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CP Flashcards

1
Q

lipophilic means

A

ability of a chemical compound to dissolve in fats/oil/lipids/nonpolar solvents

i.e. hexane

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2
Q

what makes lidocaine lipophilic

A
  • dominated by large, nonpolar aromatic ring
  • alkyl groups
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3
Q

molality equation

A

m = mol / Kg

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4
Q

molality means

A

calculating moles of solute per kg of solvent

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5
Q

molarity equation

A

M = moles / L

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6
Q

molarity means

A

moles calculated per liter of solution

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7
Q

distinct mark of a fatty acid chain

A

long alkyl chain + ends in a carboxylic acid

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8
Q

explain alpha decay

A

atomic nucleus emits alpha particle

daughter is an atom with a mass number 4 less and atomic number 2 less than parents

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9
Q

beta plus decay

A

aka positron emission

positron emitted from parent nucleus

daughter has 1 less proton

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10
Q

beta minus decay

A

neutron converts into proton

electron emitted

daughter has atomic number that increases by 1

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11
Q

why would PO4^3- molecules utilize proton-coupled transport mechanisms to enter the cell

A

PO4^3- is hydrophilic (neg charge ion)

cannot cross hydrophobic interior of membrane

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12
Q

inspiration comes from

A

initially increasing volume of lungs

pressure gradient created

air pressure in lungs is less than the air pressure in environment

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13
Q

when air pressure gradient is not as great…

A

less air enters lungs with every breath

difficulty breathing occurs at high altitudes for this reason

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14
Q

how to calculate mechanical work

A

Fdcos(θ)

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15
Q

surface tension decreases as

A

temperature rises

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16
Q

when warmer solutions are being ejected sooner, what is the reason

A

either electrical forces increase or surface tension decreases

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17
Q

why is very unlikely that the lactam in penicilin would covert to an ester

A

not thermodynamically favorable to transform from a more stable form (amide) to a more reactive one (ester)

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18
Q

due to what reason are beta-lactams more susceptible to nucleophilic attacks than amides?

A

DUE TO RING STRAIN

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19
Q

positive ions flow down voltage gradients from

A

high to low voltage

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20
Q

when the voltage inside cell is more negative, sodium ions will

A

flow passively down the voltage gradient

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21
Q

extracellular concentration of sodium ions is

A

greater than their intracellular concentration

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22
Q

explain “salty bananas”

A

extracellular concentration of sodium > intracellular (“salty”)

intracellular concentration of potassium > extracellular (“bananas”)

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23
Q

proteases cleaves…

A

peptide bonds at the carboxyl terminal of acidic AAs

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24
Q

name the two AAs that are acidic

A

aspartic acid (Asp) / (D)

glutamic acid (Glu) / (E)

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25
Q

what would have the largest decrease in entropy? melting, condesation, sublimation or deposition?

A

deposition

goes from highest to lowest entropy

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26
Q

sublimation goes from

A

solid to gas (low to high entropy)

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27
Q

liquid exhibit a small or large change in volume when temperature increases

A

small

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28
Q

gases exhibit what kind of change with temperature increase

A

large

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29
Q

heat of fusion and heat of vaporization do not involve a

A

phase change

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30
Q

liquids are more what compared to vapors

A

ordered

smaller entropy

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31
Q

ideal gas law solely pertains to

A

gases

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32
Q

heat (q) =

A

mc Δ T

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33
Q

equation for heat required to vaporize liquid

A

mΔHvap

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34
Q

Intensity (I) =

A

P/A (Power/Area)

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35
Q

Power (P) =

A

IA

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36
Q

relationship between power and energy

A

P = W/t

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37
Q

energy received by ear

A

W = Pt = IAt

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38
Q

Doppler effect shifts

A

frequency

cannot dampen sounds

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39
Q

fundamental rules of waves is that frequency does not…

A

change when wave travels from medium to another

having a different medium b/w air and ear wouldn’t change the frequency

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40
Q

constructive interferences would increase or decrease intensity of sounds

A

INCREASE

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41
Q

destructive interference can occur by adding wave energy out of phase with…

A

the incoming sound

decreasing amplitude

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42
Q

which of the following have no charge?

alpha particles

proton beams

gamma photons

beta particles

A

gamma photons

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43
Q

magnetic fields exert forces on

A

moving charged particles

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44
Q

do magnetic fields have any effect on photons?

