A Level Chemistry 2019 Course overview

A Level Chemistry

2019

Course overview

Woodbridge High School

______________________________________________________________

Know the course you are following…. You are studying the new A level course that is examined by EDEXCEL. It started in September 2015. It has terminal exam papers; no A level is modular anymore. Know where to find your specification….

From the EDEXCEL web-site. 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 text-book. 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 lesson-time. 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.

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

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 = 80

50

(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 = 80

50

(120 UMS)

To be taken June 2019

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: Acid-base Equilibria

Topic 13: Energetics II

Topic 14: Redox II

Topic 15: Transition Metals

1 hour 45

minutes. Some (10) objective spread throughout,

short open,

open-

response,

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

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 2-methylpropan-2-ol 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 12

9. Finding the K

value for a weak acid

CP10

Topic 14

10. Investigating some

electrochemical cells

CP11

Topic 14

11. 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’ (Harcourt-Esson, iodine clock)

CP14

Topic 16

14. Finding the activation

energy of a reaction

CP15

Topic 18

15. Analysis of some inorganic and organic

unknowns

CP16

Topic 18

16. The preparation of

aspirin

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.

2. Applies investigative

approaches and methods when

using instruments and equipment

a) Correctly uses appropriate instrumentation, apparatus and materials (including ICT) to carry out investigative activities, experimental techniques and procedures with minimal assistance or prompting.

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.

3. Safely uses a range of practical equipment

and materials

a) Identifies hazards and assesses risks associated with these hazards when carrying out experimental techniques and procedures in the lab or field.

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.

A level Chemistry. ½ termly review date / / .

Student Name Teacher & Group ALPS target grade_______

½ term:

Teacher Comment / Check

Notes & hand-outs.

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

Supplementary notes produced

1. Clear evidence of additional notes. 2. Some additions to notes have been made. 3. No evidence of supplementary notes

Other Practical Work - write-ups

1. Done & corrections made 2. Done 3. Missing write ups or 4. Write ups are incomplete

Teacher set questions

1. Those set are done & checked 2. Those set are done, checked & corrected 3. Missing answers.

Additional questions

1. Those set are done & checked 2. Those set are done, checked & corrected 3. Additional Qs done, checked & corrected 4. Missing answers.

Response to Teacher/Peer Marking

1. Some written response to marking. 2. Thorough written response to marking so that student is now on Target

Topic Test (if applicable)

Score Remark

Teacher initials & Date

Any further comment from teacher:

Student Response

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 A-level chemistry course. Calculate the relative formula mass of the follow compound – show your working

1. H2O 2. CO2 3. MgCO3 4. Al2O3 5. CH3COOH 6. CuSO4.5H2O 7. (NH4)SO4.FeSO4.6H2O

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 H2O 2. The mass of 1.5 moles of CO2 3. The mass of 0.25 moles of MgCO3 4. The mass of 2000 moles Al2O3

Calculate: (moles for mass)

1. The number of moles in 30g of CH3COOH 2. The number of moles in 0.15g of CuSO4.5H2O 3. The number of moles in 9.2g of (NH4)SO4.FeSO4.6H2O

Balance these equations

1) Ca + O2 → CaO

2) Na2O + H2O → NaOH

3) Al + O2 → Al2O3

4) Na + Cl2 → NaCl

5) Na2CO3 → Na2O + CO2

6) K + O2 → K2O

8) C4H8 + O2 → CO2 + H2O

9) Fe2O3 + HCl → FeCl3 + H2O

10) F2 + KBr → KF + Br2

11) C5H12 + O2 → CO2 + H2O 12) NH3 + O2 → NO + H2O

13) HNO3 → NO2 + H2O + O2

Reaction quantity questions 1. What is the maximum mass of calcium carbonate that will react with 25.0cm3 of 2.00moldm-3 HCl(aq)?

