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Chemistry 102 Final Exam (Chp 10 - 17) > Chemistry 102 Final Exam > Flashcards

Chemistry 102 Final Exam Flashcards

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1
Q

Define Intermolecular Forces

A

Forces of ATTRACTION between atoms and substances

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2
Q

Dispersion

A

Type of attraction seen in EVERY substance

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3
Q

Dipole-Dipole

A

Type of attraction seen only in POLAR substances

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4
Q

Hydrogen Bonds

A

Only bond with F.O.N

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5
Q

The strongest intermolecular force is

A

Dipole - Dipole Bonds

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6
Q

Phase Transitions

A

Changing from phases to phases

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7
Q

Phase Transitions (Name and Formula) : Liquid to Gas

A

Vapor to Condensation - ^Hvap

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8
Q

Phase Transitions (Name and Formula) : Solid to Liquid

A

Melting to Boiling - ^Hfus

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9
Q

Phase Transitions (Name and Formula) : Solid to Gas

A

Sublimation to Deposition - ^Hfus + ^Hvap

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10
Q

Endothermic or Exothermic

A 
Exo = Vapor to Condensation
End = Sublimation to Deposition and Melting to Boiling
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11
Q

Triple Point (1) and Critical Point (2)

A

(1) Point where all phases are equal

(2) Highest temperature which substance exist in liquid

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12
Q

Heat during a phase transition

A
  1. Q1 = ms^t
  2. (Grams/Molar Mass) * ^Hvap
  3. Q2 = ms^t
  4. Combine
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13
Q

Clausius-Clapeyron equation

A

Heat and Pressure of Vaporization

ln(P2/P1)= ∆Hvap/R * (1/T1 - 1/T2)

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14
Q

Crystalline structure: Simple Cubic

A

Unit Cell = 8 cn * 1/8 atom = 1 atom

Coordination Number = 6 atoms inside

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15
Q

Crystalline structure: Body-centered Cubic

A

Unit Cell = 8 cn with 1 * 1/8 atoms = 2 atoms

Coordination Number = 8 atoms inside

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16
Q

Crystalline structure: Face-Centered Cubic

A

Unit Cell = 8 cn with 1 * 1/18 and 6 cn * 1/2 = 4

Coordination Number = 12 atoms inside

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17
Q

Electrolytes

A

Substances that dissolves in H20 and goes though a chemical/physical change

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18
Q

IONIC electrolytes

A

Electrolytes that occur when water and polar molecules combine with IONs and go through dissociation

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19
Q

Henry’s law

A

Solubility of a gas in a liquid will always be PROPORTIONAL to the pressure of the gas over the solution

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20
Q

Cg = kPg

A

Formula for Henry’s Law
Cg = Concentration of dissociation
k = Constant
Pg = Pressure of the gas

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21
Q

Molarity

A

mole of SOLUTE / liter of SOLUTION

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22
Q

Molality

A

mole of SOLUTE / mass of SOLVENT

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23
Q

Percent by mass

A

mass of SOLUTE / mass of SOLUTION

solution = solute + solvent

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24
Q

Mole fraction

A

moles of substance A / moles of all substances

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25
Q

Roult’s law

A

The PARTIAL pressure exerted by any component of an IDEAL solution is EQUAL to the pressure of the PURE component MUTLIPLIED by MOLE FRACTION

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26
Q

Roult’s Law Formula

A

Pure(vapor) - Pure(amount) = Mole fraction (solute) * Pure(vapor)

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27
Q

Boiling Point Elevation

A

a. Have to find Change in Tb = Boiling Point of solution - Boling Point of Pure
b. Change Tb = Molality * Boiling Point constant (K)

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28
Q

Freezing Point Depression

A

a. Have to find Change in Tf = Freezing Point of solution - Freezing Point of Pure
b. Change Tf = Molality * Freezing Point constant (K)

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29
Q

Osmotic Pressure Definition

A

The osmotic pressure is the right about pressure enough to preventing osmosis

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30
Q

Osmotic Pressure Formula

A

Osmotic P = the molarity (mol/l) * 0.0821 L/atm * temperature K

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31
Q

Van’t Hoff factor definition

A

True number of particles AFTER dissolved / Formula number INITALLY dissolved

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32
Q

Van’t Boiling Point Formula

A

Tb = iKbm

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33
Q

Van’t Freezing Point Formula

A

Tf = iKfm

34
Q

Van’t Osmotic

A

Osmotic = iMRT

35
Q

“Reaction Rate” definition

A

a. Change in the CONCERTATRATION of a reactant/product with time
b. ALWAYS expressed in M/s

36
Q

Different type of Reaction Rates

A

Average - Reaction PROCCEEDS over time

Instantaneous - Reaction PROCCEDS at a SPECIEC time

Initial - Occurs at START

37
Q

“Rate Law” definition

A

Express the relationship between REACTION RATE to the RATE CONSTANT

38
Q

Rate Law: Order 0

A

Standard Formula: -∆A/∆T=K

Formula to find “A”: [A] =Aln -KT

39
Q

Rate Law: Order 1

A

Formula to find “K” or the rate constant = ln (A0)/ln(A)*(1/T)

