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Curriculum-aligned learning support — not an official school, university, or ministry-approved course, and not a replacement for official credit.

Grade 11 · Chemistry · Core

Chemistry 11

BC Chemistry 11 across measurement and dimensional analysis, chemical nomenclature, the mole, chemical reactions, stoichiometric calculations, atomic structure and bonding, and solution chemistry and organic chemistry, plus a foundations-review unit for safety and physical changes and units in development for green chemistry, applications and analysis techniques.

Contents

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1

Measurement and Dimensional Analysis

5 of 5 published

  1. 1.1
    The factor-label method

    The factor-label method: single and multi-step conversions using conversion factors.

    Published

  2. 1.2
    SI base units and metric prefixes

    Base units, prefixes and converting between metric prefixes.

    Published

  3. 1.3
    Derived quantities and density

    Combining units into derived quantities; density and floating vs sinking.

    Published

  4. 1.4
    Significant figures in calculations

    Counting significant figures and rounding correctly in calculations.

    Published

  5. 1.5
    Reading scales and uncertainty

    Reading a measuring scale and reporting a value with its experimental uncertainty.

    Published

2

Nature of Science and Matter

2 of 2 published

  1. 2.1
    Qualitative and quantitative observation

    Qualitative vs quantitative; observation, hypothesis, theory and law.

    Published

  2. 2.2
    Physical and chemical properties of matter

    Physical vs chemical properties; intensive vs extensive properties.

    Published

3

Chemical Nomenclature

4 of 4 published

  1. 3.1
    Element names and symbols

    Element names and the rules behind their one- and two-letter symbols.

    Published

  2. 3.2
    Valence electrons, ions and ionic formulas

    Monatomic and polyatomic ions; building a formula from a compound name.

    Published

  3. 3.3
    Naming ionic compounds and hydrates

    Naming from a formula (Stock system) and naming hydrates.

    Published

  4. 3.4
    Naming molecular compounds and acids

    The prefix-naming system, common acids and the colours of aqueous ions.

    Published

4

The Mole Concept

6 of 6 published

  1. 4.1
    Atomic masses and Avogadro's hypothesis

    Relative atomic mass and how equal gas volumes reveal atomic masses.

    Published

  2. 4.2
    The mole and molar mass

    Defining the mole and finding the molar mass of a compound.

    Published

  3. 4.3
    Moles, mass, volume and particles

    Converting between moles, mass, gas volume at STP and number of particles.

    Published

  4. 4.4
    Percentage composition

    Finding the mass percent of each element in a compound.

    Published

  5. 4.5
    Empirical and molecular formulae

    Finding the simplest ratio and then the true molecular formula.

    Published

  6. 4.6
    Molar concentration and dilution

    Molarity, making up solutions and dilution calculations.

    Published

5

Chemical Reactions

5 of 5 published

  1. 5.1
    Equations and the conservation laws

    What a chemical equation shows and the laws it must obey.

    Published

  2. 5.2
    Balancing chemical equations

    Balancing by inspection, step by step.

    Published

  3. 5.3
    Phases and word equations

    Adding state symbols and translating chemical word equations.

    Published

  4. 5.4
    Predicting the products of chemical reactions

    Synthesis, decomposition, single/double replacement, neutralization, combustion.

    Published

  5. 5.5
    Reactions and energy changes (ΔH)

    Endothermic vs exothermic reactions and enthalpy.

    Published

6

Stoichiometric Calculations

4 of 4 published

  1. 6.1
    Mole ratios from balanced equations

    Reading mole ratios from a balanced equation.

    Published

  2. 6.2
    Mass, gas-volume and molecule stoichiometry

    The mole bridge: converting between two chemicals in a reaction.

    Published

  3. 6.3
    Stoichiometry in aqueous solutions: titration

    Reaction calculations involving solutions and titration.

    Published

  4. 6.4
    Limiting and excess reactants, yield and purity

    Limiting and excess reactants, percentage yield and percentage purity.

    Published

7

Atomic Structure and Chemical Bonding

6 of 7 published

  1. 7.1
    The structure of the atom

    Early models through the Rutherford-Bohr nuclear atom.

    Published

  2. 7.2
    Atomic number, mass and isotopes

    Protons, neutrons, electrons, isotopes and average atomic mass.

    Published

  3. 7.3
    Quantum model and electron configuration

    Energy levels, orbitals and writing electron configurations.

    Published

  4. 7.4
    Periodic trends and electronegativity

    Organizing the elements; trends in size, ionization energy and electronegativity.

    Published

  5. 7.5
    Valence electrons, Lewis structures and chemical bonding

    Ionic, covalent and metallic bonding; drawing Lewis structures.

    Published

  6. 7.6
    Chemical families

    Properties of the noble gases, alkali metals, alkaline earth metals and halogens.

    Published

  7. 7.7
    Molecular geometry and VSEPR theory

    Predicting the shape of a molecule from its electron domains using VSEPR (valence shell electron pair repulsion) theory.

