7 Full Lesson Bundle + A Bonus Revision Lesson which covers the Kinetics (How Fast?) chapters from the OCR A Level Chemistry Specification (also suitable for the AQA and Edexcel Spec- see Learning Objectives below) Lesson 1: Order of Reactants Lesson 2: The Rate Equation Lesson 3&4 Concentration-Time Graphs Lesson 5: Initial Rates and Clock Reactions Lesson 6: The Rate Determining Step Lesson 7: The Arrhenius Equation Lesson 8: Revision Lesson Learning Objectives: Lesson 1: LO1: To recall the terms rate of reaction, order, overall order and rate constant LO2: To describe how orders of reactants affect the rate of a reaction LO3: To calculate the overall order of a reaction Lesson 2: LO1: To determine the order of a reactant from experimental data LO2: To calculate the rate constant, K, from a rate equation LO3: To calculate the units of the rate constant Lesson 3&4: LO1: To know the techniques and procedures used to investigate reaction rates LO2: To calculate reaction rates using gradients from concentration-time graphs LO3: To deduce zero & first order reactants from concentration-time graphs LO4: To calculate the rate constant of a first order reactant using their half-life Lesson 5: LO1: To determine the rate constant for a first order reaction from the gradient of a rate- concentration graph LO2: To understand how rate-concentration graphs are created LO3: To explain how clock reactions are used to determine initial rates of reactions Lesson 6: LO1: To explain and use the term rate determining step LO2: To deduce possible steps in a reaction mechanism from the rate equation and the balanced equation for the overall reaction LO3: To predict the rate equation that is consistent with the rate determining step Lesson 7: LO1: Explain qualitatively the effect of temperature change on a rate constant,k, and hence the rate of a reaction LO2: To Know the exponential relationship between the rate constant, k and temperature, T given by the Arrhenius equation, k = Ae–Ea/RT LO3: Determine Ea and A graphically using InK = -Ea/RT+ InA derived from the Arrhenius equation Lesson 8: This is an engaging KS5 revision lesson the Kinetics topic in A Level Chemistry (Year 13) Students will be able to complete three challenging question rounds on kinetics covering: Measuring Reaction Rates Orders of reactants Concentration-time graphs Rate-concentration graphs Clock Reactions Initial rates Arrhenius Equation Declaimer: Please refrain from purchasing this popular resource for an interview lesson or a formal observation. This is because planning your own lessons, including using your own lesson PowerPoints, is a fundamental skill of a qualified/unqualified teacher that will be assessed during the scenarios outlined above

8 Full Lesson Bundle which covers the redox and electrode potential section of the OCR Energy Chapter: Lesson 1 & 2: Redox Reactions Lesson 3& 4: Redox Titrations Lesson 5&6: Standard Electrode & Cell Potentials Lesson 7: Limitations of Cell Potentials Lesson 8: Storage & Fuel Cells Learning Objectives: Lesson 1: LO1: To identify the oxidation numbers of elements in ions and compounds LO2: To construct half-equations from redox equations LO3: To explain and use the terms oxidising agent and reducing agent Lesson 2: LO1: To understand that the overall increase in oxidation number will equal the overall decrease in oxidation number LO2: To construct balanced half equations and overall redox equations from reactions in acidic conditions LO3: To construct balanced half equations and overall redox equations from reactions in alkaline conditions (stretch & challenge) Lesson 3: LO1: To understand what a redox titration is. LO2: To describe the practical techniques and procedures used to carry out redox titrations involving Fe2+ /MnO4- LO3: To calculate structured titration questions based on experimental results of redox titrations involving Fe2+ /MnO4- and its derivatives Lesson 4: LO1: To describe the practical techniques and procedures used to carry out redox titrations for I2/S2O32- LO2: To calculate structured titration questions based on experimental results of redox titrations involving I2/S2O32- and non familiar redox systems LO3: To calculate non-structured titration questions based on experimental results of I2/S2O32- Lesson 5: LO1: To describe techniques and procedures used for the measurement of : i) Cell potentials of metals or non-metals in contact with their ions in aqueous solution ii) Ions of the same element in different oxidation states in contact with a Pt electrode Lesson 6: LO1: To use the term standard electrode potential E⦵ including its measurement using a hydrogen electrode LO2: To calculate a standard cell potential by combining two standard electrode potentials LO3: To predict the feasibility of electrode potentials to modern storage cells Lesson 7: LO1. To understand the limitations of predicting the feasibility of a reaction using cell potentials due to kinetics and non-standard conditions LO2. To explain why electrochemical cells may not work based on the limitations of using cell potentials Lesson 8: LO1: To understand the application of the principles of electrode potentials to modern storage cells LO2: To explain that a fuel cell uses the energy from a reaction of a fuel with oxygen to produce a voltage LO3: To derive the reactions that take place at each electrode in a hydrogen fuel cell The teacher will be able to check students have met these learning objectives through starter activities, discussion questions, mini AfL tasks and practice questions for students to complete Declaimer: Please refrain from purchasing this popular resource for an interview lesson or a formal observation. This is because planning your own lessons, including using your own lesson PowerPoints, is a fundamental skill of a qualified/unqualified teacher that will be assessed during the scenarios outlined above

