CHEMISTRY PART 11
Covalent Compounds
Remember...


Metals want to lose electrons and non-metals
want to gain them.
These are ionic bonds.
Covalent Compounds

A compound made of only non-metals
 Also


called a molecular compound.
Electrons are shared between the atoms to
have full valence shells.
Hydrogen counts as a non-metal.
Covalent Compounds

Covalent Compounds Animation

Sharing of electrons forms a covalent bond.
 Single
bond  2 electron shared
 Double bond  4 electrons shared
 Triple bond  6 electrons shared
Covalent Compounds

Example:
 Hydrogen
and chlorine both want 1 electron to
fill their valence shell.
 They will share 1 electron.
H now has 2e- in its valence shell
and Cl has 8, so they are both full.
Indicates a single bond
This is the structural formula.
Practice

1.
2.
3.
4.
Draw the structural formula for each covalent
compound created from the following pairs of
electrons.
bromine and iodine
nitrogen and chlorine
carbon and fluorine
sulfur and bromine
Practice
Atoms
bromine and iodine
nitrogen and chlorine
carbon and fluorine
sulfur and bromine
Structural Formula
Practice
1.
2.
3.
4.
5.
6.
7.
8.
H2O
CO2
NH3
SCl2
CH4
C2H6
CBr4
CH2Cl2
Practice
1.
2.
3.
4.
5.
6.
7.
8.
K and Se
C and Cl
C and O
Sr and Br
N and I
B and H
Ca and N
Al and S
Naming Covalent Compounds

Determine if it is a covalent compound:
 Is
1.
2.
it non-metal and non-metal?
Name the first element. Use a prefix if there
is more than one.
Name the second element. Use a prefix to
indicate the number of atoms (even if there
is only 1). Add the ending “ide”.
Naming Covalent Compounds
Number of Atoms
Prefix
1
mono(only used for second element)
2
di-
3
tri-
4
tetra-
5
penta-
6
hexa-
7
hepta-
8
octa-
9
nona-
10
deca-
Practice

Examples:
 NO
 nitrogen
monoxide
 N2O
 dinitrogen
monoxide
Practice
7.
NO2
CO
PI3
SO2
SO3
S2F10
CCl4
8.
N2O5
1.
2.
3.
4.
5.
6.
nitrogen dioxide
carbon monoxide
phosphorus triiodide
sulfur dioxide
sulfur trioxide
disulfur decafluoride
carbon tetrachloride
dinitrigoen pentoxide
Formula Writing

Use the prefixes to write the formula.

Example:
 phosphorus
 PCl5
pentachloride
Practice
1.
2.
3.
nitrogen tribromide
nitrogen dioxide
sulfur pentoxide
NBr3
NO2
SO5
Diatomic Molecules


HOFBrINCl
When alone in nature, these elements exist in
a diatomic form.
 The
atoms come in pairs, as gases.
 H2 (g)
= hydrogen
 O2 (g) = oxygen
 N2 (g) = nitrogen
Diatomic Molecules

Draw covalent bond diagrams for:

H2, O2, F2, Br2 , I2, N2 and Cl2
Practice


Worksheet
Page 127 # 8, 15