Functional
Group
Formula
Naming
Example
Types of
Intermolecular
Forces
London
dispersion
forces only
(weak)
Melting
Point (oC)
Hydrocarbons
R
-ane
-ene
-yne
CH4
= methane
Low
Halo-alkane
R-X
(X=halogen)
Prefix
depends
on
halogen
H3CCl
=
chloromethane
London, dipoledipole
Alcohol
R-OH
–ol
H3COH
= methanol
Aldehydes
R-C=O
H
-al
H3C=O
= methanal
Ketones
R-C=O
R
-one
H3C-C=O
CH3
=propanone
Carboxylic
Acids
R-C=O
OH
-oic acid
HC=O
OH
=methanoic acid
Boiling
Point (oC)
Polarity
Properties
Low
Nonpolar
Higher than
alkane
Higher than
alkane
polar
Very low
solubility in
polar solvents,
good non-polar
solvents
Solubility in
water
increases as
size decreases
London, DipoleDipole,
Hydrogen
Greater than
alkanes and
halo-alkanes
Greater than
alkanes and
halo-alkanes
OH group
is polar
London, D-D,
can accept
Hydrogen from
H2O
London, D-D,
can accept
Hydrogen from
H2O
London, D-D.
Hydrogen
Lower than
alcohol
Lower than
alcohol
Polar
Lower than
alcohol
Lower than
alcohol
polar
Higher than
alcohol
Higher than
alcohol
Polar
Solubility in
water
increases as
size decreases,
Ideal solvents
(dissolved both
polar and nonpolar)
Solubility in
waterincreases
as size
decreases
Weak acid,
conductor
Acidic,
Volatile-smell
Esters
R-C =O
OR
Ethers
R-O-R
Amines
R-N-R
R
Amides
R-C=O
N-R
R
-oate
-C
attached
to O is
side
chain
-parent
chain
attached
to =O
-oxy (on
smaller
chain)
-longer
chain is
parent
-amine
-longest
chain is
parent
-other 2
are side
chains
-amide
-longest
chain
with =O
is parent
-other 2
are side
chains
H2C-C=O
O-CH3
=methyl
ethanoate
London, D-D,
can accept
hydrogen from
H2O
Lower than
alcohol and
Acid
Lower than
alcohol and
Acid
Somewhat
Polar
Solubility in
water
increases as
size decreases
H3C-O-C H3
Propoxypropane
London, D-D,
can accept
hydrogen from
H2O
Lower than
alcohol,
greater than
hydrocarbon
Lower than
alcohol,
greater than
hydrocarbon
Somewhat
Polar
H3C-N-H
H
=methanamine
London, D-D,
primary and
secondary can
hydrogen bond,
Less than
alcohols,
higher than
those that
can’t h-bond
Less than
alcohols,
higher than
those that
can’t h-bond
Polar
Smaller are
soluble in
water
C-C=O
N-H
H
ethanamide
London, D-D,
primary and
secondary can
Hydrogen
Higher than
alcohols but
less than
acid
Higher than
alcohols but
less than
acid
Polar
Small are very
soluble in
water
MELTING AND BOILING POINT FROM HIGHEST TO LOWEST
Amide >
Form 2 Hbonds
(primary
amine has 2 NH groups),
And accept Hbonds on both
O and N and
have 2
Carboxylic
Acid >
H-bond and
2 oxygens
Alcohol >
Amine>
H-bond,
Only 1 oxygen
H-bond,
Dipoledipole (N
weaker
than O)
Ketone/Al
dehyde>
Dipoledipole,
can’t do Hbonding
but can
accept Hbonds
Ester>
Ether>
No Hbonding,
Dipole-dipole
(2 oxygens)
No Hbonding,
weak
polarity,
weak
dipoledipole (1
oxygen)
Haloalkane>
Polar,
weak
dipole
dipole
(except
F>O)
Alkane
Non-polar,
only London
dispersion
forces
INTERMOLECULAR FORCES (between two molecules) FROM STRONGEST TO WEAKEST
Hydrogen Bonding (H-bond) >
Dipole-Dipole bonds (D-D) >
Strongest intermolecular forces.
Strong intermolecular force.
Occurs with a hydrogen bonded to an O, N
or F (most EN elements)
Occurs between molecules that have a
polar dipole.
Creates a very strong dipole
To have a polar dipole, the EN difference
has to be between 0.4-1.7 and the
molecule’s VSEPR shape cannot be
symmetrical (dipoles cannot cancel out).
Molecules with an O, N and F bonded to
an H can form H-bonds with themselves
(very strong intermolecular forces leading
to higher melting and boiling points). They
can also form H-bonds with water, making
them very soluble.
London Dispersion Forces/Van der
Waals forces
Between EVERY molecule.
Weak forces that occur due to constant the
movement of electrons creating
flickering/momentary dipoles.
The larger the molecule, the greater than
force.
Molecules with a highly EN atom that
has a lone pair (O, N, F) and is bonded to
a carbon but not a hydrogen cannot Hbond with themselves but can H-bond
with water by accepting the positively
charge H atom in water on their lone pair,
making them highly soluble.