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Chem/Phys Flashcards

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MCAT flashcards
1
Q

Relate ohms law and power

A

P=IV=V²/R=I²R

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2
Q

Energy of a capacitor

A

U = 1/2QV

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3
Q

Charge of a capacitor

A

C = Q/V

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4
Q

Work

A

ΔKE
PΔV
FdCosθ

Si unit: Joule = Nm

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5
Q

Power

A

Work/Time
P=IV

Si Unit: Watt = J/s

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6
Q

Joules

A

Unit for Energy or Work

also, N*m

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7
Q

Watt

A

Unit for Power

also, J/s & Nm/s

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8
Q

kilo

A

10^3

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9
Q

micro

A

10^-6

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10
Q

nano

A

10^-9

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11
Q

milli

A

10^-3

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12
Q

Which is the limiting reagent

4A + 2B -> C

A

A
the one that produces the least amount of product
the one that has a greater mol ratio of react:prod

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13
Q

7*4

A

28

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14
Q

wavelength of a harmonic?

A 
λ = 2L/n
n = harmonic

1st harmonic has 2 nodes and 1 antinode
2nd harmonic has 3 nodes and 2 antinodes
3rd harmonic has 4 nodes and 3 antinodes

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15
Q

wavelength of a harmonic in a closed tube?

A 
λ = 4L/n
n = harmonic

closed tube is the distance from one node to one antinode aka 1/4 of a total wave

open tube is the distance from one antinode to another antinode aka 1/2 of a total wave

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16
Q

Period of a wave

A

the time it takes for a sound particle to complete one oscillation
1/f
measured in SECONDS

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17
Q

decibel equation and threshold of human hearing

A

Decibel = 10 log intensity/threshold intensity (10^-12)

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18
Q

Note than an increase of 10 dB is an increase in
intensity by a factor of __. An increase of 20 dB is an
increase in intensity by a factor of __.

A

10; 100

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19
Q

Intensity

equation, units

A

Power/Area

Units: Watts/m²

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20
Q

Doppler Effect equation

A

f′ = f (v±vd)/(v±vs)

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21
Q

Gibbs Free Energy equation

A

ΔG = ΔH - TΔS

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22
Q

Ionization Energy

A

energy required to remove an electron. goes up with electronegativity. I > Br > Cl > F

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23
Q

the energy of activation for a reaction is given by

A

the energy of the activated complex - the reactants

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24
Q

current is measured in

A

Amperes
Q/t
charge/time
coulombs/sec

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25
Q

log 1000

A

3 (10^3=1000)

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26
Q

log 1

A

0 (10^0=1)

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27
Q

sound travels fastest in a ___ ___ and slowest in a ___ ___

A

not dense solid; dense gas

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28
Q

Frequency

A

number of cycles a sound particles has made (oscillations from equilibrium and back) in one sec
measured in Hz

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29
Q

What happens in alpha decay

A

emits a 4|2 He

move to the left on the ptable to find the new compound

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30
Q

What happens in beta decay

A

a neutron decays into a proton
an 0|-1 electron is emitted
move to the right on the ptable to find the new compound

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31
Q

What happens in gamma decay

A

compound emits a high energy particle. no change to mass or atomic number

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32
Q

NADH and FADH2 and NADPH are ____ agents. They help bring about the ____ of another compound

A

reducing agents; oxidation

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33
Q

If the reaction is spontaneous, the value of K must __ 1

A

By ΔG = –RTln(Keq), the value of K is greater than 1

As K goes up, ΔG gets more negative

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34
Q

Calcium and Magnesium belong to what group on the ptable?

A

alkaline earth metals

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35
Q

Ca2+(aq) + CO32–(aq) CaCO3(s)

Whats the Ksp equation?

A

Ksp = [Ca2+][CO32–]

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36
Q

How do you calculate flow rate?

A

speed * area

Q = VA

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37
Q

Which properties of a wave are dependent on the medium? Which are not

A

are: speed, wavelength, amplitude

are not: frequency (energy is constant)

38
Q

“photon.” what equation do you use?

A

E = hc/λ

39
Q

sp2 hybridization. # bonds, geometry, angles, example?

A

3 bonds, trigonal planar, 120 degree angles, BH3

40
Q

sp3 hybridization. # bonds, geometry, angles, example?

A

4 bonds, tetrahedral, 109.5, CH4

41
Q

trigonal bipyramidal example

A

PCl5. 5 bonds to central atom. 90, 120, and 180 degree angles

42
Q

Octahedral example

A

SF6. 6 bonds to central atom

90 and 180 degree angles

43
Q

You have a nonpolar eluent in a column chromatograph. what compound will you see come out first

A

alkane first. most polar compound last

44
Q

In silica gel chromatography, silica is a ____ stationary phase so ____ compounds will travel farther and have a ____ Rf

A

polar, nonpolar, greater

45
Q

carboxylic acid has a < or > boiling point than a primary alcohol

A

higher. more polar = tighter bonds = higher bp

46
Q

CHO

A

Aldehyde Group

47
Q

Henderson Hasselbach

A

pH = pKa + log (base/acid)

48
Q

migration of a hydrogen atom from an α-carbon atom to an oxygen atom

A

tautomerism

49
Q

if a base is added to a solution of acid and base the pH will go up or down?

