Physical chemistry 3.1.1 Atomic structure The chemical properties of elements depend on their atomic structure and in particular on the arrangement of electrons around the nucleus. The arrangement of electrons in orbitals is linked to the way in which elements are organised in the Periodic Table. Chemists can measure the mass of atoms and molecules to a high degree of accuracy in a mass spectrometer. The principles of operation of a modern mass spectrometer are studied. 3.1.1.1 Fundamental particles 3.1.1.2 Mass number and isotopes 3.1.1.3 Electron configuration 3.1.2 Amount of substance When chemists measure out an amount of a substance, they use an amount in moles. The mole is a useful quantity because one mole of a substance always contains the same number of entities of the substance. An amount in moles can be measured out by mass in grams, by volume in dm3 of a solution of known concentration and by volume in dm3 of a gas. 3.1.2.1 Relative atomic mass and relative molecular mass 3.1.2.2 The mole and the Avogadro constant 3.1.2.3 The ideal gas equation 3.1.2.4 Empirical and molecular formula 3.1.2.5 Balanced equations and associated calculations 3.1.3 Bonding The physical and chemical properties of compounds depend on the ways in which the compounds are held together by chemical bonds and by intermolecular forces. Theories of bonding explain how atoms or ions are held together in these structures. Materials scientists use knowledge of structure and bonding to engineer new materials with desirable properties. These new materials may offer new applications in a range of different modern technologies. 3.1.3.1 Ionic bonding 3.1.3.2 Nature of covalent and dative covalent bonds 3.1.3.3 Metallic bonding 3.1.3.4 Bonding and physical properties 3.1.3.5 Shapes of simple molecules and ions 3.1.3.6 Bond polarity 3.1.3.7 Forces between molecules 3.1.4 Energetics The enthalpy change in a chemical reaction can be measured accurately. It is important to know this value for chemical reactions that are used as a source of heat energy in applications such as domestic boilers and internal combustion engines. 3.1.4.1 Enthalpy change 3.1.4.2 Calorimetry 3.1.4.3 Applications of Hess’s law 3.1.4.4 Bond enthalpies 3.1.5 Kinetics The study of kinetics enables chemists to determine how a change in conditions affects the speed of a chemical reaction. Whilst the reactivity of chemicals is a significant factor in how fast chemical reactions proceed, there are variables that can be manipulated in order to speed them up or slow them down. 3.1.5.1 Collision theory 3.1.5.2 Maxwell–Boltzmann distribution 3.1.5.3 Effect of temperature on reaction rate 3.1.5.4 Effect of concentration and pressure 3.1.5.5 Catalysts 3.1.6 Chemical equilibria, Le Chatelier’s principle and Kc In contrast with kinetics, which is a study of how quickly reactions occur, a study of equilibria indicates how far reactions will go. Le Chatelier’s principle can be used to predict the effects of changes in temperature, pressure and concentration on the yield of a reversible reaction. This has important consequences for many industrial processes. The further study of the equilibrium constant, Kc , considers how the mathematical expression for the equilibrium constant enables us to calculate how an equilibrium yield will be influenced by the concentration of reactants and products. 3.1.6.1 Chemical equilibria and Le Chatelier's principle 3.1.6.2 Equilibrium constant Kc for homogeneous systems 3.1.7 Oxidation, reduction and redox equations Redox reactions involve a transfer of electrons from the reducing agent to the oxidising agent. The change in the oxidation state of an element in a compound or ion is used to identify the element that has been oxidised or reduced in a given reaction. Separate half-equations are written for the oxidation or reduction processes. These half-equations can then be combined to give an overall equation for any redox reaction. 3.1.8 Thermodynamics (A-level only) The further study of thermodynamics builds on the Energetics section and is important in understanding the stability of compounds and why chemical reactions occur. Enthalpy change is linked with entropy change enabling the free-energy change to be calculated. 