Chemistry

Atomic Structure

• Recall calculating relative atomic mass and rearranging this calculation 
• Explain how mass spectrometer works and what it measures 
• Calculate TOF for given ions 
• Interpret simple mass spectra of elements and calculate relative atomic mass 
• Write electron configurations of atoms and ions in terms of s, p and d electrons 
• Identify an element from its successive ionisation energies 
• Describe general trends in ionisation energies 

Amount of Substances

• Define relative atomic mass (Ar), relative molecular mass (molecular compounds) (Mr) or formula mass (ionic compounds) (Mr) in terms of 12C. 
• Use the expression n=m/Mr to calculate mass of substance, Mr, and amount in moles 
• Use the expression n=C/V to calculate concentration, volume and amount of substance (moles) in a solution. 
• Use the ideal gas equation  pV = nRT  to calculate any of the variables p, V n, R or T converting units correctly. 
• Calculate Empirical Formula given data on composition by mass or percentage by mass.
• Calculate Molecular Formula from the Empirical Formula and relative molecular mass. 

Bonding

• Explain the properties of ionic compounds using an understanding of ionic bonding. Draw dot and cross diagrams for covalently bonded compounds with multiple bonds. 
• Explain why some molecules are polar and deduce whether a molecule has a permanent dipole 
• Explain why electronegativity trends. 
• Explain how melting and boiling points are influenced by these intermolecular forces. 
• Predict the shape and give bond angles of simple molecules and ions up to six electron pairs. 

Energetics

• How do we draw enthalpy diagrams and perform calorimetry calculations
• Construct hesses cycles and perform hesses cycle calculations for the enthalpy of combustion and formation  
• Conduct Bond enthalpy calculations and calculate missing bond enthalpy values

Oxidation, Reduction and REDOX

Periodicity, Group 2 and Group 4

• Describe and explain the trends across Period 3 
• Write equations for group 2 metals and explain trends in solubility of group 2 sulphates and hydroxides 
• Explain the uses of group 2 compounds 
• Describe and explain the trends down group 7 and in oxidising power of the halogens, illustrated by displacement reactions of halide ions an construct half and ionic equations.  
• Describe and explain the trends in reducing power of the halide ions, illustrated by reactions of concentrated sulfuric acid with solid sodium halides.
• Describe disproportionation reactions and describe the reactions of chlorine with water. 
• Determine the oxidation of elements in a compounds and practice half equations and combining them  

Introduction to Organic Chemistry

• Apply IUPAC rules for nomenclature to name and draw structural and skeletal organic compounds limited to chains and rings with up to six carbon atoms each 
• Draw the structures of chain, position and functional group isomers 
• Draw the structural formulas of E and Z isomers 

Alkanes and Haloalkanes

• To be to write equations for initiation, propagation, and termination and explain the formation of a mixture of organic products.  
• Explain the how fractional distillation, catalytic and thermal cracking work 
• Describe the combustion of alkanes  
• Explain how and why Halogenoalkanes undergo substitution reactions with the nucleophiles  
• Outline the nucleophilic substitution mechanisms of reactions and explain the relative rates of reactions 
• Show the mechanism for elimination reactions in haloalkanes 
• Explain the conditions that favour an elimination reaction rather than substitution 
• Use equations, such as the following, to explain how chlorine atoms catalyse decomposition of ozone 

Alkenes and alcohols

Organic Analysis

• Explain how alkenes undergo addition reactions with electrophiles 
• Outline the addition mechanisms of reactions 
• Explain the formation of major and minor products by reference to the relative stabilities of primary, secondary and tertiary carbocation intermediates. 
• Explain why making bioethanol from fermentation of glucose is carbon neutral, using balanced symbol equations. 
• Outline the mechanism for the formation of an alcohol by the reaction of an alkene with steam in the presence of an acid catalyst and the dehydration of a alcohol 
• Write equations for these oxidation reactions for primary, secondary or tertiary alcohols (equations showing [O] as oxidant are acceptable)
• Use chemical tests to distinguish between aldehydes and ketones including Fehling’s solution and Tollens’ reagent 

Kinetics

• Describe what must happen before a reaction will take place. Explain why factors affect the rate of reaction. Explain why all collision do not result in a reaction 
• Explain how temperature affects the number of molecules with energy equal to or more than the activation energy 
• Explain why a small increase in temperature has a large effect on rate of reaction 
• To use a Maxwell–Boltzmann distribution to help explain how a catalyst increases the rate of a reaction involving a gas. 
• To describe homogeneous and heterogenous catalyst

Equilibria 

• Use Le Chatelier’s principle to predict qualitatively 
• The effect of changes in temperature, pressure and concentration on the position of equilibrium 
• Explain why, for a reversible reaction used in an industrial process, a compromise temperature and pressure maybe used. 
• To construct an expression for Kc for a homogenous system in equilibrium  
• To calculate a value for Kc from the equilibrium concentrations at constant temperature using ICE Tables  
• Predict qualitative effects of changes if temp, conc., pressure, catalyst on the value of Kc 

Thermodynamics

• How do we define, represent and calculate parts of the Born-Haber cycle. 
• Explain the perfect ionic model provide evidence for covalent character in ionic compounds.
• How do we calculate and define enthalpies of solution for ionic compounds from lattice enthalpies and enthalpies of hydration. 
• Use a graph and ∆G = ∆H – T∆S to determine entropy, enthalpy and temperature to when a reaction becomes feasible. 