A

no b/c they have no chart

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45
Q

terminal species in the ETC

A

oxygen

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46
Q

NADH donates its electrons to

A

the first electron carrier in the ETC

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47
Q

product of NADH oxidation

A

NAD+

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48
Q

NAD+ has what electron affinity

A

LOW

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49
Q

FADH2 enters ETC by

A

donating its electron directly to CoQ

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50
Q

oxidized FAD will have a lower or higher affinity than CoQ?

A

LOWER

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51
Q

saponification is the

A

basic hydrolysis of ester bonds in a triglyceride

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52
Q

what do liver enzymes employ to produce bile acids?

A

oxidation by adding new carboxylic acid that contains 3 new bonds to oxygen atoms

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53
Q

what contributes to the fact that the small intestine cannot passively absorb bile salts?

A

1) taurine and glycine have low pKa values

2) pancreatic secretions increase intestinal pH

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54
Q

how do pancreatic secretions increase intestinal pH?

A

pancreatic secretions contain bicarbonate (a base) which raises the pH

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55
Q

lipase works to hydrolyze which functional group?

A

ester

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56
Q

sources of degrees of unsaturation

A

rings and multiple bonds

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57
Q

shorter wavelengths equate to photons of

A

larger energies

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58
Q

excited state and ground state have the same

A

overall charge (no electron transfer)

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59
Q

once in the excited state, the molecule can…

A

relax a bit of its energy as heat

before losing what’s left of its energy as an emitted photon

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60
Q

nucleophilicity increases going which way on the periodic table?

A

down

due to greater size/polarizability

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61
Q

stronger nucleophile slows or speeds up reaction?

A

speeds up

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61
Q

a cyclic sugar w/ 5 atoms in the ring is in what form?

A

furanose form

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62
Q

D-sugar has an R or S configuration?

A

R configuration at the last stereocenter

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63
Q

L sugar has what configuration?

A

S configuration

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64
Q

lipases are produced by the

A

pancreas

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65
Q

liver is responsible for

A

regulation of carbohydrate metabolism (glycogenolysis, glycogenesis, gluconeogenesis)

deamination of AA and conversion of resulting ammonia to urea

lipid metabolism (cholesterol and lipoprotein synthesis)

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66
Q

torque =

A

Fd sin θ

F = force creating torque

d = distance from force to rotation point

θ = angle between F and d

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67
Q

define centripetal force

A

force pointing into center of the circle

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68
Q

how do crown ether molecules affect polarity?

A

don’t significantly affect polarity of an ether solvent

will be miscible with it

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69
Q

crown ether molecules don’t contain any protic hydrogens to….

A

hydrogen bond w/ the solvent

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70
Q

crown ethers shield the

A

amine from h-bonding interactions w/ the solvent

decreasing amine’s solubility

71
Q

all mammalian AAs have what configuration?

A

L configuration except achiral glycine

72
Q

L configuration means

A

there’s a S stereocenter at the alpha carbon

73
Q

creatine phosphokinase is the enzyme used to

A

catalyze the reversible rxn b/w creatine and creatine phosphate

74
Q

when a rxn is reversible, it cannot have a

A

committed step

75
Q

catalysts DON’T AFFECT what in kinetics?

A

ΔG and spotaneity

76
Q

positive charges undergo what from higher to lower electric potential?