3.1.8.1 Born–Haber cycles (A-level only) 3.1.8.2 Gibbs free-energy change, ∆G, and entropy change, ∆S (A-level only) 3.1.9 Rate equations (A-level only) 3.1.9.1 Rate equations (A-level only) 3.1.9.2 Determination of rate equation (A-level only) 3.1.10 Equilibrium constant Kp for homogeneous systems (A-level only) The further study of equilibria considers how the mathematical expression for the equilibrium constant Kp enables us to calculate how an equilibrium yield will be influenced by the partial pressures of reactants and products. This has important consequences for many industrial processes. 3.1.11 Electrode potentials and electrochemical cells (A-level only) Redox reactions take place in electrochemical cells where electrons are transferred from the reducing agent to the oxidising agent indirectly via an external circuit. A potential difference is created that can drive an electric current to do work. Electrochemical cells have very important commercial applications as a portable supply of electricity to power electronic devices such as mobile phones, tablets and laptops. On a larger scale, they can provide energy to power a vehicle. 3.1.11.1 Electrode potentials and cells (A-level only) 3.1.11.2 Commercial applications of electrochemical cells (A-level only) 3.1.12 Acids and bases (A-level only) Acids and bases are important in domestic, environmental and industrial contexts. Acidity in aqueous solutions is caused by hydrogen ions and a logarithmic scale, pH, has been devised to measure acidity. Buffer solutions, which can be made from partially neutralised weak acids, resist changes in pH and find many important industrial and biological applications. 3.1.12.1 Brønsted–Lowry acid–base equilibria in aqueous solution (A-level only) 3.1.12.2 Definition and determination of pH (A-level only) 3.1.12.3 The ionic product of water, Kw (A-level only) 3.1.12.4 Weak acids and bases Ka for weak acids (A-level only) 3.1.12.5 pH curves, titrations and indicators (A-level only) 3.1.12.6 Buffer action (A-level only) 3.2 Inorganic chemistry 3.2.1 Periodicity The Periodic Table provides chemists with a structured organisation of the known chemical elements from which they can make sense of their physical and chemical properties. The historical development of the Periodic Table and models of atomic structure provide good examples of how scientific ideas and explanations develop over time. 3.2.1.1 Classification 3.2.1.2 Physical properties of Period 3 elements 3.2.2 Group 2, the alkaline earth metals The elements in Group 2 are called the alkaline earth metals. The trends in the solubilities of the hydroxides and the sulfates of these elements are linked to their use. Barium sulfate, magnesium hydroxide and magnesium sulfate have applications in medicines whilst calcium hydroxide is used in agriculture to change soil pH, which is essential for good crop production and maintaining the food supply. 3.2.3 Group 7(17), the halogens The halogens in Group 7 are very reactive non-metals. Trends in their physical properties are examined and explained. Fluorine is too dangerous to be used in a school laboratory but the reactions of chlorine are studied. Challenges in studying the properties of elements in this group include explaining the trends in ability of the halogens to behave as oxidising agents and the halide ions to behave as reducing agents. 3.2.3.1 Trends in properties 3.2.3.2 Uses of chlorine and chlorate(I) 3.2.4 Properties of Period 3 elements and their oxides (A-level only) The reactions of the Period 3 elements with oxygen are considered. The pH of the solutions formed when the oxides react with water illustrates further trends in properties across this period. Explanations of these reactions offer opportunities to develop an in-depth understanding of how and why these reactions occur. 3.2.5 Transition metals (A-level only) The 3d block contains 10 elements, all of which are metals. Unlike the metals in Groups 1 and 2, the transition metals Ti to Cu form coloured compounds and compounds where the transition metal exists in different oxidation states. Some of these metals are familiar as catalysts. The properties of these elements are studied in this section with opportunities for a wide range of practical investigations. 3.2.5.1 General properties of transition metals (A-level only) 3.2.5.2 Substitution reactions (A-level only) 3.2.5.3 Shapes of complex ions (A-level only) 3.2.5.4 Formation of coloured ions (A-level only) 3.2.5.5 Variable oxidation states (A-level only) 3.2.5.6 Catalysts (A-level only) 3.2.6 Reactions of ions in aqueous solution (A-level only) The reactions of transition metal ions in aqueous solution provide a practical opportunity for students to show and to understand how transition metal ions can be identified by test-tube reactions in the laboratory. 