A Level Chemistry 2018 Course overview

Transcription

1 A Level Chemistry 2018 Course overview Woodbridge High School

2 This booklet should give you an overview of your course and some ideas of where to find resources. Page 2 & 3 summarises how you will be examined & assessed. Page 4. As this is a practical subject there will be a number of Core Practicals that you will have to know about for the exam. These are listed here. Page 5 is a list of the CPAC skills you will be tested on throughout the course Every half term you will be asked to present your folders Page 6 is an example to the sheet your teacher will use to assess this. Some activities to complete over the summer The remaining pages contain important reference data Know the course you are following. You are studying the new A level course that is examined by EDEXCEL. It started in September It has terminal exam papers; no A level is modular anymore. Know where to find your specification. From the EDEXCEL website. This is how you can access resources from some of your lessons, Core Practicals tasks, support materials from practical work, test papers, and your data booklet. (Your teacher will talk to you about each of these.) READ & USE your textbook. Your use of your Curtis, Hill and Hunt text book may be infrequent in class but you should always have it with you & refer to it between lessons. AS Chemistry, by George Facer is worth using. We can loan you a lab coat although you may want one invest in one of your own your notes, text book, calculator and lab coat with you at all times. You will need to do more than just the work set in lessontime. It is essential for you to consolidate work covered in class. You will want to get the best possible grade and will hope to be predicted a high grade. You will want to write remarks on your Personal Statement about what extra you have done. It is very competitive to get university places. You need to produce A standard work straight away if you are ambitious. In short, it pays, from the start, to be an independent learner! Read plenty. Attend lectures. Apply for courses. Volunteer for things.

3 EDEXCEL CHEMISTRY AS level You will have mock exams based on AS papers and content UNIT CONTENT ASSESSMENT DETAILS WEIGHTING % AS AVAILABILITY Unit 1 8CH0/01 Core Inorganic & Physical Chemistry. Topic 1: Atomic Structure and the Periodic Table Topic 2: Bonding and Structure Topic 3: Redox I Topic 4: Inorganic Chemistry and the Periodic Table Topic 5: Formulae, Equations and Amounts of Substance 1 ½ hr written exam Some (10) objective & the rest structured. 20% of Qs based on practical work. 20% mathematical. Raw score = (120 UMS) To be taken June 2019 Unit 2 6CH02 Core Organic & Physical Chemistry. Topic 2: Bonding and Structure Topic 3: Redox I Topic 5: Formulae, Equations and Amounts of Substance Topic 6: Organic Chemistry I Topic 7: Modern Analytical Techniques I Topic 8: Energetics I Topic 9: Kinetics I Topic 10: Equilibrium 1 ½ hr written exam Some (10) objective & the rest structured. 20% of Qs based on practical work. 20% mathematical. Raw score = (120 UMS) To be taken June 2019

4 EDEXCEL CHEMISTRY A level UNIT CONTENT ASSESSMENT DETAILS WEIGHTING % AVAILABILITY Unit 1 9CH0/01 Advanced Inorganic & Physical Chemistry. Topic 1: Atomic Structure and the Periodic Table Topic 2: Bonding and Structure Topic 3: Redox I Topic 4: Inorganic Chemistry and the Periodic Table Topic 5: Formulae, Equations and Amounts of Substance Topic 8: Energetics I Topic 10: Equilibrium I Topic 11: Equilibrium II Topic 12: Acidbase Equilibria Topic 13: Energetics II Topic 14: Redox II Topic 15: Transition Metals 1 hour 45 minutes. Some (10) objective spread throughout, short open, openresponse, calculations and extended writing questions. 20% mathematical. Raw score = 90 (30%) To be taken June 2020 Unit 2 9CH0/02 Advanced Organic & Physical Chemistry. Topic 2: Bonding and Structure Topic 3: Redox I Topic 5: Formulae, Equations and Amounts of Substance Topic 6: Organic Chemistry I Topic 7: Modern Analytical Techniques I Topic 9: Kinetics I Topic 16: Kinetics II Topic 17: Organic Chemistry II Topic 18: Organic Chemistry III Topic 19: Modern Analytical Techniques II 1 ¾ hr written exam Some (10) objective & the rest structured. 20% mathematical. Raw score = 90 (30%) To be taken June 2020 Unit 3 9CH0/03 General & Practical Principles in Chemistry Tests the entire content of the specification. Synoptic problems & Qs that relating to practical Chemistry. Will draw on students experience of core practicals 2 ½ hrs Some multiple choice, short response, open response, calculations & extended writing Raw score = 120 (40%) (~ ½ of questions relate to practical work) June 2020

