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MCAT > Physics and Chem II (SIMPLE EDITOR) > Flashcards

Physics and Chem II (SIMPLE EDITOR) Flashcards

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1
Q

When calculating the density of a volatile liquid, must take what into account

A

some will evaporate – so will lose mass

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2
Q

Mass % of a solute * Density =

A

(Mass Solute/Mass Soln)*(Mass Soln/Vol Soln) = Mass Solute/Vol Soln

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3
Q

How to convert from grams or moles of a gas to get to liters of an ideal gas at STP?

A

22.4 Liters of gas / 1 mol gas(so would need to convert grams of gas to mols first if given grams)

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4
Q

Molecular Formula vs Empirical Formula

A

Molecular Formula is the actual mole ratio of the elements within the compound.Empirical Formula uses the smallest whole number ratio of the atoms in each compound.

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5
Q

How to calculate empirical formula

A

Assume 100–gram sample so the percentages can easily be changed into mass figuresthen convert mass into moles (using atomic masses of each element)the empirical formula is then the whole number ratio of these mol values

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6
Q

How to convert between molecular and empirical formulas

A

Multiply the empirical formula by the whole number ratio of the molecular mass to the empirical mass

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7
Q

What is a combustion reaction?

A

Hydrocarbon + Excess Oxygen ––––combusted–––> Carbon Dioxide + Water VaporCxHy + O2 –––> CO2 + H2O(Hydrocarbon is oxidized)

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8
Q

Molality (m)

A

Moles Solute / Mass Solvent (kg)

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9
Q

Which of the following are affected by temperature changes?MolarityMolalityMass Percent”

A

Molarity = IS affectedMolality = IS NOT affectedMass Percent = IS NOT affected

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10
Q

Mass Percent (in soln)

A

Mass Solute / Mass Solution *100%

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11
Q

Trick for calculating dilution

A

Recognize that total moles of a solute remain constant when a solvent is added, so M*V remains constant:MiVi = MfVf

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12
Q

What is a simple dilution?

A

Addition of pure solvent

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13
Q

What is Beer’s Law?–idea behind it–equation for it–trick for solving problems

A

States that you can pass electromagnetic radiation through a solution and the solution may absorb some of the light – the light absorbed will be a specific wavelength range and the absorbance intensity will vary directly with the concentration of the solute:

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14
Q

What is Beer’s Law?–equation for it

A

Abs = εClwhere ε = a constant for the soln at λmax C = [solute] l = width of cuvette (length of pathway through which light passes)

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15
Q

What is Beer’s Law?–trick for solving problems

A

Absi * Vi = Absf*Vf

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16
Q

the limiting reagent is the reactant with _______________

A

the lowest ratio of actual moles to needed moles

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17
Q

What are the solubility rules?

A

(1) Most salts containing alkali metal cations (Li+, Na+, K+, Cs+, Rb+) and Ammonium (NH4+) are water soluble(2) Most nitrate (NO3–) salts are water–soluble(3) Most salts containing halide ions (Cl–, Br–, I–) are water–soluble (except with heave metals such as Ag+ and Pb2+)(4) Most salts containing Sulfate anions (SO42–) are water–soluble(5) Most hydroxide anion (OH–) salts are only slightly water–soluble. (KOH ad NaOH are substantially soluble, while Ca(OH)2, Sr(OH)2, and Ba(OH)2 are fairly soluble)(6) Most carbonate anion (CO32–), chromate anion (CrO42–), phosphate anion (PO43–), and sulfide anions (S2–) salts are only slightly water–soluble

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18
Q

CaCO3 is a(n) ____________

A

BASE

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19
Q

In composition reactions, what is happening (and how is entropy affected)

A

Reactants combining to form a product:More bonds formed, so entropy decreases

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20
Q

In decomposition reactions,what is happening (and how is entropy affected)

A

Reactants decompose to form multiple products:More bonds broken = entropy increases

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21
Q

Which atom (or compound) is the reducing agent (reductant) and which is the oxidizing agent (oxidant)

