Home All Resources Login

Home All Resources Past Papers Syllabus Notes Revision Qns Tutors Login

Chemistry

0620

Describe the properties of alkenes in terms of addition reactions with: (a) bromine or aqueous bromine (b) hydrogen in the presence of a nickel catalyst (c) steam in the presence of an acid catalyst and draw the structural or displayed formulae of th State that some of these substances are potentially harmful, including: (a) some metal compounds are toxic (b) some plastics harm aquatic life (c) sewage contains harmful microbes which cause disease (d) nitrates and phosphates lead to deoxygenation State the source of each of these air pollutants, limited to: (a) carbon dioxide from the complete combustion of carbon-containing fuels (b) carbon monoxide and particulates from the incomplete combustion of carbon-containing fuels (c) methane from t State and explain strategies to reduce the effects of these environmental issues, limited to: (a) climate change: planting trees, reduction in livestock farming, decreasing use of fossil fuels, increasing use of hydrogen and renewable energy, e.g. wi Describe the manufacture of ethanol by: (a) fermentation of aqueous glucose at $25-35^{circ} mathrm{C}$ in the presence of yeast and in the absence of oxygen (b) catalytic addition of steam to ethene at $300^{circ} mathrm{C}$ and $6000 mathrm{kPa} / Name the uses of the fractions as: (a) refinery gas fraction for gas used in heating and cooking (b) gasoline/petrol fraction for fuel used in cars (c) naphtha fraction as a chemical feedstock (d) kerosene/paraffin fraction for jet fuel (e) diesel oi Calculate stoichiometric reacting masses, limiting reactants, volumes of gases at r.t.p., volumes of solutions and concentrations of solutions expressed in $mathrm{g} / mathrm{dm}^3$ and $mathrm{mol} / mathrm{dm}^3$, including conversion between $mat Describe the formation of covalent bonds in simple molecules, including $mathrm{H}_2, mathrm{Cl}_2, mathrm{H}_2 mathrm{O}, mathrm{CH}_4, mathrm{NH}_3, mathrm{HCl}, mathrm{CH}_3 mathrm{OH}, mathrm{N}_2, mathrm{O}_2, mathrm{CO}_2$ and $mathrm{N}_2$. Us Describe the extraction of iron from hematite in the blast furnace, limited to: (a) the burning of carbon (coke) to provide heat and produce carbon dioxide (b) the reduction of carbon dioxide to carbon monoxide (c) the reduction of iron(III) oxide by Describe the general solubility rules for salts: (a) sodium, potassium and ammonium salts are soluble (b) nitrates are soluble (c) chlorides are soluble, except lead and silver (d) sulfates are soluble, except barium, calcium and lead (e) carbonates Explain in terms of structure and bonding the properties of simple molecular compounds: (a) low melting points and boiling points in terms of weak intermolecular forces (specific types of intermolecular forces are not required) (b) poor electrical co State the adverse effect of these air pollutants, limited to: (a) carbon dioxide: higher levels of carbon dioxide leading to increased global warming, which leads to climate change (b) carbon monoxide: toxic gas (c) particulates: increased risk of re Name and draw the structural and displayed formulae of unbranched: (a) alkanes (b) alkenes, including but-1-ene and but-2-ene (c) alcohols, including propan-1-ol, propan-2-ol, butan-1-ol and butan-2-ol (d) carboxylic acids containing up to four carbo Describe the reactions, if any, of: (a) potassium, sodium and calcium with cold water (b) magnesium with steam (c) magnesium, zinc, iron, copper, silver and gold with dilute hydrochloric acid and explain these reactions in terms of the position of th Describe the uses of metals in terms of their physical properties, including: (a) aluminium in the manufacture of aircraft because of its low density (b) aluminium in the manufacture of overhead electrical cables because of its low density and good e Describe the general characteristics of a homologous series as: (a) having the same functional group (b) having the same general formula (c) differing from one member to the next by a $-mathrm{CH}_2$ - unit (d) displaying a trend in physical properti Describe and explain the effect on the rate of reaction of: (a) changing the concentration of solutions (b) changing the pressure of gases (c) changing the surface area of solids (d) changing the temperature (e) adding or removing a catalyst, includi Describe the substitution reaction of alkanes with chlorine as a photochemical reaction, with ultraviolet light providing the activation energy, $E_{mathrm{a}}$, and draw the structural or displayed formulae of the products, limited to monosubstituti State the symbol equations for the extraction of iron from hematite (a) $mathrm{C}+mathrm{O}_2 ightarrow mathrm{CO}_2$ (b) $mathrm{C}+mathrm{CO}_2 ightarrow 2 mathrm{CO}$ (c) $mathrm{Fe}_2 mathrm{O}_3+3 mathrm{CO} ightarrow 2 mathrm{Fe}+3 mathrm{C Describe tests using aqueous sodium hydroxide and aqueous ammonia to identify the aqueous cations: (a) aluminium, $mathrm{Al}^{3+}$ (b) ammonium, $mathrm{NH}_4{ }^{+}$ (c) calcium, $mathrm{Ca}^{2+}$ (d) chromium(III), $mathrm{Cr}^{3+}$ (e) copper(II) Define structural isomers as compounds with the same molecular formula, but different structural formulae, including $mathrm{C}_4 mathrm{H}_{10}$ as $mathrm{CH}_3 mathrm{CH}_2 mathrm{CH}_2 mathrm{CH}_3$ and $mathrm{CH}_3 mathrm{CH}left(mathrm{CH}_3 i Identify redox reactions by changes in oxidation number using: (a) the oxidation number of elements in their uncombined state is zero (b) the oxidation number of a monatomic ion is the same as the charge on the ion (c) the sum of the oxidation number Describe tests to identify the anions: (a) carbonate, $mathrm{CO}_3{ }^{2-}$, by reaction with dilute acid and then testing for carbon dioxide gas (b) chloride, $mathrm{Cl}^{-}$, bromide, $mathrm{Br}^{-}$, and iodide, $mathrm{I}^{-}$, by acidifying w Describe a: (a) solvent as a substance that dissolves a solute (b) solute as a substance that is dissolved in a solvent (c) solution as a mixture of one or more solutes dissolved in a solvent (d) saturated solution as a solution containing the maximu Describe tests to identify the gases: (a) ammonia, $mathrm{NH}_3$, using damp red litmus paper (b) carbon dioxide, $mathrm{CO}_2$, using limewater (c) chlorine, $mathrm{Cl}_2$, using damp litmus paper (d) hydrogen, $mathrm{H}_2$, using a lighted spli Identify the products formed at the electrodes and describe the observations made during the electrolysis of: (a) molten lead(II) bromide (b) concentrated aqueous sodium chloride (c) dilute sulfuric acid using inert electrodes made of platinum or car State the distinguishing properties of solids, liquids and gases Describe the structures of solids, liquids and gases in terms of particle separation, arrangement and motion Describe changes of state in terms of melting, boiling, evaporating, freezing and condensing Describe the effects of temperature and pressure on the volume of a gas Explain changes of state in terms of kinetic particle theory, including the interpretation of heating and cooling curves Explain, in terms of kinetic particle theory, the effects of temperature and pressure on the volume of a gas Describe and explain diffusion in terms of kinetic particle theory Describe and explain the effect of relative molecular mass on the rate of diffusion of gases Describe the differences between elements, compounds and mixtures Describe the structure of the atom as a central nucleus containing neutrons and protons surrounded by electrons in shells State the relative charges and relative masses of a proton, a neutron and an electron Define proton number/atomic number as the number of protons in the nucleus of an atom Define mass number / nucleon number as the total number of protons and neutrons in the nucleus of an atom Determine the electronic configuration of elements and their ions with proton number 1 to 20, e.g. 2,8,3 State that: (a) Group VIII noble gases have a full outer shell (b) the number of outer shell electrons is equal to the group number in Groups I to VII (c) the number of occupied electron shells is equal to the period number Define isotopes as different atoms of the same element that have the same number of protons but different numbers of neutrons Interpret and use symbols for atoms, e.g. ${}_6^{12} mathrm{C}$, and ions, e.g. ${}_{17}^{35} mathrm{Cl}^{-}$ State that isotopes of the same element have the same chemical properties because they have the same number of electrons and therefore the same electronic configuration Calculate the relative atomic mass of an element from the relative masses and abundances of its isotopes Describe the formation of positive ions, known as cations, and negative ions, known as anions State that an ionic bond is a strong electrostatic attraction between oppositely charged ions Describe the formation of ionic bonds between elements from Group I and Group VII, including the use of dot-and-cross diagrams Describe the properties of ionic compounds: (a) high melting points and boiling points (b) good electrical conductivity when aqueous or molten and poor when solid State that a covalent bond is formed when a pair of electrons is shared between two atoms leading to noble gas electronic configurations Describe the giant covalent structures of graphite and diamond Relate the structures and bonding of graphite and diamond to their uses, limited to: (a) graphite as a lubricant and as an electrode (b) diamond in cutting tools Describe the