Formula to find “A” or final amount = (A0)*e-KT

40
Q

Rate Law: Order 2

A

Standard Formula :

-∆A/∆T=KA2

41
Q

Activation Energy

A

The minimum energy necessary to form product during a collision between reactants

42
Q

Arrhenius Definition

A

Shows the temperature depending on the rate

43
Q

Arrhenius Formula

A

Standard Formula - K= A* e-EA/R(8.314)*T

Formula to find one K - [ln K] = (-EA/R)*(1/T) + ln A

Formula to find two Ks - ln [K2/K1] = (EA/R) * (1/T1 - 1/T2)

44
Q

In EXO reaction “EA” is

A

Less than EAR (EAR > EA)

45
Q

In END reaction “EA” is

A

More than EAR (EA > EAR)

46
Q

Equilibrium Constant “K” Definition

A

The reaction quotient at the equilibrium

47
Q

Reaction Quotient “Q” Formula

A

Use same as Reaction Formula
K > 1 (to the right) =Favor products
K< 1 (to the left) = Favor reactants

48
Q

Reaction Quotient “Q” Definition

A

The amounts of recants and products present at any point in a reversable reaction

49
Q

Reaction Quotient “Q” Formula

A

C(x)D(y) / A(a)B(b) expressed in MOLARITY (Products / Reactants )

50
Q

Le Chatelier Definition

A

When a chemical system @ equilibrium is disturbed, returns by countering

51
Q

Le Chatelier Add/Remove

A

a. Distributed by ADD = Proceeds to the side that consumes added material
b. Distributed by REMOVE = Proceeds to the side that restores removed material
c. Doesn’t work for pure liquid or solid UNLESS already in the equation

52
Q

Le Chatelier Rules Concertation

A

a. Increase Product = Left shift
b. Decrease Product = Right shift
c. Increase Reactants = Right shift
d. Decrease Reactants = Left shift

53
Q

Le Chatelier Rules Pressure/Volume

A

a. Increase Pressure = Shift to fewest
b. Increase Volume = Shift to most
c. Decrease Pressure = Shift to most
d. Decrease Volume = Shift to fewest

54
Q

Calculate pH

A

-log(OH) or -log(H)

55
Q

pH + pOH = ?

A

ALWAYS equal to 14

56
Q

Kw will always = ?

A

1.0 * 10 to the -14

57
Q

Formula for Kw with OH and H

A

OH + H = Kw (1.0 * 10 to the -14)

To find H = Kw/OH

58
Q

Ka/Kb Formula

A

Reactions/ Products

59
Q

Formula for Kw with Ka and Kb

A

Kw = Ka* Kb

If given Kw - use “Kw/Kb or Ka”

60
Q

Henderson-Hasselbalch equation

A

Used to calculate BUFFER pH

pH = pKa + log (A-/HA)

61
Q

Titration Steps

A

a. Before = The O.G substance/chemical will have Higher concertation
b. Equivalent = The O.G and added will have the SAME concertation
c. After = The O.G will have a LOWER concertation

62
Q

Complex Ion Equilibria

A

Use the formula - K = Ksp * Kf

63
Q

Precipitation Predictions

A

a. Q > K = will precipitate
b. Q < K = unsaturated
c. Q = K = saturated

64
Q

Solubility (gram/liter)

A

Number of GRAMS in solute dissolved in 1 LITER of saturated solution

65
Q

Molar Solubility (mols/liter)

A

Number of MOLES is solute dissolved in 1 LITER of saturated solution

66
Q

Product Solubility Constant (Ksp)

A

The equilibrium between precipitates: A (to power of moles) * B (to power of moles)

67
Q

Complex Ion Equilibria

A

Use the formula - K = Ksp * Kf

68
Q

Entropy

A

Measure of RANDOMNESS of a system

Formula - Change in S = Sf -SI

69
Q

Entropy relations to State

A

Solid < Liquid < Gas

70
Q

Cause Spontaneous Process

A

a. H < 0
b. EXO
c. - G
d. S > 0

71
Q

Formula for Surrounding

A

Surrounding = -H of system / Temperature
Exo = Surr> 0
End = Surr < 0

72
Q

Gibbs Free Energy

A

G = H of system - Tempture * S systems

73
Q

Gibbs Free Energy @ Equilibrium

A

G = -RTlnK
R = 8.314
T = always in K

74
Q

Oxidation verse Reduction

A

a. Oxidation is the one LOSING an e-

b. Reduction is the one GAINING an e-

75
Q

Reducing verse Oxidizing Agent

A

a. Reducing Agent = Oxidation

b. Oxidizing Agent =Reduction

76
Q

Cathode verse Anode

A

a. Cathode = Reduction

b. Anode = Oxidation

77
Q

Cell Notation

A

a. On the left (the 1st chemical) = the anode

b. On the right = the cathode

78
Q

Standard Potential

A

E cell = E cathode - E anode

Always positive in Galvanic cell

79
Q

Standard Potential and Free Energy Formula 1

A

G = - mol * F * Ecell

F = 9.648 *10 to 4

80
Q

Standard Potential and Free Energy Formula 2

A

E cell = (0.0257/mol )*ln K

Chemistry 102 Final Exam (Chp 10 - 17) (1 decks)

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