A

Atoms losing electrons = reducing agent (reductant)Atoms gaining electrons = oxidizing agent (oxidant)

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22
Q

Loss of Electrons in a reaction = a(n) _______Gain of Electrons in a reaction = a(n) ______

A

Loss of Electrons = OxidationGain of Electrons = ReductionLEO the lion goes GER

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23
Q

In combustion reaction, oxygen serves as the _______

A

oxidizing agent

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24
Q

Oxidation state of an atom an be determined by ________

A

looking at bonds it forms with less electronegative atoms (gives it a –1 for every bond) and bonds it forms with more electronegative atoms (gives it a +1 for every bond)

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25
Q

general rules for assigning oxidation states

A

O = –2 (except in molecular oxygen and peroxides)H = +2 (except in molecular hydrogen and hydrides)Halides = –1 (except when they are a central atom in an oxyacid)

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26
Q

1/5

A

0.2

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27
Q

1/6

A

0.1166

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28
Q

1/7

A

0.143

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29
Q

1/8

A

0.125

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30
Q

1/9

A

0.111

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31
Q

1/11

A

0.091

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32
Q

1/12

A

0.083

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33
Q

conduction vs convection

A

conduction = transfer of heat through direct contactconvection = transfer of heat through a liquid or gas medium

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34
Q

sublimation

A

solid –––––> gas

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35
Q

giga =

A

10^9

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36
Q

mega =

A

10^6

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37
Q

deci =

A

10^ –1

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38
Q

centi =

A

10^ –2

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39
Q

milli =

A

10^ –3

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40
Q

micron =

A

1 micron = 10^ –6 meters

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41
Q

Angstrom =

A

1 Angstrom = 10^ –10 meters

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42
Q

pico =

A

10^ –12

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43
Q

fempto =

A

10^ –12

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44
Q

calorie to joule conversion

A

1 calorie = 4.18 Joules

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45
Q

kilogram to pound conversion

A

1 kg = 2.2 pounds (on earth)

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46
Q

liter to meter conversion

A

1000 liters = 1 cubic meter

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47
Q

Mile to meter conversion

A

1 mile = roughly 1600 meters

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48
Q

foot to meter conversion

A

1 meter is a little over 3 feet

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49
Q

inch to cm conversion

A

1 inch = roughly 2.5 cm

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50
Q

Important Trig function to remember

A

cos^2(theta) + sin^2(theta) = 1

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51
Q

cos 0 =

A

1

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52
Q

cos 30 =

A

sqrt(3) / 2 = 0.86

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53
Q

cos 45 =

A

sqrt(2) / 2=0.71

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54
Q

cos 60 =

A

1/2 =0.50

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55
Q

cos 90 =

A

0

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56
Q

sin0 =

A

0

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57
Q

sin 30 =

A

1/2=0.50

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58
Q

sin 45 =

A

sqrt(2) / 2=0.71

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59
Q

sin 60 =

A

sqrt(3) / 2=0.86

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60
Q

sin 90 =

A

1

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61
Q

tan =

A

sin/cos=opp/adj

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62
Q

What is the kinematic equation to use when:you don’t have Vfinal?(assume all are in x direction)

A

Δx = viΔt + 1/2 a(Δt)^2

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63
Q

What is the kinematic equation to use when: you don’t have dx(displacement of x)? (assume all are in x direction)

A

vf = vi + a(Δt)

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64
Q

What is the kinematic equation to use when: you don’t have a? (assume all are in x direction)

A

Δx = (1/2)(vi + vf)Δt

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65
Q

What is the kinematic equation to use when: you don’t have t? (assume all are in x direction)

A

(vf)^2 =(vi)^2 + 2aΔx

66
Q

Without air resistance, a ball will fall _____ meters in 1 second, _____ meters in 2 seconds, and so forth (_______)

A

Will fall 5 meters in 1 second and 20 meters in 2 seconds (and 80 meters in 4 seconds) Δy = 5t^2*assuming starts with zero velocity

67
Q

Estimate (disregarding air resistance) the velocity of a ball falling after 1 second, 2 seconds, etc.