3.3 Organic chemistry 3.3.1 Introduction to organic chemistry Organic chemistry is the study of the millions of covalent compounds of the element carbon. These structurally diverse compounds vary from naturally occurring petroleum fuels to DNA and the molecules in living systems. Organic compounds also demonstrate human ingenuity in the vast range of synthetic materials created by chemists. Many of these compounds are used as drugs, medicines and plastics. Organic compounds are named using the International Union of Pure and Applied Chemistry (IUPAC) system and the structure or formula of molecules can be represented in various different ways. Organic mechanisms are studied, which enable reactions to be explained. In the search for sustainable chemistry, for safer agrochemicals and for new materials to match the desire for new technology, Chemistry plays the dominant role. 3.3.1.1 Nomenclature 3.3.1.2 Reaction mechanisms 3.3.1.3 Isomerism 3.3.2 Alkanes Alkanes are the main constituent of crude oil, which is an important raw material for the chemical industry. Alkanes are also used as fuels and the environmental consequences of this use are considered in this section. 3.3.2.1 Fractional distillation of crude oil 3.3.2.2 Modification of alkanes by cracking 3.3.2.3 Combustion of alkanes 3.3.2.4 Chlorination of alkanes 3.3.3 Halogenoalkanes Halogenoalkanes are much more reactive than alkanes. They have many uses, including as refrigerants, as solvents and in pharmaceuticals. The use of some halogenoalkanes has been restricted due to the effect of chlorofluorocarbons (CFCs) on the atmosphere. 3.3.3.1 Nucleophilic substitution 3.3.3.2 Elimination 3.3.3.3 Ozone depletion 3.3.4 Alkenes In alkenes, the high electron density of the carbon–carbon double bond leads to attack on these molecules by electrophiles. This section also covers the mechanism of addition to the double bond and introduces addition polymers, which are commercially important and have many uses in modern society. 3.3.4.1 Structure, bonding and reactivity 3.3.4.2 Addition reactions of alkenes 3.3.4.3 Addition polymers 3.3.5 Alcohols Alcohols have many scientific, medicinal and industrial uses. Ethanol is one such alcohol and it is produced using different methods, which are considered in this section. Ethanol can be used as a biofuel. 3.3.5.1 Alcohol production 3.3.5.2 Oxidation of alcohols 3.3.5.3 Elimination 3.3.6 Organic analysis Our understanding of organic molecules, their structure and the way they react, has been enhanced by organic analysis. This section considers some of the analytical techniques used by chemists, including test-tube reactions and spectroscopic techniques. 3.3.6.1 Identification of functional groups by test-tube reactions 3.3.6.2 Mass spectrometry 3.3.6.3 Infrared spectroscopy 3.3.7 Optical isomerism (A-level only) Compounds that contain an asymmetric carbon atom form stereoisomers that differ in their effect on plane polarised light. This type of isomerism is called optical isomerism. 3.3.8 Aldehydes and ketones (A-level only) Aldehydes, ketones, carboxylic acids and their derivatives all contain the carbonyl group which is attacked by nucleophiles. This section includes the addition reactions of aldehydes and ketones. 3.3.9 Carboxylic acids and derivatives (A-level only) Carboxylic acids are weak acids but strong enough to liberate carbon dioxide from carbonates. Esters occur naturally in vegetable oils and animal fats. Important products obtained from esters include biodiesel, soap and glycerol. 3.3.9.1 Carboxylic acids and esters (A-level only) 3.3.9.2 Acylation (A-level only) 3.3.10 Aromatic chemistry (A-level only) Aromatic chemistry takes benzene as an example of this type of molecule and looks at the structure of the benzene ring and its substitution reactions. 3.3.10.1 Bonding (A-level only) 3.3.10.2 Electrophilic substitution (A-level only) 3.3.11 Amines (A-level only) Amines are compounds based on ammonia where hydrogen atoms have been replaced by alkyl or aryl groups. This section includes their reactions as nucleophiles. 