Kinetics

• Construct, define and perform calculations with rate equations 
• Use given rate data and deduce a rate equation, determine the rate constant and its units 
• Perform calculations, rearrange and plot a straight-line graph to find Ea using the Arrhenius equation k = Ae-Ea/RT 
• Use the order with respect to reactants to provide information about the rate determining step of a reaction and vice versa 

Acid and Bases

• What is a  Bronsted-Lowry acid and bases and determine conjugate acid-base pairs 
• Determine and perform calculations of strong acids using pH = –log10[H+] and weak acids using Ka =[A-][H+]/[HA] 
• Prove Kw ionisation of water KW = [H+][OH–] and use it to find the pH of strong bases 
• Explain the action of buffers and find the pH of buffer solutions  
• Sketch and explain shapes of pH curves and use pH curves to select appropriate indicators 

Animes

• Explain the difference in base strength between ammonia, primary, secondary, tertiary and aromatic amines  
• Explain how primary amines can be produced from reactions of halogenoalkanes and the reduction of nitriles. 
• Explain how phenylamines are produced from reduction of nitrobenzene's 
• Outline the mechanisms nucleophilic substitution reactions involving amines and nucleophilic addition–elimination reactions of ammonia and primary amines with acyl chlorides. 
• Explain the use of quaternary ammonium salts as cationic surfactants. 

Amino Acids, Proteins and DNA, Chromatography & polymers

• How do we draw chemical structures of DNA strands and different amino acid in different conditions. 
• How can we explain how amino acids are hydrolysed and form peptides 
• How is thin layer chromatography used to separate out and identify amino acids 
• How do we represent and dispose of condensation & addition polymer's  

Organic synthesis and Structure Determination

• Practice applying all the knowledge of reagents and mechanisms in organic chemistry to planning sequences for producing organic compounds 
• How do we use HNMR and CNMR used to determine structures and how can these rules be used to apply to more challenging spectra and problems  

Transition Metals

• How do we explain characteristics of transition metal complexes including bidentate and multidentate ligands and write electronic configurations for TM metals atoms and ions. 
• Explain what happens and what you observe during ligand substitution reactions and explain the chelate effect in terms of entropy and enthalpy 
• Sketch shapes of transition metal complex ions and explain how cis-trans and optical isomerism arise 
• Understand why transition metal ions are coloured and what affects the colour and use colorimetry to measure concentration of solutions. 
• What are the variable oxidation states when Vanadate ions are reduced 
• How do we do calculations of redox titrations including MnO4– with Fe2+ and C2O42– in acidic solution. 
• How do homogenous and heterogenous catalysts work and how are they poisoned  

Electrochemical Cells

Transition Metals & Reactions of Inorganic Compounds

• What are the reaction of metal-aqua ions (Fe2+, Cu2+, Al3+, Fe3+) with bases OH–, NH3, CO32– 
• Explain why [M(H2O)6]3+ ions are more acidic than [M(H2O)6]2+ ions. 
• How do we write and apply the conventional representation of cells    
• What are the standard electrode potential conditions
• How do we use the electrode potential values to calculate and predict the direction of simple redox reactions  

Revision Programme - Physical and Organic

• How do we apply basic calculations involving moles to more complex processed such as titrations, percentage by mass, reacting masses/limiting reagents How do we perform long answer back redox titrations 
• How do we perform empirical and molecular formula calculations and apply this to calculations around waters of crystallization  
• How do we recall reacting masses and density to find theoretical mass then percentage yield  
• Recall conditions and draw the mechanisms for nitration of benzene and acylation of a benzene ring 
• Apply IUPAC rules for nomenclature to name and draw organic compounds limited to chains and rings with up to six carbon atoms each 
• Revise how we draw a dipeptide and reactions with amino acids, How are zwitterions represented in different pH and How do the draw a nucleotide and complementary base pairs 

Revision Programme - Physical and Inorganic

• Recall and practice isomerism, Ligand exchange, colorimetry calculations, catalysis and redox titrations 
• Recap calculations involving Ka and Kw and applying this to buffer calculations 
• How do we use EMF values to predict the feasibility of redox reactions and review 
• Use Born Haber cycles to successfully complete calculations and use the Gibbs free energy equation to find feasible temperatures, enthalpy and entropy. 
• Rearrange and substitute equations on TOF calculations.  
• Explain the reactions of group 7 halides in terms of their reducing and oxidising ability 
• To recall finding equilibrium constants(Kc), molar fractions and Kp