Ch.5 Classification & Balancing of Chemical ReactionsWorksheetSee all chapters
All Chapters
Ch.1 Matter and Measurements
Ch.2 Atoms and the Periodic Table
Ch.3 Ionic Compounds
Ch.4 Molecular Compounds
Ch.5 Classification & Balancing of Chemical Reactions
Ch.6 Chemical Reactions & Quantities
Ch.7 Energy, Rate and Equilibrium
Ch.8 Gases, Liquids and Solids
Ch.9 Solutions
Ch.10 Acids and Bases
Ch.11 Nuclear Chemistry

Spontaneous Redox Reactions occur when an element displaces another element within a compound. 

Activity Series Chart

Concept #1: Spontaneous Redox Reactions

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Example #1: Based on Activity Series Chart, determine if the following reaction represents a spontaneous redox reaction. 

Ca (s) + AgCl (s)  →

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Practice: Which element is the best reducing agent?

Practice: Determine whether which of the following redox reactions will occur spontaneously in the forward direction?

a) Ni(s) + Zn2+(aq) → Ni2+(aq) + Zn(s)
b) Fe(s) + Pb4+(aq) →   Fe2+(aq) + Pb(s)
c) Al(s) + Ag+(aq) →  Al3+(aq) + Ag(s)
d) Pb(s) + Mn2+ (aq) → Pb2+(aq) + Mn(s)

Practice: Suppose you wanted to cause Ni2+ ions to come out of solution as solid Ni. Which metal could you use to accomplish this?

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