6 Full Lesson Bundle covering the first 6 chapters in the OCR A Level Chemistry Chapter on Energy Lesson 1: Lattice Enthalpy **By the end of the lesson students will: Explain the term lattice enthalpy Understand the factors that determine the size of lattice enthalpy Explain the terms standard enthalpy change of formation and first ionisation energy** Lesson 2: Born-Haber Cycles **By the end of the lesson students will: **1. Construct Born Haber Cycle diagrams for ionic compounds from enthalpy change values **2. Calculate the value for lattice enthalpy from Born Haber Cycle diagrams **3. Calculate other enthalpy change values from Born Haber Cycle diagrams Lesson 3: Enthalpy Changes of Solution & Hydration **By the end of the lesson students will: **1. Define the terms enthalpy change of solution and hydration **2. Construct enthalpy cycles using the enthalpy change of solution of a simple ionic solid 3. Qualitatively explain the effect of ionic charge and ionic radius on the exothermic value of lattice enthalpy and enthalpy change of hydration Lesson 4: Entropy **By the end of lesson students will: **1. Know that entropy is a measure of the dispersal of energy in a system, which is greater the more disordered a system **2. Explain the difference in entropy of solids, liquids and gases **3. Calculate the entropy change of a reactant based on the entropies provided for the reactants and products Lesson 5: Gibbs Free Energy (Part 1) **By the end of the lesson students will: **1. Explain that the feasibility of a process depends upon ΔG being negative which in turn depends upon ΔS, ΔH and the T of the system **2. Recall the Gibbs’ Equation and calculate ΔG, ΔH, ΔS or T **3.Calculate ΔG, ΔH, ΔS or T using the Gibbs’ Equation Lesson 6: Gibbs Free Energy (Part 2) By the end of the lessons students will: 1. Explain that the feasibility of a process depends upon ΔG being negative which in turn depends upon ΔS, ΔH and the T of the system 2. Recall the Gibbs’ Equation and calculate ΔG, ΔH, ΔS or 3. Calculate ΔG, ΔH, ΔS or T using the Gibbs’ Equation The teacher will be able to check students have met these learning objectives through starter activities, discussion questions, mini AfL tasks and practice questions for students to complete Declaimer: Please refrain from purchasing this popular resource for an interview lesson or a formal observation. This is because planning your own lessons, including using your own lesson PowerPoints, is a fundamental skill of a qualified/unqualified teacher that will be assessed during the scenarios outlined above

10 Full Lesson Bundle + BONUS lesson on Acids, bases & buffers. This bundle covers the OCR A Level Chemistry specification. Please review the learning objectives below. Lesson 1: Bronsted-Lowry Acid and Bases To describe the difference between a BrØnsted Lowry acid and base To identify conjugate acid-base pairs To explain the difference between monobasic, dibasic and tribasic acids To understand the role of H+ in the reactions of acids with metals and bases (including carbonates, metal oxides and alkalis), using ionic equations Lesson 2: Strong Acids & The pH Scale To calculate the pH of a strong acid To convert between pH and [H+(aq)] To apply the relationship between pH and [H+(aq)] to work out pH changes after dilution **Lesson 3 - The Acid Dissociation Constant ** To understand the acid dissociation constant, Ka, as the extent of acid dissociation To know the relationship between Ka and pKa To convert between Ka and pKa Lesson 4- pH of weak acids To recall the expression of pH for weak monobasic acids To calculate the pH of weak monobasic acids using approximations To analyse the limitations of using approximations to Ka related calculations for ‘stronger’ weak acids Lesson 5 - The ionic product of water To recall the expression for the ionic product of water, Kw (ionisation of water) To calculate the pH of strong bases using Kw To apply the principles for Kc, Kp to Kw Lesson 6-9 - Buffer Solutions (3 part lesson) Part 1: Explaining How Buffer Solutions Work To know a buffer solution is a system that minimises pH changes on addition of small amounts of an acid or base To describe how a buffer solution is formed using weak acids, salts and strong alkalis To explain the role of the conjugate acid-base pair in an acid buffer solution such as how the blood pH is controlled by the carbonic acid–hydrogencarbonate buffer system Part 2: Buffer Solution Calculations (Part 1) To calculate the pH of a buffer solution containing a weak acid and the salt of a weak acid by using the Ka expression and pH equation To calculate equilibrium concentrations, moles or mass of the components of a weak acid-salt of a weak acid buffer solution Part 3: Buffer Solution Calculations (Part 2) To calculate the pH of a weak acid-strong alkali buffer solution To calculate equilibrium concentrations, moles