3.3.11.1 Preparation (A-level only) 3.3.11.2 Base properties (A-level only) 3.3.11.3 Nucleophilic properties (A-level only) 3.3.12 Polymers (A-level only) The study of polymers is extended to include condensation polymers. The ways in which condensation polymers are formed are studied, together with their properties and typical uses. Problems associated with the reuse or disposal of both addition and condensation polymers are considered. 3.3.12.1 Condensation polymers (A-level only) 3.3.12.2 Biodegradability and disposal of polymers (A-level only) 3.3.13 Amino acids, proteins and DNA (A-level only) Amino acids, proteins and DNA are the molecules of life. In this section, the structure and bonding in these molecules and the way they interact is studied. Drug action is also considered. 3.3.13.1 Amino acids (A-level only) 3.3.13.2 Proteins (A-level only) 3.3.13.3 Enzymes (A-level only) 3.3.13.4 DNA (A-level only) 3.3.13.5 Action of anticancer drugs (A-level only) 3.3.14 Organic synthesis (A-level only) 3.3.15 Nuclear magnetic resonance spectroscopy (A-level only) Chemists use a variety of techniques to deduce the structure of compounds. In this section, nuclear magnetic resonance spectroscopy is added to mass spectrometry and infrared spectroscopy as an analytical technique. The emphasis is on the use of analytical data to solve problems rather than on spectroscopic theory. 3.3.16 Chromatography (A-level only) Chromatography provides an important method of separating and identifying components in a mixture. Different types of chromatography are used depending on the composition of mixture to be separated.
Grade 6 in Chem or 6-6 in Combined Science and grade 6 in Mathematics.
Paper 1 Relevant physical chemistry topics • Inorganic chemistry • Relevant practical skills Assessed • written exam: 2 hours • 105 marks • 35% of A-level Questions 105 marks of short and long answer questions Paper 2 What's assessed • Relevant physical chemistry topics • Organic chemistry • Relevant practical skills Assessed • written exam: 2 hours • 105 marks • 35% of A-level Questions 105 marks of short and long answer questions Paper 3 What's assessed • Any content • Any practical skills Assessed • written exam: 2 hours • 90 marks • 30% of A-level Questions 40 marks of questions on practical techniques and data analysis 20 marks of questions testing across the specification 30 marks of multiple choice questions
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Physical chemistry 3.1.1 Atomic structure The chemical properties of elements depend on their atomic structure and in particular on the arrangement of electrons around the nucleus. The arrangement of electrons in orbitals is linked to the way in which elements are organised in the Periodic Table. Chemists can measure the mass of atoms and molecules to a high degree of accuracy in a mass spectrometer. The principles of operation of a modern mass spectrometer are studied. 3.1.1.1 Fundamental particles 3.1.1.2 Mass number and isotopes 3.1.1.3 Electron configuration 3.1.2 Amount of substance When chemists measure out an amount of a substance, they use an amount in moles. The mole is a useful quantity because one mole of a substance always contains the same number of entities of the substance. An amount in moles can be measured out by mass in grams, by volume in dm3 of a solution of known concentration and by volume in dm3 of a gas. 3.1.2.1 Relative atomic mass and relative molecular mass 3.1.2.2 The mole and the Avogadro constant 3.1.2.3 The ideal gas equation 3.1.2.4 Empirical and molecular formula 3.1.2.5 Balanced equations and associated calculations 3.1.3 Bonding The physical and chemical properties of compounds depend on the ways in which the compounds are held together by chemical bonds and by intermolecular forces. Theories of bonding explain how atoms or ions are held together in these structures. Materials scientists use knowledge of structure and bonding to engineer new materials with desirable properties. These new materials may offer new applications in a range of different modern technologies. 3.1.3.1 Ionic bonding 3.1.3.2 Nature of covalent and dative covalent bonds 3.1.3.3 Metallic bonding 3.1.3.4 Bonding and physical properties 3.1.3.5 Shapes of simple molecules and ions 3.1.3.6 Bond polarity 3.1.3.7 Forces between molecules 3.1.4 Energetics The enthalpy change in a chemical reaction can be measured accurately. It is important to know this value for chemical reactions that are used as a source of heat energy in applications such as domestic boilers and internal combustion engines. 