STAR Review
Standard 2:
Chemical Bonds
Polarity:
Formation:
Covalent Bonds
Ionic Bonds
Low
High
A covalent bond is formed
between two non-metals
that have similar
electronegativity's.
An ionic bond is formed between
a metal and a non-metal. Nonmetals(-ve ion) are "stronger" than
the metal(+ve ion) and can get
electrons very easily from the
For stabilization, they share metal. These two opposite ions
their electrons from outer attract each other and form the
molecular orbit with others ionic bond.
Melting point:
Low
High
Boiling point:
Low
High
Examples:
Methane (CH4), Hydro
Chloric acid (HCl)
Sodium chloride (NaCl), Sulphuric
Acid (H2SO4 )
Occurs between:
Two non-metals
One metal and one non-metal
State at room
temperature:
Liquid or gaseous
Solid
Drawing Lewis Dot Structures
Naming Compounds
 List
the first element by name.
 The second element is by name but ends
in –ide
Example:
Barium Chloride
Naming Molecules
Greek Prefixes
Number
mono-
1
di-
2
tri-
3
tetra-
4
penta-
5
hexa-
6
hepta-
7
octa-
8
nona-
9
deca-
10
 Use
prefixes
 End last
element
in –ide
Compound
Systematic name
Common name
(if it has one)
NF3
nitrogen trifluoride
NO
nitrogen monoxide
NO2
nitrogen dioxide
N2O
dinitrogen monoxide
N2O4
dinitrogen tetraoxide
PCl5
phosphorous
pentachloride
SF6
sulfur hexafluoride
S2F10
disulfur decafluoride
H2O
dihydrogen monoxide
water
H2S
dihydrogen monosulfide
hydrogen sulfide
NH3
nitrogen trihydride
ammonia
N2H4
dinitrogen tetrahydride
hydrazine
PH3
phosphorous trihydride
phosphine
nitric oxide
laughing gas