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MCAT > GEN CHEM > Flashcards

GEN CHEM Flashcards

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MCAT flashcards
1
Q

as much solute that can be dissolved in solution

A

saturated

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2
Q

electron potential energy increases or decreases when e- is taken away

A

increases

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3
Q

what type of pair differs by only one proton

A

conj. acid/base pairs

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4
Q

Keq>1 means

A

products favored

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5
Q

more can still be dissolved in a solution

A

unsaturated

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6
Q

precipitation occurs in solution

A

supersaturated

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7
Q

common ion effect increases or decreases molar solubility

A

decreases

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8
Q

lewis acid

A

e- pair acceptor

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9
Q

lewis base

A

e- pair donor

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10
Q

Brons. Lowry acid

A

proton donor

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11
Q

Brons. Lowry base

A

proton acceptor

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12
Q

in a conj. pair, the acid form is w/ or without proton

A

w/ proton; basic is without

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13
Q

same atoms but differ in connectivity

A

constitutional isomers (structural)

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14
Q

same connectivity but differ in rotation of a single bond

A

conformation isomers

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15
Q

Formal Charge equation

A

FC= VE-NBE-(1/2)BE

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16
Q

same connectivity but arranged differently in space (S and R)

A

stereoisomers

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17
Q

order of Newman projections from most stable to least

A

anti-staggered>gauche>eclipse

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18
Q

for n chiral centers, there are how many configurations

A

2^n

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19
Q

a diastereomer that differs at only 1 chiral center

A

epimer

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20
Q

done by separating 2 immiscible liquids (one polar and one nonpolar)

A

liquid-liquid extraction

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21
Q

separates 2 liquids if the difference in bp is large

A

simple distillation

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22
Q

can separate 2 liquids with small differences in bp and uses fractioning column

A

fractional distillation

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23
Q

done under lower pressure and lowers the bp for all liquid components so temp. doesn’t have to go so high

A

vacuum distillation

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24
Q

gas part is mobile phase, liquid part is stationary phase coated to inside walls of column; those with greater affinity for stationary phase come out slower

A

gas-liquid chromatography

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25
Q

separates based on polarity and charge

A

chromatography

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26
Q

separates pigments in dyes; solvent is the mobile phase and paper is the stationary phase; those with greater affinity to paper stay behind, those with greater affinity to solvent get washed along

A

paper chromatography

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27
Q

instead of paper, you have a plate coated with a specific stationary phase

A

thin-layer chromatography

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28
Q

barely dissolving your compound, then let it recrystallize out of solution, making compound more pure; impurities should remain dissolved in solvent

A

recrystallization

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29
Q

can easily evaporate, meaning lower boiling points

A

volatile compounds

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30
Q

the stronger the intermolecular forces, the ____ the boiling point

A

higher

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31
Q

separates molecules by size; size of pores in column- those that can’t fit in, elute faster

A

size-exclusion chromatography

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32
Q

strong acid =

A

inert conj. base

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33
Q

greater atomic radius means what

A

longer bond b/t two atoms (nucleus to nucleus)

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34
Q

if you compress, then volume decreases, what increases?

A

density

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35
Q

1 N =

A

1 kg*m/s^2

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36
Q

of electrons in shell

A

2n^2

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37
Q

of electrons in subshell

A

4L+2

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38
Q

more protons than electrons means positive charge pulls electrons in, which will do what to radius

A

decrease radius

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39
Q

increase intermolecular forces, increase what

A

boiling point

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40
Q

if atom is lacking in electrons by greater number, say lacking by 2 instead of 1, then its ionization energy is

A

greater b/c holding on tight to those electrons

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41
Q

considers arrangement of bonded atoms only

A

molecular arrangement

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42
Q

p< 0.05

A

statistically significant

43
Q

type I error

A

false +

44
Q

type II error

A

false -

45
Q

movement of + charge

A

current

46
Q

atomic orbital’s overall size

A

n

47
Q

shape of the orbital

A

l

48
Q

direction of spin

A

s

49
Q

distinguishes b/t 2 electrons in an atomic subshell

A

ms

50
Q

conductivity is proportional to what

A

total concentrations of ions in solution; ex. MgCl2 will dissociate into 3 ions

51
Q

method only used for separations/purifications, NOT used to drive equilibrium rxn

A

extraction

52
Q

when K< 1, what happens

A

reactants undergo little ionization and dissociation

53
Q

in a more basic environment than an acid’s pKa, say 7.4 and the pKa is 6.4, what form predominates (deprotonated or protonated?)

