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Chemistry A IFNJTUSZ OCR

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Exciting resources developed in exclusive partnership to support the new GCE Chemistry A specification

Heinemann is working exclusively with OCR to produce an exciting suite of resources tailored to the new OCR GCE Chemistry A specification. Written by experienced examiners, OCR AS and A2 Chemistry provide you with tailored support for teaching the revised specification. Comprehensive support for AS and A2, and motivating exam preparation in our unique Exam Café, will give your students every chance of success.

Course Structure AS

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AS

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Exclusively endorsed by OCR for GCE Chemistry A

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AS

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$IFNJTUSZ Exclusively endorsed by OCR for GCE Chemistry A

Exclusively endorsed by OCR for GCE Chemistry A

Second Edition

This revision guide is tailored to the OCR specification and exclusively endorsed by OCR for GCE Chemistry A. It is written by experienced examiners and teachers, giving you: complete coverage of the specification for the exams content organised by module and unit to follow the structure of the specification and exams bite-sized chunks of information to make it easier to organise your revision time quick-check revision questions so that you can test your own knowledge easily hints and tips from examiners to help you avoid common errors lots of practice exam-style questions for each unit all the answers to questions so that you can check that you’re on the right track. Titles in this series: OCR AS Chemistry student book and exam café CD-ROM OCR A2 Chemistry student book and exam café CD-ROM OCR AS Chemistry Teacher Support CD-ROM OCR A2 Chemistry Teacher Support CD-ROM OCR AS Chemistry revision guide OCR A2 Chemistry revision guide

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978 0 435691 81 3 978 0 435691 98 1 978 0 435691 83 7 978 0 435691 93 6 978 0 435583 71 2 978 0 435583 74 3

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Sarah Baldwin Christopher Wood Series Editor: Rob Ritchie

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A2 Revision Guide

What you can expect from Heinemann’s OCR AS and A2 Chemistry A l OCR and Heinemann working in exclusive partnership to provide better support for you. l Engaging resources written by experienced examiners and tailored to the new specification. l A full ready-to-use teaching scheme that can be customised to give you total freedom and flexibility. l Innovative Exam Café CD-ROM provided FREE in the back of every Student Book.

Authors itor Series Ed ie Rob Ritch

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Student Book Exam Café Teacher Support Revision CD-ROM CD-ROM Guide

AS Dave Gent Rob Clarke Rob Ritchie Rob King Chris Wood

Rob Clarke Peter Haigh Rob King Chris Wood

Mike Wooster Helen Eccles

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Peter Haigh Rob Clarke Ruth Bartlett

Mike Wooster Helen Eccles

Rob Clarke Rob King Chris Wood

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Student Books

Exclusively endorsed by OCR for GCE Chemistry A

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We listen to teachers’ needs... Exclusively endorsed by OCR, these Student Books offer accessible and engaging material to help students understand the underlying principles of science. Careful explanations of key equations, plenty of worked examples, practice questions and exam-style questions all ensure that students have plenty of opportunities to improve their skills. Learning objectives are taken from the specification to highlight what students need to know and understand.

s 13 Titration

1.1

By the end of thi

s spread, you

... should be able to

ons.

uctured calculati

, and carry out str

d–base titrations

✱ Perform aci

t reacts e solution tha tions volume of on Acid–baseetrtitic ra measure the analysis, you ion.

with a

solut During volum nd, different u react a , in which yo lume of a seco etric analysis measured vo type of volum ial ec sp a is titration se. is is usually a An acid–base lution of a ba o solutions. Th acid with a so one of the tw solution of an ncentration of co the ow kn ation about • You must d 1.1.7). known inform ion (see sprea to find out un standard solut ndard solution sta s thi e us ion. sis, you second solut • In the analy dissolved in the the substance : be y ma information The unknown solution tration of the • the concen ss • a molar ma stallisation. • a formula of water of cry of molecules • the number al flask. s. low ion to a conic fol e of one solut t a titration as asured volum You carry ou you add a me e, ett pip til the reaction a un te. k • Using ced in a buret the conical flas the solution is pla the solution in The volume of • The other te is added to the titration. ret of bu int po the d in the en lled ca is • The solution is completed. Th ured. has just been lume of the rette is meas d from the bu cts with the vo solution adde that exactly rea ion lut so e e of on lum vo the ow You now kn . lution. other solution tor. in the basic so ing an indica solution than end point us r in the acidic lour lou co co t the We identify the en s fer dif s. It also show tor must be a base indicator • The indica the acidic common acid– the colours in n me ee ng so tw usi of is be rs in titration the colou int colour is s acid–base Table 1 lists t this end po Figure 1 Thi . Methyl int. Notice tha as an indicator at the end po ns methyl orange acidic solutio in s. red ion lut ed so our End point colour and basic orange is col The end in base ns. basic solutio and yellow in en – orange. our in betwe ve point is the col ical flask abo con the in n The solutio nt the end poi d che rea has

