Physical Sciences

Question 1

The four kinematic equations are:

Answer 1

∆d = V_ot + 1/2at²

∆d = (V_avg)t

V_f² = V_o² + 2a∆x

V_f = V_o + at

Question 2

Centripetal force:

Answer 2

F_c = (mv²)/r

Question 3

Centripetal acceleration:

Answer 3

a_c = v²/r

Question 4

Power:

Answer 4

P = Work/time

Question 5

Spring mechanics:

Answer 5

F_spring = kx

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

Question 6

Elastic potential energy:

Answer 6

PE_spring = 1/2kx²

Question 7

Simple harmonic motion (mass on a spring):

Answer 7

T = 2π√(m/k)

Period = 2π√(mass/spring constant)

Question 8

Simple harmonic motion (pendulum):

Answer 8

T = 2π√(L/g)

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

Question 9

Angular velocity:

Answer 9

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

Question 10

Young’s Modulus:

Answer 10

stress/strain

(F/A)/(∆L/L)

Question 11

Period of circular motion:

Answer 11

T = 2π/ω

(Period = 2π/angular velocity)

Question 12

Ramp force:

Answer 12

F = mg(h/d)

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

Question 13

Lever force:

Answer 13

F = mg(L_m/L_f)

(L_m and L_f refer to lever arms for mass and applied force)

Question 14

Hydraulic lift force:

Answer 14

F = mg(d_l/d_s) or F = mg(A_s/A_l)

(d_l and d_s refer to distances traveled by large and small plunger; A_sand A_l refer to cross-sectional areas of small and large plunger)

Question 15

Orbital velocity:

Answer 15

v = √(GM/r)

Question 16

Angular momentum:

Answer 16

L = Iω

(angular momentum = moment of inertia X angular velocity)

Question 17

Second quantum number:

Answer 17

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

Question 18

Third quantum number:

Answer 18

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

Question 19

Fourth quantum number:

Answer 19

s – spin; two values, +1/2 and -1/2

Question 20

Work function (chemistry):

Answer 20

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

Question 21

Alpha decay:

Answer 21

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

Question 22

Beta decay:

Answer 22

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

Question 23

Electron capture:

Answer 23

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

Question 24

Positron emission:

Answer 24

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

Question 25

Gamma emission:

Answer 25

Gamma rays emitted as a byproduct of other types of decay

Question 26

Neutron =

Answer 26

proton + electron

Question 27

Proton =

Answer 27

neutron + positron

Question 28

Condosity of a solution:

Answer 28

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

Question 29

Nitrite:

Answer 29

NO₂^-

Question 30

Chlorate:

Answer 30

ClO₃^-

Question 31

Perchlorate:

Answer 31

ClO₄^-

Question 32

Chlorite:

Answer 32

ClO₂^-

Question 33

Hypochlorite:

Answer 33

ClO^-

Question 34

Carbonate:

Answer 34

CO₃^2-

Question 35

Bicarbonate:

Answer 35

HCO₃^-

Question 36

Sulfate:

Answer 36

SO₄^2-

Question 37

Phosphate:

Answer 37

PO₄^3-

Question 38

Manganate:

Answer 38

MnO₄^2-

Question 39

Permanganate:

Answer 39

MnO₄^-

Question 40

Nitrate:

Answer 40

NO₃^-

Question 41

Specific heat of a substance:

Answer 41

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)

Question 42

Pressure-volume work:

Answer 42

∆W_system = -P_ext∆V

Question 43

pKa:

Answer 43

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

Question 44

Specific gravity:

Answer 44

SG = D_substance/D_water

Question 45

Density of water:

Answer 45

1000kg/m³ or 1.0g/cm³

Question 46

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

Answer 46

D_object/D_liquid

Question 47

Buoyant force:

Answer 47

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

Question 48

Apparent weight:

Answer 48

AW = aW (actual weight) - F_buoyant

Question 49

Units of pressure:

Answer 49

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

Question 50

Fluid pressure formula:

Answer 50

P_fluid = density x g x h

Question 51

Flow rate:

Answer 51

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

Question 52

Bernoulli's equation:

