Edexcel AS Chemistry Target sheets pages Chapter 1.1 Formulae, equations and amount of substance At the 10-11 I understand the terms atom, element, ion, molecule, compound, empirical & molecular formula (1.3a) 12-13 I can write balanced equations (full & ionic) for simple reactions, including the use of state symbols 14-15 16-17 (1.3b) I understand the terms relative atomic mass, amount of substance, molar mass & parts per million (ppm) (1.3c) 24-25 I can calculate the amount of substance in a solution of known concentration (1.3d) 18-19 I can use chemical equations to calculate reacting masses & vice versa using the concepts of amount of substance and molar mass(1.3e) 20-21 I can use chemical equations to calculate volumes of gases & vice versa using the concepts of amount of substance and molar volume of gases (1.3f) 30-31 I can use chemical equations & experimental results to deduce percentage yields & atom economies in laboratory and industrial processes and understand why they are important(1.3g) 16-17 I understand, and can carry out, calculations using the Avogadro constant (1.3h) 22-23 28-29 I can analyse & evaluate results obtained from finding a formula or confirming an equation by experiment, e.g. the reaction of lithium with water and deducing the equation from the amounts in moles of lithium and hydrogen (1.3i) 30-31 I can make a salt & calculate the percentage yield of product, e.g. preparation of a double salt (ammonium iron (II) sulphate from iron, ammonia and sulphuric acid) (1.3j) 28-29 I can carry out & interpret results of simple test tube reactions, such as replacements, reactions of acids, precipitations, to relate the observations to the state symbols used in equations and to practise writing full and ionic equations (1.3k)
pages Chapter 1.2 Energetics At the 32-33 I understand the term enthalpy change, ΔH (1.4a) 34-35 34-35 I can construct simple enthalpy level diagrams showing the enthalpy change (1.4b) 34-35 I can recall the signs for ΔH exothermic and endothermic reactions, eg illustrated by the use of exo- and endothermic reactions in hot and cold packs (1.4c) 36-39 I know the definitions of standard enthalpy changes of reaction, formation, combustion, neutralization & atomization and can use experimental data to calculate energy transferred in a reaction and hence the enthalpy change of the reaction (1.4d) 42-45 I know Hess's Law & can apply this to calculating enthalpy changes of reaction from data provided, selected from a table of data or obtained from experiments. I understand why standard data is necessary to carry out calculations of this type (1.4e) 36-39 46-47 I can evaluate the results obtained from experiments using the expression: energy transferred in joules = mass x specific heat capacity x temp change. I can comment on sources of error and assumptions made in the experiments (1.4f) 48-49 I understand the terms bond enthalpy and mean bond enthalpy, and can use bond enthalpies in Hess cycle calculations and recognise their limitations (1.4g) 48-49 I understand that bond enthalpy data gives some indication about which bond will break first in a reaction, how easy or difficult it is and therefore how rapidly a reaction will take place at room temperature (1.4g)
pages Chapter 1.3 Atomic structure and the periodic table At the 52-53 I know the definitions of relative atomic mass, relative isotopic mass & relative molecular mass and understand that they are measured relative to 1/12 mass 12 C atom (1.5a) 52-53 I understand the basic principles of a mass spectrometer & can interpret data to i) determine isotopic comp of a sample of an element, e.g. polonium ii) deduce relative atomic mass of an element iii) measure relative molecular mass of a compound(1.5b) 56-59 I can describe some uses of mass spectrometers, e.g. in radioactive dating, in space research, in sport to detect the use of anabolic steroids, in the pharmaceutical industry to provide and identifier for compounds synthesised for possible identification as drugs(1.5c) 62-63 I understand the definition of ionization energies of gaseous atoms and that they are endothermic processes(1.5d) 62-63 I can recall ideas about electronic structure developed from i) an understanding that successive ionization energies provide evidence for the existence of quantum shells and the group to which the elements belong, ii) an understanding that the first ionization energy of successive elements provides evidence for electron sub shells(1.5e) 66-67 I can describe the shapes of electron density plots (or maps) for s and p orbitals(1.5f) 64-65 I can predict electronic structure and configuration of atoms of the elements from hydrogen to krypton inclusive using 1s notation and electron in-boxes notation (recall electrons populate orbits singly before pairing up) (1.5g) 68-73 I understand that electronic structure determines the chemical properties of an element(1.5h) 68-73 I know that the periodic table is divided into blocks such as s, p and d(1.5i) 74-77 I can represent data for the elements in graphical form for elements 1 to 36 and use this to explain the meaning of the term periodic property (1.5j) 74-77 I can explain trends from periods 2 & 3 i) melting temp of elements based on given data using the structure and the bonding between the atoms or molecules of the element ii) ionization energy based on given data or recall of the shapes of the plots of ionisation energy versus atomic number using ideas of electronic structure and the way that electron energy levels vary across the period(1.5k)
