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MCAT > Chemistry > Flashcards

Chemistry Flashcards

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MCAT flashcards
1
Q

Titration end point

A

When indicator changes color

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2
Q

Titration equivalence point

A

amount of titrant has neutralized analyte (moles of acid= moles of base) - vertical on curve

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3
Q

electronegativity

A

atom attraction of electron to self

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4
Q

heiseberg uncertainty principle

A

cant know position and momentum at the same time

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5
Q

principal quantum number

A

n, main energy level

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6
Q

angular momentum quantum number

(Azimuthal)

A

l, shape, 0 to n-1, 0=s, 1=p

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7
Q

magnetic quantum number

A

ml, orientation of orbital, -l to l

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8
Q

spin quantum number

A

ms, +1/2 or -1/2

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9
Q

Total orbitals

A

Total= n^2

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10
Q

Number of electrons in an orbital

A

2 max

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11
Q

Number of electrons in a shell

A

2n^2

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12
Q

Afbau principle

A

fill lowest to highest energy

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13
Q

pauli exclusion

A

no 2 electrons can have the same 4 quantum numbers

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14
Q

paramagnetism

A

one or more unpaired electrons- pulled into external magnetic field

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15
Q

diamagentism

A

all electrons are paired. repelled by magnetic field

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16
Q

atomic number

A

Z, number of protons

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17
Q

mass number

A

A, protons and neutrons in the nucleus

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18
Q

atomic mass

A

average mass of all isotopes

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19
Q

Mass defect

A

difference between predicted and actual mass.. mass is converted through energy when nucleus is made…. E=Mc^2 is energy released

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20
Q

Nuclear binding energy

A

energy to break nucleus or form nucleus (causes mass defect)

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21
Q

Nuclear strong force

A

holds nucleus, stable, stronger than electrostatics of repelling protons

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22
Q

Nucleons

A

protons and neutrons in nucleus

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23
Q

Visible spectrum ranges

A

red= longer and lower frequency, violet= shorter wavelength, higher frequency

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24
Q

Common ion effect

A

move system away from extra ion, will decrease solubility

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25
Q

How does pH affect solubility

A

increasing H+/OH alters other ions, increasing H will alter baisic anions and decrease it so shift towards basic anion

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26
Q

Sigma vs. pi bonds

A

head on orbital overlap, pi bonds are side by side unhybridized p

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27
Q

formal charge

A

number of valence electrons in free atom - number of bonds - number of nonbonded electrons

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28
Q

VSEPR

A

negative charges repel, forces molecule to a shape - form to move electrons far apart

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29
Q

sp3 hybrid

A

109.5, tetradhedral

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30
Q

sp2 hybrid

A

120, trigonal planar

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31
Q

Triple bonds

A

shortest and strongest

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32
Q

intermolecular bonds

A

between molecules

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33
Q

Dipole- dipole bonds

A

electrostatic via permanent dipole

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34
Q

hydrogen bonds

A

dipole-dipole, hydrogen with an EN atom (F,O,N)

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35
Q

Dispersion

A

weak, transient dipole due to EN difference. Temporary induced dipole

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36
Q

Constitutional isomers

A

differ in connectivty and structure

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37
Q

Chiral

A

non superimposable mirror images, 4 different groups

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38
Q

Achiral

A

superimposable miror images

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39
Q

stereoisomers

A

differ in 3D arrangements

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40
Q

Enantiomers

A

chiral mirror images, not superimposable, opposite configuration at all chiral centers

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41
Q

How to tell R vs. S

A

prioritize (Higher priority is higher atomic number), then out lower priority in the back, Clockwise is R

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42
Q

Optical activity

A

plane polarized light rotates

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43
Q

diastereomers

A

non-superimposable, non mirror images, opposite configuration at some chiral centers

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44
Q

number of stereoisomers

A

2^n where n=chiral centers

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45
Q

cis isomer

A

same group on same side of double bond

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46
Q

E/Z system

A

Z= high priority on same side of double bond

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47
Q

Atomic radius

A

increases down group (due to more electrons) and increases from right to left (less protons) shielding is due to electrons

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48
Q

Zeff

A

Charge felt by added electrons. Increases from left to right (more protons) and bottom to top (further away from protons at bottom)

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49
Q

Ionization energy

A

energy to remove electrons (increases left to right and bottom to top) - farther away feels less protons, and at right has more protons

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50
Q

electronegativity

A

tendency of atoms to attract a bonding pair of electrons, increases left to right and up a group

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51
Q

Electron affinity

A

accept electrons, increases left to right and up a group (increase in affinity means more exothermic)

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52
Q

Huckels rule

A

planar monocyclic rings with pi electrons 4n+2 are aromatic

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53
Q

nucleophillic functional groups

A

lewis base, amines, negative charges, lower EN, more EDG

54
Q

electrophillic functional groups

A

positive, carbonyl C, lewis acid

55
Q

conformational isomers

A

different spatial arrangment, different energy levels due to strain

56
Q

Polar protic solvents

A

stabilize nucleophile. Increase rate of SN1

57
Q

EWG

A

stabilize negative charge and increase acidity

58
Q

EDG examples

A

OH, NR2, OR, R

59
Q

How do mesylate and tosylate act as protecting groups

A

they protect alcohol from being nucleophile or acid

60
Q

tautomer

A

shift carbonyl (keto) to alkene (enol)

61
Q

How do acetals/ ketals protect

A

protect aldehydes or ketones from nucleophillic reaction

62
Q

hemi vs. full acetal or ketal

A

hemi has an OH, full has 2 OR

63
Q

furanose vs. pyranose

A

furanose has 5 membered ring, pyranose has 6 membered ring

64
Q

triglyceride synthesis

A

OH on glycerol is nucleophile, attack carbonyl on carboxylic acid. Makes ester bond

