Principles of Chemistry 2. Edexcel GCSE; Edexcel IGCSE; Edexcel A Level; AQA GCSE; AQA A Level; Edexcel IGCSE Chemistry Past Papers; Edexcel IGCSE Science (Double Award) Past Papers; IGCSE Physics Past Papers: June 2018. Match. January-2013-MA-M1-Edexcel Find all available grade boundaries. Also, it is much better to spend 1 hour per day for 5 days, compared to doing 5 hours on 1 day. Test. The sooner you start testing yourself, the sooner youll start putting the facts and concepts into your long-term memory. This could be a. Liquid - Particles are in contact but they are free to move January 2012 QP C1 Edexcel You should feel squirmy. January-2016-(IAL) MA-M1-Edexcel This is absolutely the key point. November-2003 MS-M1-Edexcel January 2010 MS C1 Edexcel The quantity amount of substance is a measure of how many elementary entities of a given substance are in an object or sample. Questions from P1-P3 MS January 2014 (IAL) MS C2 Edexcel Step 2. tutorMyself Chemistry is all you need to get to grips with the latest Edexcel iGCSE Chemistry Specification (2017). All rights reserved. Exam Papers: Mark Schemes: Model Answers: New Spec: Jun 19 Paper 1F (QP) Jun 19 Paper 1F (MS) Jun 19 Paper 1FR (QP) Jun 19 Paper 1FR (MS) GCSE Revision Notes IGCSE Revision Notes A Level Revision Notes Biology Chemistry Physics Maths 2022 Advance Information January 2021 4CH1/1C June 2020 4CH1/1C January 2020 4CH1/1C June 2019 4CH1/1C. Download Matriculation & Intermediate (Class 9th, 10th, 11th & 12th) all subjects updated guess papers in PDF. Match. Cambridge IGCSE Chemistry 3rd Edition PDF, A Level Chemistry Revision Guide PDF (Cambridge), Cambridge A Level Biology Revision Guide PDF, A Level Physics Revision Guide PDF Free Download, Cambridge International AS and A Level Accounting by Ian Harrison, Cambridge International AS/A level Accounting Revision Guide PDF, Cambridge International AS and A Level Biology Coursebook. June 2016 MA C2 Edexcel June-2005 MS-M1-Edexcel June-2004 MS-M1-Edexcel There are so many ways of doing this, but all of the best ways include these steps: Keep practising by testing yourself, but make sure you are mixing up and spacing out your practice. The AQA A level Biology specification is a challenging course with a wide range of content, data analysis and mathematical skills now a core part of the course. Multiple Choice Progress tracking Questions & model answers made by experienced teachers GET STARTED Theory Topic questions & Mark schemes GET STARTED Theory Topic questions & June 2013 (R) MS C1 Edexcel June-2014 MS-M1-Edexcel The qualification supports progression to further study, with up-to-date content reflecting the latest thinking in the subject. Edexcel IGCSE Chemistry Revision Guide Cliff Curtis Pearson 978-0-435046-72-910,90 IGCSE Chemistry Booklet Chemistry Department 11,00 Reprinting December [Filename: Year 4 - English School Book Lists 2012-13(1).pdf] - Read File Online - Report Abuse. June-2012 MA-M1-Edexcel January 2012 MS C2 Edexcel June 2015 MA C2 Edexcel June 2008 MS C1 Edexcel It totally replaced the 2009 specification in June this year, the 2009 is no longer being assessed. Edexcel Igcse Chemistry Student Book written by Jim Clark and has been published by Heinemann International Incorporated this book supported file pdf, txt, epub, kindle and other format this book has been release on 2009-06-01 with Chemistry categories. June-2008 QP-M1-Edexcel January 2005 MS C2 Edexcel When you have worked out why you didnt get the best possible answer, make a note of this. Edexcel IGCSE Chemistry: Past Papers Home / IGCSE / Chemistry / Edexcel / Past Papers Concise resources for the IGCSE Edexcel Chemistry: course. June 2009 MS C1 Edexcel June-2016 (IAL) MA-M1-Edexcel January 2010 QP C1 Edexcel It contains notes and questions for the Chemistry syllabus topics and many questions for you to revise for your IGCSE exams If your memory of the material is sketchy, it doesnt matter. If you find yourself doing any of these, then you are not spending your time in the most efficient way, and your time is the most important thing in the world. January 2011 MS C2 Edexcel Hodder Education June 2014 (R) MS C2 Edexcel Specimen (IAL) QP-M1-Edexcel June-2016 MA-M1-Edexcel January-2001-QP-M1-Edexcel The exam board are quite good at putting most of the spec in each exam paper, so to do well youve got to make sure you really know everything in the spec. June-2013 QP-M1-Edexcel June 2010 MS C2 Edexcel June-2016 (IAL) MS-M1-Edexcel January 2012 MS C1 Edexcel Find Edexcel IGCSE Biology Past Papers and Mark Scheme Download Past exam papers for Edexcel Biology IGCSE. June 2005 QP C2 Edexcel You may search online for other sources for past exam papers if you cant find what you want here. January-2002-MA-M1-Edexcel Edexcel IGCSE Chemistry Paper 1. Another easy way of testing yourself is to play a little game called spec point roulette. All candidates will study the following topics: KINETIC THEORY AND DIFFUSION. The term intermolecular forces of attraction can be used to represent all forces between molecules, 1:48 explain why the melting and boiling points of substances with simple molecular structures increase, in general, with increasing relative molecular mass, 1:49 explain why substances with giant covalent