Electrochemistry notes
Chemistry 3202
Unit 4 Electrochemistry
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Define the terms: oxidation and reduction in terms of loss or gain of electrons. P.714
Identify electron transfer in redox equations. P.714
Identify oxidation and reduction half-reaction equations in an oxidation-reduction (redox) equation. P.715- 716
Identify a redox equation as the sum of the oxidation half-reaction and the reduction halfreaction. P.715- 716
Identify the species oxidized, the species reduced, the oxidizing agent and the reducing agent in simple redox equations. P.715- 716
Define oxidation number. P.721- 728
Use oxidation number rules to find the oxidation numbers of the atoms in molecules or ions.
P.721- 728
Identify changes in oxidation number in half-reactions and in redox equations. P.721- 728
Given an equation for composition or decomposition of simple ionic compounds identify oxidation and reduction half reactions by balancing the number of electrons lost and gained.
P.721- 728
Write and balance half-reactions and complete redox reactions. P.730 - 736
Write and balance equations for complex oxidation reduction reactions occurring in acidic or basic solutions. P.736 - 739
Solve redox stoichiometry problems for redox reactions. P.742 - 745
Define electrochemical cells. P.757-760
Draw and label an electrochemical cell. Include: P.757-760
(i) anode
(ii) cathode
(iii) salt bridge
(iv) direction of flow of electrons
(iv) direction of flow of ions
Use electrochemical cell notation to represent an electrochemical cell. P.757-760
Draw and label an electrochemical cell using electrochemical cell notation. P.757-760
Identify electrochemical cells as cells which produce electrical energy in spontaneous oxidationreduction reactions. P.757-760
Define half-cell voltage, standard half-cell, cell voltage, Eo. P.761, 768 - 773
Define a spontaneous reaction as one
Unit 4 Electrochemistry
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
21.
22.
23.
24.
Define the terms: oxidation and reduction in terms of loss or gain of electrons. P.714
Identify electron transfer in redox equations. P.714
Identify oxidation and reduction half-reaction equations in an oxidation-reduction (redox) equation. P.715- 716
Identify a redox equation as the sum of the oxidation half-reaction and the reduction halfreaction. P.715- 716
Identify the species oxidized, the species reduced, the oxidizing agent and the reducing agent in simple redox equations. P.715- 716
Define oxidation number. P.721- 728
Use oxidation number rules to find the oxidation numbers of the atoms in molecules or ions.
P.721- 728
Identify changes in oxidation number in half-reactions and in redox equations. P.721- 728
Given an equation for composition or decomposition of simple ionic compounds identify oxidation and reduction half reactions by balancing the number of electrons lost and gained.
P.721- 728
Write and balance half-reactions and complete redox reactions. P.730 - 736
Write and balance equations for complex oxidation reduction reactions occurring in acidic or basic solutions. P.736 - 739
Solve redox stoichiometry problems for redox reactions. P.742 - 745
Define electrochemical cells. P.757-760
Draw and label an electrochemical cell. Include: P.757-760
(i) anode
(ii) cathode
(iii) salt bridge
(iv) direction of flow of electrons
(iv) direction of flow of ions
Use electrochemical cell notation to represent an electrochemical cell. P.757-760
Draw and label an electrochemical cell using electrochemical cell notation. P.757-760
Identify electrochemical cells as cells which produce electrical energy in spontaneous oxidationreduction reactions. P.757-760
Define half-cell voltage, standard half-cell, cell voltage, Eo. P.761, 768 - 773
Define a spontaneous reaction as one