Grade 10 CIE Chemistry 0620 Objectives

• State the distinguishing properties of solids, liquids and gases
  
• Describe the structure of solids, liquids and gases in terms of particle separation, arrangement and types of motion
  
• Describe changes of state in terms of melting, boiling, evaporation, freezing, condensation and sublimation
  
• Describe qualitatively the pressure and temperature of a gas in terms of the motion of its particles
  
• Show an understanding of the random motion of particles in a suspension (sometimes known as Brownian motion) as evidence for the kinetic particle (atoms, molecules or ions) model of matter
  
• Describe and explain diffusion
  

• Explain changes of state in terms of the kinetic theory
  
• Describe and explain Brownian motion in terms of random molecular bombardment
  
• State evidence for Brownian motion
  
• Describe and explain dependence of rate of diffusion on molecular mass
  

• Name appropriate apparatus for the measurement of time, temperature, mass and volume, including burettes, pipettes and measuring cylinders
  

• State the relative charges and approximate relative masses of protons, neutrons and electrons
  
• Define proton number (atomic number) as the number of protons in the nucleus of an atom
  
• Define nucleon number (mass number) as the total number of protons and neutrons in the nucleus of an atom
  
• Use proton number and the simple structure of atoms to explain the basis of the Periodic Table (see section 9), with special reference to the elements of proton number 1 to 20
  
• Define isotopes as atoms of the same element which have the same proton number but a different nucleon number
  
• State the two types of isotopes as being radioactive and non-radioactive
  
• State one medical and one industrial use of radioactive isotopes
  
• Describe the build-up of electrons in ‘shells’ and understand the significance of the noble gas electronic structures and of the outer shell electrons. (The ideas of the distribution of electrons in s and p orbitals and in d block elements are not required.)
  

NOTE: a copy of the Periodic Table, as shown in the Appendix, will be available in Papers 1, 2, 3 and 4.

• Understand that isotopes have the same properties because they have the same number of electrons in their outer shell
  

• Use the symbols of the elements and write the formulae of simple compounds
  
• Deduce the formula of a simple compound from the relative numbers of atoms present
  
• Deduce the formula of a simple compound from a model or a diagrammatic representation
  
• Construct word equations and simple balanced chemical equations
  
• Define relative atomic mass, Ar, as the average mass of naturally occurring atoms of an element on a scale where the 12C atom has a mass of exactly 12 units
  
• Define relative molecular mass, Mr, as the sum of the relative atomic masses. (Relative formula mass or Mr will be used for ionic compounds.)
  

NOTE: Calculations involving reacting masses in simple proportions may be set. Calculations will not involve the mole concept.

• Determine the formula of an ionic compound from the charges on the ions present
  
• Construct equations with state symbols, including ionic equations
  
• Deduce the balanced equation for a chemical reaction, given relevant information
  

• Define the mole and the Avogadro constant
  
• Use the molar gas volume, taken as 24 dm3 at room temperature and pressure
  
• Calculate stoichiometric reacting masses, volumes of gases and solutions, and concentrations of solutions expressed in g / dm3 and mol / dm3. (Calculations involving the idea of limiting reactants may be set. Questions on the gas laws and the conversion of gaseous volumes to different temperatures and pressures will not be set.)
  
• Calculate empirical formulae and molecular formulae
  
• Calculate percentage yield and percentage purity
  

• Define electrolysis as the breakdown of an ionic compound, molten or in aqueous solution, by the passage of electricity
  
• Describe the electrode products and the observations made during the electrolysis of:
  
  • molten lead(II) bromide
    
  • concentrated hydrochloric acid
    
  • concentrated aqueous sodium chloride
    
  • dilute sulfuric acid
    
• between inert electrodes (platinum or carbon) State the general principle that metals or hydrogen are formed at the negative electrode (cathode), and that non-metals (other than hydrogen) are formed at the positive electrode ( anode )
  