3.1.4.1 Enthalpy change 3.1.4.2 Calorimetry 3.1.4.3 Applications of Hess’s law 3.1.4.4 Bond enthalpies 3.1.5 Kinetics The study of kinetics enables chemists to determine how a change in conditions affects the speed of a chemical reaction. Whilst the reactivity of chemicals is a significant factor in how fast chemical reactions proceed, there are variables that can be manipulated in order to speed them up or slow them down. 3.1.5.1 Collision theory 3.1.5.2 Maxwell–Boltzmann distribution 3.1.5.3 Effect of temperature on reaction rate 3.1.5.4 Effect of concentration and pressure 3.1.5.5 Catalysts 3.1.6 Chemical equilibria, Le Chatelier’s principle and Kc In contrast with kinetics, which is a study of how quickly reactions occur, a study of equilibria indicates how far reactions will go. Le Chatelier’s principle can be used to predict the effects of changes in temperature, pressure and concentration on the yield of a reversible reaction. This has important consequences for many industrial processes. The further study of the equilibrium constant, Kc , considers how the mathematical expression for the equilibrium constant enables us to calculate how an equilibrium yield will be influenced by the concentration of reactants and products. 3.1.6.1 Chemical equilibria and Le Chatelier's principle 3.1.6.2 Equilibrium constant Kc for homogeneous systems 3.1.7 Oxidation, reduction and redox equations Redox reactions involve a transfer of electrons from the reducing agent to the oxidising agent. The change in the oxidation state of an element in a compound or ion is used to identify the element that has been oxidised or reduced in a given reaction. Separate half-equations are written for the oxidation or reduction processes. These half-equations can then be combined to give an overall equation for any redox reaction. 3.1.8 Thermodynamics (A-level only) The further study of thermodynamics builds on the Energetics section and is important in understanding the stability of compounds and why chemical reactions occur. Enthalpy change is linked with entropy change enabling the free-energy change to be calculated. 3.1.8.1 Born–Haber cycles (A-level only) 3.1.8.2 Gibbs free-energy change, ∆G, and entropy change, ∆S (A-level only) 3.1.9 Rate equations (A-level only) 3.1.9.1 Rate equations (A-level only) 3.1.9.2 Determination of rate equation (A-level only) 3.1.10 Equilibrium constant Kp for homogeneous systems (A-level only) The further study of equilibria considers how the mathematical expression for the equilibrium constant Kp enables us to calculate how an equilibrium yield will be influenced by the partial pressures of reactants and products. This has important consequences for many industrial processes. 3.1.11 Electrode potentials and electrochemical cells (A-level only) Redox reactions take place in electrochemical cells where electrons are transferred from the reducing agent to the oxidising agent indirectly via an external circuit. A potential difference is created that can drive an electric current to do work. Electrochemical cells have very important commercial applications as a portable supply of electricity to power electronic devices such as mobile phones, tablets and laptops. On a larger scale, they can provide energy to power a vehicle. 3.1.11.1 Electrode potentials and cells (A-level only) 3.1.11.2 Commercial applications of electrochemical cells (A-level only) 3.1.12 Acids and bases (A-level only) Acids and bases are important in domestic, environmental and industrial contexts. Acidity in aqueous solutions is caused by hydrogen ions and a logarithmic scale, pH, has been devised to measure acidity. Buffer solutions, which can be made from partially neutralised weak acids, resist changes in pH and find many important industrial and biological applications. 3.1.12.1 Brønsted–Lowry acid–base equilibria in aqueous solution (A-level only) 3.1.12.2 Definition and determination of pH (A-level only) 3.1.12.3 The ionic product of water, Kw (A-level only) 3.1.12.4 Weak acids and bases Ka for weak acids (A-level only) 3.1.12.5 pH curves, titrations and indicators (A-level only) 3.1.12.6 Buffer action (A-level only) 3.2 Inorganic chemistry 3.2.1 Periodicity The Periodic Table provides chemists with a structured organisation of the known chemical elements from which they can make sense of their physical and chemical properties. The historical development of the Periodic Table and models of atomic structure provide good examples of how scientific ideas and explanations develop over time. 3.2.1.1 Classification 3.2.1.2 Physical properties of Period 3 elements 3.2.2 Group 2, the alkaline earth metals The elements in Group 2 are called the alkaline earth metals. The trends in the solubilities of the hydroxides and the sulfates of these elements are linked to their use. Barium sulfate, magnesium hydroxide and magnesium sulfate have applications in medicines whilst calcium hydroxide is used in agriculture to change soil pH, which is essential for good crop production and maintaining the food supply. 