1
Q
Bronsted-Lowry definition of acids and bases
A
acids donate protons
bases accept protons
2
Q
Lewis definition of acids and bases
A
acids accept electrons
bases donate electrons
3
Q
where does the conjugate base come from
A
the reacting acid
4
Q
where does the conjugate acid come from
A
the reacting base
5
Q
what does amphoteric mean
A
ability to act as an acid or base (water does this)
6
Q
What is a strong acid/base
A
completely ionize (break apart) when dissolved in water
7
Q
what is a weak acid/base
A
partially ionize when dissolved in water
8
Q
strong acids have _________ conjugate ________
A
weak, bases
9
Q
weak acids have ______ conjugate ________
A
strong, bases
10
Q
weak bases have _______ conjugate _________
A
strong, acids
11
Q
strong bases have ________ conjugate __________
A
weak, acids
12
Q
HCl is a
A
strong acid
13
Q
HBr is a
A
strong acid
14
Q
HI is a
A
strong acid
15
Q
HNO3 is a
A
strong acid
16
Q
HClO4 is a
A
strong acid
17
Q
H2SO4 is a
A
strong diprotic acid (has 2 protons)
18
Q
HF is a
A
weak acid
19
Q
H2CO3 is a
A
weak acid
20
Q
H3PO4 is a
A
weak acid
21
Q
carboxylic acids are
A
weak acids
22
Q
LiOH is a
A
strong base
23
Q
NaOH is a
A
strong base
24
Q
KOH is a
A
strong base
25
Sr(OH)2 is a
strong base
26
Ca(OH)2 is a
strong base
27
Ba(OH)2 is a
strong base
28
Mg(OH)2 is a
weak base
29
NH3 is a
weak base
30
transition metal hydroxides are
weak bases
31
organic amines (NH2, NH, N-R) are
weak bases
32
what is the water constant
Kw= measure of the self-ionization of water
33
pOH+pH =
14
34
hydroxides are
bases
35
pH scale
0-7 = acidic
8-14 = basic
36
pOH scale
0-7 = basic
8-14 = acidic
37
the larger the Ka
the easier it is to remove a proton
38
the larger the Kb
the easier it is to add a proton (bases)
39
acidic functional groups
carboxylic acid, phenols, sulfonamides, amides (most to least acidic)
40
basic functional groups
amines
41
the more bonds a nitrogen has with an R group the ______
less basic (example, triple bonded N's are the least basic)
42
does resonance decrease or increase basicity
decrease
43
pyrrole are
never basic
44
stability of conjugate base rules
1. the larger the atom, the more stable
2. the more electronegative, the more stable it is
3. is there resonance (no resonance means the molecule is more acidic and more reactive)
4. inductive effects (proximity of electroneg atoms to a negative charge)
5. Orbitals (number of single, double, or triple bonds. the more bonds, the more stable.)
45
what is resonance
spreading negative charges across the molecule (requires at least a double bond)
46
the more R groups on a basic molecule, the
more basic it is
47
definition of pharmacology
the study of the interactions between a drug and organism
48
definition of pharmacodynamics
the study of how a drug affects the organism; the study of the biochemical, physiological, and molecular effects of drugs on the body
49
definition of pharmacokinetics
the study of how an organism affects the drug
50
pharmacodynamics includes
site of action, mechanism of action, receptor binding, post receptor effects, and chemical interactions
51
pharmacodynamics can be affected by
disease, disorder, age, and drug-drug interactions
52
receptor subtypes include
enzymes, ion channels, and membrane receptors
53
drugs bind due to chemical interactions such as
electrostatic (intermolecular) forces, hydrophobic interactions, covalent bonds, and stereospecific interactions (enantiomers)
54
drug properties
affinity (how well the drug binds to the receptor
efficacy (how well the drug produces its desired effect)
potency (compares the affinity of competing drugs)
55
principles of pharmacokinetics
absorption
distribution
metabolism
excretion
toxicity
ADME-TOX
56
what determines time to maximal concentration at the receptor to produce a peak effect
absorption rate
57
factors affecting bioavailability
molecular weight of drug, drug formulation, drug stability, first pass metabolism, blood flow, gastric emptying and motility, and drug interactions
58
what influences distribution
MEMBRANES, blood, total body water, ECF, lymphatic and cerebrospinal fluids, protein-binding (drugs have to be free to exert effects)
59
what helps determine the ability of a drug to be distributed to the desired receptor
drug solubility
60
LeChatlier's Principle
if equilibrium is disturbed then the reaction will act in the opposite direction of the change made to return the system to equilibrium (example as free drug is use, protein-bound drug will become free)
61
common pathways of metabolism
hydrolysis (esters, amides, and nitriles)
REDOX reactions
62
main routes of excretion
kidneys, feces, lungs, and sweat
63
what phase do most drugs fail
discovery phase
64
90% of drugs fail in the
clinical testing
65
30% of drugs fail before
they reach human trials
66
Lipinski Rule of 5 (drug development)
describes drug potential for a new chemical entity and measures bioavailability. based on hydrogen bond donors (goal <5)/acceptors (goal <10), molecular weight (500g/mol upper limit), and cLog P (goal <5)
67
what does violation of more than 1 Lipinski Rule mean
predicts a NCE is not orally-available
68
what are hydrogen donors
any N-H or O-H group
69
what are hydrogen acceptors
N or O
70
N-H is both
a hydrogen donor and acceptor
71
what is cLogP
the calculated partition coefficient;
suspend a drug between water and octanol and see which the drug moves toward. this determines if a drug is water or lipid soluble. Less than or equal to 5 indicates the NCE is both water and lipid soluble
72
low MW drugs with a low cLogP can
easily cross membranes
73
what functional groups are linked to increased toxicity
aromatic anilines, nitroaromatics, aliphatic halides(alkanes), polycyclic aromatic hydrocarbons, and thiophenes
74
drug efficacy is directly related to
the concentration of the drug at its site of action
75
drug concentration must be
high enough to elicit the desired effect but not high enough to cause negative effects