A

a force

77
Q

positive charge lowers or increases potential energy

A

lowers

78
Q

electric field lines point in a direction that a positive charge would

A

undergo a force

79
Q

electric field lines would point in the direction of

A

lower electric potential

e.g. 200 V to 100 V

80
Q

concentration is given by

A

M = mol/L

81
Q

rate is given by units

A

M/s

82
Q

M/s is the same as

A

mol/(L x s)

83
Q

second order rate law

A

rate = k[A]^2

84
Q

when does an aldehyde gains an oxygen?

A

when it’s converted to a -COOH

85
Q

which of the following could affect any of the dissociation constants for hemoglobin?

1) decreasing temp
2) adding NH3
3) increasing [O2]

A

decreasing temp
adding NH3

86
Q

K’ is what for any equilibrium at a certain temperature

A

constant

87
Q

what alters K’

A

changing temperature

88
Q

AHED mneomnic

A

Absorb Light
Higher potential
Excited
Distant from nucleus

89
Q

diamagnetic means all electrons are

A

PAIRED

90
Q

electrons are repelled by an external magnetic field in diamagnetic or paramagnetic?

A

diamagnetic

91
Q

1 or more unpaired electrons in diamagnetic or paramagnetic?

A

paramagnetic

92
Q

in paramagnetic, electrons are

A

pulled into an external magnetic field

93
Q

follow (what) to build the atom’s electron configuration

A

Hund’s Rule

94
Q

quantum number n =

A

principal number

95
Q

n labels

A

electron energy level or shell number

96
Q

possible values for n

A

1,2,3…

97
Q

l =

A

azimuthal

3D shape of orbital

98
Q

possible values for l

A

0,1,2,…. n-1

99
Q

ml =

A

magnetic

orbital sub-type

100
Q

s orbital =

A

0

101
Q

p orbital =

A

1

102
Q

d orbital =

A

2

103
Q

f orbital =

A

3

104
Q

g orbital =

A

4

105
Q

ms =

A

spin

electron spin

106
Q

rank the IM forces from weakest to strongest

A

London Dispersion

Dipole-Dipole

Hydrogen

107
Q

coordinate covalent bonds involve

A

a single atom providing both bonding electrons

most often found in Lewis acid-base chemistry

108
Q

suffix for acids with MORE oxygen

A

-ic

109
Q

suffix for acids with LESS oxygen (than -ic)

A

-ous

110
Q

equivalent mass is the

A

mass of an acid that yields 1 mole of H+

or

mass of a base that reacts w/ 1 mole of H+

111
Q

combination reaction form

A

ONE product from two or more reactants

112
Q

decomposition reaction involves

A

a single reactant breaking down

113
Q

combustions involves

A

a fuel (usually a hydrocarbon) and O2 (g)

commonly forms CO2 and water

114
Q

what type of reaction involves an atom or ion in a compound replaced by another atom or ion?

A

single displacement

115
Q

what type of reaction has elements from 2 compounds swap places?

A

double displacement (metathesis)

116
Q

neutralization rxn:

A

a type of double-replacement rxn

117
Q

-ΔG =

A

exergonic

spontaneous

118
Q

+ΔG =

A

endergonic

not spontaneous

119
Q

ΔG =

A

Ea - Ea rev

120
Q

which products are higher in free energy?

A

kinetic

121
Q

kinetic products can form at lower or higher temps

A

lower

122
Q

kinetic products are known as

A

“fast” products b/c they can form more quickly under such conditions

123
Q

thermodynamic products are lower or higher in free E?

A

lower

more stable

slower but more spontaneous

124
Q

isolated systems exchange

A

neither matter nor energy w/ the environment

125
Q

closed system can exchange

A

energy but not matter w/ the environment

126
Q

open system can exchange

A

both energy and matter with the environment

127
Q

isothermal process =

A

constant temp

128
Q

adiabatic process exchanges

A

no heat w/ the environment

129
Q

isobaric process =

A

constant pressure

130
Q

isovolumetric =

A

constant volume

131
Q

state functions describe the

A

physical ppties of an equilibrium state

pathway independent

132
Q

state functions

A

pressure

density

temp

volume

enthalpy

internal energy

gibbs free E

entropy

133
Q

standard conditions

A

298 K

1 atm

1 M

134
Q

fusion =

A

solid to liquid

135
Q

freezing =

A

liquid to solid

136
Q

vaporization =

A

liquid to gas

137
Q

sublimation =

A

solid to gas

138
Q

deposition =

A

gas to solid

139
Q

triple point =

A

point in phase diagram where all 3 phases exist

140
Q

supercritical fluid =

A

density of gas = density of liquid

no distinction b/w two phases

141
Q

F =

A

(9/5 C) + 32

142
Q

solid –> liquid –> gas is endo or exothermic?