3.2.3 Group 7(17), the halogens The halogens in Group 7 are very reactive non-metals. Trends in their physical properties are examined and explained. Fluorine is too dangerous to be used in a school laboratory but the reactions of chlorine are studied. Challenges in studying the properties of elements in this group include explaining the trends in ability of the halogens to behave as oxidising agents and the halide ions to behave as reducing agents. 3.2.3.1 Trends in properties 3.2.3.2 Uses of chlorine and chlorate(I) 3.2.4 Properties of Period 3 elements and their oxides (A-level only) The reactions of the Period 3 elements with oxygen are considered. The pH of the solutions formed when the oxides react with water illustrates further trends in properties across this period. Explanations of these reactions offer opportunities to develop an in-depth understanding of how and why these reactions occur. 3.2.5 Transition metals (A-level only) The 3d block contains 10 elements, all of which are metals. Unlike the metals in Groups 1 and 2, the transition metals Ti to Cu form coloured compounds and compounds where the transition metal exists in different oxidation states. Some of these metals are familiar as catalysts. The properties of these elements are studied in this section with opportunities for a wide range of practical investigations. 3.2.5.1 General properties of transition metals (A-level only) 3.2.5.2 Substitution reactions (A-level only) 3.2.5.3 Shapes of complex ions (A-level only) 3.2.5.4 Formation of coloured ions (A-level only) 3.2.5.5 Variable oxidation states (A-level only) 3.2.5.6 Catalysts (A-level only) 3.2.6 Reactions of ions in aqueous solution (A-level only) The reactions of transition metal ions in aqueous solution provide a practical opportunity for students to show and to understand how transition metal ions can be identified by test-tube reactions in the laboratory. 3.3 Organic chemistry 3.3.1 Introduction to organic chemistry Organic chemistry is the study of the millions of covalent compounds of the element carbon. These structurally diverse compounds vary from naturally occurring petroleum fuels to DNA and the molecules in living systems. Organic compounds also demonstrate human ingenuity in the vast range of synthetic materials created by chemists. Many of these compounds are used as drugs, medicines and plastics. Organic compounds are named using the International Union of Pure and Applied Chemistry (IUPAC) system and the structure or formula of molecules can be represented in various different ways. Organic mechanisms are studied, which enable reactions to be explained. In the search for sustainable chemistry, for safer agrochemicals and for new materials to match the desire for new technology, Chemistry plays the dominant role. 3.3.1.1 Nomenclature 3.3.1.2 Reaction mechanisms 3.3.1.3 Isomerism 3.3.2 Alkanes Alkanes are the main constituent of crude oil, which is an important raw material for the chemical industry. Alkanes are also used as fuels and the environmental consequences of this use are considered in this section. 3.3.2.1 Fractional distillation of crude oil 3.3.2.2 Modification of alkanes by cracking 3.3.2.3 Combustion of alkanes 3.3.2.4 Chlorination of alkanes 3.3.3 Halogenoalkanes Halogenoalkanes are much more reactive than alkanes. They have many uses, including as refrigerants, as solvents and in pharmaceuticals. The use of some halogenoalkanes has been restricted due to the effect of chlorofluorocarbons (CFCs) on the atmosphere. 3.3.3.1 Nucleophilic substitution 3.3.3.2 Elimination 3.3.3.3 Ozone depletion 3.3.4 Alkenes In alkenes, the high electron density of the carbon–carbon double bond leads to attack on these molecules by electrophiles. This section also covers the mechanism of addition to the double bond and introduces addition polymers, which are commercially important and have many uses in modern society. 