giant covalent structure of silicon(IV) oxide, $mathrm{SiO}_2$ Describe the similarity in properties between diamond and silicon(IV) oxide, related to their structures Describe metallic bonding as the electrostatic attraction between the positive ions in a giant metallic lattice and a 'sea' of delocalised electrons Explain in terms of structure and bonding the properties of metals: (a) good electrical conductivity (b) malleability and ductility State the formulae of the elements and compounds named in the subject content Define the molecular formula of a compound as the number and type of different atoms in one molecule Deduce the formula of a simple compound from the relative numbers of atoms present in a model or a diagrammatic representation Construct word equations and symbol equations to show how reactants form products, including state symbols Define the empirical formula of a compound as the simplest whole number ratio of atoms or ions in a compound Deduce the formula of an ionic compound from the relative numbers of the ions present in a model or a diagrammatic representation or from the charges on the ions Construct symbol equations with state symbols, including ionic equations Deduce the symbol equation with state symbols for a chemical reaction, given relevant information Describe relative atomic mass, $A_r$ as the average mass of the isotopes of an element compared to $1 / 12$ th of the mass of an atom of ${ }^{12} mathrm{C}$ Define relative molecular mass, $M_r$ as the sum of the relative atomic masses. Relative formula mass, $M_r$ will be used for ionic compounds Calculate reacting masses in simple proportions. Calculations will not involve the mole concept State that concentration can be measured in $mathrm{g} / mathrm{dm}^3$ or $mathrm{mol} / mathrm{dm}^3$ State that the mole, mol, is the unit of amount of substance and that one mole contains $6.02 imes 10^{23}$ particles, e.g. atoms, ions, molecules; this number is the Avogadro constant Use the relationship amount of substance $(mathrm{mol})=frac{ ext { mass }(mathrm{g})}{ ext { molar mass } (mathrm{g} / mathrm{mol})}$ Use experimental data from a titration to calculate the moles of solute, or the concentration or volume of a solution Calculate empirical formulae and molecular formulae, given appropriate data Calculate percentage yield, percentage composition by mass and percentage purity, given appropriate data Define electrolysis as the decomposition of an ionic compound, when molten or in aqueous solution, by the passage of an electric current Identify in simple electrolytic cells: (a) the anode as the positive electrode (b) the cathode as the negative electrode (c) the electrolyte as the molten or aqueous substance that undergoes electrolysis State that metals or hydrogen are formed at the cathode and that non-metals (other than hydrogen) are formed at the anode Predict the identity of the products at each electrode for the electrolysis of a binary compound in the molten state State that metal objects are electroplated to improve their appearance and resistance to corrosion Describe how metals are electroplated Describe the transfer of charge during electrolysis to include: (a) the movement of electrons in the external circuit (b) the loss or gain of electrons at the electrodes (c) the movement of ions in the electrolyte Identify the products formed at the electrodes and describe the observations made during the electrolysis of aqueous copper(II) sulfate using inert carbon/graphite electrodes and when using copper electrodes Predict the identity of the products at each electrode for the electrolysis of a halide compound in dilute or concentrated aqueous solution Construct ionic half-equations for reactions at the anode (to show oxidation) and at the cathode (to show reduction) State that a hydrogen-oxygen fuel cell uses hydrogen and oxygen to produce electricity with water as the only chemical product Describe the advantages and disadvantages of using hydrogen-oxygen fuel cells in comparison with gasoline/petrol engines in vehicles State that an exothermic reaction transfers thermal energy to the surroundings leading to an increase in the temperature of the surroundings State that an endothermic reaction takes in thermal energy from the surroundings leading to a decrease in the temperature of the surroundings Interpret reaction pathway diagrams showing exothermic and endothermic reactions State that the transfer of thermal energy during a reaction is called the enthalpy change, $Delta H$, of the reaction. $Delta H$ is negative for exothermic reactions and positive for endothermic reactions Define activation energy, $E_{a}$, as the minimum energy that colliding particles must have to react Draw and