Overall Expectations
D1. analyse technologies and chemical processes that are based on energy changes, and evaluate them in terms of their efficiency and their effects on the environment
D2. investigate and analyse energy changes and rates of reaction in physical and chemical processes, and solve related problems
D3. demonstrate an understanding of energy changes and rates of reaction
D2. investigate and analyse energy changes and rates of reaction in physical and chemical processes, and solve related problems
D3. demonstrate an understanding of energy changes and rates of reaction
Specific Expectations
D1.1 analyse some conventional and alternative energy technologies (e.g., fossil fuel–burning power plants, hydro-powered generators, solar panels, wind turbines, fuel cells), and evaluate them in terms of their efficiency and impact on the environment [AI, C]
D1.2 analyse the conditions (e.g. temperature, pressure, presence of a catalyst) required to maximize the efficiency of some common natural or industrial chemical reactions (e.g., decomposition, combustion, neutralization), and explain how the improved efficiency of the reaction contributes to environmental sustainability [AI, C]
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 [C]
D2.2 write thermochemical equations, expressing the energy change as a ∆H value or as a heat term in the equation [AI, C]
D2.3 solve problems involving analysis of heat transfer in a chemical reaction, using the equation Q = mc∆T (e.g., calculate the energy released in the combustion of an organic com- pound, and express the results in energy per mole of fuel [J/mol]) [AI, C]
D2.4 plan and conduct an inquiry to calculate, using a calorimeter, the heat of reaction of a substance (e.g., the heat of solution of ammonium nitrate, or of combustion of a hydrocarbon), compare the actual heat of reaction to the theoretical value, and suggest sources of experimental error [IP, PR, AI, C]
D2.5 solve problems related to energy changes in a chemical reaction, using Hess’s law [AI]
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 ∆H value of the reaction) [PR, AI]
D2.7 calculate the heat of reaction for a formation reaction, using a table of standard enthalpies of formation and applying Hess’s law [AI]
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 [IP, PR, AI]
D3. Understanding Basic Concepts
By the end of this course, students will:
D3.1 compare the energy changes resulting from physical change (e.g., boiling water), chemical reactions (e.g., bleaching a stain), and nuclear reactions (e.g., fission, fusion), in terms of whether energy is released or absorbed
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
D3.3 explain how mass, heat capacity, and change in temperature of a substance determine the amount of heat gained or lost by the substance
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 temper- ature, 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
D3.6 describe simple potential energy diagrams of chemical reactions (e.g., the relationships between the relative energies of reactants and products and the activation energy of the 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
D1.2 analyse the conditions (e.g. temperature, pressure, presence of a catalyst) required to maximize the efficiency of some common natural or industrial chemical reactions (e.g., decomposition, combustion, neutralization), and explain how the improved efficiency of the reaction contributes to environmental sustainability [AI, C]
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 [C]
D2.2 write thermochemical equations, expressing the energy change as a ∆H value or as a heat term in the equation [AI, C]
D2.3 solve problems involving analysis of heat transfer in a chemical reaction, using the equation Q = mc∆T (e.g., calculate the energy released in the combustion of an organic com- pound, and express the results in energy per mole of fuel [J/mol]) [AI, C]
D2.4 plan and conduct an inquiry to calculate, using a calorimeter, the heat of reaction of a substance (e.g., the heat of solution of ammonium nitrate, or of combustion of a hydrocarbon), compare the actual heat of reaction to the theoretical value, and suggest sources of experimental error [IP, PR, AI, C]
D2.5 solve problems related to energy changes in a chemical reaction, using Hess’s law [AI]
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 ∆H value of the reaction) [PR, AI]
D2.7 calculate the heat of reaction for a formation reaction, using a table of standard enthalpies of formation and applying Hess’s law [AI]
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 [IP, PR, AI]
D3. Understanding Basic Concepts
By the end of this course, students will:
D3.1 compare the energy changes resulting from physical change (e.g., boiling water), chemical reactions (e.g., bleaching a stain), and nuclear reactions (e.g., fission, fusion), in terms of whether energy is released or absorbed
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
D3.3 explain how mass, heat capacity, and change in temperature of a substance determine the amount of heat gained or lost by the substance
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 temper- ature, 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
D3.6 describe simple potential energy diagrams of chemical reactions (e.g., the relationships between the relative energies of reactants and products and the activation energy of the 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
Ontario Ministry of Education. (2008). The Ontario Curriculum Grades 11 and 12: Science.