Ms. Tessy
Secondary Chemistry
Secondary Chemistry
Year 10 IGCSE Chemistry Topics for the Final Exam
Syllabus references and Standard/Learning Objectives Chapters Chapter 2- 2.3 to 2.5 Chapter 3 – 3.1- 3.5 Chapter 10 and 11 3.1 State the relative charges and approximate relative masses of protons, neutrons and electrons 3.1 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 3.1 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 3.1 Define isotopes as atoms of the same element which have the same proton number but a different nucleon number 3.1(S) Understand that isotopes have the same properties because they have the same number of electrons in their outer shell 3.1 State the two types of isotopes as being radioactive and non-radioactive 3.1 Describe the build-up of electrons in ‘shells’ and understand the significance of the noble gas electronic structures and of the outer shell electrons 3.1(S) Understand that isotopes have the same properties because they have the same number of electrons in their outer shell 3.2.1 Describe the differences between elements, mixtures and compounds, and between metals and non-metals 3.2.1 Describe an alloy, such as brass, as a mixture of a metal with other elements 10.1 Identify representations of alloys from diagrams of structure 3.2.2 Describe the formation of ions by electron loss or gain 3.2.2 Describe the formation of ionic bonds between elements from Groups I and VII 3.2.2(S) Describe the formation of ionic bonds between metallic and non-metallic elements 3.2.2(S) Describe the lattice structure of ionic compounds as a regular arrangement of alternating positive and negative ions 9.1 Describe the Periodic Table as a method of classifying elements and its use to predict properties of elements 9.2 Describe the change from metallic to non-metallic character across a period 9.2(S) Describe and explain the relationship between Group number, number of outer shell electrons and metallic/non-metallic character 4.1 Use the symbols of the elements and write the formulae of simple compounds 4.1 Deduce the formula of a simple compound from the relative numbers of atoms present 14.1 Name and draw the structures of methane, ethane, ethene, ethanol, ethanoic acid and the products of the reactions stated in syllabus references 14.4–14.6 14.1(S) Name and draw the structures of the unbranched alkanes, alkenes, alcohols and acids containing up to four carbon atoms per molecule 14.1 State the type of compound present, given a chemical name ending in -ane, -ene, -ol, or -oic acid, or a molecular structure 14.3 Describe the concept of homologous series as a ‘family’ of similar compounds with similar properties due to the presence of the same functional group 14.3(s) Describe the general characteristics of a homologous series 14.3(S) Recall that the compounds in a homologous series have the same general formula 14.3(S) Describe and identify structural isomerism 6.1 State the use of hydrogen as a fuel 14.2 Name the fuels coal, natural gas and petroleum 14.2 Name methane as the main constituent of natural gas 14.2 Describe petroleum as a mixture of hydrocarbons and its separation into useful fractions by fractional distillation 14.2 Describe the properties of molecules within a fraction 14.2 Name the uses of the fractions as:
14.4 Describe the properties of alkanes (exemplified by methane) as being generally unreactive, except in terms of burning 14.4(S) Describe substitution reactions of alkanes with chlorine 14.4 Describe the bonding in alkanes 14.5 Describe the manufacture of alkenes and of hydrogen by cracking 14.5(S) Describe the properties of alkenes in terms of addition reactions with bromine, hydrogen and steam 14.5 Distinguish between saturated and unsaturated hydrocarbons
14.5 Describe the formation of poly(ethene) as an example of addition polymerisation of monomer units 14.6 Describe the manufacture of ethanol by fermentation and by the catalytic addition of steam to ethane 14.6(s) Outline the advantages and disadvantages of these two methods of manufacturing ethanol 14.6 Describe the properties of ethanol in terms of burning 14.6 Name the uses of ethanol as a solvent and as a fuel 14.7(S) Describe the formation of ethanoic acid by the oxidation of ethanol by fermentation and with acidified potassium manganate(VII 14.7 Describe the properties of aqueous ethanoic acid 14.7(S) Describe ethanoic acid as a typical weak acid 14.7(S) Describe the reaction of a carboxylic acid with an alcohol in the presence of a catalyst to give an ester 14.1(S) 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 Comments are closed.
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Ms TessyYear 7-9 Global Studies Archives
May 2017
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