Electrochemistry notes

Topics: Redox, Electrochemistry, Electrochemical cell Pages: 5 (623 words) Published: January 19, 2014
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 that produces a positive cell potential. P 768 - 773 Write and balance equations for oxidation-reduction reactions using half-reaction equations

obtained from a standard reduction potential table for simple redox reactions. P. 768 - 773 Use a standard reduction potential table to predict cell voltage and to predict if the redox reaction is spontaneous (occurs as is written). P. 768 - 773

Develop a table of redox half-reactions from experimental results. Explain the historical development of electrolysis, e.g. Sir Humphry Davy used electrolysis to separate table salt into sodium and chlorine. P. 776 - 777

Define electrolytic cells as requiring electrical energy to cause non-spontaneous oxidationreduction reactions to occur. P. 776 - 777, 780

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Draw and label an electrolytic cell. Include: p. 780
(i) anode
(ii) cathode
(iii) salt bridge
(iv) power supply
(v) direction of flow of electrons and ions
Predict and write balanced half-reactions for reactions at the cathode and the anode of electrolytic cells. P. 778 - 783
Compare electrochemical and electrolytic cells in terms of energy efficiency, electron flow/ transfer, and chemical change. P 780
Write equations for electrolytic cells from half-reactions. P. 778 - 783 Perform stoichiometry calculations related to electroplating using Q=It and Q=nF. P. 790 - 793 Define metallurgy, pyrometallurgy and hydrometallurgy using scientific principles. STSE Differentiate between the terms mineral and ore. STSE

Define and describe the process of flotation, as it applies to the mining industry. STSE Define the terms flotation, slag, and leaching, as they apply to pyrometallurgy and hydrometallurgy. STSE
Identify and describe, using chemical reactions and chemical equations, the purification of copper metal using an electrolytic cell. STSE
Identify the risks and benefits to society and the environment of pyrometallurgy. STSE Describe the process...
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