label reaction pathway diagrams for exothermic and endothermic reactions using information provided, to include: (a) reactants (b) products (c) enthalpy change of the reaction, $Delta H$ (d) activation energy, $E_{mathrm{a}}$ State that bond breaking is an endothermic process and bond making is an exothermic process and explain the enthalpy change of a reaction in terms of bond breaking and bond making Calculate the enthalpy change of a reaction using bond energies Identify physical and chemical changes, and describe the differences between them Describe the effect on the rate of reaction of: (a) changing the concentration of solutions (b) changing the pressure of gases (c) changing the surface area of solids (d) changing the temperature (e) adding or removing a catalyst, including enzymes State that a catalyst increases the rate of a reaction and is unchanged at the end of a reaction Describe practical methods for investigating the rate of a reaction including change in mass of a reactant or a product and the formation of a gas Interpret data, including graphs, from rate of reaction experiments Describe collision theory in terms of: (a) number of particles per unit volume (b) frequency of collisions between particles (c) kinetic energy of particles (d) activation energy, $E_{mathrm{a}}$ State that a catalyst decreases the activation energy, $E_a$, of a reaction Evaluate practical methods for investigating the rate of a reaction including change in mass of a reactant or a product and the formation of a gas State that some chemical reactions are reversible as shown by the symbol $ ightleftharpoons$ Describe how changing the conditions can change the direction of a reversible reaction for: (a) the effect of heat on hydrated compounds (b) the addition of water to anhydrous compounds limited to copper(II) sulfate and cobalt(II) chloride State that a reversible reaction in a closed system is at equilibrium when: (a) the rate of the forward reaction is equal to the rate of the reverse reaction (b) the concentrations of reactants and products are no longer changing Predict and explain, for a reversible reaction, how the position of equilibrium is affected by: (a) changing temperature (b) changing pressure (c) changing concentration (d) using a catalyst using information provided State the typical conditions in the Haber process as $450^{circ} mathrm{C}, 20000 mathrm{kPa} / 200 mathrm{~atm}$ and an iron catalyst State the symbol equation for the conversion of sulfur dioxide to sulfur trioxide in the Contact process, $2 mathrm{SO}_2(mathrm{~g})+mathrm{O}_2(mathrm{~g}) ightleftharpoons 2 mathrm{SO}_3(mathrm{~g})$ State the sources of the sulfur dioxide (burning sulfur or roasting sulfide ores) and oxygen (air) in the Contact process State the typical conditions for the conversion of sulfur dioxide to sulfur trioxide in the Contact process as $450^{circ} mathrm{C}, 200 mathrm{kPa} / 2 mathrm{~atm}$ and a vanadium(V) oxide catalyst Explain, in terms of rate of reaction and position of equilibrium, why the typical conditions stated are used in the Haber process and in the Contact process, including safety considerations and economics Use a Roman numeral to indicate the oxidation number of an element in a compound Define redox reactions as involving simultaneous oxidation and reduction Define oxidation as gain of oxygen and reduction as loss of oxygen Identify redox reactions as reactions involving gain and loss of oxygen Identify oxidation and reduction in redox reactions Define oxidation in terms of: (a) loss of electrons (b) an increase in oxidation number Define reduction in terms of: (a) gain of electrons (b) a decrease in oxidation number Identify redox reactions as reactions involving gain and loss of electrons Identify redox reactions by the colour changes involved when using acidified aqueous potassium manganate(VII) or aqueous potassium iodide Define an oxidising agent as a substance that oxidises another substance and is itself reduced Define a reducing agent as a substance that reduces another substance and is itself oxidised Identify oxidising agents and reducing agents in redox reactions Describe the characteristic properties of acids in terms of their reactions with: (a) metals (b) bases (c) carbonates Describe acids in terms of their effect on: (a) litmus (b) thymolphthalein (c) methyl orange State that bases are oxides or hydroxides of metals and that alkalis are soluble bases Describe the characteristic properties of bases in terms of their reactions with: (a) acids (b) ammonium salts Describe alkalis in terms of their effect on: (a) litmus (b) thymolphthalein (c) methyl orange State that aqueous solutions of acids contain $mathrm{H}^{+}$ ions and aqueous solutions of