Chemistry Final Exam Review Guide

Unit 4: Chemical Bonds

Objectives

1. Electronegativity and Bond Formation
   • Connection between electronegativity and ionic/covalent bond formation.
2. Types of Bonds
   • Differentiate single, double, and triple bonds.
3. VSEPR Theory
   • Impact on drawing Lewis structures for molecular compounds.
4. Intermolecular Forces
   • Create a summary chart of types: dipole-dipole, hydrogen bonding, London dispersion.
5. Bond Identification
   • Identify bonds/compounds as ionic, covalent, or metallic using electronegativity or examples.
6. Lewis Structures
   • Illustrate formation of ionic/covalent bonds using Lewis structures.
7. Nomenclature Rules
   • Apply rules to determine chemical formulas/names for covalent/ionic compounds, including polyatomic ions and transition metals.
8. Intermolecular Forces Prediction
   • Predict forces using pictures, descriptions, models, or examples.
9. Ranking Intermolecular Forces
   • Rank substances based on strength of intermolecular forces from given data.

Practice

• Naming Compounds
  • (NH4)2S: Ammonium sulfide
  • CuCO3: Copper(II) carbonate
• Writing Chemical Formulas
  • Magnesium sulfate: MgSO4
  • Gold(II) chloride: AuCl2
• Lewis Structures
  • Draw and name PCl3: Phosphorus trichloride
• Naming Additional Compounds
  • P2S3: Diphosphorus trisulfide
  • BBr3: Boron tribromide
• Writing Additional Formulas
  • Dinitrogen monosulfide: N2S
  • Carbon tetrahydride: CH4
• Molecular Compounds Lewis Structures
  • H2O, HCN, PH3, CH4: Draw structures, count electron domains, identify lone pairs, predict shapes.

Vocabulary

• Chemical bond, Molecule, Ionic bond, Polyatomic ion, Transition metal, Metallic bond, Covalent bond, Electron domain, Lone pairs, Bonding pairs, Polar/Nonpolar molecules, Intermolecular forces.

Unit 5: Chemical Reactions

Objectives

1. Law of Conservation of Mass
   • Relationship to chemical reactions.
2. Chemical Equations
   • Label, interpret, and write equations with correct notation.
3. Balancing Reactions
   • Balance according to conservation of mass.
4. Writing Balanced Reactions
   • From written descriptions.

Practice

• Balancing and Classifying Reactions
  • Decomposition example: Ca(OH)2 → CaO + H2O
  • Single replacement example: Al + Pb(NO3)2 → Pb + Al(NO3)3
• Predicting Products and Balancing
  • Combustion, synthesis, decomposition, single and double replacement reactions.
• Reaction Analysis
  • N2 + 3H2 ↔ 2NH3 + heat: Endothermic vs exothermic, equilibrium changes under different conditions.

Vocabulary

• Chemical equilibrium, Le Chatelier’s Principle.

Unit 6: Stoichiometry

Objectives

1. Limiting Reactant
   • Determines amount of product.
2. Stoichiometry Calculations
   • Moles/mass conversions.
3. Limiting and Excess Reactants
   • Determining quantities and leftovers.
4. Product Formation
   • Calculate potential product amount.
5. Percent Yield
   • Calculate using actual yield and reactant quantity.

Practice

• Be + HCl Reaction
  • Balance, classify, identify limiting reactant, calculate excess, determine product amount.
• Double Replacement Reaction
  • Write reaction, calculate theoretical yield, and percent yield from actual yield.

Vocabulary

• Mole, Molar mass, Limiting reactant, Excess reactant, Actual yield, Theoretical yield, Percent yield.

Unit 7: Acids and Bases

Objectives

1. Acid-Base Reactions
   • Definition, example, and neutralization explanation.
2. Definitions of Acids and Bases
   • Differentiation and examples.
3. Ionization vs Dissociation
   • Differences and effects.
4. Acid/Base Strength
   • Strong vs weak.
5. Polarity and Dissociation
   • Relationship to acid/base strength.
6. Concentration Graphs
   • Sketch for strong/weak bases.
7. pH and pOH Relationships
   • How they relate to ion concentration.
8. Identifying Acids/Bases
   • Strong vs weak from models/descriptions.

Practice

• pOH Calculation
  • Determine from given pH (e.g., pH = 3.5).

Vocabulary

• Salt, Arrhenius acid/base, Bronsted-Lowry acid/base, Amphoteric, pH, pOH.