A

pH will go up a little, become slightly more basic

50
Q

Why is NaNO2 basic?

A

NO2 reacts with water to form HNO2

51
Q

dielectric

A

an electrical insulator that can be polarized by an applied electric field.
An uncharged substance that can increase the capacitance of a capactor by decreasing the voltage separation (C=Q/V)

52
Q

two compounds are made, one bigger than the other. what is the yield in mL of one relative to the other?

A

the bigger one will take more moles to make, so it will have a smaller volumetric yield by PV=nRT

53
Q

a weak acid has an ionization constant of what?

A

much less than 1. eg. acetic acid (CH3COOH) has a pka of 1 x 10^-5

54
Q

in Denver there is a ___ atm and liquid boils at a ___ temp and freezes at a ___ temperature

A

Denver has lower atm; lower; higher

55
Q

Molar Solubility

A

How many moles of solute will dissolve in 1L. Derived from Ksp (Solubility product equilibrium constant)

PbI2(s) ⇆ Pb(aq) + I2(aq) Ksp = [Pb][I]^2

aka [Pb] or 2 x [I]

56
Q

A low Ksp means your compound is ____ reactive

A

not very

57
Q

You see an aromatic double bond. What do you think?

A

conjugated system, color
delocalization of electrons
planar
2n+1 pi electrons (2,6,10,14)

58
Q

Kcat

A

catalytic turnover

kcat = vmax/km
kcat/km is catalytic efficiency

59
Q

Km

A

substrate concentration when rate of reaction (v) is 1/2 vmax

a small km, means a high catalytic efficiency

60
Q

density equation

A

mass/volume kg/m^3

61
Q

specific gravity

concept and quantity

A

density of the substance/density of water. water has a density of 10^3 kg/m^3

62
Q

weight

A

F=ma
F=mg
and since ρ=m/v… m=ρv

F= ρgV

63
Q

pressure

A

Force/area N/m^2

64
Q

for static fluids of uniform density in a sealed vessel, pressure is

A

P=ρgz

65
Q

Absolute Pressure

A

P= Po + ρgz

66
Q

Gauge Pressure

A

Pg = P - Patm

67
Q

Continuity Equation

A

A1V1 = A2V2

68
Q

Bernoulli’s Equation

A

P + 1/2ρv^2 + ρgh = constant

69
Q

Archimedes Principle

concept and equation

A

F = ρgV, V=volume submerged

Buoyant force is equal to the weight of the displaced fluid

70
Q

Pascal’s Principle

concept and equation

A

Hydraulic Lift. A change in the pressure applied to an enclosed fluid is transmitted undiminished to every portion of the fluid and to the walls of the containing vessel. Aka you can lift heavy shit if yo uincrease distance

P = F1/A1 = F2/A2 ; A1d1 = A2d2 so
W= F1/d1 = F2/d2
71
Q

Poiseuille’s law equation

A

R = 8hl/πr^4

72
Q

Reactivity hierarchy of carboxylic acid derivatives

A

acyl halide > anhydride > ester/acid > amide

73
Q

creating a bond ____ energy

A

releases

74
Q

amide

A

R(C=O)NR’R’’

75
Q

ester

A

R(C=O)OR’

76
Q

acid anhydride

A

R(C=O)O(C=O)R’

77
Q

acid halide

A

R(C=O)X

78
Q

Amine

A

R-NH2, R-NHR’, or R-NR’R”
medium melting/boiling point
can act as weak base

79
Q

imine

A

R=NH or R=NR
medium melting, boiling point
can act as weak base

80
Q

enamine

A

C=C-NH2, C=C-NHR, C=C-NRR’
medium melting, boiling point
can act as weak base

81
Q

azide

A

N3- powerful nucleophile (like OH-)

82
Q

thiol

A

R-S-H

sulfur containing analogy of alcohol

83
Q

thioether

A

R-S-R’

sulfur containing analog of ether

84
Q

Raoult’s Law

concepts (3) and equations (2)

A

heterogeneous solute-solvent interactions result in vapor pressure depression –> boiling point elevation and freezing point depression

dTb = iKbm
dTf = iKfm
85
Q

Complex ion

A

extremely stable cations bonded to at least one electron pair donor. held together with coordinate covalent bonds. eg. hemoglobin

86
Q

chelation

A

complexes in which central cation bonds to 1 ligand in multiple different places. used to sequester toxic materials

87
Q

dissolution of solute into solution depends on what two factors

A

change in enthalpy (go = exothermic, -dH)
change in entropy (go = ^ entropy, +dS)

equation: dG = dH - TdS

88
Q

6*4

A

24

89
Q

dissolution of gas into liquid is what in terms of enthalpy?

A

exothermic

90
Q

dissolution of solid is what in terms of enthalpy

A

endothermic

91
Q

molar solubility

A

direct measure of how much solid dissolves in solution
aka Molarity
measured in: mol solute/ L soln

92
Q

6*3

A

18

MCAT (4 decks)

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