MULTIPLE BONDS AND
NAMING MOLECULES
OF COVALENT BONDS
Chemistry
Unit 3, Day 6
MULTIPLE COVALENT BONDS
 Sharing multiple pairs of electrons results in multiple covalent
bonds
 Double Bond (a.k.a. pi bond π)
 2 pairs of electrons involved in bonding
 O2
O + O
 O=O
 Triple Bond
 3 pairs of electrons involved in bonding
 N2
N + N
 N
N
NAMING BINARY MOLECULAR
COMPOUNDS

There are three rules
1. The first element is given its full name
2. The second element uses the root of its
name, but the suffix –ide
3. Both elements use prefixes to express
the number of atoms present, but the
first element never uses the prefix
mono-
PREFIXES IN COVALENT
COMPOUNDS
Number of Atoms
Prefix
1
2
3
4
MonoDiTriTetra-
5
6
7
PentaHexaHepta-
8
9
10
OctaNonaDeca-
EXAMPLE PROBLEMS

N2O – covalent bond
1. First element = nitrogen
2. Second element = oxygen

Change oxygen to oxide
3. Add prefixes for the number of atoms


Dinitrogen monoxide
CO – covalent bond
1. First element = carbon
2. Second element = oxygen

Change oxygen to oxide
3. Add prefixes for the number of atoms

Carbon monoxide
NAME THE FOLLOWING
COMPOUNDS:
1.

CO2
Carbon dioxide
2. SO2

Sulfur dioxide
3. NF3

Nitrogen trifluoride
4. CCl4

Carbon tetrachloride
5. P2O5

Diphosphorous pentaoxide
PROVIDE THE FOLLOWING
FORMULAS:
1.
Dihydrogen monoxide
 H 2O
2. Chlorine trifluoride
 ClF3
3. Diphosphorous trioxide
 P2O3
4. Disulfur decafluoride
 S2F10
GUIDED PRACTICE –
THINK, PAIR, SHARE

Work with a partner. Give the name And the Lewis
Structure:
1.
2.
3.
4.

SiF4
HBr
B2H4
NBr3
Work with your partner. Give the compound and the
Lewis Structure:
1.
2.
3.
4.
Sulfur Dichloride
Iodine Monofluoride
Dicarbon Dihydride
Silicon Dioxide
INDEPENDENT PRACTICE – EXIT
TICKET
1.
Provide the name:
C2H6
2.
Provide the Lewis Structure:
C2H6
3.
Provide the formula:
Tricarbon octahydride
4.
Provide the Lewis Structure:
Tricarbon octahydride