• Predict the products of the electrolysis of a specified binary compound in the molten state
  
• Describe the electroplating of metals
  
• Outline the uses of electroplating
  
• Describe the reasons for the use of copper and (steel-cored) aluminium in cables, and why plastics and ceramics are used as insulators
  

• Relate the products of electrolysis to the electrolyte and electrodes used, exemplified by the specific examples in the Core together with aqueous copper(II) sulfate using carbon electrodes and using copper electrodes (as used in the refining of copper)
  
• Describe electrolysis in terms of the ions present and reactions at the electrodes in the examples given
  
• Predict the products of electrolysis of a specified halide in dilute or concentrated aqueous solution Construct ionic half-equations for reactions at the cathode
  
• Describe the transfer of charge during electrolysis to include:
  
  • the movement of electrons in the metallic conductor
    
  • the removal or addition of electrons from the external circuit at the electrodes
    
  • the movement of ions in the electrolyte
    
• Describe the production of electrical energy from simple cells, i.e. two electrodes in an electrolyte. (This should be linked with the reactivity series in section 10.2 and redox in section 7.4.)
  
• Describe, in outline, the manufacture of:
  
  • aluminium from pure aluminium oxide in molten cryolite (refer to section 10.3)
    
  • chlorine, hydrogen and sodium hydroxide from concentrated aqueous sodium chloride
    

NOTE: Starting materials and essential conditions should be given but not technical details or diagrams.

• Describe the meaning of exothermic and endothermic reactions
  
• Interpret energy level diagrams showing exothermic and endothermic reactions
  

• Describe bond breaking as an endothermic process and bond forming as an exothermic process
  
• Draw and label energy level diagrams for exothermic and endothermic reactions using data provided
  
• Calculate the energy of a reaction using bond energies
  

• Describe the release of heat energy by burning fuels
  
• State the use of hydrogen as a fuel
  
• Describe radioactive isotopes, such as 235U, as a source of energy
  

• Describe the use of hydrogen as a fuel reacting with oxygen to generate electricity in a fuel cell. (Details of the construction and operation of a fuel cell are not required.)
  

• Identify physical and chemical changes, and understand the differences between them
  

• Describe and explain the effect of concentration, particle size, catalysts (including enzymes) and temperature on the rate of reactions
  
• Describe the application of the above factors to the danger of explosive combustion with fine powders (e.g. flour mills) and gases (e.g. methane in mines)
  
• Demonstrate knowledge and understanding of a practical method for investigating the rate of a reaction involving gas evolution
  
• Interpret data obtained from experiments concerned with rate of reaction
  

NOTE: Candidates should be encouraged to use the term rate rather than speed.

• Devise and evaluate a suitable method for investigating the effect of a given variable on the rate of a reaction
  
• Describe and explain the effects of temperature and concentration in terms of collisions between reacting particles. (An increase in temperature causes an increase in collision rate and more of the colliding molecules have sufficient energy (activation energy) to react whereas an increase in concentration only causes an increase in collision rate.)
  
• Describe and explain the role of light in photochemical reactions and the effect of light on the rate of these reactions. (This should be linked to section 14.4.)
  
• Describe the use of silver salts in photography as a process of reduction of silver ions to silver; and photosynthesis as the reaction between carbon dioxide and water in the presence of chlorophyll and sunlight (energy) to produce glucose and oxygen
  

• Understand that some chemical reactions can be reversed by changing the reaction conditions. (Limited to the effects of heat and water on hydrated and anhydrous copper(II) sulfate and cobalt(II) chloride.) (Concept of equilibrium is not required.)
  

• Predict the effect of changing the conditions (concentration, temperature and pressure) on other reversible reactions
  
• Demonstrate knowledge and understanding of the concept of equilibrium
  

• Define oxidation and reduction in terms of oxygen loss/gain. (Oxidation state limited to its use to name ions, e.g. iron(II), iron(III), copper(II), manganate(VII).)
  

