Ontario Curriculum
B.2.1: use appropriate terminology related to chemical trends and chemical bonding, including, but not limited to: atomic radius, effective nuclear charge, electronegativity, ionization energy, and electron affinity
Charge Launcher
Covalent Bonds
Electron Configuration
Ionic Bonds
B.2.2: analyse data related to the properties of elements within a period (e.g., ionization energy, atomic radius) to identify general trends in the periodic table
Electron Configuration
Element Builder
B.2.5: predict the nature of a bond (e.g., non-polar covalent, polar covalent, ionic), using electronegativity values of atoms
B.2.6: build molecular models, and write structural formulae, for molecular compounds containing single and multiple bonds (e.g., CO2, H2O, C2H4), and for ionic crystalline structures (e.g., NaCl)
Covalent Bonds
Dehydration Synthesis
Ionic Bonds
B.2.7: write chemical formulae of binary and polyatomic compounds, including those with multiple valences, and name the compounds using the International Union of Pure and Applied Chemistry (IUPAC) nomenclature system
Covalent Bonds
Dehydration Synthesis
Ionic Bonds
Stoichiometry
B.3.1: explain the relationship between the atomic number and the mass number of an element, and the difference between isotopes and radioisotopes of an element
Electron Configuration
Element Builder
Nuclear Decay
B.3.2: explain the relationship between isotopic abundance of an element?s isotopes and the relative atomic mass of the element
B.3.3: state the periodic law, and explain how patterns in the electron arrangement and forces in atoms result in periodic trends (e.g., in atomic radius, ionization energy, electron affinity, electronegativity) in the periodic table
Bohr Model of Hydrogen
Bohr Model: Introduction
Electron Configuration
Element Builder
Ionic Bonds
B.3.4: explain the differences between the formation of ionic bonds and the formation of covalent bonds
Covalent Bonds
Dehydration Synthesis
Ionic Bonds
C.2.1: use appropriate terminology related to chemical reactions, including, but not limited to: neutralization, precipitate, acidic, and basic
C.2.2: write balanced chemical equations to represent synthesis, decomposition, single displacement, double displacement, and combustion reactions, using the IUPAC nomenclature system
Balancing Chemical Equations
Chemical Equation Balancing
Dehydration Synthesis
C.2.3: investigate synthesis, decomposition, single displacement, and double displacement reactions, by testing the products of each reaction (e.g., test for products such as gases, the presence of an acid, or the presence of a base)
Balancing Chemical Equations
Dehydration Synthesis
C.2.4: predict the products of different types of synthesis and decomposition reactions (e.g., synthesis reactions in which simple compounds are formed; synthesis reactions of metallic or non-metallic oxides with water; decomposition reactions, in which a chemical compound is separated into several compounds)
Balancing Chemical Equations
Dehydration Synthesis
Ionic Bonds
C.2.5: predict the products of single displacement reactions, using the metal activity series and the halogen series
C.2.6: predict the products of double displacement reactions (e.g., the formation of precipitates or gases; neutralization)
C.2.8: plan and conduct an inquiry to compare the properties of non-metal oxide solutions and metal oxide solutions (e.g., carbon dioxide reacts with water to make water acidic; magnesium oxide reacts with water to make water basic)
Electron Configuration
Element Builder
Ionic Bonds
C.2.10: plan and conduct an inquiry to demonstrate a single displacement reaction, using elements from the metal activity series
Balancing Chemical Equations
Element Builder
C.3.1: identify various types of chemical reactions, including synthesis, decomposition, single displacement, double displacement, and combustion
Balancing Chemical Equations
Dehydration Synthesis
C.3.3: explain the chemical reactions that result in the formation of acids and bases from metal oxides and non-metal oxides (e.g., calcium oxide reacts with water to produce a basic solution; carbon dioxide reacts with water to produce an acidic solution)
Electron Configuration
Ionic Bonds
pH Analysis
pH Analysis: Quad Color Indicator
D.1.1: analyse processes in the home, the workplace, and the environmental sector that involve the use of chemical quantities and calculations (e.g., mixing household cleaning solutions, calculating chemotherapy doses, monitoring pollen counts)
Covalent Bonds
Dehydration Synthesis
Ionic Bonds
D.2.1: use appropriate terminology related to quantities in chemical reactions, including, but not limited to: stoichiometry, percentage yield, limiting reagent, mole, and atomic mass
Limiting Reactants
Stoichiometry
D.2.2: conduct an inquiry to calculate the percentage composition of a compound (e.g., a hydrate)
Covalent Bonds
Dehydration Synthesis
Ionic Bonds
D.2.3: solve problems related to quantities in chemical reactions by performing calculations involving quantities in moles, number of particles, and atomic mass
Limiting Reactants
Stoichiometry
D.2.4: determine the empirical formulae and molecular formulae of various chemical compounds, given molar masses and percentage composition or mass data
Covalent Bonds
Dehydration Synthesis
Ionic Bonds
Stoichiometry
D.2.5: calculate the corresponding mass, or quantity in moles or molecules, for any given reactant or product in a balanced chemical equation as well as for any other reactant or product in the chemical reaction
Balancing Chemical Equations
Chemical Equation Balancing
Dehydration Synthesis
Ionic Bonds
Stoichiometry