A

Velocity = 10Δt*assuming starts with zero velocityso after 1 second, v = 10 m/s2 seconds, v = 20 m/s3 seconds, v = 30 m/sand so on

68
Q

Calculate how much time (disregarding air resistance) it will take a ball to reach the top given an initial velocity

A

Δt = vi / 10

69
Q

Throwing a projectile: Calculate the height the projectile travels

A

h = (viy)^2 / 10or (viy)^2 /g

70
Q

Throwing a projectile: Calculate the time it takes the projectile to reach the top

A

t = viy / 10or t = viy / g

71
Q

Calculate the range of a projectile

A

r = 2voxvoy / gr = (vo)^2 sin2Θ / g

72
Q

When does a projectile have maximum range? What is the formula for its range in that case?

A

when Θ = 45 degreesr = (vo)^2 sin(90) / g = (vo)^2 / g

73
Q

What is the relationship between r and f at given thetas (from the horizontal):30 degrees45 degrees60 degrees”

A

30 degrees:r/h = 6.745 degrees:r/h = 460 degrees:r/h = 2.4

74
Q

Static friction vs kinetic friction

A 
Static = when there is no sliding (keeps object at rest; also can accelerate an object from rest)
Kinetic = when there is sliding (slows object down)
75
Q

Calculating Torque

A

T = rFsin(theta)
or
T = rF(perpendicular)

76
Q

Calculating mechanical advantage of a system

A

= Weight of object / Applied force needed to support object

77
Q

What is the Normal force of an object on an inclined plane (with horizontal angle theta)

A

F = mgscos(theta)

78
Q

What is the acceleration of an object down an inclined plane (With horizontal angle theta, and no friction)

A

a = gsin(theta)

79
Q

Relate distance traveled to acceleration and time

A

x = vit + (1/2)a*(t^2)

80
Q

An object is moving in a circle at a constant speed, what is the net Force experienced by the object?

A

Towards the center of the circle

81
Q

An object turns without changing speed, what is the net force applied to the object?

A

Net force is perpendicular to the object’s motion

82
Q

Calculate the Static Friction Force

A

F(max static friction) = (mu)N

  • Where mu = the static friction coefficient
  • N = Normal Force on an inclined plane = mgcos(theta)
83
Q

Calculate Force of a Spring

A

F = kx

  • where k is the spring constant (N/m)
  • x is the displacement of the string
84
Q

How does static friction relate to an applied force?

A

It is a REACTIONARY force –> so it is equal and opposite to applied force

85
Q

Calculate mechanical advantage for a pulley system

-Use mechanical advantage to determine the amount of force needed to lift an object (with Weight W Newtons)

A

MA = (# pulleys)*(sin(theta))

Force needed = W / MA

86
Q

Coloumb’s Law:

A

Relates the magnitude of force to the distance between two charges:

F = kq(1)q(2) / (r^2)
*so, if you triple the distance, the strength of the electric field is 1/9th

**can modify for the strength of an electric field around a point charge: E = kq / (r^2)

87
Q

Units for electric field strength

A

N/C —or—- V/m

88
Q

Calculate change in voltage given for a point charge that moved in an electric field

A

Delta(V) = E * d(parallel or antiparallel)

*where E = electric field strength (N/m) and d(parallel or antiparallel) = distance traveled that is parallel or antiparallel to the electric field

89
Q

When will a point charge experience a voltage change in an electric field?

A

Only when moving parallel or antiparallel to the electric field

90
Q

Calculate the work done by an electric field on a point charge

A

W = delta(V) * q

Where delta(V) = the change in voltage and q = charge on the point charge

91
Q

An electric field points towards _____ charge.

So a positive charge will move in the same/opposite direction of the electric field lines?

