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Organic Chem > Test 1 Ch. 7-8 > Flashcards

Test 1 Ch. 7-8 Flashcards

1
Q

The study of energy, work, and heat

A

THERMODYNAMICS

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2
Q

molecules and atoms in a reaction mixture are in constant, random motion

A

KINETIC MOLECULAR THEORY

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3
Q

molecules and atoms frequently collide with each other

A

KINETIC MOLECULAR THEORY

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4
Q

Only some collision, those with sufficient energy, will break bonds in molecules.

A

KINETIC MOLECULAR THEORY

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5
Q

When reactants bonds are broken, new bonds are formed and products result

A

KINETIC MOLECULAR THEORY

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6
Q

System vs. surroundings = contains the process under study

A

SYSTEM

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7
Q

System vs. surroundings = the rest of the universe

A

SURROUNDINGS

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8
Q

Energy of the universe is constant

A

FIRST LAW OF THERMODYNAMICS

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9
Q

First law of thermodynamics aka

A

LAW OF CONSERVATION OF ENERGY

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10
Q

The energy required to break the bond is less than the energy released when the bonds are formed

A

EXOTHERMIC REACTION

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11
Q

The energy required to break the bond is greater than the energy released when the bonds are formed

A

ENDOTHERMIC REACTION

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12
Q

/\ H. represents heat energy

A

ENTHALPY

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13
Q

Change in enthalpy will be ____ in Exothermic reactions

A

NEGATIVE

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14
Q

Change in enthalpy will be ____ in Endothermic reactions

A

POSITIVE

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15
Q

Most, but not all, ______ reactions are spontaneous

A

EXOTHERMIC

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16
Q

Most, but not all, ______ reactions are nonspontaneous

A

ENDOTHERMIC

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17
Q

The universe spontaneously tends towards increasing disorder and randomness

A

SECOND LAW OF THERMODYNAMICS

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18
Q

Measure of randomness of a chemical system

A

ENTROPY

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19
Q

Highly disordered system the absence of a regular repeating pattern

A

HIGH ENTROPY

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20
Q

well organized system such as a crystalline structure

A

LOW ENTROPY

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21
Q

/\ G. represents the combined contribution of the enthalpy and entropy values for a chemical reaction

A

FREE ENERGY

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22
Q

negative /\ G

A

ALWAYS SPONTANEOUS

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23
Q

positive /\ G

A

NEVER SPONTANEOUS

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24
Q

/\ G = ….

A

/\ H - [ T (kevlin) * /\ S ]

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25
The measurement of heat energy changes in a reaction
calorimetry
26
Q = Ms * /\ T * SHs what do all values mean
- specific heat (SHs) - change in temp (/\ T) - Mass of the solutions
27
The number of calories of heat needed to raise the temp of 1g of the substance 1c
Q = Ms * /\ T * SHs
28
the study of the rate/speed of chemical reactions
KINETICS
29
the difference between the energy of the reactants and that of the activation complex
ACTIVATION ENERGY (Ea)
30
process that can occur in both direction
REVERSIBLE REACTION
31
the rate of forward process in a reversible reaction is exactly balanced by the rate of the reverse process
DYNAMIC EQUILIBRIUM
32
Keq = aA + bB <--> cC + dD
[C]^c[D]^d --------------- [A]^a [B]^b
33
Keq greater than 1 x 10 ^3
- at equilibrium mostly product present.
34
Keq less than 1 x 10^ -3
- at equilibrium mostly reactants present
35
Keq between 1 x 10^-3 and 1 x 10 ^ 3
- mixture contains sigificant concentration between both reactants and products
36
If a stress is placed on a system at equilibrium, the system will respond by alternating the equilibrium composition in such a way as to minimize the stress
LECHATELIERS PRINCIPLE
37
Increase reactants
SHIFT TO PRODUCTS
38
Increase products
SHIFT TO REACTION
39
Increase pressure
SHIFT TO SIDE WITH LESS MOLES
40
decrease pressure
SHIFT TO SIDE WITH MORE MOLES
41
increase temp in an exothermic reaction
SHIFT TO REACTANTS
42
decrease temp in an exothermic reaction
SHIFT TO PRODUCTS
43
molecular collision, activation energy, molecular orientation
COLLISION THEORY
44
Bronsted Lower Acid
Proton H+ Donator
45
Bronsted Lowery Base
Proton H+ Acceptor
46
a substance, when dissolved in water dissociated to produce hydrogen ions
Arrhenius Acid
47
a substance, when dissolved in H20, dissociates to produce Hydroxide ions
Arrhenius Base
48
A substance poessing both acid and base properties
Amphiprotic
49
When NH3 dissolves in water it has ___ properties, however it does not have ____ ions in it
BASIC, OH-
50
6 strong acids (NEED TO KNOW IN THIS CLASS) and charge
HCL HBr HI HNO3 +1 H2SO4 HClO4 +3
51
2 weak acids (NEED TO KNOW IN THIS CLASS)
CH3COOH H2CO3
52
acetic acid
CH3COOH
53
Carbonic acid
H2CO3
54
3 Strong bases
NaOH KOH Ba(OH)2
55
3 Weak bases
NH3 C5H5NH2 C6H5NH2
56
Nitric Acid
HNO3
57
Sulfuric Acid
H2SO4
58
HCLO4
Perchloric Acid
59
only a small percent dissociates
Weak acid/bases
60
Calculating the pH of a buffer solution
pH = pKa + log ( Cb / Acid )
61
pKa =
-log(Ka)
62
- gain of electrons - gain of H2 - loss of O2
REDUCTION
63
High pKa
Low ACID STRENGTH
64
Low pKa
High ACID STRENGTH
65
electrochemical cell that converts stored chemical energy
VOLTAIC CELLS
66
Mg -> Mg 2+ + 2e-
OXIDATION HALF REACTION
67
Cl + 2e- --> 2Cl
REDUCTION HALF REACTION
68
uses electrical energy to cause non-spontaneous oxidation-reduction reactions to occur
ELECTROLYSIS
69
Fill in the blank question. The spontaneity of a chemical reaction depends on the relative magnitude of the __ and ____ values
ENTHALPY, ENTROPY
70
Decomposition of a liquid to form gaseous molecules ____ in entropy
INCREASE
71
Separation of a gaseous mixture into individual components ___ in entropy
DECREASE
72
Vaporization --> ___ in entropy
INCREASE
73
Condensation --> ___ in entropy
DECREASE
74
/\ S > 0
process moves to a state of increased disorder
75
T or F: gases have a higher entropy than solids
TRUE
76
Products have a higher potential energy than reactants
ENDOTHERMIC
77
Chemical kinetics is the study of the _____ of chemical reactions and gives an indication of the _____ of a reaction.
RATE ; MECHANISM

Organic Chem (4 decks)

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