The
bond that forms from the
sharing of valence electrons
Atoms
1
2
3
4
5
6
7
8
9
10
Prefix
monoditritetrapentahexaheptaoctanonadeca-
Name
first element
Name the second element and
add –ide
Use prefixes to indicate the
number of atoms in the molecule
 Exception…if
there is only one of
the first atom, mono is left out!
N2F6
CO2
SiF4
CBr4
NCl3
P 2 S3
CO
NO2
SF2
PF5
SO2
NO
CCl4
P 2 O5
Dinitrogen Hexafluoride
Carbon Dioxide
Silicon Tetrafluoride
Carbon Tetrabromide
Nitrogen Trichloride
Diphosphorous Trisulfide
Carbon Monoxide
Nitrogen Dioxide
Sulfur Difluoride
Phosphorous Pentafluoride
Sulfur Dioxide
Nitrogen Monoxide
carbon tetrachloride
diphosphorus pentoxide
Antimony
tribromide
Hexaboron monosilicide
Chlorine dioxide
Hydrogen monoiodide
Iodine pentafluoride
Dinitrogen trioxide
Phosphorus triiodide
SbBr3
B6Si
ClO2
HI
IF5
N2O3
PI3
Ammonia
Water
– NH3
- H2O
Methane
- CH4
Electron
dot notation is used to
shown how electrons are shared
Molecules are formed
Each molecule has 8 valence
electrons
 Except
Hydrogen!
Each line represents the
sharing of 2 electrons
Lone Pair
PH3
H2S
HCl
CCl4
SiH4
 H2
HF
F 2
Single Bonds
Symbol : σ

Draw
O3
Draw
O2
N2
C2H2
CO2
 Xe,Si,


Sometimes have more than 8 electrons
PF5
 Be

P, S, Cl, Br, and I
and B often only have 6 electrons
BeCl3
Draw
CH4
Label all bonds as sigma or pi
A
single electron, not paired
As
the number of shared
electrons increases, bond length
decreases
Breaking
the bond of a short
bond is larger than a long bond
What
is an ionic bond and how does
it differ from an ionic bond?
What is the difference between a
sigma bond and a pi bond?
Predict the bond energy of each of
the bonds in CH2.