A

Points towards NEGATIVE.
___________
Positive charge will more SAME direction as the electric field (e.g., in the direction of +E; the same direction the electric field lines point)

92
Q

Calculate the Force on a point charge in an electric field

A

F = Eq

*where E = Electric Field, and q = charge on the point charge

93
Q

Calculate the energy of a photon

A

E = hf = hc/(lamda)

*where lamda = the wavelength of the photon

94
Q

sp hybridization = what geometry and bond angle

A

linear; 180 degrees

95
Q

sp2 hybridization = what geometry and bond angle

– and what possible molecular shapes given the # of lone pairs

A

trigonal planar; 120 degrees

  • -shapes:
  • 0 lone pairs = trigonal planar
  • 1 lone pair = bent
96
Q

sp3 hybridization = what geometry and bond angle

– and what possible molecular shapes given the # of lone pairs

A

tetrahedral; 109.5 degrees

  • -shapes:
  • 0 lone pairs = tetrahedral
  • 1 lone pair = trigonal pyramidal
  • 2 lone pairs = bent
97
Q

sp3d hybridization = what geometry and bond angle

– and what possible molecular shapes given the # of lone pairs

A

trigonal bipyramidal; 90 degrees, 120 degrees, and 180 degrees

  • -shapes:
  • 0 lone pairs = trigonal bipyramidal
  • 1 lone pair = trigonal-based pyramid
  • 2 lone pairs = trigonal planar or T-shaped
98
Q

sp3d2 hybridization = what geometry and bond angle

– and what possible molecular shapes given the # of lone pairs

A

octahedral; 90 degrees

  • -shapes:
  • 0 lone pair = octahedral
  • 1 lone pair =square-based pyramid
  • 2 lone pairs = square planar
99
Q

Rate the following from LONGEST wavelength to SHORTEST wavelength:

  • AM/FM/TV waves
  • Infrared
  • Gamma Rays
  • Microwaves
  • Ultraviolet
  • Visible - Red
  • Visible - Purple
  • X-Rays
A

(1) AM/FM/TV waves
(2) Microwaves*
(3) Infrared*
(4a) Visible - Red
(4b) Visible - Purple
(5) Ultraviolet*
(6) X-Rays*
(7) Gamma Rays*

*note - some may have overlapping wavelengths

100
Q

Calculate Work done given Force and displacement

A

Work = displacement * Force(parallel-to-displacement)

101
Q

Calculate Zeff

A

Zeff = Z - S

Where Z = Atomic # and S = # of electrons NOT in valence shell

102
Q

2 major components affecting periodic trends

A

(1) Zeff = increases going left to right. The net charge exerted on valence electrons. takes into account -proton attraction, -interaction with neutrons, and -repulsion (shielding) due to core electrons. Zeff = proton charge - core electron repulsion
(2) Valence Shell: increases going from top to bottom

103
Q

the 4 major periodic trends to be aware of

A

As move bottom left to top right:

(1) Atomic size decreases
(2) ionization energy (energy required to remove outermost electron from atom in gas phase) increases
(3) Electron affinity increases
(4) Electronegativity increases

104
Q

ionization energy vs. electron affinity vs. electronegativity

A

Ionization energy = energy required to remove outermost electron from atom in gas phase. Becomes a cation
____
Electron Affinity = energy associated with an atom gaining an electron in its gas phase
____
Electronegativity = tendency to hold shared electrons with another atom within a bond

105
Q

Major periodic trend - rule that is broken

A

1/2 fulled and fulled subshells have special stability

N ionization energy is greater than O b/c N loses its 1/2 filled subshell and O gains a 1/2 filled subshell

106
Q

Radius within a period: compare neutral atoms with cations and anions

A

Cations < neutral atoms < anions

because losing electrons means less repulsion, and gaining electrons means more repulsion

107
Q

Radius trends in periods and groups

A
  • radius decreases left to right b/c Zeff increases

- radius increases top to bottom b/c # of electron shells increase

108
Q

Radii of transition metals: trend in a row

A

have ~the same radii in the same row

109
Q

major periodic trend - rule that is broken about radii size

A

He > H (likely due to shielding)

110
Q

Low ionization energy —- what that means for reduction and oxidation potential

A

Smaller value for reduction potential and larger value for oxidation potential (b/c easier to oxidize)