alkalis contain $mathrm{OH}^{-}$ ions Describe how to compare hydrogen ion concentration, neutrality, relative acidity and relative alkalinity in terms of colour and $mathrm{pH}$ using universal indicator paper Describe the neutralisation reaction between an acid and an alkali to produce water, $mathrm{H}^{+}(mathrm{aq})+mathrm{OH}^{-}(mathrm{aq}) ightarrow mathrm{H}_2 mathrm{O}(l)$ Classify oxides as acidic, including $mathrm{SO}_2$ and $mathrm{CO}_2$, or basic, including $mathrm{CuO}$ and $mathrm{CaO}$, related to metallic and non-metallic character Describe amphoteric oxides as oxides that react with acids and with bases to produce a salt and water Classify $mathrm{Al}_2 mathrm{O}_3$ and $mathrm{ZnO}$ as amphoteric oxides Describe the preparation, separation and purification of soluble salts by reaction of an acid with: (a) an alkali by titration (b) excess metal (c) excess insoluble base (d) excess insoluble carbonate Define a hydrated substance as a substance that is chemically combined with water and an anhydrous substance as a substance containing no water Describe the preparation of insoluble salts by precipitation Define the term water of crystallisation as the water molecules present in hydrated crystals, including $mathrm{CuSO}_4 cdot 5 mathrm{H}_2 mathrm{O}$ and $mathrm{CoCl}_2 cdot 6 mathrm{H}_2 mathrm{O}$ Describe the Periodic Table as an arrangement of elements in periods and groups and in order of increasing proton number / atomic number Describe the change from metallic to non-metallic character across a period Describe the relationship between group number and the charge of the ions formed from elements in that group Explain similarities in the chemical properties of elements in the same group of the Periodic Table in terms of their electronic configuration Explain how the position of an element in the Periodic Table can be used to predict its properties Identify trends in groups, given information about the elements Describe the Group I alkali metals, lithium, sodium and potassium, as relatively soft metals with general trends down the group, limited to: (a) decreasing melting point (b) increasing density (c) increasing reactivity Predict the properties of other elements in Group I, given information about the elements Describe the Group VII halogens, chlorine, bromine and iodine, as diatomic non-metals with general trends down the group, limited to: (a) increasing density (b) decreasing reactivity State the appearance of the halogens at r.t.p. as: (a) chlorine, a pale yellow-green gas (b) bromine, a red-brown liquid (c) iodine, a grey-black solid Describe and explain the displacement reactions of halogens with other halide ions Predict the properties of other elements in Group VII, given information about the elements Describe the transition elements as metals that: (a) have high density (b) have high melting points (c) form coloured compounds (d) often act as catalysts as elements and in compounds Describe transition elements as having ions with variable oxidation numbers, including iron(II) and iron(III) Describe the Group VIII noble gases as unreactive, monatomic gases and explain this in terms of electronic configuration Compare the general physical properties of metals and non-metals, including: (a) thermal conductivity (b) electrical conductivity (c) malleability and ductility (d) melting points and boiling points Describe the general chemical properties of metals, limited to their reactions with: (a) dilute acids (b) cold water and steam (c) oxygen Describe an alloy as a mixture of a metal with other elements, including: (a) brass as a mixture of copper and zinc (b) stainless steel as a mixture of iron and other elements such as chromium, nickel and carbon State that alloys can be harder and stronger than the pure metals and are more useful Describe the uses of alloys in terms of their physical properties, including stainless steel in cutlery because of its hardness and resistance to rusting Identify representations of alloys from diagrams of structure Explain in terms of structure how alloys can be harder and stronger than the pure metals because the different sized atoms in alloys mean the layers can no longer slide over each other State the order of the reactivity series as: potassium, sodium, calcium, magnesium, aluminium, carbon, zinc, iron, hydrogen, copper, silver, gold Deduce an order of reactivity from a given set of experimental results Describe the relative reactivities of metals in terms of their tendency to form positive ions, by displacement reactions, if any, with the aqueous ions of magnesium, zinc, iron, copper and silver Explain the apparent unreactivity of aluminium in terms of its oxide layer State the conditions required for