Quiz 3 Flashcards
PHYSICAL PROPERTIES
- Strong intermolecular forces generally result in higher boiling & melting points
- High degree of polarity generally results in substantial water solubility
IMF
- LDFs (increases with MW, decreases slightly with branching)
- Dipole-dipole (increases with polarity)
- Hydrogen bonding
non-polar
• C – C and C – H
are polar
• C – O and O – H
hydrogen bonding
• O – H
LDFs only
propane= -42 C
butane= -1 C
pentane=36 C
2-methylbutane= 28
di-di
dimethyl ether= -24 C
ethyl methyl ether= 7C
diethyl ether= 35 C
isopropyl methyl ether= 56 C
H-bonding
ethanol= 78 C (very water soluble) 1-propanol= 97 C 1-butanol= 118 C 2-butanol= 99 C (slightly water soluble)
• Hydrocarbons
Not miscible with water
• Ethers:
Smaller ethers are slightly miscible with water
• Alcohols
Small to mid-size are very miscible with water
ether
[ – O – R “alkoxyl group”
alcohol*
[ – O H “hydroxyl group”
if a compound contains both an alkoxyl AND a hydroxyl group, it is considered
an alcohol.
C – F BONDS
• Polar & very strong (doesn’t typically react)
• C-F – containing drugs
Resisitant to metabolism (i.e. being broken down), and thus last longer in the body
• PTFE (teflon):
strong and inert; does not bind to materials
• CFCs (chlorofluorocarbons
Higher BP, higher density, less volatile & flammable than corresponding alkane
diethyl ether
old anesthetic
methyl tert-butyl ether
MTBE; old gasoline additive
methanol
wood alcohol”, toxic, flammable
CH3OH
ethanol
CH3CH2OH
from fermentation; causes inebriation; disinfectant; flammable
2-propanol
AKA isopropanol
