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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
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Sections
Chemical Reaction: Chemical Change
Law of Conservation of Mass
Balancing Chemical Equations (Simplified)
Solubility Rules
Molecular Equations
Types of Chemical Reactions
Complete Ionic Equations
Calculate Oxidation Numbers
Redox Reactions
Spontaneous Redox Reactions
Balancing Redox Reactions: Acidic Solutions
Balancing Redox Reactions: Basic Solutions
Balancing Redox Reactions (Simplified)
Galvanic Cell (Simplified)

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

Activity Series Chart

Concept #1: Spontaneous Redox Reactions

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

Ca (s) + AgCl (s)  →

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?