the rusting of iron and steel to form hydrated iron(III) oxide State some common barrier methods, including painting, greasing and coating with plastic Describe how barrier methods prevent rusting by excluding oxygen or water Describe the use of zinc in galvanising as an example of a barrier method and sacrificial protection Explain sacrificial protection in terms of the reactivity series and in terms of electron loss Describe the ease in obtaining metals from their ores, related to the position of the metal in the reactivity series State that the main ore of aluminium is bauxite and that aluminium is extracted by electrolysis Describe the extraction of aluminium from purified bauxite/aluminium oxide, including: (a) the role of cryolite (b) why the carbon anodes need to be regularly replaced (c) the reactions at the electrodes, including ionic half-equations Describe chemical tests for the presence of water using anhydrous cobalt(II) chloride and anhydrous copper(II) sulfate Describe how to test for the purity of water using melting point and boiling point Explain that distilled water is used in practical chemistry rather than tap water because it contains fewer chemical impurities State that water from natural sources may contain substances, including: (a) dissolved oxygen (b) metal compounds (c) plastics (d) sewage (e) harmful microbes (f) nitrates from fertilisers (g) phosphates from fertilisers and detergents State that some of these substances are beneficial, including: (a) dissolved oxygen for aquatic life (b) some metal compounds provide essential minerals for life Describe the treatment of the domestic water supply in terms of: (a) sedimentation and filtration to remove solids (b) use of carbon to remove tastes and odours (c) chlorination to kill microbes State that ammonium salts and nitrates are used as fertilisers Describe the use of NPK fertilisers to provide the elements nitrogen, phosphorus and potassium for improved plant growth State the composition of clean, dry air as approximately $78 \%$ nitrogen, $mathrm{N}_2, 21 \%$ oxygen, $mathrm{O}_2$ and the remainder as a mixture of noble gases and carbon dioxide, $mathrm{CO}_2$ Describe photosynthesis as the reaction between carbon dioxide and water to produce glucose and oxygen in the presence of chlorophyll and using energy from light State the word equation for photosynthesis, carbon dioxide + water $ ightarrow$ glucose + oxygen Describe how the greenhouse gases carbon dioxide and methane cause global warming, limited to: (a) the absorption, reflection and emission of thermal energy (b) reducing thermal energy loss to space Describe the role of oxides of nitrogen in the formation of photochemical smog and their removal by catalytic converters, e.g. $2 mathrm{CO}+2 mathrm{NO} ightarrow 2 mathrm{CO}_2+mathrm{N}_2$ State the symbol equation for photosynthesis, $6 mathrm{CO}_2+6 mathrm{H}_2 mathrm{O} ightarrow mathrm{C}_6 mathrm{H}_{12} mathrm{O}_6+6 mathrm{O}_2$ Draw and interpret the displayed formula of a molecule to show all the atoms and all the bonds State that a homologous series is a family of similar compounds with similar chemical properties due to the presence of the same functional group State that a saturated compound has molecules in which all carbon-carbon bonds are single bonds State that an unsaturated compound has molecules in which one or more carbon-carbon bonds are not single bonds State that a structural formula is an unambiguous description of the way the atoms in a molecule are arranged, including $mathrm{CH}_2=mathrm{CH}_2$, $mathrm{CH}_3 mathrm{CH}_2 mathrm{OH}, mathrm{CH}_3 mathrm{COOCH}_3$ Name and draw the displayed formulae of: (a) methane and ethane (b) ethene (c) ethanol (d) ethanoic acid (e) the products of the reactions stated in sections 11.4-11.7 State the type of compound present, given a chemical name ending in -ane, -ene, -ol, or -oic acid or from a molecular formula or displayed formula Name and draw the displayed formulae of the unbranched esters which can be made from unbranched alcohols and carboxylic acids, each containing up to four carbon atoms Name the fossil fuels: coal, natural gas and petroleum Name methane as the main constituent of natural gas State that hydrocarbons are compounds that contain hydrogen and carbon only State that petroleum is a mixture of hydrocarbons Describe the separation of petroleum into useful fractions by fractional distillation Describe how the properties of fractions obtained from petroleum change from the bottom to the top of the fractionating column, limited to: (a) decreasing chain length (b) higher volatility (c) lower boiling points (d) lower viscosity State that the bonding in alkanes is single covalent and that alkanes are saturated