Advanced Chemistry Grade 12A Sem 1 Overview



Science Curriculum Resources Overview* – GRADE 12A – SEMESTER 1- Cluster A & BMAIN RESOURCE:ALTERNATIVE RESOURCESResources 1Resources 2Advanced Chemistry PUBLISHER: Oxford University Press Edition: 2000Advanced Chemistry for You Publisher:Nelson Thornes.Edition: 2000ISBN0-19-914633-0ISBN978-0-7487-5297-3ISBNStrandTotal Curriculum Standards (based on CORE STANDARDS in Scheme of Work(Semesters 1 & 2)Curriculum Standards forSemester 1 (Based on scheme of work)Enquiry Standards(Based on Curriculum standards)Curriculum Standards covered in textbooks for Semester 1(using main and alternative)Curriculum Standards covered inAdvanced Chemistry Curriculum Standards covered inalternative resourceNot covered by selected resources%Covered in text booksChemistry382320232300100%Please Note:*Inquiry Standards are an integral part of science teaching – every effort must be made in providing opportunities for pupils to practice these skills. AT THE END OF EACH UNIT BELOW THERE IS A SPACE FOR THE SCIENCE DEPT TO OUTLINE HOW THEY INTEND TO DO THIS. Text book references are given to help teachers teach, and also provide a reference for pupils. However this does not replace the good practice of teachers using a variety of resources to teach and explain further in order to cover the curriculum standard fully.TITLE: Advanced Chemistry GRADE: 12 AdvancedPUBLISHER: Oxford University PressEdition: 2009ISBN: 978-0-19-9146333-8UNITS – SEMESTER 1UNIT TITLE/ NUMBER from S.O.WSchemes of Work - SubtitlesSoW PAGE number112 A C.1 – The periodic tablePeriodicity in propertiesP 458s-block elementsP 458-459p-block elementsP 459-460d-block elementsP 4622.12AC.2 Rates of reactionOrder of reactionP 467Reaction rate and temperatureP 467Equilibrium constantsP 4683.12AC.3 Acids and K valuespHP 473IndicatorsP 473BuffersP 473Solubility productsP 4744.12 A C.4 Energy and entropyEnthalpy change and cyclesP 479Free energyP 481STRANDScheme of Work UnitMonth/WeekTime /SubtopicC.SSCIENCE CURRICULUM STANDARDCHAPTERPAGESNOTCOVEREDALTERNATIVE RESOURCEChemistryCluster AThe periodic table3 hoursPeriodicity in properties12A.19.1Understand and use the term ionisation energy. Explain the factors influencing the ionisation energies of elements and the trends in ionisation energies across a period and down a group of the periodic table.4Electron in atoms16The S block elements17Trends across a period52More evidence for shells and sub shells ionisation energies 282Some group trends304Effect of atomic size12A.19.2Understand the terms electron affinity and electronegativity and recognise and explain their periodic variation.10Thermochemistry 16The S block elements154Some important enthalpy change283Some group trends4 hourss-block elements12A.19.3Know the general chemistry of the s-block elements, including:?trends in the physical properties of the elements;?trends in the chemical properties of the elements;?general common properties of the compounds of the elements, including the solubility, colour and thermal stability of the nitrates, carbonates and hydroxides;?the occurrence and extraction of the elements.16The S block elements280-295Group I and group II metals ToAnomalous behaviour of Li and Be6 hoursp-block elements12A.19.5Outline and explain trends in a number of properties down group VII:?physical properties;?the reactivity of the elements as oxidising agents;?the thermal stability of the hydride;? the reaction of the halide ions with silver nitrate followed by aqueous ammonia.18The halogens318-329group The S block elementsVII elements Halogen and halides :redox behaviourHalogens in solutions The halogen halidesSome ionic halides 4 hourd-block elements12A.19.9Know that in transition metals, d-electrons can be involved in bonding as well as the outer s-electrons, resulting in multiple oxidation states. Predict from its electronic configuration, the likely oxidation states of a transition element.20The transition metal358-359The element titanium to copper364Variable oxidation states 12A.19.10Explain how the variable oxidation states can result in transition metal ions acting as oxidising and reducing agents. Give examples of transition metal redox systems.13Redox equilibrium20The transition metal213-217Oxidation numbers-1221Oxidants and reductants372Transition metal complexes :some reactions376Other reaction of complex ions12A.19.14Know the biochemical importance of cobalt and iron.20The transition metal368Catalytic activity373Transition metal complexes :some reactions377Other reaction of complex ionsScientific EnquiryActivityCluster BRates of reaction5 hoursOrder of