5 Core practicals There are 16 core practicals that you must have knowledge & understanding of for your exams. CP1 CP8 are AS based. CP9 CP16 are A2 based CP Code Topic Brief Description ~Date CP1 Topic 5 1: Measuring the molar volume of a gas CP2 Topic 5 2: Preparation of a standard solution from a solid acid CP3 Topic 5 3: Finding the concentration of a solution of hydrochloric acid CP4 Topic 6D 4: Investigation of the rates of hydrolysis of halogenoalkanes CP5 Topic 6E 5: The oxidation of ethanol CP6 Topic 6E 6: Chlorination of 2methylpropan2ol with concentrated HCl CP7 Topic 7 7: Analysis of some inorganic and organic unknowns CP8 Topic 8 8: To determine the enthalpy change of a reaction using Hess s Law CP9 Topic Finding the K value for a weak acid CP10 Topic Investigating some electrochemical cells CP11 Topic Redox titration CP12 Topic 15B 12. The preparation of a transition metal complex CP13 Topic 16 13a: Following the rate of the iodinepropanone reaction by a titrimetric method 13b investigating a clock reaction (HarcourtEsson, iodine clock) CP14 Topic 16 CP15 Topic Finding the activation energy of a reaction 15. Analysis of some inorganic and organic unknowns CP16 Topic The preparation of aspirin

6 You will have a file that is kept in school that is evidence of you achieving practical competency. This can only been awarded when you have shown mastery of the following. 1. Follows written procedures a) Correctly follows instructions to carry out the experimental techniques or procedures. a) Correctly uses appropriate instrumentation, apparatus and materials (including ICT) to carry out investigative activities, experimental techniques and procedures with minimal assistance or prompting. 2. Applies investigative approaches and methods when using instruments and equipment b) Carries out techniques or procedures methodically, in sequence & in combination, identifying practical issues & making adjustments when necessary. c) Identifies & controls significant quantitative variables where applicable, & plans approaches to take account of variables that cannot readily be controlled. d) Selects appropriate equipment & measurement strategies in order to ensure suitably accurate results. a) Identifies hazards and assesses risks associated with these hazards when carrying out experimental techniques and procedures in the lab or field. 3. Safely uses a range of practical equipment and materials b) Uses appropriate safety equipment and approaches to minimise risks with minimal prompting. c) Identifies safety issues and makes adjustments when necessary. 4. Makes and records observations a) Makes accurate observations relevant to the experimental or investigative procedure. b) Obtains accurate, precise and sufficient data for experimental and investigative procedures and records this methodically using appropriate units and conventions. 5. Researches, references and reports a) Uses appropriate software and/or tools to process data, carry out research and report findings. b) Sources of information are cited demonstrating that research has taken place, supporting planning and conclusions. Keep track of all the work you have to do. The following will be completed ½ termly.

7 A level Chemistry. ½ termly review date / /. Student Name Teacher & Group ALPS target grade Notes & handouts. ½ term: Supplementary notes produced Teacher Comment / Check 1. Notes are neat, complete & in order 2. Handouts included. 3. Notes are missing. 4. Presentation of work needs to improve. 5. Handouts are missing 1. Clear evidence of additional notes. 2. Some additions to notes have been made. 3. No evidence of supplementary notes Other Practical Work writeups Teacher set questions 1. Done & corrections made 2. Done 3. Missing write ups or 4. Write ups are incomplete 1. Those set are done & checked 2. Those set are done, checked & corrected 3. Missing answers. Additional questions Response to Teacher/Peer Marking 1. Those set are done & checked 2. Those set are done, checked & corrected 3. Additional Qs done, checked & corrected 4. Missing answers. 1. Some written response to marking. 2. Thorough written response to marking so that student is now on Target Score Remark Topic Test (if applicable) Teacher initials & Date Any further comment from teacher: Student Response

8 The next few pages contain some activities that you will need to complete over the summer. Completing them will help ensure a smooth start to your Alevel chemistry course. Calculate the relative formula mass of the follow compound show your working 1. H 2 O 2. CO 2 3. MgCO 3 4. Al 2 O 3 5. CH 3 COOH 6. CuSO 4.5H 2 O 7. (NH 4 )SO 4.FeSO 4.6H 2 O Use the molecular mass from above to answer these questions show your working Calculate: (mass from moles) 1. The mass of 4 moles of water H 2 O 2. The mass of 1.5 moles of CO 2 3. The mass of 0.25 moles of MgCO 3 4. The mass of 2000 moles Al 2 O 3 Calculate: (moles for mass) 1. The number of moles in 30g of CH 3 COOH 2. The number of moles in 0.15g of CuSO 4.5H 2 O 3. The number of moles in 9.2g of (NH 4 )SO 4.FeSO 4.6H 2 O Balance these equations 1) Ca + O 2 CaO 2) Na 2 O + H 2 O NaOH 3) Al + O 2 Al 2 O 3 4) Na + Cl 2 NaCl 5) Na 2 CO3 Na 2 O + CO 2 6) K + O 2 K 2 O 8) C 4 H 8 + O 2 CO 2 + H 2 O 9) Fe 2 O 3 + HCl FeCl 3 + H 2 O 10) F 2 + KBr KF + Br 2 11) C 5 H 12 + O 2 CO 2 + H 2 O 12) NH 3 + O 2 NO + H 2 O 13) HNO 3 NO 2 + H 2 O + O 2

