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Chemistry > Redox > Flashcards

Redox Flashcards

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1
Q

Electrochemistry

A

The study of the exchange between electrical and chemical energy

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2
Q

Battery

A

A galvanic cell or cells connected in a series with a constant amount of reagents. A battery stores energy in the form of electrical potential energy.

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3
Q

Electrorefining

A

Process by which materials, usually metals, are purified by means of an electrolytic cell. The anode is the impure metal and the cathode is the pure sample of the metal.

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4
Q

Oxidation

A

The loss of an electron from a species (an increase in its oxidation number).

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5
Q

Oxidation Number

A

A conceptual bookkeeping numbering system that allows us to track the number electrons transferred during a redox reaction.

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6
Q

Reduction

A

The gain of an electron by a species (and a decrease in the oxidation number)

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7
Q

Redox

A

A reaction involving the transfer of one or more electrons from the reducing agent to the oxidizing agent.

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8
Q

Reducing Agent

A

A reactant in a redox equation that donates an electron to the reduced species. The reducing agent is oxidized.

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9
Q

Oxidizing Agent

A

A reactant in a redox reaction that accepts an electron from the oxidized species. The oxidizing Agent is reduced.

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10
Q

Galvanic Cell

A

An electrochemical cell with a positive cell potential that allows chemical energy to be converted into electrical energy.

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11
Q

Cell Potential

A

The overall electrical potential of an electrochemical cell. It is the sum of the reduction potential of the cathode and the oxidation potential of the anode.

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12
Q

Oxidation Potential

A

The potential of a half-reaction written as an oxidation reaction, it is the opposite sign of the same reaction written as a reduction.

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13
Q

Reduction Potential

A

Arbitrarily setting the potential of the standard hydrogen electrode, SHE, to zero, all other half reactions are measured by their power to reduce hydrogen. The voltage given by the construction of a galvanic cell between the SHE and the reduction of interest gives the standard reduction potential of that reduction.

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14
Q

Work

A

Force over a distance

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15
Q

Electrolytic Cell

A

A cell that consumes electrical energy to drive a non-spontaneous redox reaction.

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16
Q

Anode

A

The electrode that is the source of the negative charge, designated by a minus sign (-); this electrode is the site of oxidation.

17
Q

Cathode

A

The electrode that is the source of positive charge, designated by a plus sign (+); this electrode is the site of reduction.

18
Q

Concentration Cell

A

A galvanic cell that has two compositionally equivalent half-cells of differing concentrations. One can calculate the potential developed by such a cell using the Nernst Equation.

19
Q

Electrode

A

A conducting material placed in physical contact with a half-reaction on which the electron transfers in the redox reaction take place.

20
Q

Fuel Cell

A

A galvanic cell with a constant flow of reagents in and products out used for the prodction of a constant supply of energy. Whereas batteries have a finite lifetime of useful energy production, fuel cells are only limited in their duration of energy production by the ammount of available fuel reagents.

21
Q

Half-Cell

A

A half-reaction and its electrode; it is half of a galvanic cell.

22
Q

Half-Reaction

A

Either an oxidation or a reduction reaction, it represents half of the redox reaction.

23
Q

Half-Reaction Method

A

The set of rules that have been developed to aid in balancing redox reactions.

24
Q

Line Notation

A

A shorthand way of describing an electrochemical cell without drawing a picture.

25
Q

pH Meter

A

A concentration cell that places a known concentration of acid in the meter’s electrode. When that probe is dipped into a solution of unknown acid concentration, a potential develops due to the differences in concentration which can be calculated by the Nernst Equation. From that potential, the meter calculates the concentration of the unknown acid and, therefore, its pH.

26
Q

Porous Disk

A

A disk placed between two half-reactions allowing ion flow between half-reactions without mixing the reactions. The mixing of the two cells would cause a short in the circuit.

27
Q

Potentiometer

A

A device that measures electrical potential.

28
Q

Reaction Quotient

A

Similar to the form of an equilibrium constant, the reaction quotient is the ratio of the product of the each product in a reaction raised to its stoichiometric power divided by the product of each reactant raised to its stoichiometric power from the balanced equation.

29
Q

Salt Bridge

A

A tube plugged with pourous material at either end (usually cotton) filled with a gel allowing ion flow between half-reactions without mixing the reactions. The actual mixing of the two cells would cause a short in the circuit.

30
Q

Standard State

A

An arbitrarily defined set of conditions–273K, 1atm for gasses, or 1M for solutions.

31
Q

Atoms in elemental form have oxidation states of zero.

A

N/A

32
Q

The charge on a monoatomic ion is equivalent to its charge.

A

N/A

33
Q

Hydrogen has an oxidation state of +1 when bonded to non-metals and -1 when bonded to metals.

A

N/A

34
Q

F, because it only forms one bond and is the most electronegative element, has an oxidation state of -1.

A

N/A

35
Q

O, unless bonded to F or itself, has an oxidation state of -2.

A

N/A

36
Q

The sum of all oxidation states in a compound must equal the total charge on the species

A

N/A

37
Q
  1. Separate oxidation and reduction half-reactions.
  2. Balance all atoms except for hydrogen and oxygen in each half-reaction.
  3. Balance oxygen by adding H2O as needed.
  4. To balance hydrogen, add H+ as needed.
  5. Balance the charge of each reaction by adding electrons to side with the greater charge.
  6. Multiply each half-reaction by the least integer factor that equalizes the number of electrons in each half-reaction. Then, add the half-reactions to obtain the overall balanced reaction in acidic solution.

If your redox reaction is in acidic solution, the above reaction is properly balanced. However, if the reaction you wish to balance is in basic solution, you need to add these three steps:

  1. If the redox reaction is one in basic solution, then add OH- to both sides of the equation to “neutralize” each H+.
  2. “React” H+ and OH- to form H2O and eliminate water molecules on both sides of the equation.
  3. Make sure that all atoms and charges are indeed balanced in your overall balanced equation for the redox reaction in basic solution.
A

How to solve redox reactions

Chemistry (3 decks)

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