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Chemistry 12 > Unit 5: Electrochemistry > Flashcards

Unit 5: Electrochemistry Flashcards

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1
Q

Metals love to ____

A

Oxidize

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2
Q

____ is a reaction in which e- are lost

A

Oxidation

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3
Q

Oxidation-reduction (redox) reactions involve a transfer of ____.

A

Electrons

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4
Q

_____ is the branch of chemistry which is concerned with the conversion of chemical energy to electrical energy, and vice versa.

A

Electrochemistry

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5
Q

A(n) _____ _____ is a half-reaction in which a species loses electrons.

A

Oxidation reaction

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6
Q

A(n) _____ _____ is a half-reaction in which a species gains electrons.

A

Reduction reaction

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7
Q

For every reduction reaction there must be an accompanying ____ ____.

A

Oxidation reaction

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8
Q

For every oxidation reaction there must be an accompanying ____ ____.

A

Reduction reaction

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9
Q

A reaction involving the loss and gain of electrons is called a ______-______ ______.

A

Reduction-oxidation reaction

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10
Q

A reduction-oxidation reaction is also called a ____ reaction

A

Redox

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11
Q

You can be certain you are dealing with a redox reaction any time you see that an atom or ion has changed ____ during the reaction

A

Charge

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12
Q

The oxidizing agent is ____ during the reaction

A

Reduced

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13
Q

The reducing agent is ____ during the reaction

A

Oxidized

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14
Q

A species being oxidized becomes more ____ charged

A

Positively

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15
Q

A species being reduced becomes more ____ charged

A

Negatively

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16
Q

Oxidation reactions are often the attachment of ____ to ____

A

Oxygen

Metals

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17
Q

The reduction process removes ____ from the metal compounds, leaving more or less pure metal behind

A

Oxygen

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18
Q

An oxidation number is the charge that an atom would posses if….

A

The species containing the atom were made of ions

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19
Q

The rule which governs oxidation numbers is

A

The sum of the positive charges and the negative charges must equal the overall charge on the species

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20
Q

The oxidation number of an atom in its elemental form is ____.

A

ZERO

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21
Q

The oxidation number of a monatomic ion is ….

A

The charge on the ion

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22
Q

When referring to an isolated half reaction, use ______ arrows to show that the reaction can go….

A

Equilibrium

Forward or backward

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23
Q

If the half reaction is made to undergo either reduction or oxidation as a result of being part of a redox reaction the use a ______ reaction arrow

A

One way

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24
Q

If two half cells are joined, the half reaction ____ on the chart will undego reduction and the one _____ chart will undergo oxidation

A

Higher

Lower

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25
Q

If both reactants are only found on the left of the table or both reactants are only found on the right then….

A

No reaction is possible

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26
Q

If the reactant to be reduced (left side) is higher on the table than the reactant to be oxidized (right side) the reaction will ____ _____

A

Occur (spontaneously)

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27
Q

If the reactant to be reduced (left side) is lower on the table than the reactant to be oxidized (right side) the reaction will ____ _____

A

Not occur

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28
Q

A disproportionation reaction is…

A

A redox reaction in which the same species is both reduced and oxidized

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29
Q

A reaction will be spontaneous if and only if there is a reactant to be reduced which is ______ a reactant to be oxidized

A

Above

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30
Q

An increase in oxidation number in one species must be balanced by a corresponding ____ in oxidation number in a second species

A

Decrease

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31
Q

In any redox equation the overall change in oxidation numbers must be ____

A

Zero

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32
Q

An electrode is (in general terms)….

A

A conductor at which a half reaction occurs

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33
Q

At which electrode does oxidation take place?

A

Anode

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34
Q

At which electrode does reduction take place?

A

Cathode

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35
Q

The electrode to which anions travel is?

A

The anode

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36
Q

A cathode ____ electrons from/to a substance being ____. The cathode receives its electrons through the wire from the ____

A

Supplies
Reduced
Anode

37
Q

Electrons flow from the ____ to the ____

A

Anode

Cathode

38
Q

The electrons are forced through the wire in an electrochemical cell because….

A

The reactants are separated

39
Q

Only ____ flow in the solution in an electrochemical cell

A

Ions

40
Q

The number of electrons involved in the oxidation reaction must equal….

A

The number of electrons involved in the reduction reaction

41
Q

As positive ions are formed at the anode they accumulate around the anode. This excess of positive charge is depleted by…. (2 factors)

A

1) random movement of the positive ion away from the anode due to the fact that there is a higher probability that the ion will move to the area of the lower concentration of the ion
2) movement of the negative ions toward the anode (due to its positivity)

42
Q

As the positive ions around the cathode are depleted by the reduction of them, the amount of positive charge is decreased around the cathode. The resulting deficiency of positive charge is corrected by…. (2 factors)

A

1) the movement of the positive ions towards the cathode by random movement. There is a great possibility that the ions will move into a low concentration from a high concentration
2) movement of negative ions away from the cathode. The greater amount of positive charge at the anode end of the cell will attract the negative ions toward the anode

43
Q

The tendency of electrons to flow in an electrochemical cell is called _____ or ____ ____ to do work.

A

Voltage

Electric potential

44
Q

The _____ is the work done per electron transferred

A

Voltage

45
Q

E° =….

A

The STANDARD REDUCTION POTENTIAL, in volts.