• Define redox in terms of electron transfer
  
• Identify redox reactions by changes in oxidation state and by the colour changes involved when using acidified potassium manganate(VII), and potassium iodide. (Recall of equations involving KMnO4 is not required.)
  
• Define oxidising agent as a substance which oxidises another substance during a redox reaction. Define reducing agent as a substance which reduces another substance during a redox reaction.
  
• Identify oxidising agents and reducing agents from simple equations
  

• Describe the characteristic properties of acids as reactions with metals, bases, carbonates and effect on litmus and methyl orange
  
• Describe the characteristic properties of bases as reactions with acids and with ammonium salts and effect on litmus and methyl orange
  
• Describe neutrality and relative acidity and alkalinity in terms of pH measured using universal indicator paper (whole numbers only)
  
• Describe and explain the importance of controlling acidity in soil
  

• Define acids and bases in terms of proton transfer, limited to aqueous solutions
  
• Describe the meaning of weak and strong acids and bases
  

• Classify oxides as either acidic or basic, related to metallic and non-metallic character
  

• Further classify other oxides as neutral or amphoteric
  

• Demonstrate knowledge and understanding of preparation, separation and purification of salts as examples of some of the techniques specified in section 2.2.2 and the reactions specified in section 8.1
  

• Demonstrate knowledge and understanding of the preparation of insoluble salts by precipitation
  
• Suggest a method of making a given salt from a suitable starting material, given appropriate information
  

Describe the following tests to identify:

• aqueous cations:
  

  • aluminium
    
  • ammonium
    
  • calcium
    
  • chromium(III)
    
  • copper(II)
    
  • iron(II)
    
  • iron(III)
    
  • zinc (using aqueous sodium hydroxide and aqueous ammonia as appropriate).
    

  NOTE: Formulae of complex ions are not required.
  

• cations: use of the flame test to identify:
  
  • lithium
    
  • sodium
    
  • potassium
    
  • copper(II)
    
• anions:
  
  • carbonate (by reaction with dilute acid and then limewater)
    
  • chloride, bromide and iodide (by reaction under acidic conditions with aqueous silver nitrate)
    
  • nitrate (by reduction with aluminium)
    
  • sulfate (by reaction under acidic conditions with aqueous barium ions)
    
  • sulfite (by reaction with dilute acids and then aqueous potassium manganate(VII))
    
• gases:
  
  • ammonia (using damp red litmus paper)
    
  • carbon dioxide (using limewater)
    
  • chlorine (using damp litmus paper)
    
  • hydrogen (using lighted splint)
    
  • oxygen (using a glowing splint)
    
  • sulfur dioxide (using aqueous potassium manganate(VII))
    

• Describe the Periodic Table as a method of classifying elements and its use to predict properties of elements
  

• Describe the change from metallic to nonmetallic character across a period
  

• Describe and explain the relationship between Group number, number of outer shell electrons and metallic/non-metallic character
  

• Describe lithium, sodium and potassium in Group I as a collection of relatively soft metals showing a trend in melting point, density and reaction with water
  
• Predict the properties of other elements in Group I, given data, where appropriate
  
• Describe the halogens, chlorine, bromine and iodine in Group VII, as a collection of diatomic non-metals showing a trend in colour and density and state their reaction with other halide ions
  
• Predict the properties of other elements in Group VII, given data where appropriate
  

• Identify trends in Groups, given information about the elements concerned
  

• Describe the transition elements as a collection of metals having high densities, high melting points and forming coloured compounds, and which, as elements and compounds, often act as catalysts
  

• Know that transition elements have variable oxidation states
  

• Describe the noble gases, in Group VIII or 0, as being unreactive, monoatomic gases and explain this in terms of electronic structure
  
• State the uses of the noble gases in providing an inert atmosphere, i.e. argon in lamps, helium for filling balloons
  