    In review

8

Solution Chemistry

5 of 6 published

  1. 8.1
    Solutions and solubility

    Solute, solvent, saturation and the meaning of solubility.

    Published

  2. 8.2
    Dissociation and electrolytes

    Electrolytes, ions and why some solutions conduct electricity.

    Published

  3. 8.3
    Bonding, electronegativity and molecular polarity

    Dipole-dipole forces and hydrogen bonding.

    Published

  4. 8.4
    Polar and nonpolar solvents

    "Like dissolves like" and how ionic solids dissolve in water.

    Published

  5. 8.5
    Stoichiometry in aqueous solutions: molarity and dilution

    Finding ion concentrations from dissociation and mixing.

    Published

  6. 8.6
    Intermolecular forces and physical properties

    Dispersion forces, dipole-dipole forces and hydrogen bonding compared, and how intermolecular forces (as distinct from intramolecular bonds) affect boiling and melting points.

    In review

9

Organic Chemistry

5 of 6 published

  1. 9.1
    Organic compounds: alkanes

    Why carbon is special; naming straight-chain, branched and cyclic alkanes.

    Published

  2. 9.2
    Alkyl halides

    Naming and properties of halogen-substituted hydrocarbons.

    Published

  3. 9.3
    Alkenes and alkynes

    Double and triple bonds, naming and cis-trans isomerism.

    Published

  4. 9.4
    Aromatic compounds

    Benzene, resonance and naming aromatic molecules.

    Published

  5. 9.5
    Functional groups

    Alcohols, aldehydes, ketones, acids, esters, ethers, amines and more.

    Published

  6. 9.6
    Applications of organic chemistry

    Pharmaceuticals, petrochemicals, polymers, cosmetics, agriculture, food and biotechnology, and the traditional plant-based medicines of First Peoples.

    In preparation

10

Chemical Processes and Green Chemistry

0 of 3 published

  1. 10.1
    Local and other chemical processes

    Smelting, pulp and paper, food chemistry, photosynthesis and respiration, petrochemical smog, and the traditional practices of First Peoples (tanning hides, food, soap, natural bleach).

    In preparation

  2. 10.2
    Green chemistry

    Sustainable processes and technologies that reduce environmental impact.

    In preparation

  3. 10.3
    Analysis techniques

    Testing water quality for dissolved oxygen, pH, nitrates and phosphorus.

    In preparation

11

Foundations Review: Safety and Physical ChangesFoundations review, not counted toward course totals

6 of 6 published

  1. 11.1
    Emergency and protective equipment

    Eyewash, safety showers, alarms, evacuation, goggles and fume hoods, including which actions require trained, authorized responders.

    Published

  2. 11.2
    Fire, hazards and safe conduct

    Handling fires, common lab hazards, safe disposal and the rules of a conscious safety attitude.

    Published

  3. 11.3
    The classification of matter

    Elements, compounds, solutions and mechanical mixtures.

    Published

  4. 11.4
    The physical separation of substances

    Filtration, distillation, extraction, chromatography and more.

    Published

  5. 11.5
    Phase changes

    Melting, boiling and the heating curve of a pure substance.

    Published

  6. 11.6
    Kinetic energy and phase changes

    How molecular kinetic energy drives physical and phase changes.

    Published

What is Chemistry 11 in British Columbia?

Short answer

Chemistry 11 is the BC senior-science course that builds the quantitative foundation of chemistry — measurement and lab safety, naming compounds, the mole and molar mass, balancing reactions, stoichiometry, atomic structure and periodic trends, solutions, and an introduction to organic chemistry. It prepares students for Chemistry 12 and AP Chemistry.

Course overview

Chemistry 11 moves students from describing matter to reasoning about it numerically. You learn to name and write chemical formulas, count particles with the mole, balance equations, and use stoichiometry to predict how much product a reaction yields. Alongside the calculations you build a mental model of the atom and the periodic table that explains why elements behave as they do.

What you will learn

  • Name ionic and molecular compounds and write correct chemical formulas
  • Convert confidently between mass, moles, and number of particles
  • Balance chemical equations and classify reaction types
  • Solve stoichiometry problems, including limiting-reactant reasoning
  • Relate atomic structure and periodic trends to chemical behaviour
  • Describe solutions quantitatively (concentration and dilution)

Who this course is for

  • • BC students taking Chemistry 11 who want deeper understanding than rote memorization
  • • Students preparing for Chemistry 12 and, later, AP Chemistry
  • • Anyone who finds the mole, nomenclature, or stoichiometry confusing and wants targeted practice

Commonly difficult topics

  • • The mole concept — treating it as a bridge between mass and particle count rather than a magic number
  • • Nomenclature — keeping ionic vs molecular naming rules straight
  • • Stoichiometry — setting up mole ratios and identifying the limiting reactant
  • • Significant figures and units in quantitative work

How Dr. Shreyank Educare teaches this course

  1. 01 · Diagnose

    Find the exact skill causing difficulty — not the chapter, the skill.

  2. 02 · Understand

    Learn it through explanations, worked examples and visual reasoning.

  3. 03 · Practice

    Work problems that adapt to how you are actually doing.

