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My MCAT decks > Chem/Phys 1 > Flashcards

Chem/Phys 1 Flashcards

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MCAT flashcards
1
Q

formula for degrees of unsaturation

A

(2C+2)-H / 2

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2
Q

Bronsted-Lowry acid vs base

A

acid gives H+, base receives H+

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3
Q

Lewis acid vs base

A

acid=electron pair acceptor, base= electron pair donor

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4
Q

epimers

A

a type of diastereomer that differs at exactly 1 chiral center

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5
Q

meso compounds

A

achiral, must contain at least 1 chiral center, have an internal plane of symmetry

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6
Q

speed of light (in a vacuum)

A

3 x 10^8 m/s

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7
Q

electric charge of a proton/electron

A

1.6 x 10^-19

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8
Q

density of water

A

1000 kg/m^3

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9
Q

3 kinematic formulas

A

Vf=Vi + at, Vf^2=Vi^2 t +2ad, d=Vi t +1/2at^2

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10
Q

Newton’s first law

A

F=ma

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11
Q

Friction formula

A

mu x normal force

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12
Q

1 cm^3= ___ L?

A

1 mL= .001 L

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13
Q

ionization energy trend

A

Ionization energy is the amount of energy required to remove an electron. As radius decreases and number of protons increases, its harder to remove an electron. So ionization energy increases towards the direction of NY where there is the most energy.

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14
Q

Electron affinity

A

Energy change (energy required/released) to add an additional electron. If energy is released, the energy change is negative and electron affinity is negative. If energy is required to add an electron, electron affinity is positive

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15
Q

relationship between visible light, energy, wavelength, frequency and which colors are highest/lowest energy

A

red has the longest wavelength and lowest energy, violet has the shortest wavelength and highest energy (E = hν = hc/λ where v=frequency and gamma is the wavelength)

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16
Q

diamagnetic vs paramagnetic

A

diamagnetic=all electrons are paired and atom is REPELLED by an external magnetic field. Paramagnetic=unpaired electrons and atom is ATTRACTED to an external magnetic field

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17
Q

alpha decay

A

alpha particle (2 protons and 2 neutrons) is emitted in order to become more stable, reducing the atomic number by 2 and teh mass number by 4

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18
Q

beta decay

A

conversion of a neutron to a proton, and an electron is emitted. Atomic number increases by one but mass number remain the same

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19
Q

electron capture

A

capture an electron from the n=1 shell and use it to convert a proton into a neutron. Atomic number is decreased by one and mass number remains the same

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20
Q

Gamma decay

A

photon is emitted which changes neither mass number nor atomic number

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21
Q

how many moles per liter of pure water

A

55 moles of water in 1 L

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22
Q

solubility rules

A

NAG SAG: Nitrates, acetates, Group 1, Sulfates, Ammonium, Group 17. Exceptions are PMS: Pb, Mercury (Hg), Silver

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23
Q

Mixing solutions formula

A

CV+CV=CV final

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24
Q

polar bonds are shorter/equal/longer than non-polar bonds

A

shorter because polar bonds are stronger than nonpolar bonds

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25
Q

what does anhydrous mean

A

anhydrous means in the absence of water

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26
Q

visible light region wavelengths

A

400 nm (violet) to 700 nm (red).

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27
Q

formal charge

A

formal charge = valence e for that element – ½(bonding electrons) – lone electrons (FC=V- B/2 - L)

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28
Q

which atoms form only 3 bonds? (6 valence electrons)

A

B and Al (and some other group 3 atoms)

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29
Q

which atoms can make 5 bonds?

A

Si, P, S, Cl

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30
Q

fusion vs vaporization vs crystallization vs condensation vs sublimation vs deposition

A

fusion=melting, vaporization=boiling, condensation=gas to liquid, crystallization=liquid to solid, sublimation=solid to gas, deposition=gas to solid

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31
Q

relationship between heat capacity/specific heat and temperature change

A

high specific heat=smaller change in temp

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32
Q

1 calorie = ___ Joules

A

4.2

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33
Q

specific heat equation

A

q=mc(delta t)

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34
Q

effect of pressure on water melting

A

increased pressure on ice results in increased melting. Increased pressure=decreased melting point, decreased pressure=increased melting point

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35
Q

volatile

A

easily evaporated, weakest IMFs

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36
Q

which gasses behave most ideally?