• List the general physical properties of metals
  
• Describe the general chemical properties of metals, e.g. reaction with dilute acids and reaction with oxygen
  
• Explain in terms of their properties why alloys are used instead of pure metals
  
• Identify representations of alloys from diagrams of structure
  

• Place in order of reactivity: potassium, sodium, calcium, magnesium, zinc, iron, (hydrogen) and copper, by reference to the reactions, if any, of the metals with:
  
  • water or steam
    
  • dilute hydrochloric acid and the reduction of their oxides with carbon
    
• Deduce an order of reactivity from a given set of experimental results
  

• Describe the reactivity series as related to the tendency of a metal to form its positive ion, illustrated by its reaction, if any, with:
  
  • the aqueous ions
    
  • the oxides of the other listed metals
    
• Describe and explain the action of heat on the hydroxides, carbonates and nitrates of the listed metals
  
• Account for the apparent unreactivity of aluminium in terms of the oxide layer which adheres to the metal
  

• Describe the ease in obtaining metals from their ores by relating the elements to the reactivity series
  
• Describe and state the essential reactions in the extraction of iron from hematite
  
• Describe the conversion of iron into steel using basic oxides and oxygen
  
• Know that aluminium is extracted from the ore bauxite by electrolysis
  
• Discuss the advantages and disadvantages of recycling metals, limited to iron/steel and aluminium
  

• Describe in outline, the extraction of zinc from zinc blende
  
• Describe in outline, the extraction of aluminium from bauxite including the role of cryolite and the reactions at the electrodes
  

• Name the uses of aluminium:
  
  • in the manufacture of aircraft because of its strength and low density
    
  • in food containers because of its resistance to corrosion
    
• Name the uses of copper related to its properties ( electrical wiring and in cooking utensils )
  
• Name the uses of mild steel (car bodies and machinery) and stainless steel (chemical plant and cutlery)
  

• Explain the uses of zinc for galvanising and for making brass
  
• Describe the idea of changing the properties of iron by the controlled use of additives to form steel alloys
  

• Describe chemical tests for water using cobalt(II) chloride and copper(II) sulfate
  
• Describe, in outline, the treatment of the water supply in terms of filtration and chlorination
  
• Name some of the uses of water in industry and in the home
  

• Discuss the implications of an inadequate supply of water, limited to safe water for drinking and water for irrigating crops
  

• State the composition of clean, dry air as being approximately 78% nitrogen, 21% oxygen and the remainder as being a mixture of noble gases and carbon dioxide
  
• Name the common pollutants in the air as being carbon monoxide, sulfur dioxide, oxides of nitrogen and lead compounds
  
• State the source of each of these pollutants:
  
  • carbon monoxide from the incomplete combustion of carbon-containing substances
    
  • sulfur dioxide from the combustion of fossil fuels which contain sulfur compounds ( leading to ‘acid rain’ )
    
  • oxides of nitrogen from car engines
    
  • lead compounds from leaded petrol
    
• State the adverse effect of these common pollutants on buildings and on health and discuss why these pollutants are of global concern
  
• State the conditions required for the rusting of iron
  
• Describe and explain methods of rust prevention, specifically paint and other coatings to exclude oxygen
  

• Describe the separation of oxygen and nitrogen from liquid air by fractional distillation
  
• Describe and explain the presence of oxides of nitrogen in car engines and their catalytic removal
  
• Describe and explain sacrificial protection in terms of the reactivity series of metals and galvanising as a method of rust prevention
  

• Describe the need for nitrogen-, phosphorus- and potassium-containing fertilisers
  
• Describe the displacement of ammonia from its salts
  

• Describe and explain the essential conditions for the manufacture of ammonia by the Haber process including the sources of the hydrogen and nitrogen, i.e. hydrocarbons or steam and air
  

• State that carbon dioxide and methane are greenhouse gases and explain how they may contribute to climate change
  
• State the formation of carbon dioxide:
  
