Ontario Curriculum
A1.1: formulate relevant scientific questions about observed relationships, ideas, problems, or issues, make informed predictions, and/or formulate educated hypotheses to focus inquiries or research
Diffusion
Sight vs. Sound Reactions
A1.5: conduct inquiries, controlling relevant variables, adapting or extending procedures as required, and using appropriate materials and equipment safely, accurately, and effectively, to collect observations and data
A1.6: compile accurate data from laboratory and other sources, and organize and record the data, using appropriate formats, including tables, flow charts, graphs, and/or diagrams
A1.8: synthesize, analyse, interpret, and evaluate qualitative and/or quantitative data; solve problems involving quantitative data; determine whether the evidence supports or refutes the initial prediction or hypothesis and whether it is consistent with scientific theory; identify sources of bias and error; and suggest improvements to the inquiry to reduce the likelihood of error
A1.10: draw conclusions based on inquiry results and research findings, and justify their conclusions with reference to scientific knowledge
A1.13: express the results of any calculations involving data accurately and precisely, to the appropriate number of decimal places and significant figures
Unit Conversions 2 - Scientific Notation and Significant Digits
B3.3: explain the chemical changes that occur during various types of organic chemical reactions, including substitution, addition, elimination, oxidation, esterification, and hydrolysis
B3.4: explain the difference between an addition reaction and a condensation polymerization reaction
C2.1: use appropriate terminology related to structure and properties of matter, including, but not limited to: orbital, emission spectrum, energy level, photon, and dipole
C2.2: use the Pauli exclusion principle, Hund’s rule, and the aufbau principle to write electron configurations for a variety of elements in the periodic table
C3.1: explain how experimental observations and inferences made by Ernest Rutherford and Niels Bohr contributed to the development of the planetary model of the hydrogen atom
C3.2: describe the electron configurations of a variety of elements in the periodic table, using the concept of energy levels in shells and subshells, as well as the Pauli exclusion principle, Hund’s rule, and the aufbau principle
C3.3: identify the characteristic properties of elements in each of the s, p, and d blocks of the periodic table, and explain the relationship between the position of an element in the periodic table, its properties, and its electron configuration
D2.1: use appropriate terminology related to energy changes and rates of reaction, including, but not limited to: enthalpy, activation energy, endothermic, exothermic, potential energy, and specific heat capacity
Calorimetry Lab
Chemical Changes
Energy Conversion in a System
D2.5: solve problems related to energy changes in a chemical reaction, using Hess’s law
D2.6: conduct an inquiry to test Hess’s law (e.g., measure heats of reaction from the combustion of magnesium, and combine them to yield the “Delta”H value of the reaction)
D2.7: calculate the heat of reaction for a formation reaction, using a table of standard enthalpies of formation and applying Hess’s law
D2.8: plan and conduct an inquiry to determine how various factors (e.g., change in temperature, addition of a catalyst, increase in surface area of a solid reactant) affect the rate of a chemical reaction
D3.2: compare the energy change from a reaction in which bonds are formed to one in which bonds are broken, and explain these changes in terms of endothermic and exothermic reactions
D3.4: state Hess’s law, and explain, using examples, how it is applied to find the enthalpy changes of a reaction
D3.5: explain, using collision theory and potential energy diagrams, how factors such as temperature, the surface area of the reactants, the nature of the reactants, the addition of catalysts, and the concentration of the solution control the rate of a chemical reaction
D3.7: explain, with reference to a simple chemical reaction (e.g., combustion), how the rate of a reaction is determined by the series of elementary steps that make up the overall reaction mechanism
E1.2: assess the impact of chemical equilibrium processes on various biological, biochemical, and technological systems (e.g., remediation in areas of heavy metal contamination, development of gallstones, use of buffering in medications, use of barium sulfate in medical diagnosis)
Equilibrium and Concentration
Equilibrium and Pressure
E2.1: use appropriate terminology related to chemical systems and equilibrium, including, but not limited to: homogeneous, closed system, reversible reaction, equilibrium constant, equilibrium concentration, molar solubility, and buffer
Equilibrium and Concentration
Equilibrium and Pressure
E2.2: predict, applying Le Châtelier’s principle or the reaction quotient for a given reaction, how various factors (e.g., changes in volume, temperature, or concentration of reactants or products in a solution) would affect a chemical system at equilibrium, and conduct an inquiry to test those predictions
Equilibrium and Concentration
Equilibrium and Pressure
E2.3: conduct an inquiry to determine the value of an equilibrium constant for a chemical reaction (e.g., Keq for iron(III) thiocyanate, Ksp for calcium hydroxide, Ka for acetic acid)
Equilibrium and Concentration
Equilibrium and Pressure
E2.4: solve problems related to equilibrium by performing calculations involving concentrations of reactants and products (e.g., Keq, Ksp, Ka, pH, pOH, Kp, Kb)
E2.5: solve problems related to acid–base equilibrium, using acid–base titration data and the pH at the equivalence point
E3.1: explain the concept of dynamic equilibrium, using examples of physical and chemical equilibrium systems (e.g., liquid–vapour equilibrium, weak electrolytes in solution, reversible chemical reactions)
Equilibrium and Concentration
Equilibrium and Pressure
E3.2: explain the concept of chemical equilibrium and how it applies to the concentration of reactants and products in a chemical reaction at equilibrium
E3.3: explain Le Châtelier’s principle and how it applies to changes to a chemical reaction at equilibrium
Equilibrium and Concentration
Equilibrium and Pressure
E3.4: identify common equilibrium constants, including Keq, Ksp, Kw, Ka, Kb, and Kp, and write the expressions for each
E3.6: explain the Brønsted-Lowry theory of acids and bases
F2.1: use appropriate terminology related to electrochemistry, including, but not limited to: half-reaction, electrochemical cell, reducing agent, oxidizing agent, redox reaction, and oxidation number
Correlation last revised: 9/16/2020