  4. 04 · Fix

    A wrong answer becomes targeted remediation for the misconception behind it.

  5. 05 · Prove

    Solve new, unseen problems independently before mastery is awarded.

Course curriculum

1Measurement and Dimensional Analysis5 topics
  • — The factor-label method
  • — SI base units and metric prefixes
  • — Derived quantities and density
  • — Significant figures in calculations
  • — Reading scales and uncertainty
2Nature of Science and Matter2 topics
  • — Qualitative and quantitative observation
  • — Physical and chemical properties of matter
3Chemical Nomenclature4 topics
  • — Element names and symbols
  • — Valence electrons, ions and ionic formulas
  • — Naming ionic compounds and hydrates
  • — Naming molecular compounds and acids
4The Mole Concept6 topics
  • — Atomic masses and Avogadro's hypothesis
  • — The mole and molar mass
  • — Moles, mass, volume and particles
  • — Percentage composition
  • — Empirical and molecular formulae
  • — Molar concentration and dilution
5Chemical Reactions5 topics
  • — Equations and the conservation laws
  • — Balancing chemical equations
  • — Phases and word equations
  • — Predicting the products of chemical reactions
  • — Reactions and energy changes (ΔH)
6Stoichiometric Calculations4 topics
  • — Mole ratios from balanced equations
  • — Mass, gas-volume and molecule stoichiometry
  • — Stoichiometry in aqueous solutions: titration
  • — Limiting and excess reactants, yield and purity
7Atomic Structure and Chemical Bonding7 topics
  • — The structure of the atom
  • — Atomic number, mass and isotopes
  • — Quantum model and electron configuration
  • — Periodic trends and electronegativity
  • — Valence electrons, Lewis structures and chemical bonding
  • — Chemical families
  • — Molecular geometry and VSEPR theory
8Solution Chemistry6 topics
  • — Solutions and solubility
  • — Dissociation and electrolytes
  • — Bonding, electronegativity and molecular polarity
  • — Polar and nonpolar solvents
  • — Stoichiometry in aqueous solutions: molarity and dilution
  • — Intermolecular forces and physical properties
9Organic Chemistry6 topics
  • — Organic compounds: alkanes
  • — Alkyl halides
  • — Alkenes and alkynes
  • — Aromatic compounds
  • — Functional groups
  • — Applications of organic chemistry
10Chemical Processes and Green Chemistry3 topics
  • — Local and other chemical processes
  • — Green chemistry
  • — Analysis techniques
11Foundations Review: Safety and Physical Changes6 topics
  • — Emergency and protective equipment
  • — Fire, hazards and safe conduct
  • — The classification of matter
  • — The physical separation of substances
  • — Phase changes
  • — Kinetic energy and phase changes

A sample learning experience

How many moles of water are produced when 4.0 g of hydrogen gas (H₂) reacts completely with oxygen? (Molar mass of H₂ ≈ 2.0 g/mol.)

  1. 1. Write the balanced equation: 2 H₂ + O₂ → 2 H₂O.
  2. 2. Convert mass of H₂ to moles: 4.0 g ÷ 2.0 g/mol = 2.0 mol H₂.
  3. 3. Use the mole ratio: 2 mol H₂ produces 2 mol H₂O, so the ratio is 1:1.
  4. 4. Therefore 2.0 mol H₂ produces 2.0 mol H₂O.

Frequently asked questions

Is Chemistry 11 hard?
The concepts are approachable, but Chemistry 11 is the first course where you must reason quantitatively. Most students find the mole and stoichiometry challenging at first; with targeted practice on those specific skills, the course becomes much more manageable.
What math do I need for Chemistry 11?
Comfort with ratios, unit conversion, scientific notation, and basic algebra is enough. You rearrange simple equations and track units carefully — the arithmetic itself is not advanced.
How is Chemistry 11 different from Chemistry 12?
Chemistry 11 builds the foundation (the mole, reactions, stoichiometry, atomic structure). Chemistry 12 goes deeper into reaction rates, equilibrium, acids and bases, and electrochemistry, assuming you can already do the Chemistry 11 quantitative work.
Do I need Chemistry 11 for AP Chemistry?
It is strongly recommended. AP Chemistry assumes fluency with moles, stoichiometry, and atomic structure — all core Chemistry 11 skills — and then adds college-level depth and problem difficulty.
What is the best way to study for Chemistry 11?
Practise the specific skill you are weak on rather than re-reading notes. Diagnose which step of a problem you miss (naming, mole conversion, mole ratio, or units), then drill that step until it is automatic.

Related courses

Chemistry 12 →AP Chemistry →

Explore all Chemistry courses →

Curriculum & sources

Content source: original lessons, worked examples and diagrams created for Dr. Shreyank Educare.

Curriculum alignment: Grade 11 Chemistry (BC curriculum).

Curriculum-aligned learning support — not an official school, ministry, or College Board course, and not a replacement for official credit.

Last updated . Authored and maintained in-house by the Dr. Shreyank Educare teaching team — see our editorial standards, methodology and source policy.