A

endothermic

gases have more heat energy than liquids and liquids have more heat energy than solids

143
Q

gas –> liquid –> solid is endo or exothermic?

A

exothermic b/c of the heat released

144
Q

ΔHrxn =

from heat of formations

A

ΔH products - ΔH reactants

145
Q

ΔH rxn =

from bond dissociation energies

A

ΔH reactants - ΔH products

146
Q

standard entropy of rxn

A

ΔSrxn = ΔS products - ΔS reactants

147
Q

gibbs free energy (G) =

A

ΔG = ΔH - TΔS

148
Q

entropy is maxed at

A

equilibrium

149
Q

gibbs free E is derived from

A

enthalpy and entropy

150
Q

ΔG < 0

A

spontaneous

151
Q

ΔG = 0

A

equilibrium

152
Q

ΔG > 0

A

non-spotaneous

153
Q

oxidizing agent is a

A

substance that causes another substance to lose electrons and undergo oxidation

154
Q

reducing agent is a

A

substance that causes another substance to gain electrons and undergo reduction

155
Q

what does thermodynamically favorable mean

A

reaction is energetically favorable and can proceed spontaneously without input of external energy

156
Q

what does thermodynamically unfavorable mean

A

rxn requires some input of energy to proceed

157
Q

reduction potential is a measure of the

A

tendency of chemical species to gain electrons (be reduced)

158
Q

more positive reduction potential means what?

A

better oxidizing agent and easier to reduce

159
Q

half-reaction is a chemical equation that either the

A

oxidation or reduction process occurring in a redox rxn

160
Q

a reduced compound has a higher number of

A

electrons than its oxidized counterpart

161
Q

atom radium increases in which direction?

A

DOWN bc you’re adding shells (principle quantum number increases)

162
Q

atom radius decreases left or right?

A

right because you add protons

increases positive charge which draws electrons closer

163
Q

fluorine will hog electrons in a bond due to

A

a highly charged nucleus

164
Q

BEAR stands for

A

basicity
electronegativity, electron affinity, ionization Energy
acidity
atomic Radius

165
Q

6 strong acids to know

A

sulfuric acid (H2SO4)
hydroiodic acid (HI)
hydrobromic acid (HBr)
nitric acid (HNO3)
hydrochloric acid (HCl)
perchloric acid (HClO4)

166
Q

good leaving groups are

A

conjugate bases of strong acids

167
Q

poor leaving groups are

A

conjugate bases of weak acids

168
Q

So I Brought No Clean Clothes stands for

A

sulfuric acid (H2SO4)
hydroiodic acid (HI)
hydrobromic acid (HBr)
nitric acid (HNO3)
hydrochloric acid (HCl)
perchloric acid (HClO4)

169
Q

nucleophiles are

A

electron-rich molecules that donate electrons to form bonds

similar to lewis bases

170
Q

examples of nucleophiles

A

carbanions, water, ammonia, cyanide ion

171
Q

electrophiles are

A

electron-poor molecules that accept electrons to form bonds

similar to lewis acids

172
Q

examples of electrophiles

A

cations (H+ and NO+), HCl, carbocations, carbonyl compounds

173
Q

in an SN1 reaction,

A

the leaving group leaves before a nucleophile takes its place

174
Q

in an SN2 reaction,

A

the LG is pushed out at the same time as the nucleophile comes in

175
Q
A

practice test review (4 decks)

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