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

Chemistry 102 Final Exam Flashcards

(80 cards)

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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
Roult’s law
The PARTIAL pressure exerted by any component of an IDEAL solution is EQUAL to the pressure of the PURE component MUTLIPLIED by MOLE FRACTION
26
Roult’s Law Formula
Pure(vapor) - Pure(amount) = Mole fraction (solute) * Pure(vapor)
27
Boiling Point Elevation
a. Have to find Change in Tb = Boiling Point of solution - Boling Point of Pure b. Change Tb = Molality * Boiling Point constant (K)
28
Freezing Point Depression
a. Have to find Change in Tf = Freezing Point of solution - Freezing Point of Pure b. Change Tf = Molality * Freezing Point constant (K)
29
Osmotic Pressure Definition
The osmotic pressure is the right about pressure enough to preventing osmosis
30
Osmotic Pressure Formula
Osmotic P = the molarity (mol/l) * 0.0821 L/atm * temperature K
31
Van’t Hoff factor definition
True number of particles AFTER dissolved / Formula number INITALLY dissolved
32
Van’t Boiling Point Formula
Tb = i*Kb*m
33
Van’t Freezing Point Formula
Tf = i*Kf*m
34
Van’t Osmotic
Osmotic = iMRT
35
“Reaction Rate” definition
a. Change in the CONCERTATRATION of a reactant/product with time b. ALWAYS expressed in M/s
36
Different type of Reaction Rates
Average - Reaction PROCCEEDS over time Instantaneous - Reaction PROCCEDS at a SPECIEC time Initial - Occurs at START
37
“Rate Law” definition
Express the relationship between REACTION RATE to the RATE CONSTANT
38
Rate Law: Order 0
Standard Formula: -∆A/∆T=K Formula to find “A”: [A] =Aln -KT
39
Rate Law: Order 1
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
Rate Law: Order 2
Standard Formula : | -∆A/∆T=KA2
41
Activation Energy
The minimum energy necessary to form product during a collision between reactants
42
Arrhenius Definition
Shows the temperature depending on the rate
43
Arrhenius Formula
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
In EXO reaction “EA” is
Less than EAR (EAR > EA)
45
In END reaction “EA” is
More than EAR (EA > EAR)
46
Equilibrium Constant “K” Definition
The reaction quotient at the equilibrium
47
Reaction Quotient “Q” Formula
Use same as Reaction Formula K > 1 (to the right) =Favor products K< 1 (to the left) = Favor reactants
48
Reaction Quotient “Q” Definition
The amounts of recants and products present at any point in a reversable reaction
49
Reaction Quotient “Q” Formula
C(x)*D(y) / A(a)*B(b) expressed in MOLARITY (Products / Reactants )
50
Le Chatelier Definition
When a chemical system @ equilibrium is disturbed, returns by countering
51
Le Chatelier Add/Remove
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
Le Chatelier Rules Concertation
a. Increase Product = Left shift b. Decrease Product = Right shift c. Increase Reactants = Right shift d. Decrease Reactants = Left shift
53
Le Chatelier Rules Pressure/Volume
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
Calculate pH
-log(OH) or -log(H)
55
pH + pOH = ?
ALWAYS equal to 14
56
Kw will always = ?
1.0 * 10 to the -14
57
Formula for Kw with OH and H
OH + H = Kw (1.0 * 10 to the -14) | To find H = Kw/OH
58
Ka/Kb Formula
Reactions/ Products
59
Formula for Kw with Ka and Kb
Kw = Ka* Kb | If given Kw - use “Kw/Kb or Ka”
60
Henderson-Hasselbalch equation
Used to calculate BUFFER pH | pH = pKa + log (A-/HA)
61
Titration Steps
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
Complex Ion Equilibria
Use the formula - K = Ksp * Kf
63
Precipitation Predictions
a. Q > K = will precipitate b. Q < K = unsaturated c. Q = K = saturated
64
Solubility (gram/liter)
Number of GRAMS in solute dissolved in 1 LITER of saturated solution
65
Molar Solubility (mols/liter)
Number of MOLES is solute dissolved in 1 LITER of saturated solution
66
Product Solubility Constant (Ksp)
The equilibrium between precipitates: A (to power of moles) * B (to power of moles)
67
Complex Ion Equilibria
Use the formula - K = Ksp * Kf
68
Entropy
Measure of RANDOMNESS of a system | Formula - Change in S = Sf -SI
69
Entropy relations to State
Solid < Liquid < Gas
70
Cause Spontaneous Process
a. H < 0 b. EXO c. - G d. S > 0
71
Formula for Surrounding
Surrounding = -H of system / Temperature Exo = Surr> 0 End = Surr < 0
72
Gibbs Free Energy
G = H of system - Tempture * S systems
73
Gibbs Free Energy @ Equilibrium
G = -RTlnK R = 8.314 T = always in K
74
Oxidation verse Reduction
a. Oxidation is the one LOSING an e- | b. Reduction is the one GAINING an e-
75
Reducing verse Oxidizing Agent
a. Reducing Agent = Oxidation | b. Oxidizing Agent =Reduction
76
Cathode verse Anode
a. Cathode = Reduction | b. Anode = Oxidation
77
Cell Notation
a. On the left (the 1st chemical) = the anode | b. On the right = the cathode
78
Standard Potential
E cell = E cathode - E anode | Always positive in Galvanic cell
79
Standard Potential and Free Energy Formula 1
G = - mol * F * Ecell | F = 9.648 *10 to 4
80
Standard Potential and Free Energy Formula 2
E cell = (0.0257/mol )*ln K

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

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