46
Q

The “o” in the E° implies this is a ____ _____

A

STANDARD STATE

47
Q

An electrochemical cell is said to be at STANDARD STATE if… (4 things)

A

1) it is at 25°
2) all gasses are at 101.3 KPa (1 atm)
3) all elements are in their standard states (that is, their normal phase at 25°c)
4) there exists a 1M concentration for ALL solutions involved in the half cell (both on the reactants and products side)

48
Q

Platinum is used because it is an ____ electrode.

A

Inert

49
Q

Being a inert electrode means…

A

It doesn’t react but it conducts electrons and allows the reaction to occur at its surface

50
Q

If a half reaction is reversed the sign of its E° value is ____.

A

Reversed

51
Q

If two half reactions can be added together to give a redox equation, the voltages associated with the half reactions can be ____

A

Added

52
Q

The potential of an electrochemical cell is just the difference between the half-cell voltages for the…..

A

Reduction reaction and the oxidation reaction.

53
Q

E°red - E°ox = ?

A

E°cell

54
Q

If E°cell is positive for a redox reaction the reaction is expected to be_____.

A

Spontaneous

55
Q

If E°cell is negative for a redox reaction, the reaction is _____.

A

Non-spontaneous

56
Q

____ is the work done per electron so DO NOT multiply the E° value

A

Voltage

57
Q

If a reaction occurs in an acidic solution, the reduction of ____ may be a possible reaction and must be considered along with any other reductions possible

A

H+ (at 0.00V)

58
Q

If a reaction occurs in an neutral solution, the reduction of ____ may be a possible reaction and must be considered along with any other reductions possible

A

Neutral water (at -0.41V)

59
Q

The surface are of an electrode has _______ (no effect/some effect) on the cell potential

A

No effect

60
Q

When the surface area of an electrode is increased, the reaction rate at the electrode ______. That is, the number of electrons per second being transferred ______.

A

Increases

Increases

61
Q

The increased reaction rate, due to increased surface area, _____ (does/ does not) increase the cell voltage.

A

Does not

62
Q

How can you increase the amount of time a battery will operate?

A

Increase the amount of electron material

63
Q

When the difference in reduction potentials is zero (Ecell=0)….

A

The reaction is at equilibrium

64
Q

If the difference in reduction potentials is zero then the reaction is….

A

At equilibrium

65
Q

Name 4 ways to prevent corrosion

A

1) apply a protective layer
2) apply a metal which is corrosion resistant to the surface of the original metal
3) cathodic protection
4) change the conditions in the chemical surroundings so as to lower the tendency of the surrounding to reduce

66
Q

Cathodic protection is…

A

The process of protecting a substance from unwanted oxidation by connecting it to a substance having a higher tendency to oxidize

67
Q

An _____ or ______ is an apparatus in which electrolysis can occur.

A

Electrolytic cell

Electrolysis cell

68
Q

_____ supplies energy to non-spontaneous electrochemical reactions (E°cell

A

Electrolysis

69
Q

Electrolysis is the process of….

A

Supplying electrical energy to a molten ionic compound or a solution containing ions so as to produce a chemical change

70
Q

What is a binary salt

A

A binary salt is a salt made of only two different elements

71
Q

In a simple electrolytic cell (electrolysis of a molten binary salt) there is no need for a salt bridge or a porous barrier to keep the reactants separated because….

A

No spontaneous reaction occurs between the reactants

72
Q

In a simple electrolytic cell (electrolysis of a molten binary salt) what are the anode and cathode made of?

A

both anode and cathode are made of inert materials such as platinum or carbon

73
Q

The anode and cathode in a simple electrolytic cell are connected by?

A

A wire with a DC current battery in its center

74
Q

During the electrolysis of aqueous solutions what must you always consider?

A

You must always consider the possibility that H2O may oxidize and/or reduce

75
Q

The preferred reaction (in electrolysis of aqueous solutions) will be the one requiring the least…..

A

Voltage input

76
Q

Which half reactions are preferred?

A

The half reactions that have the greatest tendency to reduce and the greatest tendency to oxidize

77
Q

Electrolysis of aqueous solutions containing Cl- or Br- will produce?

A

Cl2 or Br2 at the anode

78
Q

Electroplating is….

A

An electrolytic process in which a metal is reduced or “plated out” at a cathode

79
Q

In electroplating: the cathode is made of?

A

The material which will receive the metal plating

80
Q

In electroplating: the ______ solution contains ions of the metal which is to be “plated” onto the carthode

A

Electroplating

81
Q

In electroplating what is the anode made of? (2 possible answers)

A

1) the anode may be made of the same metal which is to be “plated out” onto the cathode
2) the anode can also be an inert electrode (carbon or platinum)

82
Q

Electrorefining is the process of….

A

Purifying metal by electrolysis

83
Q

When several different reduction half reactions occur the one having the _____ tendency to accept electrons or the ____ reductions potential will occur preferentially.

A

Highest

Highest

84
Q

When several different oxidation half reactions occur the one having the _____ tendency to lose electrons or the ____ reductions potential will occur preferentially.

A

Highest

Lowest

85
Q

Any ion capable of being reduced will be a _______ ion if there is another ion in the same solution which has a greater tendency to be reduced

A

Spectator

86
Q

Any ion capable of being oxidized will be a spectator ion if there is another ion in the same solution which has a _____ tendency to be _____

A

Greater

Oxidized

87
Q

Which ions are generally spectator ions? (six ions)

A 
Na+
K+
Ca2+
Mg2+
SO4 2- (in a neutral solution)
Cl-
88
Q

The anode _____ electrons from the substance being _____ and the electrons then move through the wire to the ____

A

Receive
Oxidized
Cathode

Chemistry 12 (7 decks)

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