Term 1: Module 2 - Atoms and reactions
This section builds directly from GCSE Science, starting with basic atomic structure and isotopes. Important basic chemical skills are developed: writing chemical formulae, constructing equations and calculating chemical quantities using the concept of amount of substance. The role of acids, bases and salts in chemistry is developed in the context of neutralisation reactions.
Assessment happens continuously through classwork and homework activities. There is at least one formal assessment each term to monitor progress and assess the content covered in lessons up to the assessment point. Practical activities are embedded within the learning outcomes of the course to ensure achievement of the practical endorsement. Students also assessed in their practical skills through completion of PAG 1.1- Determination of the composition of copper(II) carbonate basic.
Atom
The basic units of matter and the defining structure of elements.
Isotope
Isotopes are forms of an element that have the same number of protons but different numbers of neutrons.
Ionic bond
The electrostatic force of attraction between a positively charged metal ion and a negatively charged non-metal ion.
Mole
A standard scientific unit for measuring large quantities of very small entities such as atoms, molecules, or other specified particles.
Empirical formula
The simplest whole number ratio of atoms of each element present in a compound.
Molecular formula
The number and type of atoms of each element in a molecule.
Anhydrous
A substance, especially a crystalline compound, containing no water.
Stoichiometric
Relating to or denoting quantities of reactants in simple integral ratios, as prescribed by an equation or formula.
Yield
How much product is obtained compared to the maximum possible mass.
Atom economy
The atom economy of a reaction gives the percentage of atoms in reactants that form a desired product.
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Term 2: Bonding and structure and basics of organic chemistry.
This section introduces the concept of atomic orbitals and develops a deeper understanding of electron configurations linked to the periodic table. The central role of electrons in ionic and covalent bonding is then studied. The important role of molecules is studied, including an explanation of polarity, intermolecular forces and how bonding and structure contribute to properties of substances. Students are also introduced to the fundamentals of organic chemistry. This section introduces the various types of structures used routinely in organic chemistry, nomenclature, and the important concepts of homologous series, functional groups, isomerism and reaction mechanisms using curly arrows. The initial ideas are then developed within the context of alkanes.
Assessment happens continuously through classwork and homework activities. There is at least one formal assessment each term to monitor progress and assess the content covered in lessons up to the assessment point. Practical activities are embedded within the learning outcomes of the course to ensure achievement of the practical endorsement. Students also assessed in their practical skills through completion of PAG 2.1- Determination of the concentration of hydrochloric acid.
Electron
The negatively charged particles of atom.
Atomic Orbitals
Describe where an electron is likely to be found in an atom.
Giant ionic lattice
A structure created by the arrangement of ions.
Covalent bond
The strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms.
Ionic bond
The electrostatic attraction between positive and negative ions.
Dative covalent
A dative bond (also called a co-ordinate covalent bond) is a covalent bond (a shared pair of electrons) in which both electrons come from the same atom.
Average bond enthalpy
A measurement of covalent bond strength.
Electronegativity
The ability of an atom to attract the bonding electrons in a covalent bond.
Dipole
A molecule which has areas of asymmetrical positive and negative charge.
Intermolecular forces
Are the attractive and repulsive forces that arise between the molecules of a substance
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Term 3: The Periodic Table, Alkenes, Alcohols and haloalkanes
In this section Periodic trends are first studied to extend the understanding of structure and bonding. Group properties are then studied using Group 2 and the halogens as typical metal and non-metal groups respectively, allowing an understanding of redox reactions to be developed further. Furthermore, this unit also introduces three further functional groups: alkenes, alcohols and haloalkanes, and considers the importance of polarity and bond enthalpy to organic reactions.
Assessment happens continuously through classwork and homework activities. There is at least one formal assessment each term to monitor progress and assess the content covered in lessons up to the assessment point. Practical activities are embedded within the learning outcomes of the course to ensure achievement of the practical endorsement. There are no set PAGs for this unit, but students will complete practical work to aid understanding.
First Ionisation Energy
The removal of one mole of electrons from one mole of gaseous atoms
Giant Covalent Lattice
A network of atoms bonded by strong covalent bonds (e.g. carbon (diamond, graphite and graphene) and silicon)
Giant Metallic Lattice Structure
The structure of all metals, made up of cations and delocalised electrons.