Colour in acid

Indicator methyl orange

red

bromothymol blu phenolphthalein

e

yellow

Colour

yellow blue pink

colourless

to the aqu from the burette e has been added t the aqueous bas s colourless. * This assumes tha is complete when the solution goe base, the titration tors mon acid–base rs of some com

orange

green pale pink* eous acid. If acid

is added to

indica

sults d examples: titration re n in the worke knowns frsom ttern, as show Calculatintitrgatiun low a set pa on results fol to work out. ; Analysis of that you need ays the same the unknown o steps are alw depending on • the first tw ly to the y be different, ma uctured similar p str ste be rd l • the thi carry out wil ions that you lat lcu ca y an y, In AS chemistr low. examples be steps yourself. rk out these y have to wo For A2, you ma

28 .U1 M1.indd

4

28-29

In Exclusive Partnership

Text is structured in line with the new OCR specification by Unit and Module.

Modu

Atoms and reac Titra

tion n concentra an unknow Calculating 1: e pl d am OH(aq) reacte Worked ex

e Na –3 sodium hydroxid 3 50 mol dm ). 25.0 cm of 0.1 , SO on 4(aq H ati titr id, 2 a ac In 3 lfuric .40 cm of su ) exactly with 23 (aq)  2H2O(l ) }m Na2SO4 SO 4(aq t reacted. H  2 q) l, of NaOH tha 2NaOH(a mo in nt, ou the am –3 (a) Calculate 25.0 __ 5s10 mol ___ V 0 s 00  3.7 __ 0.15 10 s ___ . n(NaOH) c 1000 that was used in mol, of H2SO4 }}m the amount,  H2SO4(aq) q) H(a (b) Calculate 2NaO }}m  1 mol –3 mol equation l mo 2 10 uation eq –3 mol 1.875s m fro les mo id. 3.75s10 –3 of the sulfuric ac les actual mo tion, in mol dm –3 –3 mol dm the concentra –3 00 10 10 s _ 1 s (c) Calculate ___ 8.0 ___  s10 ___ 1.875___ __ ___ n s__10 __00 ___ 23.40 __ c(H2SO4)  V

Worked exam

ating an

ple 2: Calcul

Sample pages from OCR AS Chemistry A Student Book.

Notes :

For (a), we use

3 ) cm__ V (in___ ___ 1000 the balanced equ For (b), we use cting quantities work out the rea ali. acid and alk H cts with 1 mol 2 mol NaOH rea V cs_  n : nge rra For (c), we rea

s amount, n  c

Hence, c 

lution up to d made the so l dm–3 HX in water an st 0.0614 mo g of an acid3 ain 94 ag 2.7 ion d lut lve so this so reach of to ed cm ed .0 A student dis ne 25 d ) were 3 3 student titrate of Na2CO3(aq 250 cm . The ). 23.45 cm te Na2CO3(aq na rbo ca m sodiu . the end point on is: for this reacti The equation (g)  H2O(l) aX(aq)  CO2 X(aq) }m 2N 2H that reacted.  ) (aq l, of Na2CO3 Na2CO3 mo in nt, ou the am –3 (a) Calculate 23.45 ___  1.44s10 mol ___ s V 14 1000 __ 0.06 s ___ the titration. n(Na2CO3) c 1000 in that was used in mol, of HX }}m the amount,  2 HX(aq) ) (aq (b) Calculate CO Na2 3 }}m  2 mol equation –3 mol 1 mol 3 –3 m equation l 2.88s10 250 cm moles fro 1.44s10 mo make up the to les that was used actual mo in mol, of HX nt, ou am the (c) Calculate –3 mol –2 l solution. –3  2.88s10 mo ins 2.88s10 3 HX(aq) conta cm s2.88s10 .0 25 contains 10–1 3 ion . lut HX so id 0 cm the ac 25 of , l the , mo So g tion, in the concentra –1 (d) Calculate ____  97.0 g mol ___94 m ___2.7 m_ so, M  _ n_  8 s 10–2 _ 2.8 n  M