structures are solids with high melting and boiling points, 1:50 explain how the structures of diamond, graphite and C, 1:51 know that covalent compounds do not usually conduct electricity, 1:52 (Triple only) know how to represent a metallic lattice by a 2-D diagram, 1:53 (Triple only) understand metallic bonding in terms of electrostatic attractions, 1:54 (Triple only) explain typical physical properties of metals, including electrical conductivity and malleability, 1:55 (Triple only) understand why covalent compounds do not conduct electricity, 1:56 (Triple only) understand why ionic compounds conduct electricity only when molten or in aqueous solution, 1:57 (Triple only) know that anion and cation are terms used to refer to negative and positive ions respectively, 1:58 (Triple only) describe experiments to investigate electrolysis, using inert electrodes, of molten compounds (including lead(II) bromide) and aqueous solutions (including sodium chloride, dilute sulfuric acid and copper(II) sulfate) and to predict the products, 1:59 (Triple only) write ionic half-equations representing the reactions at the electrodes during electrolysis and understand why these reactions are classified as oxidation or reduction, 1:60 (Triple only) practical: investigate the electrolysis of aqueous solutions, (a) Group 1 (alkali metals) lithium, sodium and potassium, 2:01 understand how the similarities in the reactions of lithium, sodium and potassium with water provide evidence for their recognition as a family of elements, 2:02 understand how the differences between the reactions of lithium, sodium and potassium with air and water provide evidence for the trend in reactivity in Group 1, 2:03 use knowledge of trends in Group 1 to predict the properties of other alkali metals, 2:04 (Triple only) explain the trend in reactivity in Group 1 in terms of electronic configurations, (b) Group 7 (halogens) chlorine, bromine and iodine, 2:05 know the colours, physical states (at room temperature) and trends in physical properties of chlorine, bromine and iodine, 2:06 use knowledge of trends in Group 7 to predict the properties of other halogens, 2:07 understand how displacement reactions involving halogens and halides provide evidence for the trend in reactivity in Group 7, 2:08 (Triple only) explain the trend in reactivity in Group 7 in terms of electronic configurations, 2:09 know the approximate percentages by volume of the four most abundant gases in dry air, 2:10 understand how to determine the percentage by volume of oxygen in air using experiments involving the reactions of metals (e.g. June-2009 QP-M1-Edexcel June-2015 MS-M1-Edexcel June 2006 QP C1 Edexcel June 2006 MS C2 Edexcel June 2014 (R) MS C1 Edexcel Was there a calculation method you need to practice more? Vast collection of Textbooks, Helping Books, Notes, Date Sheets, Pairing Schemes, Entry Test and other exams materials. We have worked hard to compile every Edexcel IGCSE Biology past paper by topic and exam board! January-2012-MA-M1-Edexcel Company Number. magnesium, zinc and iron), 2:22 (Triple only) know that most metals are extracted from ores found in the Earths crust and that unreactive metals are often found as the uncombined element, 2:23 (Triple only) explain how the method of extraction of a metal is related to its position in the reactivity series, illustrated by carbon extraction for iron and electrolysis for aluminium, 2:24 (Triple only) be able to comment on a metal extraction process, given appropriate information, 2:25 (Triple only) explain the uses of aluminium, copper, iron and steel in terms of their properties the types of steel will be limited to low-carbon (mild), high-carbon and stainless, 2:26 (Triple only) know that an alloy is a mixture of a metal and one or more elements, usually other metals or carbon, 2:27 (Triple only) explain why alloys are harder than pure metals, 2:28 describe the use of litmus, phenolphthalein and methyl orange to distinguish between acidic and alkaline solutions, 2:29 understand how to use the pH scale, from 014, can be used to classify solutions as strongly acidic (03), weakly acidic (46), neutral (7), weakly alkaline (810) and strongly alkaline (1114), 2:30 describe the use of Universal Indicator to measure the approximate pH value of an aqueous solution, 2:31 know that acids in aqueous solution are a source of hydrogen ions and alkalis in a aqueous solution are a source of hydroxide ions, 2:32 know that bases can neutralise acids, 2:33 (Triple only) describe how to carry out an acid-alkali titration, 2:34 know the general rules for predicting the solubility of ionic compounds in water: common sodium, potassium and ammonium compounds are soluble, all nitrates are soluble, common chlorides are soluble, except those of silver and lead(II), common sulfates are soluble, except for those of barium, calcium and lead(II), common carbonates are insoluble, except for those of sodium, potassium and ammonium, common hydroxides are insoluble except for those of sodium, potassium and calcium (calcium hydroxide is slightly soluble), 2:35 understand acids and bases in terms of proton transfer, 2:36 understand that an acid is a proton donor and a base is a proton acceptor, 2:37 describe the reactions of hydrochloric