111
Q

Negative vs positive values for electron affinity

A

more negative = greater electron affinity (b/c means more energy is released, which is favorable)

112
Q

Most and least EN elements

A

Most = F (4.0); Least = Na (0.9)

113
Q

EN and ionic bonds

A

if delta(EN) > 2.0, the bond is ionic

114
Q

Reactivity of alkali metals and alkali earth metals as go down the period

A

increase as you go down, b/c ionization energy is decreasing (also, alkali metals are more reactive than alkaline earth metals)

115
Q

defining feature of strong reducing agents

A

readily lose electrons

116
Q

Reactivity of chalcogens and halogens as go down the period

A

reactivity decreases as go down b/c 1st and 2nd electron affinities decrease

117
Q

spring potential energy

A

PE(spring) = (1/2) k*(x^2)

118
Q

how to calculate the amount of energy lost to heat

A

Q= mc∆t

119
Q

Power =

A

work / time

J/s = Watts

120
Q

Calculate the mechanical advantage of an inclined plane

A

ME = 1 / sin(theta)

121
Q

Calculate the mechanical advantage of a pulley system

A

ME = W / T
___
where W = the weight of the mass and T = the tension

122
Q

Work done on a system in terms of force, displacement, pressure, and volume

A

W = F∆T = -P∆V

123
Q

Total energy change in terms of Pressure, Volume, Heat, Force, displacement, and work

A

∆E = q - Work = q - F∆d = q + P∆V

124
Q

what does positive Q vs. negative Q mean

A

+Q = heat flows from surroundings to system
____
-Q = heat flows from system to surroundings

125
Q

What does positive Work vs negative Work mean

A 
\+W = work done on system by surroundings
-W = work done on surroundings by system
126
Q

Compare: refrigerator to an engine in terms of work and heat

A

Fridge: takes in work (applied to a piston) and releases heat vs.
Engine: releases work (expands gas in a piston) and takes in heat

127
Q

Calculate Impulse

A

Impulse = F(average)*t = m∆v

128
Q

What type of reactions generate the greatest changes in free energy and enthalpy

A

Oxidation-reduction reactions

129
Q

anode vs. cathode and direction of electron flow

A

Anode = Reducing agent
Cathode = Oxidizing Agent
E- flow from anode to cathode

130
Q

Oxidation and reduction in orgo/biochem

A

Oxidation = often the gain of bonds to oxygen and/or the loss of bonds to hydrogen
___
Reduction = often the loss of bonds to oxygen and/or the gain of bonds to hydrogen

131
Q

Biological Oxidizing agents vs. biological reducing agents

A

Oxidizing = usually rich in Oxygen and poor in Hydrogen
___
Reducing = usually poor in Oxygen and rich in hydrogen

132
Q

NADH generally reduces what? And FADH2 generally reduces what?

A

NADH => carbonyls

FADH2 => alkene double bonds

133
Q

How to calculate electromotive force given two reduction potentials

A

E = E(reduction) + E(oxidation)

-Use E(reduction) of the 1/2 rxn with the HIGHER reduction potential (more positive)
-For E(oxidation), use the 1/2 rxn with the LOWER (or more negative) reduction potential - to find the E(oxidation), just take the negative of its E(red)
____
(Ered = reduction potential of the 1/2 rxns)

134
Q

Higher Reduction potential means what?

A

It can be reduced (Gain electrons) more favorably, meaning it is a stronger oxidizing agent

135
Q

Periodic trends - what is easily oxidized and what isn’t

A 
Easily oxidized (lose e-) = alkali and alkali earth etals (to form + or 2+ cations)
_
Don't easily oxidize = precious metals
136
Q

Calculate the free energy change associated with an EMF

A

∆Grxn = -nFE(cell)

F = 96500 C/mol
n = #electrons/reaction
137
Q

Unit for Work

A

J = N/m

138
Q

Universal rules for Electrical Circuits

A

(1) e- flow anode->cathode

(2) cations migrate through electric fields to the cathode, and anions migrate through electric fields to thhe anion

139
Q

Why do you need salt bridges in an electrochemical cell?

