Honors Chemistry

Chapter 19 Review

Can you:

• Define the terms oxidation, reduction, oxidizing agent, and reducing agent.
• Relate an elements tendency to lose or gain electrons to its position on the periodic table.
• Identify the form (ion or neutral atom) that would lose or gain electrons.
• Identify chemical equations as oxidation-reduction reactions.
• Determine oxidation number for elements within a compound or ion.
• Use oxidation number to identify the element oxidized and the element reduced given an equation for an oxidation-reduction reaction.
• Balance oxidation-reduction reactions using oxidation number.
• Explain what it means for a chemical reaction to be spontaneous.
• Explain why an oxidation-reduction reaction is spontaneous in terms of the desire for the elements involved to gain or lose electrons (who likes electrons better?).
• Use the table of reduction half-reactions to predict whether a reaction will be spontaneous.
• Write balanced chemical equations for oxidation-reduction reactions using the table of reduction half-reactions.
• Predict what products will be produced, if any, in an oxidation-reduction reaction using the periodic table and table of reduction half-reactions.
• Define electrochemical cell.
• Identify common examples of electrochemical cells.
• Using a diagram for an electrochemical cell:
• Identify the substance being oxidized and the substance being reduced.
• Identify the anode and the cathode.
• Write the overall reaction.
• Determine the cell potential (voltage on the voltmeter?)
• Determine which direction electrons are flowing.
• Explain the purpose of the salt bridge.
• Give the direction ions are flowing within the salt bridge.