Molecular Compounds
Molecular Compounds
• Molecular Compounds form between
nonmetals and nonmetals. (ex. S2O4 )
• Covalent bonds form when atoms share
electrons.
• Neither atoms gain or lose electrons because
their electronegativity values are very close.
Naming Binary Molecular Compounds
• To name molecular compounds, use prefixes
to show how many atoms of each element
there are.
• Exception: do not show a prefix if the first
element has only one atom.
• Note: Do NOT reduce if the element ratio is
not in lowest terms.
• Similar to ionic compounds – last element
ends in -ide
Prefix
mono
di
tri
tetra
penta
hexa
hepta
octa
nona
deca
# atoms
1
2
3
4
5
6
7
8
9
10
Name the following molecular
(covalent) compound: SiF4
1. Monosilicon fluoride
2. Sulfur fluoride
3. Monosilicon
tetrafluoride
4. Silicon tetrafluoride
5. Silicon quadfluoride
0%
Sil
i
.
df
l..
co
n
qu
a
te
tra
co
n
Sil
i
ico
n
id
.. .
M
on
os
il
0%
f. .
.
0%
te
...
0%
fu
rf
lu
or
Su
l
M
on
os
il
ico
n
fl.
.
.
0%
Name the following molecular
(covalent) compound: SO3
Sulfur trioxide
Sulfur oxide
Sulfur dioxide
Monosulfur trioxide
0%
..
0%
ri.
rt
on
os
ul
fu
M
Su
l
fu
rd
io
xid
de
e
0%
fu
ro
xi
Su
l
fu
rt
r io
xi
d.
..
0%
Su
l
1.
2.
3.
4.
Name the following molecular
(covalent) compound: S2F6
Sulfur fluoride
Sulfur hexafluoride
Disulfur fluoride
Disulfur
hexafluoride
0%
Di
su
lfu
rh
lu
o
r. .
.
ex
af
. ..
0%
lfu
rf
Di
su
Su
l
fu
rh
ex
a
id
.. .
fu
rf
lu
or
0%
flu
.. .
0%
Su
l
1.
2.
3.
4.
Acid Nomenclature
• In general, names of acids will begin with
hydrogen.
• If the anion does not contain oxygen, the acid
begins with hydro and ends in –ic
• HCl = hydrochloric acid
• HBr =
• HCN =
Acids containing oxygen
• If the acid contains oxygen, the acid does not
have hydro at the start and either ends in ic
or ous.
• If the anion ends in –ate use –ic
• HNO3 = nitric acid
• If the anion ends in –ite use –ous
• H2SO3 = sulfurous acid