Periodicity
A repeating trend in physical and chemical properties across the periods of the periodic table.
Successive Ionisation Energies
The energy required to remove each electron one-by-one from one mole of gaseous atoms / ions.
Redox
A reaction in which oxidation of one element and reduction of another occurs.
Disproportionation
The oxidation and reduction of the same element
Precipitation Reaction
A reaction in which two aqueous solutions are combined to form an insoluble salt (a precipitate)
Qualitative Analysis
Identifying the elements present in a substance, typically using test-tube reactions.
Average Bond Enthalpy
The energy required to break one mole of gaseous bonds.
Enthalpy Change (ΔH)
The change in the heat content of a system during a reaction.
Enthalpy Change of Combustion (ΔcH)
The enthalpy change that takes place when one mole of a substance is completely combusted.
Enthalpy Change of Neutralisation (ΔneutH)
The enthalpy change that takes place when one mole of water is formed from a neutralisation reaction.
Enthalpy Change of Reaction (ΔrH)
The enthalpy change that is associated with a particular chemical equation.
Boltzmann Distribution
A graph showing the distribution of the energies of molecules in relation to the activation energy. I
Heterogeneous Catalyst
A catalyst that is in a different state to the reactants (e.g. a solid catalyst with gaseous reactants).
Homogeneous catalyst
A catalyst which is in the same state as the reactants.
Le Chatelier’s Principle
When a system in dynamic equilibrium is subject to change, the position of equilibrium will shift to minimise the change
Kc
The equilibrium constant that is equal to the concentration of products raised to their stoichiometric coefficients divided by the concentration of reactants to the power of their stoichiometric coefficients.
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Term 4: Enthalpy changes and Organic synthesis
This section introduces physical chemistry within the general theme of energy. Learners first learn about the importance of enthalpy changes, their uses and determination from experimental results including enthalpy cycles. Furthermore, students learn how to devise two stage synthetic routes by applying transformations between all the functional groups they encountered so far. Throughout this section, there are many opportunities for developing organic practical skills, including preparation and purification of organic liquids
Assessment happens continuously through classwork and homework activities. There is at least one formal assessment each term to monitor progress and assess the content covered in lessons up to the assessment point. Practical activities are embedded within the learning outcomes of the course to ensure achievement of the practical endorsement. Students also assessed in their practical skills through completion of PAGs 4.1 Identifying unknowns 1 and 5.2 Preparation of cyclohexene.
Alicyclic
An aliphatic compound that is arranged in non-aromatic rings (with or without side chains).
Aliphatic
A compound containing carbon and hydrogen atoms joined in straight or branched chains or in non-aromatic rings.
Aromatic
An organic compound containing a benzene ring.
Curly arrow
Shows the movement of a pair of electrons. Curly arrows must start from a bond, a lone pair of electrons or a negative change
Displayed Formula
The relative positions of atoms and the bonds between them.
Empirical Formula
The simplest whole number ratio of atoms of each element present in a compound.
Functional Group
A group of atoms responsible for the characteristic reactions of a compound.
General Formula
The simplest algebraic formula of a member of a homologous series.
Heterolytic Fission
When a covalent bond breaks, one bonding atom receives both electrons from the bonded pair.
Homologous Series
A series of organic compounds containing the same functional group with successive members differing by -CH2 .
Reaction Mechanism
A series of steps that represent the overall reaction by showing the breaking and forming of bonds using curly arrows.
Skeletal Formula
The simplified organic formula, shown by removing hydrogen atoms from alkyl chains, leaving the carbon skeleton and the functional groups.
Radical Substitution
A type of substitution reaction in which a radical replaces another atom/ group of atoms in a compound.
Nucleophilic Substitution
A reaction in which an electron pair donor attacks an electrophilic atom (an atom with a partial or full positive charge) to replace an atom / group of atoms.
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Term 5: Reaction rates and analytical techniques
In this unit students learn about the ways in which a change in conditions can affect the rate of a chemical reaction, in terms of activation energy, the Boltzmann distribution and catalysis. Reversible reactions are then studied, including the dynamic nature of chemical equilibrium and the influence of conditions upon the position of equilibrium. Students also learn about, the integrated roles of enthalpy changes, rates, catalysts, and equilibria as a way of increasing yield and reducing energy demand, improving the sustainability of industrial processes. Students also learn about the important techniques of infrared spectroscopy and mass spectrometry and how these are used to as a valuable tool for identifying organic compounds.
Assessment happens continuously through classwork and homework activities. There is at least one formal assessment each term to monitor progress and assess the content covered in lessons up to the assessment point. Practical activities are embedded within the learning outcomes of the course to ensure achievement of the practical endorsement. Students also assessed in their practical skills through completion of PAG 3.1- Determination of the enthalpy change of neutralisation.
Enthalpy Change (ΔH)
The change in the heat content of a system during a reaction.
Enthalpy Change of Combustion (ΔcH)
The enthalpy change that takes place when one mole of a substance is completely combusted.
Enthalpy Change of Formation (ΔfH)
The enthalpy change that takes place when one mole of a compound is formed from its elements.
Enthalpy Change of Neutralisation (ΔneutH)
The enthalpy change that takes place when one mole of water is formed from a neutralisation reaction.
Enthalpy Change of Reaction (ΔrH)
The enthalpy change that is associated with a particular chemical equation.
Standard Conditions
A pressure of 100 kPa and a temperature of 298K.
Boltzmann Distribution
A graph showing the distribution of the energies of molecules in relation to the activation energy.
Collision Theory
The theory which states that molecules must collide with sufficient energy at the correct orientation for a reaction to occur.
Le Chatelier’s Principle
When a system in dynamic equilibrium is subject to change, the position of equilibrium will shift to minimise the change.
Kc
The equilibrium constant that is equal to the concentration of products raised to their stoichiometric coefficients divided by the concentration of reactants to the power of their stoichiometric coefficients.
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Term 6: Rates equilibrium and pH
The largely qualitative treatment of reaction rates and equilibria encountered in Module 3 is developed within a quantitative and graphical context. This section also allows learners to develop practical quantitative techniques involved in the determination of reaction rates and pH. There are many opportunities for developing mathematical skills, including use of logarithms and exponents, when studying the content of this section and when carrying out quantitative practical work.
Assessment happens continuously through classwork and homework activities. There is at least one formal assessment each term to monitor progress and assess the content covered in lessons up to the assessment point. Practical activities are embedded within the learning outcomes of the course to ensure achievement of the practical endorsement. Students also assessed in their practical skills through completion of PAGs 7.1 - Identifying organic unknowns 1 and 9.2- Rates of reaction. Furthermore, students sit an end of year 12 exam which covers all the content (modules 1,2,3 and 4) that students have studied in year 12.
Alcohol
An organic compound containing the OH functional group. The polarity of the OH functional group means that alcohols can form hydrogen bonds and are soluble in water (when the alkyl chain is short)..
Aldehyde
An organic compound containing the -CHO functional group.
Carboxylic Acid
An organic compound containing the -COOH functional group.
Haloalkanes
An organic compound containing a halogen atom (F/ Cl/ Br/ I) bound to an alkyl chain.
Ketone
An organic compound containing the C=O functional group in the middle of an alkyl chain.
CFC
A class of compound made up of carbon, fluorine and chlorine, used as refrigerants and aerosol propellants.
Radical
A species with an unpaired electron (e.g. •Cl).
Reflux
The continual boiling and condensing of a reaction mixture. This is to ensure that the reaction goes to completion. During reflux, the condenser must be positioned vertically.
Synthetic Route
A series of steps that are followed to make a specific compound.
Elemental Analysis
A sample is analysed to determine the proportion of elements that make up the compound present.
Fragmentation
During mass spectrometry, unstable molecular ions break down into smaller fragments.
Infrared Spectroscopy
A technique used to identify particular bonds and functional groups within a molecule
Mass spectrometry
A technique used to identify compounds and determine relative molecular mass.
M+1 Peak
A small peak on a mass spectrum caused by the presence of a small proportion of carbon-13.
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