CaCO3(s) + 2HCl(aq) CaCl2(aq) +CO2(g) + H2O(l) 2. What is the minimum volume of 0.500moldm-3 sulphuric acid needed to react with 0.240g of magnesium?

Mg(s) + H2SO4(aq) MgSO4(aq) + H2(g) 3. 25cm3 of sodium hydroxide solution, NaOH(aq), of unknown concentration was titrated with dilute sulphuric acid of concentration 0.500moldm-3. 20.0cm3 of the acid was needed to neutralise the alkali. Find its concentration in moldm-3.

2NaOH(aq) + H2SO4(aq) Na2SO4(aq) + 2H2O(l) 4. Limewater is calcium hydroxide solution. In an experiment to find the concentration of calcium hydroxide in limewater, 25.0cm3 of limewater needed 18.8cm3 of 0.0400moldm-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) CaCl2(aq) + 2H2O(l) 5. 2.10g of sodium hydrogencarbonate, NaHCO3(s), was dissolved in water and the solution was made up to 250cm3. 25.0cm3 of this solution was pipetted into a flask and an indicator was added. This solution was neutralised by 25.9cm3 of dilute hydrochloric acid added from a burette. Calculate the acid’s concentration.

NaHCO3(aq) + HCl(aq) NaCl(aq) + CO2(g) + H2O(l)

Using Avogadro’s Number, 6.02 X1023 particles per mole. Example 1 mole of Ca(NO3)2 contains 3 moles of ions; 1 mole of Ca2+ and 2 moles of NO3

– . The total number of ions in 1 mole of Ca(NO3)2 is therefore 3 X Avogadro’s number = 1.806 X 1024

1. What is the total number of atoms in 1 mole of i) H2O ii) CO2 iii) H2SO4 iv) CH3CO2H 2. What is the total number of ions in 1 mole of i) Li2O ii) Fe2(SO4)3 iii) KMnO4 iv) Na2Cr2O7 3. How many molecules of water are there in 1/4 mole of H2O? 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 H2SO4? How many atoms would there be in this number of molecules of sulphuric acid?

Empirical formula Work out the empirical formulae for the compounds made by the following combinations of elements 1. 0.72g of magnesium combines with 0.28g of nitrogen. 2. 1.68g of iron combines with 0.64g of oxygen. 3. 0.62g of phosphorus combines with 0.48g of oxygen. 4. 1.4g of nitrogen combines with 0.30g of hydrogen. 5. 9.8g of a viscous, colourless liquid contains 0.2g of hydrogen, 3.2g of sulphur and 6.4g of oxygen. 6. 3.400g of calcium formed 9.435g of a chloride compound. What is the empirical formula of this compound? 7. 2.39g of lead sulphide contains 2.07g of lead. What is the empirical formula of this compound?

Writing formula

1+ ammonium NH4 + 1- bromide Br

-

copper(I) Cu + chlorate I ClO

-

hydrogen H + chlorate V ClO3

-

lithium Li + chloride Cl

-

potassium K + cyanide CN

-

silver Ag + ethanoate CH3CO2

-

sodium Na + ethoxide CH3CH2O

-

hydrogencarbonate HCO3

-

hydroxide OH

-

iodide I

-

manganate VII MnO4

-

2+ barium Ba 2+ nitrate NO3

-

calcium Ca 2+

copper II Cu 2+ 2- carbonate CO3

2-

iron II Fe 2+ dichromate VI Cr2O7

2-

lead II Pb 2+ oxide O

2-

magnesium Mg 2+ sulphate SO4

2-

manganese Mn 2+ sulphide S

2-

strontium Sr 2+ sulphite SO3

2-

zinc Zn 2+ thiosulphate S2O3

2-

3+ aluminium Al 3+ 3- phosphate PO4

3-

iron III Fe 3+

chromium

III

Cr 3+

Use the table above to guide you Name these compounds

1. NaOH

2. KCN

3. CuSO4

4. NH4Cl

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

DATA-BOOK SECTION