breaking. Use data on use mean bond enthalpies to calculate Students should be able to: compounds containing bond enthalpies to an approximate value of for define the term mean bond that bond. ΔH calculate enthalpies of reactions in the gaseous phase enthalpy; use mean bond reaction, combustion explain why values from mean bond enthalpies to calculate an and formation. enthalpy calculations differ from those approximate value of for ΔH determined using Hess’s Law reactions in the gaseous phase; explain why values from mean bond enthalpy calculations differ from those determined using Hess’s Law. Student Required One hour lessons Learning Outcomes Specification Content Skills Covered Book Section Practicals CHAPTER 8 Kinetics (10 hours) – 1 Rate of reaction 3.1.5.1 Collision theory 8.1 Reactions can only occur when collisions take Recap of what is meant Recall the definition of rate of place between particles having sufficient by the term rate of reaction reaction and how it is energy. This energy is called the activation Describe how different factors calculated. Explain how energy. affect the rate of reaction different factors affect Explain how reactions take place Students should be able to: define the term the rate. in terms of collisions, and how activation energy; explain why most collisions various factors increase the rate. do not lead to a reaction. 2 Collision theory 8.2 8.3 Introduces the idea of describe how moving particles orientation and store energy (translational, activation. Uses these vibrational and rotational) ideas to explain why define the term activation energy most collision do not explain why most collisions do not lead to a reaction. lead to a reaction
breaking. Use data on bond enthalpies to calculate enthalpies of reaction, combustion and formation. use mean bond enthalpies to calculate an approximate value of ΔH for reactions in the gaseous phase explain why values from mean bond enthalpy calculations differ from those determined using Hess’s Law Students should be able to: define the term mean bond enthalpy; use mean bond enthalpies to calculate an approximate value of ΔH for reactions in the gaseous phase; explain why values from mean bond enthalpy calculations differ from those determined using Hess’s Law. compounds containing that bond. One hour lessons Learning Outcomes Specification Content Skills Covered Student Book Section Required Practicals CHAPTER 8 – Kinetics (10 hours) 1 Rate of reaction Recap of what is meant by the term rate of reaction and how it is calculated. Explain how different factors affect the rate. Recall the definition of rate of reaction Describe how different factors affect the rate of reaction Explain how reactions take place in terms of collisions, and how various factors increase the rate. 3.1.5.1 Collision theory Reactions can only occur when collisions take place between particles having sufficient energy. This energy is called the activation energy. Students should be able to: define the term activation energy; explain why most collisions do not lead to a reaction. 8.1 2 Collision theory Introduces the idea of orientation and activation. Uses these ideas to explain why most collision do not lead to a reaction. describe how moving particles store energy (translational, vibrational and rotational) define the term activation energy explain why most collisions do not lead to a reaction 8.2 8.3
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