3 linked lessons on the carbon cycle, the greenhouse effect and climate change.

Each lesson includes a ‘blast from the past quiz’, a range of activities and an AFL task that relates to their progress. A range of lessons are designed to relate to the future AQA syllabus as well as allowing students to apply a unit of work to novel and interesting applications e.g. Following Dr Who to the early Earth’s atmosphere, choosing an alternative fuel for a new Elon musk prototype car and narrating a climate change trailer for Leonardo Decaprio. It wa sa lot of fun teaching for what can be a very dry subject!

This resource contains 3 revision mats for the required practicals in the Chemistry section of the new AQA Science Trilogy paper 2. Answer sheets have been added. They contain questions about methodology, scientific enquiry and analysis of results. These can be given after teaching the required practical, homework or at the end of year 11 for revision before their exams. Required practicals included: Rates of Reaction Chromatography Water Purification My year 11s have found these particularly useful to go through in revision lessons and have taken extra home to use as revision tools. Please rate this resource. You can also find our other bundles for the following: Biology Paper 1 Biology Paper 2 Biology Triple Physics Paper 1 Physics Paper 2 Chemistry Paper 1 Chemistry Paper 2 Other resources and revision mats can be found in my shop by clicking the following link: https://www.tes.com/teaching-resources/shop/cal-w11

