Ontario Grade 11 Chemistry (SCH3U) lessons and practice

Atomic structure, isotopes, periodic trends, Lewis structures, bonding, nomenclature, and properties.

Balanced equations, reaction types, product prediction, combustion, acids, bases, and neutralization.

The mole, molar mass, formulas, stoichiometry, limiting reagents, and percentage yield.

Concentration, dilution, solubility, ionic equations, titration, and water quality.

Kinetic molecular theory, gas laws, gas stoichiometry, atmospheric composition, and air quality.

Plan, perform, analyse, and communicate chemistry investigations safely, and explore related careers.

• A1.1 · Form scientific questions, predictions, and testable hypotheses (published written lesson)
• A1.2 · Choose suitable chemistry equipment, materials, and procedures (published written lesson)
• A1.3 · Find appropriate print and electronic research sources (published written lesson)
• A1.4 · Plan investigations using safe laboratory practices and WHMIS (published written lesson)
• A1.5 · Conduct inquiries safely while controlling relevant variables (published written lesson)
• A1.6 · Record and organize accurate data in suitable formats (published written lesson)
• A1.7 · Organize research information and document sources (published written lesson)
• A1.8 · Analyse evidence, solve quantitative problems, and evaluate error (published written lesson)
• A1.9 · Evaluate research sources for accuracy, reliability, and bias (published written lesson)
• A1.10 · Draw and justify conclusions from inquiry and research evidence (published written lesson)
• A1.11 · Communicate chemistry procedures, results, and conclusions clearly (published written lesson)
• A1.12 · Use suitable numeric, symbolic, graphical, and unit representations (published written lesson)
• A1.13 · Report calculations with suitable precision and significant figures (published written lesson)
• A2.1 · Explore chemistry-related careers and required education (published written lesson)
• A2.2 · Describe contributions of chemists, including Canadians (published written lesson)

Connect atomic structure and periodic trends to bonding, nomenclature, structures, and material properties.

• B1.1 · Analyse a potentially harmful chemical and propose safer use or alternatives (published written lesson)
• B1.2 · Evaluate health risks and benefits of common chemicals (published written lesson)
• B2.1 · Use periodic-trend and chemical-bonding terminology (published written lesson)
• B2.2 · Analyse element data to identify periodic trends (published written lesson)
• B2.3 · Investigate element reactions and develop an activity series (published written lesson)
• B2.4 · Draw Lewis structures for ionic and molecular compounds (published written lesson)
• B2.5 · Predict bond type using electronegativity (published written lesson)
• B2.6 · Build molecular and ionic models and write structural formulas (published written lesson)
• B2.7 · Write formulas and IUPAC names for binary and polyatomic compounds (published written lesson)
• B3.1 · Relate atomic number, mass number, isotopes, and radioisotopes (published written lesson)
• B3.2 · Relate isotopic abundance to relative atomic mass (published written lesson)
• B3.3 · Explain periodic law and trends from electron arrangement and forces (published written lesson)
• B3.4 · Compare formation of ionic and covalent bonds (published written lesson)
• B3.5 · Compare physical properties of ionic and molecular compounds (published written lesson)

Represent, classify, predict, and investigate common chemical reactions and their impacts.

• C1.1 · Analyse industrial reactions that affect community health and safety (published written lesson)
• C1.2 · Assess chemical reactions used to address social and environmental problems (published written lesson)
• C2.1 · Use terminology for reaction types, acids, bases, and precipitates (published written lesson)
• C2.2 · Write balanced equations for common reaction types (published written lesson)
• C2.3 · Investigate reaction types by testing their products (published written lesson)
• C2.4 · Predict products of synthesis and decomposition reactions (published written lesson)
• C2.5 · Predict single-displacement products using activity series (published written lesson)
• C2.6 · Predict double-displacement products (published written lesson)
• C2.7 · Design an inquiry comparing complete and incomplete combustion (published written lesson)
• C2.8 · Compare solutions formed by metal and non-metal oxides (published written lesson)
• C2.9 · Investigate a neutralization reaction (published written lesson)
• C2.10 · Plan and conduct a single-displacement inquiry (published written lesson)
• C3.1 · Identify synthesis, decomposition, displacement, and combustion reactions (published written lesson)
• C3.2 · Explain complete and incomplete combustion (published written lesson)
• C3.3 · Explain acid and base formation from metal and non-metal oxides (published written lesson)

Use the mole and balanced equations to calculate composition, formulas, stoichiometry, limiting reagents, and yield.

