Test 1 Review Flashcards
alcohol functional group
R-OH
- polar
- primary alcohol is attached to one carbon. secondary alcohol attached to 2 carbons. tertiary alcohol attached to 3 carbons
- named -ol ex) ethanol
- IMF: H bonds, dipole dipole, LDF
thiol functional group
CH3-CH2-CH2-SH
- nonpolar
- no dipol (sulfur and water have similar electronegativities)
- not soluble in water
- covalent
- named -thiol ex) propanethiol
ether functional group
R-O-R (O in middle of hydrocarbon chain) "hydrocarbons on ether side" 1. polar because oxygen and carbon 2. can be aromatic or aliphatic 3. named -ether ex)methyl propyl ether
aldehyde functional group
R-(C=O)-H. have a carbonyl group (C=O). ends in H 1. super polar 2. soluble in water 3. named -al ex) ethanal
ketone functional group
R-(C=O)-R. have a carbonyl group (C=O).
- super polar
- soluble in water
- named -one ex)butanone
carboxylic acid
CH3-(C=O)-OH
can donate hydrogen (acid is a proton donor)
contains carboxyl group (carbonyl, alcohol)
1. polar (electronegativity between C+O, O+H)
2. soluble in water unless R=mucho hydrocarbons
3. named “-oic acid” ex)ethanoic acid
4. IMF: H bonds, dipole, dipole, LDF
5. boiling point 118 degrees
esters
CO-O-CH "esters got a COOCH" 1. polar 2. make this with carboxylic acid and ETOH 3. named -oate ex)methyl ethanoate
amines
CH3-CH2-CH2-(N-CH2)-CH3
- primary attached to one hydrocarbon and likely two hydrogens
- secondary attached to two hydrocarbon and likely one hydrogens
- tertiary attached to 3 hydrocarbon, most lipophilic. least polar of the 3 (because difference between N-C is smaller than N-H)
- lipophilic but derivative of ammonia
- must have nitrogen
- act as bases in water, will accept proton (H+)
- named -amine. ex) dimethyl propyl amine
amides
CH3-(C=O)-NH2
- derivative of carboxylic acids in which nitrogen group (NH2) replaces hydroxyl group
1. carbonyl group makes it polar
2. -amide. ex)ethanamide
3. primary and secondary amides
4. IMF: h-bond, dipole-dipole, LDF
5. H bonds with H20
6. boiling point 222 degrees
Chirality
- only describing center carbon
- chiral carbon is stereogenic, everything rotates around it
- this carbon is connected to 4 different things
- cannot superimpose on itself
stereoisomer
more than one way to rearrange group. usually because more than one of the same thing
ex) C attached to H+, H+, Cl, Br
constitutional isomer
made up of same things but function as two different molecules
enantiomer
- prioritize 4 groups attached to chiral center based on atomic number
- orient so lowest priority group is projecting away
- determine if highest to lower priority is going clockwise (R) or counterclockwise (L)
alkanes
C-C
- nonpolar
- not water soluble
alkenes
C=C
- no chirality anymore
- nonpolar and hydrophobic
- only SLIGHT water solubility
alkynes
C(3lines)C
- most soluble but still not soluble
- nonpolar
aromatic rings
can have - or = bonds
great stability
can have N, S, O
in larger structures, called a phenyl group
phenol
OH group with phenyl ring
much more soluble than non aromatic alcohols
-lipid soluble until it binds to molecules that create polarity
least to most polar functional groups
lowest to highest boiling point
most soluble in water
- hydrocarbons (exist naturally as a gas)
- ethers
- esters, aldehydes, ketones
- amines
- alcohol
- carboxylic acid
- amides
Quarternary Ammonium Cation
loss of N outer shell electron makes N+, no H+, pH independent because no H+.
attraction of H+ means reversible charge to ammonium. pH dependent.
Amide Local Anesthetics
licocaine, bupivicaine, ropivicaine, mepivicaine (all are tertiary amines). amide linker broken down by liver
ester local anesthetics
chloropocaine, procaine, tetracaine. ester linker broken down by esterases
chemical structure of local anesthetics
phenyl group for lipophilicity
ester or amide group for degradation.
protonation state affects its solubility (amine portion, affected by acid base balance)
nano equivalents of H+ in blood
40x 10^-9Eq/L
how to assess electroneutrality
mg has to be converted to moles of ions and valence to assess this
BH+ B + H+
BH+ is protonated acid, B + H+ is a weak base.
intramolecular forces
covalent, ionic, polar covalent, nonpolar covalent
intermolecular forces
hydrogen (O-H dipol), van der waals
strongest to least strong types of chemical bonds
covalent ionic hydrogen hydrophobic van der waals
covalent bonds
different atoms can support different numbers of covalent bonds. number of covalent bonds formed is equal to the number of unpaired electrons in outermost shell
daltons laws describing behavior of atoms
- atoms of different elements have different properties
- atoms are neither created nor destroyed in chemical reactions
- atoms of different elements form compounds in whole number ratios