reaction12A.20.1Recognise that different reactions proceed at different rates and explain reaction rate in terms of particle collisions and particle energy.15Chemical kinetic255-258Reaction rateSome practical techniquesInstantaneous reaction rate260Reaction rate and collision theory12A.20.2Derive and use rate expressions of the form rate = k[A]m[B]n from data and draw and analyse graphical representations for zero, first- and second-order reactions in a specified reactant.15Chemical kinetic262-263Rate reaction and order of reaction266-267Using calculus to find order12A.20.3Calculate the half-life of first-order reactions and show an understanding of why it is concentration independent.15Chemical kinetic267Using calculus to find order3 hoursReaction rate and temperature12A.20.4Describe qualitatively the relationship between the rate constant and temperature.15Chemical kinetic254Reaction rate261Reaction rate and collision theory2 hoursEquilibrium constants12A.20.7Deduce expressions for forward and backward rate constants for a simple bimolecular reaction and hence deduce expressions for equilibrium constants in terms of concentrations (Kc) and partial pressures (Kp).11Chemical equilibrium165The nature of dynamic equilibrium 172The equilibrium constant Kc174An experimental determination of Kc 178Gas mixtures and the equilibrium constant Kp12A.20.8Calculate the values of equilibrium constants in terms of concentrations or partial pressures from appropriate data, and calculate the quantities present at equilibrium, given appropriate data.11Chemical equilibrium172The equilibrium constant Kc174An experimental determination of Kc 178Gas mixtures and the equilibrium constant Kp12A.20.9Understand and use the term position of equilibrium as applied to a reversible reaction and know that the size of an equilibrium constant is an indication of the extent to which a reaction nears completion.11Chemical equilibrium168-171Le chatelier's principals -1&2179Gas mixtures and the equilibrium constant KpScientific EnquiryActivityCluster BAcids and K values2 hourspH12A.20.10Show an understanding of the Br?nsted–Lowry theory of acidity. Derive and explain the terms pH, Ka, pKa and Kw, and use these concepts in calculations such as the calculation of the pH of solutions of weak acids and bases12acid – base equilibrium186-199Acids and bases and their properties188Acids and bases and proton transfer190Aqueous hydrogen ion concentration and pH192Strong acids194Weak acids2 hoursIndicators12A.20.11Know that indicators are weak acids and explain the choice of suitable indicators in acid–base titrations, in terms of the dissociation constant of the indicator.12acid – base equilibrium200-203Acids bases titrations-1&22 hoursBuffers12A.20.12Understand how buffer solutions control pH (including the role of HCO3– in controlling blood pH) and calculate the pH of buffer solutions, given appropriate data12acid – base equilibrium204Buffer solutions 206Buffer solutionsCalculations 1 hourSolubility products12A.20.13Apply quantitatively the concept of dynamic equilibrium to the solubility of ionic compounds by calculating the solubility product Ksp from concentrations, and vice versa, and demonstrate an understanding of the common ion effect.11Chemical equilibrium180Heterogeneous equilibrium 182solubility product and precipitates ChemistryCluster BEnergy and entropy8 hoursEnthalpy change and cycles12A.21.1Explain and use the concept of standard enthalpy change (ΔH), with particular reference to combustion, formation, solution and neutralisation. Calculate enthalpy changes from experimental results.10Thermo chemistry144-146Enthalpy change154Some important enthalpy change12A.21.2Use Hess’s law to construct simple energy cycles and determine enthalpy changes that cannot be found by direct experiment, such as enthalpies of formation and of ionisation.10Thermo chemistry150Standard enthalpy change and Hess's low152Hess's law examples12A.21.5State and explain the factors that lead to an increase in the entropy (disorder) of a chemical system.14Spontaneous change242-245Entropy 1&212A.21.6Calculate the standard entropy change for a reaction using absolute entropy values and recognise and explain the impact of changes of state on this value.14Spontaneous change242-245Entropy 1&24 hoursFree energy12A.21.7Calculate standard free energy changes for reactions from enthalpy and entropy changes and use this to predict the spontaneity of a reaction at a particular temperature.14Spontaneous change246-248Standards Gibbs energy changeScientific EnquiryActivity ................
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