hydrocarbons Describe the properties of alkanes as being generally unreactive, except in terms of combustion and substitution by chlorine State that in a substitution reaction one atom or group of atoms is replaced by another atom or group of atoms State that the bonding in alkenes includes a double carbon-carbon covalent bond and that alkenes are unsaturated hydrocarbons Describe the manufacture of alkenes and hydrogen by the cracking of larger alkane molecules using a high temperature and a catalyst Describe the reasons for the cracking of larger alkane molecules Describe the test to distinguish between saturated and unsaturated hydrocarbons by their reaction with aqueous bromine State that in an addition reaction only one product is formed Describe the combustion of ethanol State the uses of ethanol as: (a) a solvent (b) a fuel Describe the advantages and disadvantages of the manufacture of ethanol by: (a) fermentation (b) catalytic addition of steam to ethene Describe the reaction of ethanoic acid with: (a) metals (b) bases (c) carbonates including names and formulae of the salts produced Describe the formation of ethanoic acid by the oxidation of ethanol: (a) with acidified aqueous potassium manganate(VII) (b) by bacterial oxidation during vinegar production Describe the reaction of a carboxylic acid with an alcohol using an acid catalyst to form an ester Define polymers as large molecules built up from many smaller molecules called monomers Describe the formation of poly(ethene) as an example of addition polymerisation using ethene monomers State that plastics are made from polymers Describe how the properties of plastics have implications for their disposal Describe the environmental challenges caused by plastics, limited to: (a) disposal in land fill sites (b) accumulation in oceans (c) formation of toxic gases from burning Identify the repeat units and/or linkages in addition polymers and in condensation polymers Deduce the structure or repeat unit of an addition polymer from a given alkene and vice versa Deduce the structure or repeat unit of a condensation polymer from given monomers and vice versa, limited to: (a) polyamides from a dicarboxylic acid and a diamine (b) polyesters from a dicarboxylic acid and a diol Describe the differences between addition and condensation polymerisation Describe and draw the structure of: (a) nylon, a polyamide (b) PET, a polyester State that PET can be converted back into monomers and re-polymerised Describe proteins as natural polyamides and that they are formed from amino acid monomers with the general structure Describe and draw the structure of proteins as Name appropriate apparatus for the measurement of time, temperature, mass and volume, including: (a) stopwatches (b) thermometers (c) balances (d) burettes (e) volumetric pipettes (f) measuring cylinders (g) gas syringes Suggest advantages and disadvantages of experimental methods and apparatus Describe an acid-base titration to include the use of a: (a) burette (b) volumetric pipette (c) suitable indicator Describe how to identify the end-point of a titration using an indicator Describe how paper chromatography is used to separate mixtures of soluble coloured substances, using a suitable solvent Interpret simple chromatograms to identify: (a) unknown substances by comparison with known substances (b) pure and impure substances Describe how paper chromatography is used to separate mixtures of soluble colourless substances, using a suitable solvent and a locating agent State and use the equation for $R_{mathrm{f}}$ : $R_{mathrm{f}}=frac{ ext { distance travelled by substance }}{ ext { distance travelled by solvent }}$ Describe and explain methods of separation and purification using: (a) a suitable solvent (b) filtration (c) crystallisation (d) simple distillation (e) fractional distillation Suggest suitable separation and purification techniques, given information about the substances involved Identify substances and assess their purity using melting point and boiling point information Describe the use of a flame test to identify the cations: (a) lithium, $mathrm{Li}^{+}$ (b) sodium, $mathrm{Na}^{+}$ (c) potassium, $mathrm{K}^{+}$ (d) calcium, $mathrm{Ca}^{2+}$ (e) barium, $mathrm{Ba}^{2+}$ (f) copper(II), $mathrm{Cu}^{2+}$

State that ammonium salts and nitrates are used as fertilisers

Revision

Log in to practice.

50 views 0 suggestions

e-Consult

Secure online learning platform connecting students with expert tutors across Kenya.

Contact Us

Off Limuru Road, Parklands
Nairobi, Kenya
+254 708 495 677
info@e-consult.co.ke

Legal

Terms & Conditions
Privacy Policy
Cookie Policy

© 2026 e-Consult. All rights reserved. We are not affiliated with any examination body.