A

weakest IMFs and smallest molecular weights/volumes

37
Q

structure of diamond

A

all carbon- only covalent bonds

38
Q

Standard temperature and pressure

A

1 atm and 0 degrees C

39
Q

volume of an ideal gas (per mole)

A

22.4 L per 1 mole sample of gas

40
Q

Avogadro’s number (# of particles in a mole) approximated

A

6x10^23

41
Q

1 atm = ___ torr

A

760

42
Q

760 torr= ___mmHG

A

760

43
Q

1 atm=___kPa

A

101

44
Q

celcius to kelvin

A

C+273=K

45
Q

2 factors relevant to gas behavior

A

IMFs and molecular weight

46
Q

where on a heating curve can you get the specific heat (c)

A

the slope

47
Q

prefix for 4 carbons

A

but-

48
Q

prefix for 2 carbons

A

eth-

49
Q

Rf value

A

distance traveled by individual component / distance traveled by solvent

50
Q

IR stretch of carbonyls (C=O)

A

1700 cm-1, very strong and intense “v” shape

51
Q

IR stretch of alkenes (C=C)

A

1650 cm-1

52
Q

IR stretch of triple bond (C≡C)

A

2260-2100 cm-1

53
Q

IR stretch of alcohols (O-H)

A

2600-3200 cm-1 very strong and very broad “U” shape (broadness is due to H bonding)

54
Q

IR stretch of N-H bond

A

3150-2500

55
Q

which base only deprotonates carboxylic acids?

A

weak base solvents like NaHCO3 (sodium bicarbonate)

56
Q

which base deprotonates phenols AND carboxylic acids?

A

strong base solvents like NaOH

57
Q

which acid protonates amines?

A

strong acids (HCl)

58
Q

are amines nucleophiles or electrophiles?

A

nucleophiles because they have a lone pair to donate

59
Q

isochoric process

A

constant volume so deltaE=Q

60
Q

units of Pa

A

J/m^3

61
Q

in a closed system, if internal energy increases, what happens to temperature?

A

temperature increases

62
Q

L amino acid vs D amino acid

A

amino group on the left=L, amino group on the right=D

63
Q

acidic amino acids

A

D (aspartate) and E (glutamate)

64
Q

basic amino acids

A

lysine (K), arginine (R), histidine (H)

65
Q

amino acids with aromatic side chains

A

Tryptophan (W), Phenylalanine (F), Tyrosine (Y)

66
Q

Strecker synthesis of amino acids

A

aldehyde becomes an immine, then H is replaced with CN, then acid workup to become COOH

67
Q

Gabriel Malonic ester synthesis

A

phthalimide + KOH is deprotonated, then attacks alkyl halide via SN2, decarboxylation

68
Q

Zwitterion

A

amino acid ion where net charge is 0, at pI

69
Q

determining L or D of carbohydrates

A

look at second to last (penultimate) carbon with an OH. OH groups attacks the anomeric carbon to form a ring.

70
Q

Anomeric carbon of a carbohydrate

A

the carbon attached to 2 oxygens in a ring which was initially a COOH group on the end.

71
Q

Benedict’s test

A

Cu2+ reagent reduces aldehyde of a sugar into a COO- group and Cu precipitate

72
Q

a vs b glycosidic linkages

A

a is when oxygen group is down, b is when oxygen group is up. look at carbon attached to 2 oxygens

73
Q

Size exclusion chromatography

A

used to separate proteins, small proteins get stuck in beads, large proteins eluded

74
Q

Thin-Layer chromatography and column chromatography

A

used to separate based on polarity, stationary phase is polar, mobile phase is nonpolar

75
Q

reverse phase HPLC (reverse phase High performance liquid chromatography)

A

nonpolar stationary phase and polar mobile phase, polar eludes first

76
Q

Ion Exchange Chromatography

A

used to separate proteins based on charges

77
Q

Affinity Chromatography

A

lock and key interactions drive separation. Used to separate proteins from a biochemical mixture

78
Q

ELISA

A

used to determine the presence of antigens or antibodies

79
Q

Blotting (South, North, West)

A

South=DNA, North=RNA, West/East=proteins (SNOW DRoP)

80
Q

Gas chromatography and distillation

A

separation based on volatility/boiling point, low boiling point substances get stuck and are eluded as liquids

81
Q

extraction (solvents)

A

separation based on solubility on polar/nonpolar solvents

82
Q

Resolution of enantiomers techniques

A

convert enantiomers to diasteriomeric salts, separate salts, then revert salts to their original enantiomers

83
Q

Mass spectroscopy

A

used to determine molecular weight and elemental/isotopic composition

84
Q

UV/Vis spectroscopy

A

indicates the presence of a conjugated pi system. As conjugation increases, wavelength absorbed increases (appears more green)

85
Q

IR spectroscopy

A

used to distinguish between molecules with different functional groups

86
Q

H-NMR

A

measures nonequivalent hydrogens. Splitting pattern=n+1=number of nonequivalent neighboring hydrogens. Area under signal (integration)=# of Hs represented by the signal

87
Q

isochoric

A

volume is constant, no work being done

88
Q

isobaric

A

pressure is constant, expansion. Work done is the area under the curve of pressure and volume.

89
Q

isothermal

A

temperature is constant, work is done as volume increases

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