Answer 52

Pressure + *p*gh + 1/2*p*v² = constant value (conservation of energy for flowing fluids)

Question 53

Charge of an electron:

Answer 53

e^- = 1.6 x 10^-19 C | (charge is _quantized_)

Question 54

Constant electric field voltage =

Answer 54

Ed (strength of electric field X distance)

Question 55

Point charge electric field voltage =

Answer 55

Kq/r (K constant X charge/distance)

Question 56

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

Answer 56

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

Question 57

Current =

Answer 57

∆q/∆t

Question 58

Formula for resistance:

Answer 58

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

Question 59

Formula for capacitance:

Answer 59

C = Q/V | (capacitance = charge on plate/voltage)

Question 60

Potential energy stored by a capacitor:

Answer 60

U = 1/2CV²

Question 61

Total resistance of resistors in series:

Answer 61

R = R₁ + R₂ + R₃...

Question 62

Total resistance of resistors in parallel:

Answer 62

1/R = 1/R₁ + 1/R₂ + 1/R₃...

Question 63

Total capacitance of capacitors in parallel:

Answer 63

C = C₁ + C₂ + C₃...

Question 64

Total capacitance of capacitors in series:

Answer 64

1/C = 1/C₁ + 1/C₂ + 1/C₃...

Question 65

Total voltage of batteries in series:

Answer 65

add individual voltages directly

Question 66

Total voltage of batteries in parallel:

Answer 66

the highest voltage of any one of the batteries in parallel

Question 67

Formula for electrical power:

Answer 67

P = IV

Question 68

RMS voltage/current/etc:

Answer 68

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

Question 69

Intensity:

Answer 69

power/unit area | (Watts/4πr²)

Question 70

Decibel system:

Answer 70

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)

Question 71

Speed of light:

Answer 71

3 x 10⁸ m/s

Question 72

Speed of sound:

Answer 72

340 m/s

Question 73

Doppler effect formulas:

Answer 73

∆f/f_s = v/c or ∆wavelength/wavelength_s = v/c (v = relative velocity, c = speed of wave)

Question 74

Wave rules for non-dispersive medium:

Answer 74

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

Question 75

Harmonics (matching ends):

Answer 75

wavelength = 2L/n

Question 76

Harmonics (one node, one antinode):

Answer 76

wavelength = 4L/n (gives only the odd harmonics - 1, 3, 5...)

Question 77

The frequency of the first harmonic is called the \_\_.

Answer 77

fundamental frequency | (f = v/2L)

Question 78

The 2nd harmonic can also be called the \_\_.

Answer 78

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

Question 79

The frequency of any harmonic is equal to:

Answer 79

n(fundamental frequency)

Question 80

Energy of a photon:

Answer 80

E = hf | (h = Planck's constant)

Question 81

Young's double-slit experiment:

Answer 81

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

Question 82

Electromagnetic radiation - decreasing frequency:

Answer 82

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

Question 83

Visible light wavelength range:

Answer 83

390 - 700 nm

Question 84

Index of refraction:

Answer 84

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

Question 85

Mirror magnification equation:

Answer 85

M = -d_i/d_o = h_i/h_o (d = distance, h = height, i = image, o = object)

Question 86

Thin lens / mirror equation:

Answer 86

1/f = 1/d_i + 1/d_o

Question 87

Focal point - convex/concave mirrors:

Answer 87

f = 1/2r

Question 88

Lens/mirror rules:

Answer 88

1. d_o is always positive 2. d_i 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)

Question 89

Optical power:

Answer 89

inverse of focal point (P = 1/f)

Question 90

Two lens systems:

Answer 90

M = m₁m₂ P = p₁ + p₂

Question 91

Amphoteric:

Answer 91

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

Question 92

Arrhenius acid/base definitions:

Answer 92

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

Question 93

Bronsted-Lowry acid/base definitions:

Answer 93

acids donate protons, bases acept protons

Question 94

Lewis acid/base definitions:

Answer 94

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

Question 95

Strong acids:

Answer 95

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

Question 96

Strong bases:

Answer 96

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

Question 97

What is the salt of a weak acid or base?

