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MCAT > Physical Sciences > Flashcards

Physical Sciences Flashcards

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MCAT flashcards
1
Q

The four kinematic equations are:

A

∆d = Vot + 1/2at2

∆d = (Vavg)t

Vf2 = Vo2 + 2a∆x

Vf = Vo + at

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2
Q

Centripetal force:

A

Fc = (mv2)/r

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3
Q

Centripetal acceleration:

A

ac = v2/r

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4
Q

Power:

A

P = Work/time

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5
Q

Spring mechanics:

A

Fspring = kx

(Force of compression or stretch = spring constant X displacement of spring from equilibrium position)

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6
Q

Elastic potential energy:

A

PEspring = 1/2kx2

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7
Q

Simple harmonic motion (mass on a spring):

A

T = 2π√(m/k)

Period = 2π√(mass/spring constant)

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8
Q

Simple harmonic motion (pendulum):

A

T = 2π√(L/g)

Period = 2π√(pendulum length/acceleration of gravity)

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9
Q

Angular velocity:

A 
ω = 2πf (angular velocity = 2π X frequency)
ω = v/r (angular velocity = tangential velocity/radius)
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10
Q

Young’s Modulus:

A

stress/strain

(F/A)/(∆L/L)

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11
Q

Period of circular motion:

A

T = 2π/ω

(Period = 2π/angular velocity)

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12
Q

Ramp force:

A

F = mg(h/d)

(Force = mg(height of ramp/distance along its hypotenuse)

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13
Q

Lever force:

A

F = mg(Lm/Lf)

(Lm and Lf refer to lever arms for mass and applied force)

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14
Q

Hydraulic lift force:

A

F = mg(dl/ds) or F = mg(As/Al)

(dl and ds refer to distances traveled by large and small plunger; Asand Al refer to cross-sectional areas of small and large plunger)

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15
Q

Orbital velocity:

A

v = √(GM/r)

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16
Q

Angular momentum:

A

L = Iω

(angular momentum = moment of inertia X angular velocity)

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17
Q

Second quantum number:

A

l – designates sub-shell; value can be positive integer from 0-(n-1); 0 = s orbital, 1 = *p *orbital, 2 = *d *orbital, 3 = *f *orbital

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18
Q

Third quantum number:

A

m – values range from -l to l; designates orientation of corresponding orbital

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19
Q

Fourth quantum number:

A

s – spin; two values, +1/2 and -1/2

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20
Q

Work function (chemistry):

A

The amount of energy required to eject valence electrons from the surface of a solid metal

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21
Q

Alpha decay:

A

loss of one He nucleus (mass number 4, atomic number 2)

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22
Q

Beta decay:

A

A neutron is changed into a proton with the ejection of an electron

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23
Q

Electron capture:

A

A proton is changed into a neutron via capture of an electron

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24
Q

Positron emission:

A

A proton is changed into a neutron via expulsion of a positron

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25
Q

Gamma emission:

A

Gamma rays emitted as a byproduct of other types of decay

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26
Q

Neutron =

A

proton + electron

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27
Q

Proton =

A

neutron + positron

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28
Q

Condosity of a solution:

A

the concentration of NaCl that will conduct electricity exactly as well as the solution in question

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29
Q

Nitrite:

A

NO2-

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30
Q

Chlorate:

A

ClO3-

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31
Q

Perchlorate:

A

ClO4-

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32
Q

Chlorite:

A

ClO2-

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33
Q

Hypochlorite:

A

ClO-

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34
Q

Carbonate:

A

CO32-

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35
Q

Bicarbonate:

A

HCO3-

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36
Q

Sulfate:

A

SO42-

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37
Q

Phosphate:

A

PO43-

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38
Q

Manganate:

A

MnO42-

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39
Q

Permanganate:

A

MnO4-

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40
Q

Nitrate:

A

NO3-

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41
Q

Specific heat of a substance:

A

the amount of heat per unit mass required to raise the temperature by one degree Celsius

Q = mc∆t

(heat added = mass X specific heat X change in temp)

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42
Q

Pressure-volume work:

A

∆Wsystem = -Pext∆V

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43
Q

pKa:

A

measurement of the relative ability of a molecule to give up a proton; a low pKa value indicates that the compound is acidic and will easily give up its proton to a base

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44
Q

Specific gravity:

A

SG = Dsubstance/Dwater

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45
Q

Density of water:

A

1000kg/m3 or 1.0g/cm3

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46
Q

For objects floating in liquids, the fraction of the object submerged =

A

Dobject/Dliquid

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47
Q

Buoyant force:

A

Fbuoyant = pvg = weight of the amount of fluid displaced by object

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48
Q

Apparent weight:

A

AW = aW (actual weight) - Fbuoyant

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49
Q

Units of pressure:

A

1 x 105 Pascals = 1 atm = 760 mmHg = 760 Torr

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50
Q

Fluid pressure formula:

A

Pfluid = density x g x h

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51
Q

Flow rate:

A

Q = A (total cross-section area) X V (flow velocity)

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52
Q

Bernoulli’s equation:

A

Pressure + pgh + 1/2pv2 = constant value

(conservation of energy for flowing fluids)

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53
Q

Charge of an electron:

A

e- = 1.6 x 10-19 C

(charge is quantized)

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54
Q

Constant electric field voltage =

A

Ed (strength of electric field X distance)

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55
Q

Point charge electric field voltage =

A

Kq/r (K constant X charge/distance)

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56
Q

Formula for magnetic force exerted on a charged particle moving in a magnetic field:

A

F = qvBsinØ

[Force = charge X velocity of particle X magnetic field (in Tesla) X angle between v & B]

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57
Q

Current =

A

∆q/∆t

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58
Q

Formula for resistance:

A

R = pL/A

(Resistance = resistivity X length/cross-sectional area)

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59
Q

Formula for capacitance:

A

C = Q/V

(capacitance = charge on plate/voltage)

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60
Q

Potential energy stored by a capacitor:

A

U = 1/2CV2

61
Q

Total resistance of resistors in series:

A

R = R1 + R2 + R3…

62
Q

Total resistance of resistors in parallel:

A

1/R = 1/R1 + 1/R2 + 1/R3…

63
Q

Total capacitance of capacitors in parallel:

A

C = C1 + C2 + C3…

64
Q

Total capacitance of capacitors in series:

A

1/C = 1/C1 + 1/C2 + 1/C3…

65
Q

Total voltage of batteries in series:

A

add individual voltages directly

66
Q

Total voltage of batteries in parallel:

A

the highest voltage of any one of the batteries in parallel

67
Q

Formula for electrical power:

A

P = IV

68
Q

RMS voltage/current/etc:

A

‘root mean square’ - take readings from several time intervals, square those values, find the average of those squares, determine square root of that average

69
Q

Intensity:

A

power/unit area

(Watts/4πr2)

70
Q

Decibel system:

A

10-fold increases in intensity are represented by 10 unit increases on Richter scale (e.g., sound 100 times more intense = 20 points higher on Richter scale)

71
Q

Speed of light:

A

3 x 108 m/s

72
Q

Speed of sound:

A

340 m/s

73
Q

Doppler effect formulas:

A

∆f/fs = v/c or ∆wavelength/wavelengths = v/c

(v = relative velocity, c = speed of wave)

74
Q

Wave rules for non-dispersive medium:

A
  1. frequency never changes when a wave moves from medium to medium
  2. wavelength does change when a wave moves from medium to medium
75
Q

Harmonics (matching ends):

A

wavelength = 2L/n

76
Q

Harmonics (one node, one antinode):

A

wavelength = 4L/n

(gives only the odd harmonics - 1, 3, 5…)

77
Q

The frequency of the first harmonic is called the __.

