and follows the octet rule: the 7 it originally had and 1 from the other atom. Cl Cl

9. Covalent Bonding
This sharing of electrons is called a covalent bond. Because only one electron is being shared from each atom in this example, it is called a single covalent bond.
When atoms bond covalently, they form molecules. Cl Cl
This is the Lewis structure for the Cl2 molecule.

10. Covalent Bonding
Let’s look at another molecule, O2. Draw the Lewis structures for the two oxygen atoms separately. O O
How do you think these two atoms can bond?
How many electrons does each atom need to gain or share to achieve an octet?

11. Covalent Bonding
Let’s look at another molecule, O2. Draw the Lewis structures for the two oxygen atoms separately. O O
How do you think these two atoms can bond?
How many electrons does each atom need to achieve an octet?

12. Covalent Bonding
Let’s look at another molecule, O2. Draw the Lewis structures for the two oxygen atoms separately. O O
How do you think these two atoms can bond?
How many electrons does each atom need to achieve an octet?

13. Covalent Bonding
Let’s look at another molecule, O2. Draw the Lewis structures for the two oxygen atoms separately. O O
How do you think these two atoms can bond?
How many electrons does each atom need to achieve an octet?

14. This is the Lewis structure for the O2 molecule.
Covalent Bonding
Look at each atom now. Each atom is sharing two electrons with the other atom and now each has 8 valence electrons. O O
This is the Lewis structure for the O2 molecule.
Because each atom is sharing 2 valence electrons, this is called a double covalent bond.

15. Covalent Bonding
Look at each atom now. Each atom is sharing two electrons with the other atom and now each has 8 valence electrons. O O
We can also draw it this way. This is called the structural formula for O2. Each line represents two electrons.

16. Covalent Bonding Important covalent bonding notes:
sharing of electrons to achieve an octet
(hydrogen is a notable exception because it
only needs two valance electrons)
occur between non-metal atoms
can be single, double, or triple bond

17. Practice NaCl C6H12O6 H2O SrBr2 Li3P Al2O3 CO2 PCl5
Which of the following compounds will have covalent bonds?
NaCl
C6H12O6
H2O
SrBr2
Li3P
Al2O3
CO2
PCl5

18. Practice
Draw the Lewis structure for water. Are the bonds single, double, or triple covalent bonds.
Steps
1) Draw each atom’s Lewis structure.
2) Pair up unpaired electrons. H O H

19. Practice
Draw the Lewis structure for water. Are the bonds single, double, or triple covalent bonds.
Steps
1) Draw each atom’s Lewis structure.
2) Pair up unpaired electrons.
3) Rearrange atoms so that electron pairs are connected. H O H

20. Practice
Draw the Lewis structure for water. Are the bonds single, double, or triple covalent bonds.
Steps 1) Draw each atom’s Lewis structure. 2) Pair up unpaired electrons. 3) Rearrange atoms so that electron pairs are connected. H O H

21. Practice
Draw the Lewis structure for water. Are the bonds single, double, or triple covalent bonds. H
There are two single covalent bonds in a water molecule. O H

22. P Cl Practice Draw the Lewis structure for PCl3.
Steps 1) Draw each atom’s Lewis structure. 2) Pair up unpaired electrons. 3) Rearrange atoms so that electron pairs are connected. P Cl

23. C H N Practice Draw the Lewis structure for HCN.
Steps 1) Draw each atom’s Lewis structure. 2) Pair up unpaired electrons. 3) Rearrange atoms so that electron pairs are connected. C H N
Single bond
Triple bond