D.2.6: solve problems related to quantities in chemical reactions by performing calculations involving percentage yield and limiting reagents
D.2.7: conduct an inquiry to determine the actual yield, theoretical yield, and percentage yield of the products of a chemical reaction (e.g., a chemical reaction between steel wool and copper(II) sulfate solution), assess the effectiveness of the procedure, and suggest sources of experimental error
D.3.1: explain the law of definite proportions
D.3.2: describe the relationships between Avogadro?s number, the mole concept, and the molar mass of any given substance
D.3.3: explain the relationship between the empirical formula and the molecular formula of a chemical compound
Covalent Bonds
Dehydration Synthesis
Ionic Bonds
Stoichiometry
D.3.4: explain the quantitative relationships expressed in a balanced chemical equation, using appropriate units of measure (e.g., moles, grams, atoms, ions, molecules)
Balancing Chemical Equations
Chemical Equation Balancing
Stoichiometry
E.1.1: analyse the origins and cumulative effects of pollutants that enter our water systems (e.g., landfill leachates, agricultural run-off, industrial effluents, chemical spills), and explain how these pollutants affect water quality
E.2.1: use appropriate terminology related to aqueous solutions and solubility, including, but not limited to: concentration, solubility, precipitate, ionization, dissociation, pH, dilute, solute, and solvent
Colligative Properties
Solubility and Temperature
pH Analysis
pH Analysis: Quad Color Indicator
E.2.2: solve problems related to the concentration of solutions by performing calculations involving moles, and express the results in various units (e.g., moles per litre, grams per 100 mL, parts per million or parts per billion, mass, volume per cent)
Colligative Properties
Density Laboratory
E.2.3: prepare solutions of a given concentration by dissolving a solid solute in a solvent or by diluting a concentrated solution
Colligative Properties
Freezing Point of Salt Water
E.2.4: conduct an investigation to analyse qualitative and quantitative properties of solutions (e.g., perform a qualitative analysis of ions in a solution)
Colligative Properties
Solubility and Temperature
E.2.5: write balanced net ionic equations to represent precipitation and neutralization reactions
Balancing Chemical Equations
Chemical Equation Balancing
E.2.6: use stoichiometry to solve problems involving solutions and solubility
E.2.8: conduct an investigation to determine the concentrations of pollutants in their local treated drinking water, and compare the results to commonly used guidelines and standards (e.g., provincial and federal standards)
E.3.2: explain the process of formation for solutions that are produced by dissolving ionic and molecular compounds (e.g., salt, oxygen) in water, and for solutions that are produced by dissolving non-polar solutes in non-polar solvents (e.g., grease in vegetable oil)
Dehydration Synthesis
Ionic Bonds
Pond Ecosystem
E.3.3: explain the effects of changes in temperature and pressure on the solubility of solids, liquids, and gases (e.g., explain how a change in temperature or atmospheric pressure affects the solubility of oxygen in lake water)
Phase Changes
Relative Humidity
Solubility and Temperature
E.3.4: identify, using a solubility table, the formation of precipitates in aqueous solutions (e.g., the use of iron or aluminum compounds to precipitate and remove phosphorus from wastewater)
E.3.5: explain the Arrhenius theory of acids and bases
pH Analysis
pH Analysis: Quad Color Indicator
E.3.6: explain the difference between strong and weak acids, and between strong and weak bases, in terms of degree of ionization
pH Analysis
pH Analysis: Quad Color Indicator
F.2.1: use appropriate terminology related to gases and atmospheric chemistry, including, but not limited to: standard temperature, standard pressure, molar volume, and ideal gas
F.2.2: determine, through inquiry, the quantitative and graphical relationships between the pressure, volume, and temperature of a gas
F.2.3: solve quantitative problems by performing calculations based on Boyle?s law, Charles?s law, Gay-Lussac?s law, the combined gas law, Dalton?s law of partial pressures, and the ideal gas law
F.2.4: use stoichiometry to solve problems related to chemical reactions involving gases (e.g., problems involving moles, number of atoms, number of molecules, mass, and volume)
Balancing Chemical Equations
Boyle's Law and Charles' Law
Chemical Equation Balancing
Limiting Reactants
Stoichiometry
F.2.5: determine, through inquiry, the molar volume or molar mass of a gas produced by a chemical reaction (e.g., the molar volume of hydrogen gas from the reaction of magnesium with hydrochloric acid)
F.3.2: describe the different states of matter, and explain their differences in terms of the forces between atoms, molecules, and ions
Covalent Bonds
Dehydration Synthesis
Ionic Bonds
Limiting Reactants
Phase Changes
F.3.3: use the kinetic molecular theory to explain the properties and behaviour of gases in terms of types and degrees of molecular motion
Boyle's Law and Charles' Law
Phase Changes
Temperature and Particle Motion
F.3.4: describe, for an ideal gas, the quantitative relationships that exist between the variables of pressure, volume, temperature, and amount of substance
F.3.5: explain Dalton?s law of partial pressures, Boyle?s law, Charles?s law, Gay-Lussac?s law, the combined gas law, and the ideal gas law
F.3.6: explain Avogadro?s hypothesis and how his contribution to the gas laws has increased our understanding of the chemical reactions of gases
Correlation last revised: 8/18/2015