R—OH
alcohol
R—Cl
Alkyl halide
R—NH2
Amine
R2C—CR2
\ /
O
Epoxide
R—O—R
Ether
RC≡N
Nitrile
R—NO2
Nitroalkane
R—S—R
Sulfide
R—SH
Thiol
. O
||
R—CH
Aldehyde
. O
||
R—C—R
Ketone
. O
||
R—C—OH
Carboxylic acid
. O
||
R—CX
Acyl halide
. O O
|| ||
R—C—O—C—R
Acid anhydride
. O
||
R—C—O—R
Ester
…..O
…..||
R—C—N—R2
Amide
What are intermolecular forces?
IMFS, the forces of attraction that may exist between the atoms and molecules of a substance (WEAK)
- hold multiple molecules together
- determine many of a substance’s properties
- the result of electrostatic phenomena
- non covalent forces
What provides the energy required to overcome IMFs?
Kinetic energy
What are intramolecular forces
the forces that hold atoms together in a molecule (STRONG)
What are the three types of IMFs?
- Dispersion forces
- Dipole-Dipole attractions
- Hydrogen bonding
What are van der Waals forces?
the three intermolecular forces collectively
Describe dispersion forces
- result from the formation of temporary dipoles
- heavier molecules and atoms exhibit stronger dispersion forces than do lighter molecules and atoms
—–> because larger atoms have greater polarizability due to the valence electrons being farther from the nucleus - the strength of dispersion forces increases with the contact area between molecules
What is polarizability?
The measure of how easy or difficult it is for another electrostatic charge to distort a molecule’s charge distribution.
What are dipole-dipole attractions?
- molecules with permanent dipoles display dipole-dipole attractions
- this type of attraction is present only in polar molecules
- dipole-dipole attractions are stronger than dispersion forces
- polar molecules contain dipole dipole and dispersion forces
- adjacent molecules line up such that the partial negative pole of one molecule is as close as possible to the partial positive pole of another molecule.