Answer 97

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

Question 98

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

Answer 98

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

Question 99

Titration: 1 equivalent =

Answer 99

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

Question 100

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

Answer 100

[titrant] = [analyte]

Question 101

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

Answer 101

[HA] = [A^-] (only true for weak conjugate acid/base pairs)

Question 102

Electrical potential =

Answer 102

E^o - reduction potential (larger number = higher potential for reduction)

Question 103

Hydrogen half cell:

Answer 103

2H⁺ + 2e^- = H², E^o = 0.00V

Question 104

Cell potential:

Answer 104

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

Question 105

Cathode:

Answer 105

positive terminal

Question 106

Anode:

Answer 106

negative terminal

Question 107

Cell potential for a Galvanic cell is always \_\_.

Answer 107

positive

Question 108

Cell potential for an electrolytic cell will always be \_\_.

Answer 108

negative

Question 109

Electrolytic cell:

Answer 109

external voltage applied to galvanic cell, forcing the reverse results

Question 110

Nernst equation:

Answer 110

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

Question 111

Concentration cell:

Answer 111

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

Question 112

Relationship between free energy and chemical energy:

Answer 112

∆G^o = -nFE^o (n = moles of electrons transferred, F = Faraday's constant)

Question 113

Faraday's constant:

Answer 113

the charge on one mole of electrons

Question 114

R gas constant:

Answer 114

R = 0.08 L•atm/mol•K = 8.31 J/mol•K

Question 115

Ideal gas assumptions:

Answer 115

gas molecules have no volume and no intermolecular forces

Question 116

Ideal Gas Standard Temperature and Pressure:

Answer 116

P = 1 atm V = 22.4 L n = 1 mole R = 0.08 Latm/molK or 8.31 J/molK T = 273 K

Question 117

Combined Gas Law:

Answer 117

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)

Question 118

Real gas deviations from Ideal Gas Law:

Answer 118

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

Question 119

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

Answer 119

Rate₁/Rate₂ = √MW₂/√MW₁ | (MW = molecular weight)

Question 120

Liquids boil when the vapor pressure of the liquid equals \_\_.

Answer 120

atmospheric pressure

Question 121

∆H_fusion =

Answer 121

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

Question 122

∆H_vaporization =

Answer 122

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

Question 123

Sublimation:

Answer 123

solid → gas

Question 124

Deposition =

Answer 124

gas → solid

Question 125

Triple point (chemistry):

Answer 125

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

Question 126

Critical point (chemistry):

Answer 126

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

Question 127

Supercritical fluid (chemistry):

Answer 127

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

Question 128

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

Answer 128

shorter

Question 129

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

Answer 129

directly

Question 130

Vapor pressure w/ a non-volatile solute:

Answer 130

Vp = XVp^o | (x = mole fraction of pure solvent)

Question 131

Total vapor pressue w/ a volatile solute:

Answer 131

XVp^o_solvent + XVp^o_solute

Question 132

Gas solubility: polar and non-polar gases together:

Answer 132

easily form homogenous mixtures

Question 133

Boiling point elevation:

Answer 133

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

Question 134

Freezing point depression:

Answer 134

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

Question 135

More solute = __ osmotic pressure

Answer 135

higher

Question 136

Osmotic pressure formula:

Answer 136

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

Question 137

Molality:

Answer 137

moles solute / kg solvent

Question 138

Parts per million:

Answer 138

mass solute/total mass solution x 10⁶

Question 139

Colloid:

Answer 139

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

Question 140

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

Answer 140

greater

Question 141

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

Answer 141

common, spectator

Question 142

Prefix: tera-

Answer 142

T - 10¹²

Question 143

Prefix: giga-

Answer 143

G - 10⁹

Question 144

Prefix: mega-

Answer 144

M - 10⁶

Question 145

Prefix: kilo-

Answer 145

k - 10³

Question 146

Prefix: hecto-

Answer 146

h - 10²

Question 147

Prefix: micro-

Answer 147

µ - 10^-6

Question 148

Prefix: nano-

Answer 148

n - 10^-9

Question 149

Prefix: pico-

Answer 149

p - 10^-12