or mass of the components of a weak acid- strong alkali buffer solution BONUS Lesson 9 : Revision on Buffer Solutions To review how to calculate the pH of a buffer solution containing a weak acid and a strong alkali To review how to calculate the pH of a buffer solution containing a weak acid and the salt of the weak acid Lesson 10- Neutralisation & Titration Curves To interpret titration curves of strong and weak acids and strong and weak bases To construct titration curve diagrams of strong and weak acids and strong and weak bases **Lesson 11- pH indicators & Titration Curves ** To explain indicator colour changes in terms of equilibrium shift between the HA and A- forms of the indicator To explain the choice of suitable indicators given the pH range of the indicator To describe an experiment for creating a titration curve Declaimer: Please refrain from purchasing this popular resource for an interview lesson or a formal observation. This is because planning your own lessons including using your own lesson PowerPoints is a fundamental skill of a qualified/unqualified teacher that will be reviewed during these scenarios outlined above

6 Full Lesson Bundle (includes a bonus lesson) on the topic of Equilibrium from the OCR A Level Chemistry specification plus an end of topic test. See below for the lessons and learning objectives Lesson 1: Le Chatelier’s Principle To explain the term dynamic equilibrium To apply le Chatelier’s principle to homogeneous equilibria in order to deduce qualitatively the effect of a change in temperature, pressure or concentration on the position of equilibrium To explain why catalysts do not change the position of equilibrium To explain the importance to the chemical industry of a compromise between chemical equilibrium and reaction rate in deciding the operational conditions Lesson 2: The Equilibrium Constant Kc (Part 1) To construct expressions for the equilibrium constant Kc for homogeneous reactions To calculate the equilibrium constant Kc from provided equilibrium concentrations To estimate the position of equilibrium from the magnitude of Kc To know the techniques and procedures used to investigate changes to the position of equilibrium for changes in concentration and temperature Lesson 3: The Equilibrium Constant Kc (Part 2) To construct expressions for the equilibrium constant Kc for homogeneous and heterogeneous reactions To calculate units for Kc To calculate quantities present at equilibrium and therefore kc given appropriate data Lesson 4: Controlling The Position of Equilibrium (Kc) To understand and explain the effect of temperature, concentration, pressure and catalysts on Kc and controlling the position of equilibrium Lesson 5: The Equilibrium Constant Kp To use the terms mole fraction and partial pressure To construct expressions for Kp for homogeneous and heterogeneous equilibria To calculate Kp including determination of units To understand the affect of temperature, pressure, concentration and catalysts on Kp and controlling the position of equilibrium Lesson 6 (BONUS): Chemical Equilibirum (Practical Skills): To understand how a titration experiment can be used to calculate the equilibrium constant, Kc To understand how a colorimeter can be used to calculate the equilibrium constant, Kc To analyse exam questions based on titration experiments in order to calculate out Kc End of Topic Test: A 45 minute end of chapter test on chemical equilibrium. The test covers content from both year 12 and 13 OCR on chemical equilibrium. A markscheme with model answers is also included which enables students self assess their answers in class with their teacher or as a homework task. The test is based on the following learning objectives: Apply le Chatelier’s principle to deduce qualitatively (from appropriate information) the effect of a change in temperature, concentration or pressure, on a homogeneous system in equilibrium. Explain that a catalyst increases the rate of both forward and reverse reactions in an equilibrium by the same amount resulting in an unchanged position of equilibrium Deduce, for homogeneous and heterogeneous reactions, expressions for the equilibrium constant Kc. Calculate the values of the equilibrium constant, Kc (from provided or calculated equilibrium moles or concentrations), including determination of units. Estimate the position of equilibrium from the magnitude of Kc. Calculate, given appropriate data, the concentration or quantities present at equilibrium. Deduce, for homogeneous and heterogeneous reactions, expressions for the equilibrium constant Kp. Calculate the values of the equilibrium constant, Kp (from provided or calculated equilibrium moles or pressures), including determination of units. Explain the effect of changing temperature on the value of Kc or Kp for exothermic and endothermic reactions. State that the value of Kc or Kp is unaffected by changes in concentration or pressure or by the presence of a catalyst. Explain how Kc or Kp controls the position of equilibrium on changing concentration, pressure and temperature Declaimer: Please refrain from purchasing this popular resource for an interview lesson or a formal observation. This is because planning your own lessons including using your own lesson PowerPoints is a fundamental skill of a qualified/unqualified teacher that will be reviewed during these scenarios outlined above