acid, sulfuric acid and nitric acid with metals, bases and metal carbonates (excluding the reactions between nitric acid and metals) to form salts, 2:38 know that metal oxides, metal hydroxides and ammonia can act as bases, and that alkalis are bases that are soluble in water, 2:39 describe an experiment to prepare a pure, dry sample of a soluble salt, starting from an insoluble reactant, 2:40 (Triple only) describe an experiment to prepare a pure, dry sample of a soluble salt, starting from an acid and alkali, 2:41 (Triple only) describe an experiment to prepare a pure, dry sample of an insoluble salt, starting from two soluble reactants, 2:42 practical: prepare a sample of pure, dry hydrated copper(II) sulfate crystals starting from copper(II) oxide, 2:43 (Triple only) practical: prepare a sample of pure, dry lead(II) sulfate, 2:44a describe tests for these gases: hydrogen, carbon dioxide, 2:44 describe tests for these gases: hydrogen, oxygen, carbon dioxide, ammonia, chlorine, 2:45 describe how to carry out a flame test, 2:46 know the colours formed in flame tests for these cations: Li is red, Na is yellow, K is lilac, Ca is orange-red, Cu is blue-green, 2:47 describe tests for these cations: NH using sodium hydroxide solution and identifying the gas evolved, Cu, Fe and Fe using sodium hydroxide solution, 2:48 describe tests for these anions: Cl, Br and I using acidified silver nitrate solution, SO using acidified barium chloride solution, CO using hydrochloric acid and identifying the gas evolved, 2:49 describe a test for the presence of water using anhydrous copper(II) sulfate, 2:50 describe a physical test to show whether a sample of water is pure, 3:01 know that chemical reactions in which heat energy is given out are described as exothermic, and those in which heat energy is taken in are described as endothermic, 3:02 describe simple calorimetry experiments for reactions such as combustion, displacement, dissolving and neutralisation, 3:03 calculate the heat energy change from a measured temperature change using the expression Q = mcT, 3:04 calculate the molar enthalpy change (H) from the heat energy change, Q, 3:05 (Triple only) draw and explain energy level diagrams to represent exothermic and endothermic reactions, 3:06 (Triple only) know that bond-breaking is an endothermic process and that bond-making is an exothermic process, 3:07 (Triple only) use bond energies to calculate the enthalpy change during a chemical reaction, 3:08 practical: investigate temperature changes accompanying some of the following types of change: salts dissolving in water, neutralisation reactions, displacement reactions and combustion reactions, 3:09 describe experiments to investigate the effects of changes in surface area of a solid, concentration of a solution, temperature and the use of a catalyst on the rate of a reaction, 3:10 describe the effects of changes in surface area of a solid, concentration of a solution, pressure of a gas, temperature and the use of a catalyst on the rate of a reaction, 3:11 explain the effects of changes in surface area of a solid, concentration of a solution, pressure of a gas and temperature on the rate of a reaction in terms of particle collision theory, 3:12 know that a catalyst is a substance that increases the rate of a reaction, but is chemically unchanged at the end of the reaction, 3:13 know that a catalyst works by providing an alternative pathway with lower activation energy, 3:14 (Triple only) draw and explain reaction profile diagrams showing H and activation energy, 3:15 practical: investigate the effect of changing the surface area of marble chips and of changing the concentration of hydrochloric acid on the rate of reaction between marble chips and dilute hydrochloric acid, 3:16 practical: investigate the effect of different solids on the catalytic decomposition of hydrogen peroxide solution, 3:17 know that some reactions are reversible and this is indicated by the symbol in equations, 3:18 describe reversible reactions such as the dehydration of hydrated copper(II) sulfate and the effect of heat on ammonium chloride, 3:19 (Triple only) know that a reversible reaction can reach dynamic equilibrium in a sealed container, 3:20 (Triple only) know that the characteristics of a reaction at dynamic equilibrium are: the forward and reverse reactions occur at the same rate, and the concentrations of reactants and products remain constant, 3:21 (Triple only) understand why a catalyst does not affect the position of equilibrium in a reversible reaction, 3:22 (Triple only) predict, with reasons, the effect of changing either pressure or temperature on the position of equilibrium in a reversible reaction (references to Le Chateliers principle are not required), 4:01 know that a hydrocarbon is a compound of hydrogen and carbon only, 4:02 understand how to represent organic molecules using empirical formulae, molecular formulae, general formulae, structural formulae and displayed formulae, 4:03a know what is meant by the term isomerism, 4:03 know what is meant by the terms homologous series, functional group and isomerism, 4:04 understand how to name compounds relevant to this specification using the rules of International Union of Pure and Applied Chemistry (IUPAC) nomenclature.