Predicting Redox Reactions Chapter 9.3

Mg

Mg

Some redox reactions are spontaneous Mg2+

Mg2+

Pb

Pb

Other redox reactions are not spontaneous Mg2+ Mg2+ Mg2+

Mg2+

Mg2+ Mg2+

Experiments can be run…

…and the results can be summarized in tables like the one below

Redox table (standard reduction potentials table): A table listing standard reduction potentials of common oxidizing agents and reducing agents in order from strongest to weakest p.729-730 of your textbook

The Spontaneity Rule

Example • Use the redox table to predict whether the following reactions will be spontaneous: a) Cr (s) + NiSO4 (aq)  ? b) Ag(s) + Pb(NO3)2 (aq)  ?

Predicting Redox Reactions Using a Redox Table 1. List all of the entities present 2. Classify the entities as either oxidixing agents (left side of the table) or reducing agents (right side of the table) 3. Identify the strongest oxidizing agent (top left) and the strongest reducing agent (bottom right) 4. Predict whether the reaction is spontaneous 5. Write the half-reaction equations (reverse the direction of the oxidation reaction) 6. Use multipliers to balance the electrons 7. Combine the half reactions to give the overall equation

Example • A strip of tin is placed in a solution of silver nitrate

Practice • Iodic acid is poured into an aluminum pop can

Practice • Tin (II) bromide solution is poured into acidified sodium dichromate solution

HOMEWORK Required Reading: p. 618-623 (remember to supplement your notes!)

Questions: p. 622 #1-4 p. 623 #1-9

9.3 Predicting Redox Reactions

Write the half-reaction equations (reverse the direction of the oxidation reaction). 6. Use multipliers to balance the electrons. 7. Combine the half reactions to give ...

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