A

fundamental frequency

(f = v/2L)

78
Q

The 2nd harmonic can also be called the __.

A

first overtone

(and 3rd harmonic is 2nd overtone, etc.)

79
Q

The frequency of any harmonic is equal to:

A

n(fundamental frequency)

80
Q

Energy of a photon:

A

E = hf

(h = Planck’s constant)

81
Q

Young’s double-slit experiment:

A

x = (wavelength)L/d

(x = distance between fringes, L = distance between slits and screen, d = distance between slits)

82
Q

Electromagnetic radiation - decreasing frequency:

A

gamma rays > x-rays > UV > visible light > infrared > microwaves > radio waves > long waves

83
Q

Visible light wavelength range:

A

390 - 700 nm

84
Q

Index of refraction:

A

n = c/v

(c = speed of light in vacuum, v = speed of light in that medium)

85
Q

Mirror magnification equation:

A

M = -di/do = hi/ho

(d = distance, h = height, i = image, o = object)

86
Q

Thin lens / mirror equation:

A

1/f = 1/di + 1/do

87
Q

Focal point - convex/concave mirrors:

A

f = 1/2r

88
Q

Lens/mirror rules:

A
  1. do is always positive
  2. di and f are positive if on same side as observer, negative if on opposite side
  3. RIP / VUN - real, inverted, positive / virtual, upright, negative (each trio always stay together)
89
Q

Optical power:

A

inverse of focal point (P = 1/f)

90
Q

Two lens systems:

A

M = m1m2

P = p1 + p2

91
Q

Amphoteric:

A

can act as an acid or base (e.g., H2O)

92
Q

Arrhenius acid/base definitions:

A

acids produce H+ ions in solution, bases produce OH- ions in solution

93
Q

Bronsted-Lowry acid/base definitions:

A

acids donate protons, bases acept protons

94
Q

Lewis acid/base definitions:

A

acids accept a pair of electrons, bases donate a pair of electrons

95
Q

Strong acids:

A

HI, HBr, HCl, HNO3, HClO4, HClO3, H2SO4, H3O+

96
Q

Strong bases:

A

Group IA hydroxides (NaOH, KOH, etc.), NH2-, H-, Ca(OH)2, Sr(OH)2, Ba(OH)2, Na2O, CaO

97
Q

What is the salt of a weak acid or base?

A

the conjugate base/acid of that weak acid/base combined with an ion to form a salt

98
Q

When the salts of weak acids or bases dissolve in water,

A

one of the ions will undergo hydrolysis to re-form the weak acid or base

99
Q

Titration: 1 equivalent =

A

the amount of acid or base necessary to produce or consume one mole of [H+] ions

100
Q

Titration: at the equivalence/stoichiometric point (midpoint of nearly vertical section):

A

[titrant] = [analyte]

101
Q

Titration: at the half-equivalence point (midpoint of nearly horizontal section):

A

[HA] = [A-]

(only true for weak conjugate acid/base pairs)

102
Q

Electrical potential =

A

Eo - reduction potential (larger number = higher potential for reduction)

103
Q

Hydrogen half cell:

A

2H+ + 2e- = H2, Eo = 0.00V

104
Q

Cell potential:

A

Eocell or Cell EMF - the sum of the electrical potentials for the two half-reactions that make up an electrochemical cell

105
Q

Cathode:

A

positive terminal

106
Q

Anode:

A

negative terminal

107
Q

Cell potential for a Galvanic cell is always __.

A

positive

108
Q

Cell potential for an electrolytic cell will always be __.

