Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

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

Test 1 Ch. 7-8 Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

The study of energy, work, and heat

A

THERMODYNAMICS

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

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

A

KINETIC MOLECULAR THEORY

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

molecules and atoms frequently collide with each other

A

KINETIC MOLECULAR THEORY

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

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

A

KINETIC MOLECULAR THEORY

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

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

A

KINETIC MOLECULAR THEORY

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

System vs. surroundings = contains the process under study

A

SYSTEM

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

System vs. surroundings = the rest of the universe

A

SURROUNDINGS

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Energy of the universe is constant

A

FIRST LAW OF THERMODYNAMICS

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

First law of thermodynamics aka

A

LAW OF CONSERVATION OF ENERGY

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

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

A

EXOTHERMIC REACTION

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

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

A

ENDOTHERMIC REACTION

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

/\ H. represents heat energy

A

ENTHALPY

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Change in enthalpy will be ____ in Exothermic reactions

A

NEGATIVE

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Change in enthalpy will be ____ in Endothermic reactions

A

POSITIVE

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Most, but not all, ______ reactions are spontaneous

A

EXOTHERMIC

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Most, but not all, ______ reactions are nonspontaneous

A

ENDOTHERMIC

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

The universe spontaneously tends towards increasing disorder and randomness

A

SECOND LAW OF THERMODYNAMICS

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Measure of randomness of a chemical system

A

ENTROPY

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Highly disordered system the absence of a regular repeating pattern

A

HIGH ENTROPY

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

well organized system such as a crystalline structure

A

LOW ENTROPY

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

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

A

FREE ENERGY

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

negative /\ G

A

ALWAYS SPONTANEOUS

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

positive /\ G

A

NEVER SPONTANEOUS

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

/\ G = ….

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

The measurement of heat energy changes in a reaction

A

calorimetry

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

Q = Ms * /\ T * SHs
what do all values mean

A
  • specific heat (SHs)
  • change in temp (/\ T)
  • Mass of the solutions
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

The number of calories of heat needed to raise the temp of 1g of the substance 1c

A

Q = Ms * /\ T * SHs

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

the study of the rate/speed of chemical reactions

A

KINETICS

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

the difference between the energy of the reactants and that of the activation complex

A

ACTIVATION ENERGY (Ea)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

process that can occur in both direction

A

REVERSIBLE REACTION

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

the rate of forward process in a reversible reaction is exactly balanced by the rate of the reverse process

A

DYNAMIC EQUILIBRIUM

32
Q

Keq = aA + bB <–> cC + dD

A

[A]^a [B]^b

33
Q

Keq greater than 1 x 10 ^3

A
  • at equilibrium mostly product present.
34
Q

Keq less than 1 x 10^ -3

A
  • at equilibrium mostly reactants present
35
Q

Keq between 1 x 10^-3 and 1 x 10 ^ 3

A
  • mixture contains sigificant concentration between both reactants and products
36
Q

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

A

LECHATELIERS PRINCIPLE

37
Q

Increase reactants

A

SHIFT TO PRODUCTS

38
Q

Increase products

A

SHIFT TO REACTION

39
Q

Increase pressure

A

SHIFT TO SIDE WITH LESS MOLES

40
Q

decrease pressure

A

SHIFT TO SIDE WITH MORE MOLES

41
Q

increase temp in an exothermic reaction

A

SHIFT TO REACTANTS

42
Q

decrease temp in an exothermic reaction

A

SHIFT TO PRODUCTS

43
Q

molecular collision, activation energy, molecular orientation

A

COLLISION THEORY

44
Q

Bronsted Lower Acid

A

Proton H+ Donator

45
Q

Bronsted Lowery Base

A

Proton H+ Acceptor

46
Q

a substance, when dissolved in water dissociated to produce hydrogen ions

A

Arrhenius Acid

47
Q

a substance, when dissolved in H20, dissociates to produce Hydroxide ions

A

Arrhenius Base

48
Q

A substance poessing both acid and base properties

A

Amphiprotic

49
Q

When NH3 dissolves in water it has ___ properties, however it does not have ____ ions in it

A

BASIC, OH-

50
Q

6 strong acids (NEED TO KNOW IN THIS CLASS) and charge

A

HCL
HBr
HI
HNO3 +1
H2SO4
HClO4 +3

51
Q

2 weak acids (NEED TO KNOW IN THIS CLASS)

A

CH3COOH
H2CO3

52
Q

acetic acid

A

CH3COOH

53
Q

Carbonic acid

A

H2CO3

54
Q

3 Strong bases

A

NaOH
KOH
Ba(OH)2

55
Q

3 Weak bases

A

NH3
C5H5NH2
C6H5NH2

56
Q

Nitric Acid

A

HNO3

57
Q

Sulfuric Acid

A

H2SO4

58
Q

HCLO4

A

Perchloric Acid

59
Q

only a small percent dissociates

A

Weak acid/bases

60
Q

Calculating the pH of a buffer solution

A

pH = pKa + log ( Cb / Acid )

61
Q

pKa =

A

-log(Ka)

62
Q
  • gain of electrons
  • gain of H2
  • loss of O2
A

REDUCTION

63
Q

High pKa

A

Low ACID STRENGTH

64
Q

Low pKa

A

High ACID STRENGTH

65
Q

electrochemical cell that converts stored chemical energy

A

VOLTAIC CELLS

66
Q

Mg -> Mg 2+ + 2e-

A

OXIDATION HALF REACTION

67
Q

Cl + 2e- –> 2Cl

A

REDUCTION HALF REACTION

68
Q

uses electrical energy to cause non-spontaneous oxidation-reduction reactions to occur

A

ELECTROLYSIS

69
Q

Fill in the blank question.
The spontaneity of a chemical reaction depends on the relative magnitude of the __ and ____ values

A

ENTHALPY, ENTROPY

70
Q

Decomposition of a liquid to form gaseous molecules ____ in entropy

A

INCREASE

71
Q

Separation of a gaseous mixture into individual components ___ in entropy

A

DECREASE

72
Q

Vaporization –> ___ in entropy

A

INCREASE

73
Q

Condensation –> ___ in entropy

A

DECREASE

74
Q

/\ S > 0

A

process moves to a state of increased disorder

75
Q

T or F: gases have a higher entropy than solids

A

TRUE

76
Q

Products have a higher potential energy than reactants

A

ENDOTHERMIC

77
Q

Chemical kinetics is the study of the _____ of chemical reactions and gives an indication of the _____ of a reaction.

A

RATE ; MECHANISM

Organic Chem (4 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions