5 Steps to a 5 AP Chemistry

You get 1 point for entering the values into the correct equation. The question does not

ask you to do any calculations, so there are no points for including any work beyond

what is shown.

e. Anode Cd

Cathode Ag

Oxidizing Agent Ag+

Reducing Agent Cd

You get 1 point for each correctly identified item.

Total your points; there are 10 points possible. Subtract one point if all answers do

not have the correct number of significant figures.

 Rapid Review

 In redox reactions electrons are lost and gained. Oxidation is the loss of electrons, and

reduction is the gain of electrons.

 The reactant that is being reduced is the oxidizing agent, and the reactant being oxidized

is the reducing agent.

 The same number of electrons is lost and gained in redox reactions.

 Galvanic (voltaic) cells produce electricity through the use of a redox reaction.

 The anode is the electrode at which the oxidation half-reaction takes place. The anode

compartment is the solution in which the anode is immersed.

 The cathode is the electrode at which reduction takes place, and the cathode compart-

ment is the solution in which the cathode is immersed.

 In a galvanic cell the anode is labeled as (−) and the cathode (+).

 A salt bridge is used in an electrochemical cell to maintain electrical neutrality in the cell

compartments.

 Be able to diagram an electrochemical cell.

 The cell notation is a shorthand way of representing a cell. It has the form:

anode |anode compartment ||cathode compartment |cathode

 Standard reduction potentials are used to calculate the cell potential under standard con-

ditions. All half-reactions are shown in the reduction form.

 For a galvanic cell E°cell>0.

 E°cell=E°cathode−E^0 anode>0. Know how to use this equation to calculate E°cell.

 Electrolytic cells use an external source of electricity to produce a desired redox reaction.

 Review how to diagram an electrolytic cell.

 The following relationships can be used to calculate quantitative changes that occur in

an electrochemical cell, especially an electrolytic one: 1 F =96,500 C per mole of electron

(F =96,500 C/mol e−=96,500 J/V) and 1 amp =1 C/s (A =C/s)

258  Step 4. Review the Knowledge You Need to Score High