  • as a product of complete combustion of carbon-containing substances
    
  • as a product of respiration
    
  • as a product of the reaction between an acid and a carbonate
    
  • from the thermal decomposition of a carbonate
    
• State the sources of methane, including decomposition of vegetation and waste gases from digestion in animals
  

• Describe the carbon cycle, in simple terms, to include the processes of combustion, respiration and photosynthesis
  

• Name some sources of sulfur
  
• Name the use of sulfur in the manufacture of sulfuric acid
  
• State the uses of sulfur dioxide as a bleach in the manufacture of wood pulp for paper and as a food preservative (by killing bacteria)
  

• Describe the manufacture of sulfuric acid by the Contact process, including essential conditions and reactions
  
• Describe the properties and uses of dilute and concentrated sulfuric acid
  

• Describe the manufacture of lime (calcium oxide) from calcium carbonate ( limestone) in terms of thermal decomposition
  
• Name some uses of lime and slaked lime such as in treating acidic soil and neutralising acidic industrial waste products, e.g. flue gas desulfurisation
  
• Name the uses of calcium carbonate in the manufacture of iron and cement
  

• Name and draw the structures of methane, ethane, ethene, ethanol, ethanoic acid and the products of the reactions stated in sections 14.4–14.6
  
• State the type of compound present, given a chemical name ending in -ane, -ene, -ol, or -oic acid or a molecular structure
  

• Name and draw the structures of the unbranched alkanes, alkenes (not cis-trans), alcohols and acids containing up to four carbon atoms per molecule
  
• Name and draw the structural formulae of the esters which can be made from unbranched alcohols and carboxylic acids, each containing up to four carbon atoms
  

• Name the fuels: coal, natural gas and petroleum
  
• Name methane as the main constituent of natural gas
  
• Describe petroleum as a mixture of hydrocarbons and its separation into useful fractions by fractional distillation
  
• Describe the properties of molecules within a fraction
  
• Name the uses of the fractions as:
  
  • refinery gas for bottled gas for heating and cooking
    
  • gasoline fraction for fuel (petrol) in cars
    
  • naphtha fraction for making chemicals
    
  • kerosene/paraffin fraction for jet fuel
    
  • diesel oil/gas oil for fuel in diesel engines
    
  • fuel oil fraction for fuel for ships and home heating systems
    
  • lubricating fraction for lubricants, waxes and polishes
    
  • bitumen for making roads
    

• Describe the concept of homologous series as a ‘family’ of similar compounds with similar chemical properties due to the presence of the same functional group
  

• Describe the general characteristics of a homologous series
  
• Recall that the compounds in a homologous series have the same general formula
  
• Describe and identify structural isomerism
  

• Describe the properties of alkanes (exemplified by methane) as being generally unreactive, except in terms of burning
  
• Describe the bonding in alkanes
  

• Describe substitution reactions of alkanes with chlorine
  

• Describe the manufacture of alkenes and of hydrogen by cracking
  
• Distinguish between saturated and unsaturated hydrocarbons:
  
  • from molecular structures
    
  • by reaction with aqueous bromine
    
• Describe the formation of poly(ethene) as an example of addition polymerisation of monomer units
  

• Describe the properties of alkenes in terms of addition reactions with bromine, hydrogen and steam
  

• Describe the manufacture of ethanol by fermentation and by the catalytic addition of steam to ethene
  
• Describe the properties of ethanol in terms of burning
  
• Name the uses of ethanol as a solvent and as a fuel
  

• Outline the advantages and disadvantages of these two methods of manufacturing ethanol
  

• Describe the properties of aqueous ethanoic acid
  

• Describe the formation of ethanoic acid by the oxidation of ethanol by fermentation and with acidified potassium manganate(VII)
  
• Describe ethanoic acid as a typical weak acid
  
• Describe the reaction of a carboxylic acid with an alcohol in the presence of a catalyst to give an ester