A

deprotonated

54
Q

deprotonated conj. pair

A

base

55
Q

what occurs when dealing with an indicator when the pH of the solution is around pKa of indicator; (so choose indicator with pka near estimated eq. pt. pH)

A

color change occurs

56
Q

pH at eq. pt. when strong acid is titrated with strong base

A

pH=7

57
Q

pH at eq. pt. when weak acid is titrated with strong base

A

pH>7

58
Q

pH at eq. pt. when strong acid is titrated with weak base

A

pH<7

59
Q

common strong acids:

A 
HCl
HBr
HI
H2SO4
HNO3
HClO3
HClO4
60
Q

common strong bases:

A 
NaOH
KOH
CsOH
Ca(OH)2
Ba(OH)2
Sr(OH)2
61
Q

interaction b/t a metal cation and an electron pair donor (lewis acid-base interaction)

A

coordinate covalent

electrons shared b/t the two by only one molecule providing them

62
Q

which has smaller bond:

C-H or O-N

A

C-H because hydrogen atomic radius tiny compared to other elements

63
Q

minimum energy barrier necessary to be overcome by the reactants on the path to products

A

activation energy

64
Q

adding or removing a catalyst affects the reaction rates, but NOT what

A

the position of the equilibrium

65
Q

what cannot be amphoteric species?

A

STRONG acids or bases

66
Q

intermolecular forces in NH3 gases

A

dipole-dipole and london dispersion (all molecules exhibit london dispersion)

67
Q

stable to mixing is thermodynamic or kinetic

A

kinetic

68
Q

mixing to new liposomes or molecules is thermodynamic or kinetic

A

thermodynamic

69
Q

function of air bubbles and boiling chip in vacuum distillation

A

prevent superheating

70
Q

color of solutions depends on an ion that has what and is able to absorb more light to move to higher energy orbitals

A

unfilled orbitals

71
Q

N-H bond is capable of what making it more soluble in water

A

capable of hydrogen bonding with water

72
Q

when asked to find a quantity of X that was required to reach eq. point in titration, remember “X is titrated with Y”

A

X is the unknown concentration and Y is the titrant

73
Q

involves using varying volumes of a solution of known concentration with a known volume of solution of unknown concentration

A

titration

74
Q

if passage says varying amounts of NAG, use what values

A

the other values given, not the NAG values

75
Q

finding the concentration of an unknown solution when you know the concentration of another solution- use the known to find the unknown

A

titration

76
Q

acid + base= salt + water is what type of reaction

A

neutralization

77
Q

temperature at STP

A

0C or 273K

78
Q

temperature under standard conditions

A

25C or 298 K

79
Q

rate law=

A

k[A]^x[B]^y

80
Q

Boyles law

A

PV=PV

81
Q

Charles law

A

V/T=V/T

82
Q

gay lussacs law

A

P/T=P/T

83
Q

pressure, density, temperature, volume, enthalpy, internal energy, free energy, and entropy are all what

A

state functions

84
Q

standard heat of reaction

A

heat of products- heat of reactants

85
Q

bond enthalpy equation

A

bonds broken-bonds formed

86
Q

1 mole of gas at STP=

A

22.4 L

87
Q

osmotic pressure=

A

iMRT

88
Q

gas molecules distribute randomly

A

diffusion

89
Q

gas molecules under pressure go from one compartment to another through small opening

A

effusion

90
Q

mol/kg

A

molality

91
Q

image when on opposite side of light source and has solid lines; is it perceived by the eye

A

real image; but since on opp. side, not perceived by eye

92
Q

binding site is hydrophilic or hydrophobic if a molecule is hydrophobic

A

hydrophobic; like dissolves like

93
Q

why must reactive side chains of AA’s be protected

A

to prevent unwanted side reactions

94
Q

amino acid sequence is disrupted; what structure is affected

A

primary

95
Q

what kind of pH will the salt of a weak acid acquire

A

basic pH

96
Q

The number of equivalence points in a titration curve for a polyprotic acid is equal to what

A

the number of acidic protons in the acid

97
Q

large Ksp means what

A

more soluble

98
Q

charge of an electron

A

-1.6x10^(-19) C

99
Q

why can insoluble molecules (nonpolar, hydrophobic, lipid-soluble) pass readily through lipid bilayer

A

b/c they dissolve in the nonpolar, hydrophobic portion of bilayer; like dissolves like

100
Q

buffers contain what kind of acids and bases

A

weak

101
Q

strong acids and bases vs weak acids and bases in terms of conducting electricity

A

strong conducts strongly; weak conducts weakly

102
Q

Co(II) means gain or loss of electrons

A

loss of 2 electrons; so atomic number is minus 2 from original

103
Q

what to add to get weaker acids in aqueous layer during extractions

A

a base

104
Q

purines or pyrimidines always glow

A

purines

MCAT (6 decks)

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