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

My resources now cover the whole of OCR AS Chemistry. Each download includes a list of all available lessons and bundles. This bundle is ideal for classroom or home learning and covers the whole of the OCR A level chemistry specification module 2 - Foundations in Chemistry, sections 2.1 and 2.2. Each topic includes a fully interactive PowerPoint including starter, group activities, questions and plenary along with a worksheet and a lesson plan. Answers to all exercises are provided. Some of the resources include a PowerPoint quiz. A practical activity on titration is also included. This bundle relates to the following sections of the OCR AS Chemistry specification: Module 2 – Foundations in chemistry Part 1 – Atoms and reactions (whole) 2.1.1 – Atomic structure and isotopes 2.1.2 – Compounds, formulae and equations 2.1.3 – Amount of substance 2.1.4 – Acids 2.1.5 − Redox Part 2 – Electrons, bonding and structure (whole) 2.2.1 – Electron structure 2.2.2 – Bonding and structure Module 3 – The Periodic table and energy Part 1 –The Periodic Table (part) 3.1.1 (Periodicity) (part) Content covered: The changing atom How Science Works - HSW7 - The changing accepted models of atomic structure over time. The contributions of five scientists to the development of the theory of atomic structure. Atomic structure • Protons, neutrons and electrons – mass and relative charge • Atomic number and mass number • Isotopes • Key definitions Atomic masses • Relative masses - comparison of masses to carbon-12 • Calculating relative atomic mass from the masses and abundances of the isotopes • Mass spectrometry and its use in the above • Calculating relative molecular and relative formula masses from formulae • Key definitions of relative atomic mass and relative isotopic mass Formulae and equations • Formulae of ions • Predicting ionic charges from the Periodic Table • Writing the formulae of ionic compounds and elements • Writing and balancing equations • Common types of reaction and their equations Amount of substance and the mole • Relative masses and the mole • Avogadro constant • Calculating number of atoms • Amount of substance • Molar mass • Calculating amount of substance from total mass and vice versa • Mole triangle Determining formulae • Definitions and use of the terms empirical and molecular formula • Simplest whole number ratios • Calculations of empirical and molecular formulae, from composition by mass or percentage compositions by mass and relative molecular mass • Calculating % by mass from the formula • The terms anhydrous, hydrated and water of crystallisation • Calculation of the formula of a hydrated salt from given percentage composition, mass composition or based on experimental results Moles and gas volumes • Molar volume of a gas • Moles and gas volume triangle • Summary of relationships for gases between amount of substance, volume, mass and number of molecules • Calculating amount of substance from volume of gas and vice versa • Ideal gases • The ideal gas equation Moles, concentrations and solutions • Definitions and use of the terms concentration and mass concentration • Concentrated and dilute • Relationship between concentration, amount in mol and volume including concentration triangle • Calculating concentration, amount in mol, volume and mass from given data • Example calculations • Mass concentrations • Choosing the correct glassware to measure volumes • Standard solutions • Practical activity – making up a standard solution • Diluting solutions and calculations • Practical activity – diluting solutions Moles and reactions • Balanced chemical equations and stoichiometry • Molar ratios • Using molar ratio to calculate amounts in moles of reactants and products in a chemical reaction • Using molar ratio to calculate masses of reactants and products in a chemical reaction • Using molar ratio to calculate volumes of gases in a chemical reaction • Flow diagrams showing steps in calculations involving quantities of reacting substances • Example calculations – clearly illustrated in a highly visual way Percentage yield and atom economy • Introduction to Green Chemistry • Reasons why reactions do not have 100% yield • % yield and how to calculate it • Calculations of % yield involving limiting reactant • Atom economy and its importance in the sustainability of a chemical process • Calculating atom economy • Example calculations – clearly illustrated in a highly visual way • Differences between atom economy and % yield • Comparing chemical processes in terms of sustainability (using production of ethanol as an example) Acids and bases • Definitions of acid, base, alkali and salt • Formulae of acids, bases, alkalis and salts • The relationship between bases and alkalis • The pH scale • Everyday examples of acids and bases • Weak and strong acids • Diprotic acids • Writing and balancing neutralization reactions (including acid-carbonate reactions) • Ionic equations Acid-base titrations • Titration and uses • Standard solution • Glassware and procedure for titration with detailed hints for technique • Reading burette • Recording titration results and calculating the mean • Titration calculations • Examples of structured and unstructured calculations • Revision of calculations involving masses and volumes • Practical titration activity • Evaluation of titration experiment • Uncertainties and calculating % uncertainties • Procedural errors Redox • Redox definition in terms of electron transfer • Oxidation numbers and how to calculate them • Oxidation number in chemical names • Redox definition in terms of oxidation number • Using oxidation numbers to identify redox reactions and determine what has been oxidised and reduced • Oxidising and reducing agents • Disproportionation as oxidation and reduction of the same element Electron configuration - shells, sub-shells and orbitals • Energy levels • Main shells, sub-shells and orbitals • Rules for filling orbitals • Electron configurations of atoms and ions • Deducing electron configuration using the Periodic Table • Relationship of electron configuration to the Periodic Table Ionic bonding • Bonding and the Periodic Table • Predicting ionic formulae • Definition of ionic bonding • Dot-and-cross diagrams – some of them animated • Half equations • Giant ionic lattice • Physical properties of ionic compounds including: • melting point • electrical conductivity • solubility in polar and non-polar solvents Covalent bonding • Definition of a covalent bond • Single, double and triple covalent bonds • Lone pairs • How to construct dot-and-cross diagrams • Dative covalent or coordinate bonds • The Octet Rule and exceptions • Average bond enthalpies Shapes of molecules and ions • Electron pair repulsion theory (VSEPR) • Effect of lone pairs on shape • Model answer to exam question • How to draw simple shapes in 3D • Bond angles Electronegativity and bond polarity • Definition of electronegativity • Atomic core and calculation of core charge • Factors affecting electronegativity • Pauling scale of electronegativity • Electronegativity and bond polarity • Non-polar and polar covalent bonds • Electronegativity and bonding type (including intermediate bonding) • Polarity of molecules from the bond polarities and the molecular shape • Predicting whether a molecule will have an overall dipole from its symmetry Intermolecular forces • What are intermolecular forces? • Strengths of bonds and intermolecular forces • Types of intermolecular forces • Induced dipole-dipole interactions (London (dispersion) forces) • How London forces arise • Factors affecting strength of London forces • Permanent dipole-dipole interactions • How permanent dipole-dipole interactions arise • How intermolecular forces affect properties • Hydrogen bonding • What’s special about hydrogen bonds • Effects of hydrogen bonds on properties • Special properties of water • Summary of intermolecular forces • Predicting the type of intermolecular forces Structure and bonding • Factors influencing physical properties • The way the atoms/ions are grouped together (structure) • The type of particles the solid is built up from • The bonds or forces holding these particles together • Structure and physical properties of ionic compounds (see also topic 15) • Structures and physical properties of covalent substances including giant covalent and simple molecular • Diamond and graphite – structures and properties • Graphene • Metallic bonding, structure and physical properties • Summary of types of bonding • Jigsaw discussion to summarise 4 main types of structure and their properties Links Next lesson – free resource: Topic 21 – the Periodic Table past and present http://www.tes.com/teaching-resource/periodic-table-past-and-present-ocr-as-chemistry-12964450 Next large bundle Periodic table and energy https://www.tes.com/teaching-resource/periodic-table-and-energy-13214245

Bundle for GCSE Chemistry on fuels etc.