A

They complete the cycle: allow anions to flow to anode to balance out charge distributions from e- flowing to the cathode

140
Q

Types of Electrochemical Cells, and how they differ

A

(1) Galvanic = Spontaneous (Ecell > 0) –> release energy in form of e- flow
(2) Electrolytic = Non-spontaneous (Ecell <0) –> used for storage of electrical potential

141
Q

How to maximize voltage in a galvanic cell (and what happens over time)

A

increase reactants (cathode ions) and decrease products (anode ions).

Over time, reactants are converted to products until reach equilibrium and reaction stops and gives off no more energy.

142
Q

At what conditions are Standard EMFs given at

A

25 degrees celsius, 1 atm, and 1.00m

143
Q

What is a concentration cell

A

Anode and cathode contain same species but at different concentrations

144
Q

Nernst Equation

A

E(cell) = E* - 2.3RT/nF * logQ
or, at 298K: E(cell) = E* - 0.059/n*logQ

Where Q = [anode]/[cathode]
(where E* = E not)

145
Q

What is a battery and what does it do?

A

A galvanic cell (or group of galvanic cells in series)

  • they convert electrical potential energy into direct currents,
  • by using a reversible oxidation-reduction reaction. they can act as either a galvanic cell OR an electrolytic cell
146
Q

how does a fluorescent tube work

A

(1) 2 plates create a potential ∆
(2) Gas ions accelerate towards oppositely charged plates until collide with another gas particle
(3) some KE is absorbed by the other particle which absorbs energy by exciting an electron
(4) When excited e- relaxes back to ground state, a photon is emitted. –> the tube is coated with a fluorescing agent to convert UV radiation into visible light.

147
Q

How do incandescent light bulbs work

A

They convert electrical flow into light by passing current through a resistor and a vacuum (vacuum prevents energy from being dissapated within)
–> thermal energy builds up and is released via EM radiation (causing glowing)

148
Q

How do electrical motors work

A

an electric flow (current flowing through a loop) induces a magnetic field —> by allowing the induced filed to interact with an external stationary magnetic field, a torque can be exerted on the loop. —> loop realigns with stationary field —> causes induced field to revers —> causing more torque —> and repeat

149
Q

What is electroplating

A

The process of reducing ions in solution onto the surface of a conducting material —> happens at the cathode, so cathode gains a thin film of the reduced metal on its surface

150
Q

what does it mean to galvanize a metal? And why is it done

A
  • add a more reactive metal to be preferentially oxidized over the metal being preserved —> so using a metal with a higher oxidation potential.
  • It’s done b/c metals exposed to the environment will oxidize over time, so this preserves the metal
151
Q

Formula for phosphate ion

A

PO4 (3-)

152
Q

Rusting is an example of _____ (oxidation or reduction)?

A

OXIDATION

153
Q

Aziuthal quantum number

A

determines its orbital angular momentum & describes the shape of the orbital

154
Q

farsightedness = the image forms ______ and so you need a ____ lens

A

The image forms behind the retina, so you need a converging lens

155
Q

longitudinal vs. transverse waves

A 
longitudinal = direction of wave vibration is parallel to propagation (collisions btwn neighborhing particles); 
transverse = direction of wave vibration is Perpendicular to wave propagation
156
Q

sound is what type of wave

A

longitudinal

157
Q

IR frequency of C=O bond

A

1650 - 1750 cm-1

158
Q

IR frequency of O-H bond

A

2500 - 3300 cm-1

159
Q

IR frequency of Alkane (C triple bond C)

A

2100-2260 cm-1

160
Q

IR frequency of C-O bond

A

1000 - 1320 cm-1

161
Q

What is the fingerprint region

A

IR spectrum that lies in between that of functional groups (1500 to 4000 cm-1) and Aromatic rings (under ~500 cm-1) —> so, roughly 500 - 1500 cm-1; signals here are unique to each particular molecule

MCAT (14 decks)

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