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Ontario Grade 12 Chemistry (SCH4U) course and lessons
Study Ontario SCH4U through organic chemistry, structure and properties of matter, energy changes and reaction rates, chemical equilibrium, and electrochemistry. The complete expectation map helps you find an exact topic.
Publication status
3 of 85 written lessons published
The topic map covers the course expectations. A topic marked “written lesson not published” remains available for practice and tutoring, but does not have a reviewed written lecture yet.
SCH4U study path
Build from organic molecules to electrochemical cells
Functional groups, IUPAC names, isomers, organic reactions, and polymers.
Electron configurations, VSEPR shapes, polarity, bonding, and intermolecular forces.
Calorimetry, enthalpy, Hess’s law, collision theory, and catalysts.
Dynamic systems, Le Châtelier’s principle, equilibrium constants, acids and bases, and buffers.
Redox balancing, galvanic cells, standard potentials, corrosion, and applications.
Review the SCH3U prerequisite · Compare Alberta Chemistry 30 · Browse all courses
Free published lessons
Start learning SCH4U
These lessons are public, free to read, and connected to the full course map below.
A polymer is a long molecule assembled from repeating building blocks called monomers. In SCH4U, the useful first question is what…
A calorimeter lets us estimate heat transferred during a process by measuring a temperature change in a surrounding substance, often…
A table of standard reduction potentials lists half-reactions as reductions. To predict whether a proposed redox reaction is…
SCH4U
Topics by strand
Plan, perform, analyse, and communicate chemistry investigations safely, and explore related careers.
- A1.1 · Form scientific questions, predictions, and testable hypotheses (written lesson not published)
- A1.2 · Choose suitable chemistry equipment, materials, and procedures (written lesson not published)
- A1.3 · Find appropriate print and electronic research sources (written lesson not published)
- A1.4 · Plan investigations using safe laboratory practices and WHMIS (written lesson not published)
- A1.5 · Conduct inquiries safely while controlling relevant variables (written lesson not published)
- A1.6 · Record and organize accurate data in suitable formats (written lesson not published)
- A1.7 · Organize research information and document sources (written lesson not published)
- A1.8 · Analyse evidence, solve quantitative problems, and evaluate error (written lesson not published)
- A1.9 · Evaluate research sources for accuracy, reliability, and bias (written lesson not published)
- A1.10 · Draw and justify conclusions from inquiry and research evidence (written lesson not published)
- A1.11 · Communicate chemistry procedures, results, and conclusions clearly (written lesson not published)
- A1.12 · Use suitable numeric, symbolic, graphical, and unit representations (written lesson not published)
- A1.13 · Report calculations with suitable precision and significant figures (written lesson not published)
- A2.1 · Explore chemistry-related careers and required education (written lesson not published)
- A2.2 · Describe contributions of chemists, including Canadians (written lesson not published)
Connect functional groups and molecular structures to names, properties, reactions, and environmental impacts.
- B1.1 · Assess health, social, and environmental impacts of common organic compounds (written lesson not published)
- B1.2 · Propose actions to reduce use of harmful organic compounds (written lesson not published)
- B2.1 · Use functional-group, hydrocarbon, isomer, and polymer terminology (written lesson not published)
- B2.2 · Name and draw structures of the specified organic compound classes (written lesson not published)
- B2.3 · Build models of simple organic molecules (written lesson not published)
- B2.4 · Investigate and analyse organic reactions (written lesson not published)
- B3.1 · Compare organic classes by names and structural formulas (written lesson not published)
- B3.2 · Compare physical properties within organic compound classes (written lesson not published)
- B3.3 · Explain substitution, addition, elimination, oxidation, esterification, and hydrolysis (written lesson not published)
- B3.4 · Distinguish addition from condensation polymerization (published written lesson)
- B3.5 · Relate organic isomers and their properties to molecular structures (written lesson not published)
Use electron configurations, VSEPR, polarity, and bonding forces to explain substance properties.
- C1.1 · Assess benefits of atomic- and molecular-structure technologies (written lesson not published)
- C1.2 · Evaluate benefits and environmental impacts of specialized materials (written lesson not published)
- C2.1 · Use orbital, spectrum, energy-level, photon, and dipole terminology (written lesson not published)
- C2.2 · Write electron configurations using Pauli, Hund, and aufbau rules (written lesson not published)
- C2.3 · Predict and diagram simple molecular and ionic shapes with VSEPR (written lesson not published)
- C2.4 · Predict molecular polarity from shape and electronegativity (written lesson not published)
- C2.5 · Predict solid type and properties from bonding (written lesson not published)
- C2.6 · Investigate substance properties to infer bonding type (written lesson not published)
- C3.1 · Explain evidence behind Rutherford and Bohr atomic models (written lesson not published)
- C3.2 · Explain shell and subshell electron configurations (written lesson not published)
- C3.3 · Link s-, p-, and d-block properties to electron configurations (written lesson not published)
- C3.4 · Explain physical properties using particles and inter- and intramolecular forces (written lesson not published)
- C3.5 · Describe a Canadian contribution to atomic or molecular theory (written lesson not published)
Reason with heat, enthalpy, Hess’s law, collision theory, catalysts, and reaction rates.
