AP Chemistry Unit 4: Chemical Reactions

TLDR

• Learn to identify reaction types and predict products confidently.

• Master net ionic equations, solubility rules, and reaction driving forces.

• Apply stoichiometry, limiting reactants, and percent yield correctly.

• Understand redox reactions and titrations from an exam perspective.

• Download the Unit 4 cheat sheet for quick revision before practice sets.

Why This Unit Matters

Unit 4 is where chemistry becomes procedural and logical. The AP exam frequently tests whether you can recognize what kind of reaction is happening, predict the correct products, and explain why the reaction occurs.

Strong performance here helps with later units like thermodynamics, equilibrium, and electrochemistry. If you can identify reaction type, driving force, and limiting reactant, you already control a large portion of the exam.

1. Types of Chemical Reactions

Most AP Chemistry reactions fall into predictable categories.

Synthesis: A + B → AB
Decomposition: AB → A + B
Single replacement: A + BC → AC + B
Occurs only if the free element is more reactive than the one it replaces.
Double replacement: AB + CD → AD + CB
Driven by precipitate formation, gas formation, or weak electrolyte formation.
Combustion: Hydrocarbon + O₂ → CO₂ + H₂O

Mnemonic: So Do Single, Double, Combust.

2. Net Ionic Equations

Net ionic equations focus on what actually changes in solution.

Steps:

1. Write the balanced molecular equation.

2. Dissociate all strong electrolytes into ions.

3. Remove spectator ions.

4. What remains is the net ionic equation.

Strong electrolytes include soluble ionic compounds, strong acids, and strong bases.

Tutor Tip: Always include state symbols. Missing (s), (l), (g), or (aq) can cost points on FRQs.

3. Solubility Rules and Precipitation

Precipitation reactions occur when an insoluble solid forms from aqueous ions.

High-yield rules to memorize:

• Nitrates and ammonium compounds are soluble.

• Group 1 metal salts are soluble.

• Carbonates, phosphates, and hydroxides are usually insoluble unless paired with Group 1 or ammonium.

• Sulfates are soluble except with Ba²⁺, Sr²⁺, and Pb²⁺.

Mnemonic: NAG SAG for common soluble compounds.

4. Reaction Evidence and Driving Forces

A reaction proceeds if at least one driving force is present.

Common driving forces:

• Formation of a precipitate.

• Formation of a gas.

• Formation of a weak electrolyte such as water.

• Transfer of electrons in redox reactions.

AP graders reward explanations that explicitly reference these driving forces.

5. Oxidation–Reduction Reactions

Redox reactions involve electron transfer.

• Oxidation is loss of electrons.

• Reduction is gain of electrons.

Mnemonic: OIL RIG.

To balance redox reactions:

• Assign oxidation numbers.

• Identify what is oxidized and reduced.

• Use the half-reaction method.

• Balance atoms, then charge using electrons.

In basic solutions, eliminate H⁺ by adding OH⁻ to both sides.

6. Stoichiometry and Limiting Reactants

Chemical reactions depend on mole ratios.

Process:

• Convert grams to moles.

• Use mole ratios from the balanced equation.

• Identify the limiting reactant.

• Calculate theoretical yield.

Formulas to know:

• Percent yield = (actual ÷ theoretical) × 100

• Percent error = |experimental − true| ÷ true × 100

The limiting reactant is the one that produces the least amount of product.

7. Titrations and Solution Reactions

Titrations determine unknown concentrations using neutralization or redox reactions.

Key ideas:

• Equivalence point occurs when stoichiometric amounts react.

• Endpoint is indicated by a color change.

• M₁V₁ = M₂V₂ only works for 1:1 reactions.

• For all others, use mole ratios from the balanced equation.

Common indicators:

• Phenolphthalein turns pink in base.

• Methyl orange turns red in acid.

8. Gas-Producing Reactions

Some reactions are driven by gas formation.

Examples:

• Acid + carbonate → CO₂ + H₂O + salt

• Acid + sulfite → SO₂ + H₂O + salt

• Hydrogen peroxide decomposition → O₂ + H₂O

Mnemonic: Carbonate makes CO₂, sulfite makes SO₂.

Common Pitfalls

• Forgetting to remove spectator ions in net ionic equations.

• Using M₁V₁ = M₂V₂ when coefficients are not 1:1.

• Treating weak acids as strong electrolytes.

• Forgetting state symbols.

• Not justifying reactions using driving forces.

Tutor Tip

On free-response questions, always explain why a reaction occurs. Statements like “a precipitate forms because BaSO₄ is insoluble” or “CO₂ gas evolution drives the reaction forward” earn reasoning points and separate strong answers from average ones.

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