9 Reaction quantity questions 1. What is the maximum mass of calcium carbonate that will react with 25.0cm 3 of 2.00moldm 3 HCl(aq)? CaCO 3 (s) + 2HCl(aq) CaCl 2 (aq) +CO 2 (g) + H 2 O(l) 2. What is the minimum volume of 0.500moldm 3 sulphuric acid needed to react with 0.240g of magnesium? Mg(s) + H 2 SO 4 (aq) MgSO 4 (aq) + H 2 (g) 3. 25cm 3 of sodium hydroxide solution, NaOH(aq), of unknown concentration was titrated with dilute sulphuric acid of concentration 0.500moldm cm 3 of the acid was needed to neutralise the alkali. Find its concentration in moldm3. 2NaOH(aq) + H 2 SO 4 (aq) Na 2 SO 4 (aq) + 2H 2 O(l) 4. Limewater is calcium hydroxide solution. In an experiment to find the concentration of calcium hydroxide in limewater, 25.0cm 3 of limewater needed 18.8cm 3 of moldm 3 hydrochloric acid to neutralise it. Calculate the concentration of calcium hydroxide in moldm 3 and in gdm 3. Ca(OH) 2 (aq) + 2HCl(aq) CaCl 2 (aq) + 2H 2 O(l) g of sodium hydrogencarbonate, NaHCO 3 (s), was dissolved in water and the solution was made up to 250cm cm 3 of this solution was pipetted into a flask and an indicator was added. This solution was neutralised by 25.9cm 3 of dilute hydrochloric acid added from a burette. Calculate the acid s concentration. NaHCO 3 (aq) + HCl(aq) NaCl(aq) + CO 2 (g) + H 2 O(l) Using Avogadro s Number, 6.02 X10 23 particles per mole. Example 1 mole of Ca(NO 3 ) 2 contains 3 moles of ions; 1 mole of Ca and 2 moles of NO 3. The total number of ions in 1 mole of Ca(NO 3 ) 2 is therefore 3 X Avogadro s number = X What is the total number of atoms in 1 mole of i) H 2 O ii) CO 2 iii) H 2 SO 4 iv) CH 3 CO 2 H 2. What is the total number of ions in 1 mole of i) Li 2 O ii) Fe 2 (SO 4 ) 3 iii) KMnO 4 iv) Na 2 Cr 2 O 7 3. How many molecules of water are there in 1 / 4 mole of H 2 O? How many atoms would there be in this number of molecules of water? 4. How many molecules of sulphuric acid are there in 1 / 3 mole of H 2 SO 4? How many atoms would there be in this number of molecules of sulphuric acid?

10 Empirical formula Work out the empirical formulae for the compounds made by the following combinations of elements g of magnesium combines with 0.28g of nitrogen g of iron combines with 0.64g of oxygen g of phosphorus combines with 0.48g of oxygen g of nitrogen combines with 0.30g of hydrogen g of a viscous, colourless liquid contains 0.2g of hydrogen, 3.2g of sulphur and 6.4g of oxygen g of calcium formed 9.435g of a chloride compound. What is the empirical formula of this compound? g of lead sulphide contains 2.07g of lead. What is the empirical formula of this compound? Writing formula 1+ ammonium NH bromide Br copper(i) Cu + chlorate I ClO hydrogen H + chlorate V ClO 3 lithium Li + chloride Cl potassium K + cyanide CN silver Ag + ethanoate CH 3CO 2 sodium Na + ethoxide CH 3CH 2O hydrogencarbonate HCO 3 hydroxide iodide OH I barium Ba manganate VII MnO 4 nitrate NO 3 calcium Ca copper II Cu 2 carbonate CO 3 2 iron II Fe dichromate VI Cr 2O 7 2 lead II Pb oxide O 2 magnesium Mg sulphate SO 4 2 manganese Mn sulphide S 2 strontium Sr sulphite SO 3 2 zinc Zn thiosulphate S 2O aluminium Al 3+ 3 phosphate PO 4 3 iron III chromium III Fe Cr 3+ 3+

11 Use the table above to guide you Name these compounds 1. NaOH 2. KCN 3. CuSO 4 4. NH 4 Cl 5. Mg(OH) 2 Predict the formula of the following compounds (hint remember the overall charge must be zero) 1. Calcium chloride 2. Sodium carbonate 3. Strontium nitrate 4. Iron (III) bromide 5. Potassium hydrogencarbonate

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