- D1.1 · Evaluate energy technologies for efficiency and environmental effects (written lesson not published)
- D1.2 · Analyse reaction conditions that improve efficiency and sustainability (written lesson not published)
- D2.1 · Use enthalpy, activation-energy, and heat-capacity terminology (written lesson not published)
- D2.2 · Write thermochemical equations with ΔH or heat terms (written lesson not published)
- D2.3 · Calculate reaction heat with Q = mcΔT (published written lesson)
- D2.4 · Plan calorimetry, compare measured and theoretical heat, and evaluate error (written lesson not published)
- D2.5 · Solve reaction-energy problems with Hess’s law (written lesson not published)
- D2.6 · Test Hess’s law with an investigation (written lesson not published)
- D2.7 · Find reaction enthalpy from standard enthalpies of formation (written lesson not published)
- D2.8 · Investigate how conditions affect reaction rate (written lesson not published)
- D3.1 · Compare energy transfer in physical, chemical, and nuclear changes (written lesson not published)
- D3.2 · Explain energy absorbed in bond breaking and released in bond formation (written lesson not published)
- D3.3 · Relate heat transfer to mass, heat capacity, and temperature change (written lesson not published)
- D3.4 · State and explain Hess’s law (written lesson not published)
- D3.5 · Explain reaction-rate factors with collision theory and energy diagrams (written lesson not published)
- D3.6 · Interpret simple reaction potential-energy diagrams (written lesson not published)
- D3.7 · Relate overall reaction rate to elementary reaction steps (written lesson not published)
Connect dynamic equilibrium, shifts, constants, acid–base systems, solubility, and buffers.
- E1.1 · Analyse optimal conditions for natural or industrial equilibrium processes (written lesson not published)
- E1.2 · Assess equilibrium impacts in biological and technological systems (written lesson not published)
- E2.1 · Use reversible-reaction, equilibrium-constant, solubility, and buffer terminology (written lesson not published)
- E2.2 · Predict and investigate equilibrium shifts from changing conditions (written lesson not published)
- E2.3 · Determine an equilibrium constant by inquiry (written lesson not published)
- E2.4 · Solve equilibrium-concentration, solubility, and pH calculations (written lesson not published)
- E2.5 · Solve acid–base equilibrium problems using titration and equivalence-point data (written lesson not published)
- E3.1 · Explain dynamic equilibrium in physical and chemical systems (written lesson not published)
- E3.2 · Explain reactant and product concentrations at chemical equilibrium (written lesson not published)
- E3.3 · Explain Le Châtelier’s principle and equilibrium shifts (written lesson not published)
- E3.4 · Write expressions for common equilibrium constants (written lesson not published)
- E3.5 · Use water ionization to calculate pH, pOH, and ion concentrations (written lesson not published)
- E3.6 · Explain Brønsted–Lowry acids and bases (written lesson not published)
- E3.7 · Compare strong and weak acids and bases using equilibrium (written lesson not published)
- E3.8 · Describe the chemical characteristics of buffer solutions (written lesson not published)
Balance redox reactions, model galvanic cells, predict cell potentials, and evaluate applications.
- F1.1 · Assess viability and impacts of electrochemical energy technologies (written lesson not published)
- F1.2 · Analyse electrochemistry-related health and safety issues (written lesson not published)
- F2.1 · Use half-reaction, cell, oxidant, reductant, and oxidation-number terminology (written lesson not published)
- F2.2 · Investigate a redox reaction qualitatively (written lesson not published)
- F2.3 · Balance redox equations using oxidation numbers and half-reactions (written lesson not published)
- F2.4 · Build a galvanic cell and measure its potential (written lesson not published)
- F2.5 · Draw and analyse labelled galvanic-cell diagrams (written lesson not published)
- F2.6 · Predict redox spontaneity from standard reduction potentials (published written lesson)
- F3.1 · Explain redox with electron transfer and oxidation numbers (written lesson not published)
- F3.2 · Explain the components and functions of a galvanic cell (written lesson not published)
- F3.3 · Relate half-cell voltages to overall cell potential (written lesson not published)
- F3.4 · Explain the standard hydrogen half-cell reference (written lesson not published)
- F3.5 · Explain industrial electrochemistry applications (written lesson not published)
- F3.6 · Explain electrochemical corrosion and prevention methods (written lesson not published)
Worked examples
Start with worked Grade 12 examples
These original examples introduce selected SCH4U expectations. The full expectation map is not a complete set of published written lessons or a substitute for official course materials and assignments. The strand-prefixed labels below identify the matching Ontario specific expectations; titles are concise study-guide paraphrases.
Name CH₃–CH₂–OH and identify its functional group.
