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 Dear Year 8 students,
I am posting the list of topics that will be covered in the final exam. A hard copy of the same was given to all of you last week. There is a slight change in the last topic- instead of area of parallelogram and trapezium, you will have volume of cuboid and surface area. The exam will be on 11th June. Topics for Final Exam- Year 8 Math Marks 50 Adding and subtracting numbers- Exercise 1A HCF and LCM – Exercise 1J Constructing triangles- Exercise 3B Bisecting angles- Exercise 3D Multiplying decimals- Exercise 5D Mean, median, mode and range- Exercise 6G Adding and subtracting fractions- Exercise 7A Solving linear equations- Exercise 8B All about angles- Exercise 9B Transformations-reflection- Exercise 15 A Rotation- Exercise 15 B Areas of triangles and rectangles- Exercise 17E Volumes of cuboids and surface area- Exercise 17 M and 17N Topics for the Week
Year 12 Chemistry Revision Hands on practical test- Monday, 15th May Year 11 Chemistry Revision IGCSE Chemistry Theory exam on 16th May Year 10 Chemistry Organic chemistry- Structural formulae of alkenes, general formula Chemical properties of alkenes Functional groups and Homologous series Year 8 Math Calculating Angles and angles in different shapes- Chapter 9 Unit Test- Sunday, 14th May Topics- Chapter 3 and 4 Topics for the week
Year 12 Chemistry Revision Year 11 Chemistry Revision Year 10 Chemistry Transition metals Thermal stability of compounds of group 1 and 2 metals Recycling of metals Year 8 Math Drawing nets and making 3D shapes Quadrilaterals Units of measurement and their inter-conversions (chapter 4) Topics for the Week
Year 12 Chemistry Revision Hands on Practical Year 11 Chemistry Revision Year 10 Chemistry Comparing reactivity of metals- Displacement reactions Thermite reaction Un-reactivity of aluminium Uses of aluminium Year 8 Math Geometry- Chapter 3 Constructing circles, triangles, right triangles and bisectors. Quiz on Wednesday- Topics- Probability- Chapter 18 (Experimental probability, theoretical probability, listing the outcomes and then finding the probability) Topics for the Week
Year 12 Chemistry Revision Revising Unit 2 and answering previous year’s question papers Year 11 Chemistry Revision Year 10 Chemistry Metals – Chemical properties Importance of alloys Year 8 Math Probability Experimental and Theoretical probability- (Chapter 18 in the course book) Dear year 10 students,
I am posting the syllabus standards and main points of the unit Reaction Test. This will help you prepare well for the coming test. Year 10 IGCSE Chemistry Unit- Reaction rate Standards and Topics for the Unit Test 7.2 Describe and explain the effect of concentration, particle size, catalysts (including enzymes) and temperature on the rate of reactions. Demonstrate knowledge and understanding of a practical method for investigating the rate of a reaction involving gas evolution Learners should use the term rate rather than speed. 7.2(S) Devise and evaluate a suitable method for investigating the effect of a given variable on the rate of a reaction 7.2 Interpret data obtained from experiments concerned with rate of reaction 7.2(S) 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.) 7.2 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 6.1 Interpret energy level diagrams showing exothermic and endothermic reactions 6.1(S) Draw and label energy level diagrams for exothermic and endothermic reactions using data provided Describe bond breaking as an endothermic process and bond forming as an exothermic Calculate the energy of a reaction using bond energies 7.2(S) Describe and explain the role of light in photochemical reactions and the effect of light on the rate of these reactions Topics for the week
Year 12 Chemistry Revising the units and answering past paper questions Unit Test on 27th Monday – Organic Chemistry Year 11 Chemistry Revision Year 10 Chemistry Metals and Reactivity Series- Physical and Chemical properties of Metals Metallic bonding Unit Test- Wednesday,29thMarch- Unit- Reaction rate Year 8 Math Real life graphs- Chapter 11 Reading, Interpreting and drawing real life graphs Unit Test- Monday, 27th March- Topics- Chapter 6 and Chapter 12(in the course book) Topics for the Week
Year 12 Chemistry Carbonyl compounds- Preparation and Properties Year 11 Chemistry Revision Revision Test on Tuesday- Topics- Experimental Techniques, Air and Water and Covalent Bonding Year 10 Chemistry Reaction rate- Energy level diagrams Calculating energy of reactions Year 8 Math Histograms Stem and Leaf Diagrams Comparing and Interpreting data diagrams |
Ms TessyYear 7-9 Global Studies Archives
May 2017
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