A

negative

109
Q

Electrolytic cell:

A

external voltage applied to galvanic cell, forcing the reverse results

110
Q

Nernst equation:

A

E = Eo - (0.06/n)log[lower]/[higher]

111
Q

Concentration cell:

A

same electrodes and solution used, reaction driven difference in molarities of two solutions

112
Q

Relationship between free energy and chemical energy:

A

∆Go = -nFEo

(n = moles of electrons transferred, F = Faraday’s constant)

113
Q

Faraday’s constant:

A

the charge on one mole of electrons

114
Q

R gas constant:

A

R = 0.08 L•atm/mol•K = 8.31 J/mol•K

115
Q

Ideal gas assumptions:

A

gas molecules have no volume and no intermolecular forces

116
Q

Ideal Gas Standard Temperature and Pressure:

A

P = 1 atm

V = 22.4 L

n = 1 mole

R = 0.08 Latm/molK or 8.31 J/molK

T = 273 K

117
Q

Combined Gas Law:

A

P1V1/T1 = P2V2/T2

(Because PV/T = nR and R is constant, for the same number of moles of gas the ratio of PV/T remains constant)

118
Q

Real gas deviations from Ideal Gas Law:

A

at extremely high pressure, gas molecules will occupy a greater volume; at extremely low temperature, gas molecules produce a smaller pressure

119
Q

Graham’s Law (effusion and diffusion, i.e., gas mixing):

A

Rate1/Rate2 = √MW2/√MW1

(MW = molecular weight)

120
Q

Liquids boil when the vapor pressure of the liquid equals __.

A

atmospheric pressure

121
Q

∆Hfusion =

A

the amount of energy in J/mol required or removed to go from solid to liquid or liquid to solid, respectively

122
Q

∆Hvaporization =

A

the amount of energy in J/mol required or removed to go from liquid to gas or gas to liquid, respectively

123
Q

Sublimation:

A

solid → gas

124
Q

Deposition =

A

gas → solid

125
Q

Triple point (chemistry):

A

precise temperature and pressure at which all 3 phases of a substance exist simultaneously in equilibrium with each other

126
Q

Critical point (chemistry):

A

the precise temp and pressure above which gas and liquid phases become indistinguishable

127
Q

Supercritical fluid (chemistry):

A

cannot be compressed back into a liquid by increasing pressure, nor can it be turned to gas by increasing temp

128
Q

If energy is added at a constant rate, the phase change from solid to liquid is __ than that from liquid to gas.

A

shorter

129
Q

The solubility of a gas in a liquid is __ proportional to the partial pressure of the gas over that liquid.

A

directly

130
Q

Vapor pressure w/ a non-volatile solute:

A

Vp = XVpo

(x = mole fraction of pure solvent)

131
Q

Total vapor pressue w/ a volatile solute:

A

XVposolvent + XVposolute

132
Q

Gas solubility: polar and non-polar gases together:

A

easily form homogenous mixtures

133
Q

Boiling point elevation:

A

∆T = kbmi

(m = molality, i = number of ions formed per molecule)

134
Q

Freezing point depression:

A

∆T = kfmi

(m = molality, i = number of ions formed per molecule)

135
Q

More solute = __ osmotic pressure

A

higher

136
Q

Osmotic pressure formula:

A

π = TRiM

(i = # ions formed per molecule, M = molarity)

137
Q

Molality:

A

moles solute / kg solvent

138
Q

Parts per million:

A

mass solute/total mass solution x 106

139
Q

Colloid:

A

solvents containing undissolved solute particles too small to be separated by filtration (ex: paint)

140
Q

For unsaturated solutions, the Ksp is __ than the ion product.

A

greater

141
Q

A __ ion added to a solution might cause precipitation; a __ ion added definitely will not cause precipitation.

A

common, spectator

142
Q

Prefix: tera-

A

T - 1012

143
Q

Prefix: giga-

A

G - 109

144
Q

Prefix: mega-

A

M - 106

145
Q

Prefix: kilo-

A

k - 103

146
Q

Prefix: hecto-

A

h - 102

147
Q

Prefix: micro-

A

µ - 10-6

148
Q

Prefix: nano-

A

n - 10-9

149
Q

Prefix: pico-

A

p - 10-12

MCAT (3 decks)

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