Worked method: The two-carbon parent is ethane. The –OH group makes it an alcohol, so its IUPAC name is ethanol.
فارسی · توضیح مثال
CH₃–CH₂–OH را نامگذاری کنید و گروه عاملی آن را مشخص کنید. زنجیر اصلی دو کربن دارد و اتان است. گروه –OH آن را به الکل تبدیل میکند؛ نام IUPAC آن اتانول است.
If A → B has ΔH = −40 kJ and B → C has ΔH = +15 kJ, find ΔH for A → C.
Worked method: Add the reactions so B cancels. Enthalpy is a state function, so ΔH = −40 kJ + 15 kJ = −25 kJ for A → C.
فارسی · توضیح مثال
اگر ΔH برای A → B برابر −40 kJ و برای B → C برابر +15 kJ باشد، ΔH واکنش A → C را بیابید. دو واکنش را جمع کنید تا B حذف شود. آنتالپی تابع حالت است؛ پس ΔH برای A → C برابر −40 + 15 = −25 kJ است.
A galvanic cell has a cathode reduction potential of +0.34 V and an anode reduction potential of −0.76 V. Find the standard cell potential.
Worked method: E°cell = E°cathode − E°anode = +0.34 V − (−0.76 V) = +1.10 V. The positive result is consistent with a spontaneous galvanic cell.
فارسی · توضیح مثال
پتانسیل کاهش کاتد یک پیل گالوانی +0.34 V و پتانسیل کاهش آند −0.76 V است. پتانسیل استاندارد پیل را بیابید. E°پیل = E°کاتد − E°آند = +0.34 V − (−0.76 V) = +1.10 V. نتیجه مثبت با خودبهخودی بودن پیل گالوانی سازگار است.
Try independently, then check
Write your own solution before opening each answer. If a step is unclear, review the matching expectation or a Grade 11 prerequisite.
At equilibrium, [H₂] = 0.20 mol/L, [I₂] = 0.20 mol/L, and [HI] = 0.80 mol/L for H₂(g) + I₂(g) ⇌ 2HI(g). Find Kc.
Show worked answer
Kc = [HI]²/([H₂][I₂]) = (0.80)²/((0.20)(0.20)) = 16.
فارسی · تمرین و پاسخ
در تعادل واکنش H₂(g) + I₂(g) ⇌ 2HI(g)، غلظتهای H₂ و I₂ هرکدام ۰٫۲۰ مول بر لیتر و غلظت HI برابر ۰٫۸۰ مول بر لیتر است. Kc را بیابید. Kc = [HI]²/([H₂][I₂]) = (0.80)²/((0.20)(0.20)) = 16.
A 100 g water sample warms by 5.0 °C. If c = 4.18 J/(g·°C), how much heat does the water absorb?
Show worked answer
q = mcΔT = (100 g)(4.18 J/(g·°C))(5.0 °C) = 2.09 × 10³ J, or 2.1 kJ to two significant figures.
فارسی · تمرین و پاسخ
دماى ۱۰۰ گرم آب ۵٫۰ °C افزایش مییابد. اگر c = 4.18 J/(g·°C) باشد، آب چقدر گرما جذب میکند؟ q = mcΔT = (100 g)(4.18 J/(g·°C))(5.0 °C) = 2.09 × 10³ J، یعنی با دو رقم معنادار 2.1 kJ.
Scientific investigation processes across expectations
These processes are practised throughout the course, rather than listed as separate lessons.
- Initiating and planning: ask testable questions, predict, identify variables, and select safe procedures and materials (آغاز و برنامهریزی: طرح پرسش آزمونپذیر، پیشبینی، تشخیص متغیرها و انتخاب روش و مواد ایمن)
- Performing and recording: follow safe procedures, control variables, and organize observations and measurements (اجرا و ثبت: پیروی از روش ایمن، کنترل متغیرها و سازماندهی مشاهدهها و اندازهگیریها)
- Analysing and interpreting: calculate from evidence, evaluate error and sources, and justify conclusions (تحلیل و تفسیر: محاسبه با شواهد، ارزیابی خطا و منابع و توجیه نتیجه)
- Communicating: use correct formulas, equations, states, charges, units, significant figures, tables, and graphs (ارتباط علمی: استفاده درست از فرمول، معادله، حالت، بار، یکا، ارقام معنادار، جدول و نمودار)
Source and coverage
Prerequisite: Chemistry, Grade 11, University Preparation (SCH3U). Confirm your current school timetable and admission requirements.
The expectation map follows the official Ontario chemistry curriculum. Titles are concise study-guide paraphrases; consult the official source for exact requirements. Browse all courses.
Sources and editorial process
Curriculum-aligned and reviewed before publication
This independent study guide follows the official course source. It is not an official government, school, or university publication.
Lessons may be AI-assisted or editorially prepared. Published content is checked for structure, notation, calculations, course boundaries, and readability before release. Because corrections can still be necessary, readers can report a problem.