3.3.4.1 Structure, bonding and reactivity 3.3.4.2 Addition reactions of alkenes 3.3.4.3 Addition polymers 3.3.5 Alcohols Alcohols have many scientific, medicinal and industrial uses. Ethanol is one such alcohol and it is produced using different methods, which are considered in this section. Ethanol can be used as a biofuel. 3.3.5.1 Alcohol production 3.3.5.2 Oxidation of alcohols 3.3.5.3 Elimination 3.3.6 Organic analysis Our understanding of organic molecules, their structure and the way they react, has been enhanced by organic analysis. This section considers some of the analytical techniques used by chemists, including test-tube reactions and spectroscopic techniques. 3.3.6.1 Identification of functional groups by test-tube reactions 3.3.6.2 Mass spectrometry 3.3.6.3 Infrared spectroscopy 3.3.7 Optical isomerism (A-level only) Compounds that contain an asymmetric carbon atom form stereoisomers that differ in their effect on plane polarised light. This type of isomerism is called optical isomerism. 3.3.8 Aldehydes and ketones (A-level only) Aldehydes, ketones, carboxylic acids and their derivatives all contain the carbonyl group which is attacked by nucleophiles. This section includes the addition reactions of aldehydes and ketones. 3.3.9 Carboxylic acids and derivatives (A-level only) Carboxylic acids are weak acids but strong enough to liberate carbon dioxide from carbonates. Esters occur naturally in vegetable oils and animal fats. Important products obtained from esters include biodiesel, soap and glycerol. 3.3.9.1 Carboxylic acids and esters (A-level only) 3.3.9.2 Acylation (A-level only) 3.3.10 Aromatic chemistry (A-level only) Aromatic chemistry takes benzene as an example of this type of molecule and looks at the structure of the benzene ring and its substitution reactions. 3.3.10.1 Bonding (A-level only) 3.3.10.2 Electrophilic substitution (A-level only) 3.3.11 Amines (A-level only) Amines are compounds based on ammonia where hydrogen atoms have been replaced by alkyl or aryl groups. This section includes their reactions as nucleophiles. 3.3.11.1 Preparation (A-level only) 3.3.11.2 Base properties (A-level only) 3.3.11.3 Nucleophilic properties (A-level only) 3.3.12 Polymers (A-level only) The study of polymers is extended to include condensation polymers. The ways in which condensation polymers are formed are studied, together with their properties and typical uses. Problems associated with the reuse or disposal of both addition and condensation polymers are considered. 3.3.12.1 Condensation polymers (A-level only) 3.3.12.2 Biodegradability and disposal of polymers (A-level only) 3.3.13 Amino acids, proteins and DNA (A-level only) Amino acids, proteins and DNA are the molecules of life. In this section, the structure and bonding in these molecules and the way they interact is studied. Drug action is also considered. 3.3.13.1 Amino acids (A-level only) 3.3.13.2 Proteins (A-level only) 3.3.13.3 Enzymes (A-level only) 3.3.13.4 DNA (A-level only) 3.3.13.5 Action of anticancer drugs (A-level only) 3.3.14 Organic synthesis (A-level only) 3.3.15 Nuclear magnetic resonance spectroscopy (A-level only) Chemists use a variety of techniques to deduce the structure of compounds. In this section, nuclear magnetic resonance spectroscopy is added to mass spectrometry and infrared spectroscopy as an analytical technique. The emphasis is on the use of analytical data to solve problems rather than on spectroscopic theory. 3.3.16 Chromatography (A-level only) Chromatography provides an important method of separating and identifying components in a mixture. Different types of chromatography are used depending on the composition of mixture to be separated.
Grade 6 in Chem or 6-6 in Combined Science and grade 6 in Mathematics.
Paper 1 Relevant physical chemistry topics • Inorganic chemistry • Relevant practical skills Assessed • written exam: 2 hours • 105 marks • 35% of A-level Questions 105 marks of short and long answer questions Paper 2 What's assessed • Relevant physical chemistry topics • Organic chemistry • Relevant practical skills Assessed • written exam: 2 hours • 105 marks • 35% of A-level Questions 105 marks of short and long answer questions Paper 3 What's assessed • Any content • Any practical skills Assessed • written exam: 2 hours • 90 marks • 30% of A-level Questions 40 marks of questions on practical techniques and data analysis 20 marks of questions testing across the specification 30 marks of multiple choice questions