• D1.1 · Analyse practical processes that depend on chemical quantities (published written lesson)
• D1.2 · Assess the importance of quantitative accuracy in industry (published written lesson)
• D2.1 · Use mole, stoichiometry, limiting-reagent, and yield terminology (published written lesson)
• D2.2 · Determine percent composition through inquiry (published written lesson)
• D2.3 · Convert among moles, particles, and mass (published written lesson)
• D2.4 · Determine empirical and molecular formulas (published written lesson)
• D2.5 · Calculate reactant and product quantities from balanced equations (published written lesson)
• D2.6 · Solve limiting-reagent and percentage-yield problems (published written lesson)
• D2.7 · Measure actual and theoretical yield and evaluate error (published written lesson)
• D3.1 · Explain the law of definite proportions (published written lesson)
• D3.2 · Relate Avogadro’s number, moles, and molar mass (published written lesson)
• D3.3 · Explain the relationship between empirical and molecular formulas (published written lesson)
• D3.4 · Explain quantitative relationships in balanced equations (published written lesson)

Prepare and analyse solutions, concentrations, solubility, ionic equations, acids, bases, titrations, and water quality.

• E1.1 · Analyse sources and cumulative effects of water pollutants (published written lesson)
• E1.2 · Analyse issues in drinking-water distribution, purification, and use (published written lesson)
• E2.1 · Use solution, solubility, concentration, ionization, and pH terminology (published written lesson)
• E2.2 · Calculate solution concentration in multiple units (written lesson not published)
• E2.3 · Prepare solutions by dissolving or dilution (published written lesson)
• E2.4 · Investigate qualitative and quantitative solution properties (published written lesson)
• E2.5 · Write net ionic equations for precipitation and neutralization (written lesson not published)
• E2.6 · Solve solution-stoichiometry problems (published written lesson)
• E2.7 · Determine acid or base concentration by titration (published written lesson)
• E2.8 · Investigate local drinking-water pollutant concentrations (published written lesson)
• E3.1 · Explain water polarity, hydrogen bonding, and solvent properties (published written lesson)
• E3.2 · Explain formation of ionic, molecular, and non-polar solutions (published written lesson)
• E3.3 · Explain temperature and pressure effects on solubility (published written lesson)
• E3.4 · Predict precipitates using a solubility table (published written lesson)
• E3.5 · Explain Arrhenius acids and bases (published written lesson)
• E3.6 · Distinguish strong and weak acids and bases by ionization (published written lesson)

Use kinetic molecular theory and gas laws to investigate gases, while connecting chemistry to air quality.

• F1.1 · Analyse air-quality impacts and propose carbon-footprint reductions (published written lesson)
• F1.2 · Assess air quality and Canadian pollution-reduction initiatives (published written lesson)
• F2.1 · Use gas-law and atmospheric-chemistry terminology (published written lesson)
• F2.2 · Investigate pressure, volume, and temperature relationships (published written lesson)
• F2.3 · Solve problems with major gas laws and the ideal gas law (published written lesson)
• F2.4 · Solve stoichiometry problems involving gases (published written lesson)
• F2.5 · Determine gas molar volume or molar mass through inquiry (published written lesson)
• F3.1 · Identify major and minor components of Earth’s atmosphere (published written lesson)
• F3.2 · Explain states of matter using interparticle forces (published written lesson)
• F3.3 · Explain gas behaviour using kinetic molecular theory (published written lesson)
• F3.4 · Describe relationships among ideal-gas variables (published written lesson)
• F3.5 · Explain Boyle’s, Charles’s, Gay-Lussac’s, combined, Dalton’s, and ideal gas laws (published written lesson)
• F3.6 · Explain Avogadro’s hypothesis and its contribution to gas chemistry (published written lesson)

Chlorine is 75.77% chlorine-35 and 24.23% chlorine-37. Estimate its relative atomic mass.

Worked method: Use a weighted average: (0.7577)(35 u) + (0.2423)(37 u) = 35.48 u.

Balance the synthesis reaction Al(s) + O₂(g) → Al₂O₃(s).

Worked method: Balance oxygen and aluminium without changing subscripts: 4Al(s) + 3O₂(g) → 2Al₂O₃(s). Each side has four Al atoms and six O atoms.

For 2H₂(g) + O₂(g) → 2H₂O(g), how many moles of water can form from 3.0 mol O₂ when H₂ is in excess?

Worked method: The balanced equation gives 2 mol H₂O per 1 mol O₂. Therefore 3.0 mol O₂ × 2 = 6.0 mol H₂O.

Find the number of molecules and mass in 0.50 mol CO₂.

What volume of 2.0 mol/L stock solution is needed to prepare 250 mL of a 0.40 mol/L solution?