pages Chapter 1.4 Bonding At the 1 ionic bonding 78-79 82-83 I can recall & interpret evidence for the existence of ions by reference to the physical properties of ionic compounds, electron density maps & migration of ions, e.g. electrolysis of aqueous copper chromate (VI) (1.6.1a) 78-79 I can describe the formation of ions in terms of electron loss or gain (1.6.1b) 78-79 I can draw electron configuration diagrams of cations and anions using dots or crosses to represent electrons (1.6.1c) 80-81 I can describe ionic crystals as giant lattices of ions (1.6.1d) 78-79 I can describe ionic bonding as the result of strong net electronic attraction between ions (1.6.1e) 80-81 I can recall trends in ionic radii down the group and for a set of isoelectronic ions, e.g. N 3- to Al 3+ (1.6.1f)? I can recall the stages in the formation of a solid ionic crystal from its elements & know that this leads to a measure value for the lattice energy (1.6.1g) 84-85 I can test the ionic model for ionic bonding of a particular compound by a comparison of lattice energies obtained from the experimental values in Born-Haber cycles, with provided values calculated from electrostatic theory (1.6.1h) 86-87 I can explain the meaning of the term polarization as applied to ions (1.6.1i) 86-87 I understand that the polarizing power of a cation depends on its radius and charge, and polarizaribility of an anion depends on its size (1.6.1j) 86-87 I understand that the polarization of anions by cations leads to some covalency in an ionic bond, based on evidence from Born-Haber cycles (1.6.1k) 84-85 I can use values calculated for standard heats of formation based on Born-Haber cycles to explain why particular ionic compounds exist, eg the relative stability of MgCl 2 over MgCl or MgCl 3 and NaCl over NaCl 2 (1.6.1l)
2 covalent bonding 90-91 I can demonstrate an understanding that covalent bonding is strong & arises from the electrostatic attraction between the nucleus & electrons which are between nuclei, based on the evidence: i ) the physical properties of giant atomic structures ii) electron density maps for simple molecules (1.6.2a) 88-91 I can draw electron configuration diagrams for simple covalently bonded molecules including those with multiple bonds and dative covalent bonds, using dots or crosses to represent electrons (1.6.2b) 3 metallic bonding 92-93 I understand that metals consist of giant lattices of metal ions in a sea of delocalised electrons (1.6.3a) 92-93 I can describe metallic bonding as the strong attraction between metal ions and the sea of delocalised electrons (1.6.3b) 92-93 I can use the models in 1.6.3a and 1.6.3b to interpret simple properties of metals e.g. conductivity & melting temperatures (1.6.3c)
pages Chapter 1.5 Introductory organic chemistry At the 100-103 I understand that a series of organic compounds is characterised by a general formula with one or more functional groups (1.7.1a) 100-103 I can apply the rules of IUPAC nomenclature to organic compounds and draw these compounds, as I encounter them, using structural, displayed & skeletal formulae (1.7.1b) 94-99 I appreciate the difference between hazard and risk (1.7.1c) 94-99 I understand the hazards associated with organic compounds and why it is necessary to carry out risk assessments when dealing with potentially hazardous materials (1.7.1d) 94-99 I can suggest ways that risk can be reduced and reactions can be carried out safely by: i) working on a smaller scale ii) taking specific precautions or using alternative techniques depending on properties of substances involved carrying out reaction using alternative method that involves less hazardous substances (1.7.1d) pages Chapter 1.6 The Alkanes At the 104-105 I can state the general formula of alkanes and understand that they are saturated hydrocarbons which contain single bonds only (1.7.2a) 106-107 I can explain the existence of structural isomers using alkanes (up to C 5 ) as examples (1.7.2b) 108-113 I know that alkanes are used as fuels and obtained from the fractional distillation, cracking and reformation of crude oil (1.7.2c) 120-123 I can discuss the reasons for developing alternative fuels in terms of sustainability & reducing emission of CO2 & its relationship to climate change (1.7.2d) 114-117 118-119 I can describe the reactions of alkanes in terms of combustion, substitution by chlorine showing the mechanism of free radical substitution in terms of initiation, propagation and termination, and using curly half-arrows in the mechanism to show the formation of free radicals in the initiation step using a single dot to represent the unpaired electron (1.7.2e)
Pages Chapter 1.7 The alkenes At the 124-128 I can state the general formula of alkenes and understand that they are unsaturated hydrocarbons with a carbon-carbon double bond which consists of a σ and a π bond (1.7.3a) 124-128 I can explain E-Z isomerism (geometric /cis/trans isomerism) in terms of restricted rotation around a C=C double bond and the nature of substituents on the carbon atoms (1.7.3b) 124-128 I can show an understanding of the E- Z- naming system and why it is necessary to use this when the cis- trans- naming system breaks down (1.7.3c) 129-131 I can describe the addition reactions of alkenes, limited to: i) addition of hydrogen with nickel catalyst to form alkane ii) addition of halogens to produce disubstituted halogenoalkanes iii) addition of hydrogen halides to produce mono-substituted halogenoalkanes iv) oxidation of the double bond by potassium manganate (VII) to produce a diol (1.7.3d) 132-133 I can describe the mechanism (including diagrams), giving evidence where possible of: i) electrophillic addition of bromine and hydrogen bromide to ethane ii) the electrophillic addition of hydrogen bromide to propene (1.7.3e) 129-131 I can describe the test for presence of C=C using bromine water and understand that the product is the addition of OH and Br (1.7.3f) 134-135 I can describe addition polymerization of alkenes and ID the repeat unit given the monomer and vice versa (1.7.3g) 136-141 I can interpret given information about the uses of energy and resources over the life-cycle of polymer products to show how the use of renewable resources, recycling and energy recovery can contribute to more sustainable use of materials (1.7.3h)