Chemical Bonding
II. Molecular Compounds
I
II
III
IV
B. Lewis Structures
Octet Rule
Most atoms form bonds in order to
obtain 8 valence eFull energy level stability ~ Noble
Gases
Ne
B. Lewis Structures
Nonpolar Covalent - no charges
Polar Covalent - partial charges
+
+
C. Molecular Nomenclature
Prefix System (binary compounds)
1. How do we recognize these? Because
they’re made up of 2 nonmetals? Where
are nonmetals found???
2. Add prefixes to indicate # of atoms. Omit
mono- prefix on first element.
3. Change the ending of the
second element to -ide.
C. Molecular Nomenclature
PREFIX
monoditritetrapentahexaheptaoctanonadeca-
NUMBER
1
2
3
4
5
6
7
8
9
10
Special Rules with Mono
 If there is only one of the first element, then
the prefix mono is not used.
 If there is only one of the second element,
then the prefix mono is necessary.
Ex.
 CO – Carbon Monoxide
 CO2 – Carbon Dioxide
 C2O – Dicarbon Monoxide
Also….
 There is no reducing for covalent
compounds. What you see is what you
get. If you reduced, you would change the
chemical formula and ratio of the elements
in the bond….Not good….
 C2H4 - Dicarbon Tetrahydride
 CH2 - Carbon Dihydride
 N3O6 - Trinitrogen Hexaoxide
 NO2 - Nitrogen Dioxide
C. Molecular Nomenclature
CCl4
carbon tetrachloride
N2O
dinitrogen monoxide
SF6
sulfur hexafluoride
C. Molecular Nomenclature
arsenic trichloride
AsCl3
dinitrogen pentoxide
N2O5
tetraphosphorus decoxide
P4O10
C. Molecular Nomenclature
The Seven Diatomic Elements
I2 Br2 Cl2 F2 O2 N2 H2
H
N O F
Cl
Br
I