65
Q

anomeric carbon

A

old carbonyl carbon, attatched to 2 oxygen, OH up is alpha, OH down is beta

66
Q

Zero reaction order

A

rate is independent of concentration, slope=-kf

67
Q

first reaction order

A

rate is proportional to concentration, graph ln[A], slope=-kf

68
Q

second reaction order

A

rate is proportional to reactant, graph 1/[A], slope kf

69
Q

Kinetics

A

how fast a reaction is, rate

70
Q

Thermodynamics

A

spontaneity, stability

71
Q

zero law of thermodynamics

A

temperature is a state function, in contact means in equilibrium

72
Q

first law of thermodynamics

A

energy of isolated systems is conserved, delta U= Q+W (if work done on gas then add, if by gas then subtract)

73
Q

second law of thermodynamics

A

entropy of isolated systems wont decrease, heat flows hot to cold

74
Q

third law of thermodynamics

A

entropy increases with temperature, volume

75
Q

La Chetllier

A

move to less concentration, lower P, and heat removed

76
Q

Boyles Law

A

PV= constant

77
Q

Charles Law

A

V/T= constant

78
Q

Avagadros Law

A

V/n= constant

79
Q

Isovolumetric

A

delta v=0, w=0, delta U= q- vertical line

80
Q

adiabatic

A

delta T=0, q=0, delta U=w , NO HEAT EXCHANGED

81
Q

isothermal

A

delta U= 0, delta E=0, 0=q+ w, PV=0

82
Q

isobaric

A

constant P, delta U= Q + (-PdeltaV)

83
Q

Ideal gas law

A

pV=nRT

84
Q

STP

A

1 mol= 22.4L, 1 atm, 273K

85
Q

When does real has deviate from ideal

A

when close together, high P, low temp

86
Q

normality

A

number of equivalents per L solution

87
Q

Ksp

A

solubility constant, shows how inclined compound is to dissolve, only include aq and gas

88
Q

Balance Redox

A

make hald reaction, balance all except HO, then add H2O to balance O and H+ ti balance H, add electrons to balance charge

89
Q

acidic

A

more acidic= more polar, more oxygenated.

90
Q

weak acid

A

HF, HCN, acetic acid

91
Q

weak base

A

NH3, ammonia

92
Q

pKa of amino acids

A

amino group is 9, carboxyl is 2 (acidic). pI is 5.5

93
Q

purpose of acetyl coA

A

TCA cycle, produces fatty acid when ATP is high

94
Q

anomers

A

epimers that are in their cyclic state

95
Q

Epimers

A

stereoisomers that differ in stereochem configuration at only ONE stereocenter

96
Q

Max number of stereoisomers

A

2^n where n= number of chiral centers

97
Q

Fischer projection

A

horizontal is wedged, out of page. Vertical is dashed, into page

98
Q

How does optical activity relate to configuration

A

Positive =d, negative=s

99
Q

What affects acidity

A

EWG - (stabilize the negative charge to increase acidity), more polar, more oxidized

100
Q

How does reduction occur

A

hydride attacks carbonyl (hydrogen has lone pair)

101
Q

Amino acid synthesis

A

amine is nucleophile, and carbonyl is electrophule. Can be gabriel or strecker

102
Q

Reaction quotient

A

Q, at some point in time to reach equilibrium

103
Q

Redox titration

A

strong oxiding agent is titrated and the change in voltage is measured. equivalence is when all of the reducing agent is oxidized

104
Q

Velocity

A

displacement over time

105
Q

Acceleration

A

Change in velocity over time, has force, can change in magnitude or direction

106
Q

Negative acceleration

A

slowing down when velocity is positive, speeding up when velocity is negative

107
Q

Hydrophobic effect

A

hydrophobic layer moves closer together and becomes ordered, making a smaller hydrophillic layer of water- allows higher entropy for water

108
Q

Vmax

A

shows enzyme concentration

109
Q

Kcat

A

Vmax / [Et] , lower kM means tight fit

110
Q

X intercept on Michaelis Menten

A

1/km

111
Q

Y intercept on Michaelis Menten

A

1/Vmax

112
Q

Slope on Michaelis Menten

A

Km/Vmax

113
Q

Bronsted acid vs. base

A

acid is proton donor, base is proton acceptor

114
Q

Lewis acid vs. base

A

acid is electron pair acceptor, base is electron pair donor

115
Q

geometric isomers

A

isomers that differ in orientation across a double bond

116
Q

coordinate covalent

A

both electrons come from same atom

117
Q

heat of formation

A

larger is favored (more release)

118
Q

Ka

A

Acid dissociation constant, how well something dissociates

119
Q

amplitude

A

maximum magnitude of displacement from equilibrium

120
Q

period

A

time for entire cycle, T=1/f

121
Q

how do electrochemical cells work

A

reduction at cathode, oxidation at anode

122
Q

direction of electron flow in electrochemical cells

A

electrons flow from anode to cathode

123
Q

What can oxidizing agent oxidize?

A

Any reducing agent below it on standard reduction table

124
Q

How to tell if redox is spontaneous?

A

add redox standard redox potentials - + potential is spontaneous

125
Q

ceoncentration cell

A

same electrode on both sides, different concentrations

126
Q

isotopes

A

same atom, differ in number of neutrons

127
Q

alpha particle

A

two protons and two neutrons bound, positive

128
Q

beta particles

A

high energy electrons or positrons

129
Q

beta radiation

A

protons turns into a neutron, release electron

130
Q

positron

A

electron counter part, +1

MCAT (7 decks)

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