Notes

the steps a For (a) and (b), rked exam as in the first wo example, h In this worked steps. You are two further these in a helped through le up by a For (c), we sca t, in mol, find the amoun 3 n that w 250 cm solutio nge: rra rea we For (d), __ ___ss, ___ma amount, n  molar ma m_ _ Hence, M  n In this example,

n below.

concentratio

tly reacted exac 1 to calculate Questions m hydroxide rked example aqueous sodiu method in Wo –3

3 1 Use the 25 mol dm 25.0 cm of 0.1 In a titration, 3 ic acid. of hydrochlor cm O(l) .75 22 with NaCl(aq)  H2 OH(aq) }m H X. ic acid. HCl(aq)  Na ss of the acid 2 the hydrochlor of n tio e the molar ma tra en nc solution up to le 2 to calculat Find the co and made the –3 dium Worked examp ter in wa d in tho X, me H so 2 Use the g of an acid, 2 0.125 mol dm solved 1.571 lution against end point. A student dis cm3 of this so ed to reach the 3 e titrated 25.0 (aq) were need 3 OH Na of 250 cm . Sh .30 cm 21 ). (aq OH hydroxide, Na ction is: O(l) n for this rea Na X(aq)  2H2 The equatio H2X(aq) }m 2  q) H(a aO 2N

Questions students should be able to answer after studying each spread.

0 100__ n s___ ___ V

Worked student should b

olar mass unknown m

the unknown

Table 1 Colou

935 chemistry

Dave Gent and Rob Ritchie Series Editor: Rob Ritchie

the mass of HX

is 2.7

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End-of-module summary pages help students link together all the topics within each module.

1.1

Atoms and reactions summar y

Dave Gent and Rob Ritchie Series Editor: Rob Ritchie

Practi ce quest ions 1 How many protons,

Practice q

neutrons and electrons are in the following atoms and ions ?

(a)

Moles

(c)

Mass n = mass, m molar mass, M

(e) (g)

ctions

Gas volumes

Moles

3 V n = (in dm ) = V (in cm3) 24.0 24 000

uation to of the

Solutions n = c V (in dm3) = c  V (in cm3) 1 000

Acids

Carbonate

d examples show Salt
CO2
H20 ts how calculations be set out.

Metal

Base

Base Alkali soluble base OH–

Salt
H20 Salt
H2

Reduction • Gain of electrons • Decrease in oxidation number

m __ ___ ass, M

3 Use Ar values from the Perio

dic Table to calculate the relative formula mass of the following: (a) Cr2O3; (b) Rb2S; (c) Zn(OH)2; (d) (NH4)2CO3; (e) Fe3(PO4)2.

(a) 6 mol MnO ; 2 (c) 0.60 mol Ag SO . 2 4

5 Calculate the amo unt,

(a) 8.823 g CaI ; 2 (c) 7.50 g Cu(NO ) . 32

(b) 0.25 mol Ga O ; 2 3

in mol, in: (b) 48.55 g K CrO ; 2 4

formula for the compoun d of carbon, hydrogen and oxygen atoms with the composition by mass: C, 40.0%; H, 6.7%; O, 53.3%; M 90. r

8 (a) At RTP, what amount,

794 g.

in mol dm–3, for the follow ing solutions: (a) 0.75 moles dissolved in 5 dm3 of solution; (b) 0.450 moles disso lved in 100 cm3 of solut ion.

ing equations: (a) P4(s) + O2(g) }m P 2O5(s) (b) C5H12(l) + O (aq) }m 2 CO2(g) + H2O(l) (c) NaOH(aq) + H PO 3 4(aq) }m Na2HPO (aq) + H2O(l). 4

12 Define the terms:

(a) acid;

(b) base;

in mol, of gas molecules are in: (i) 84 dm3; (ii) 300 cm3; (iii) 10 dm3? (b) At RTP, what is the volume, in dm3, of: (i) 12 mol CO (g); 2 (ii) 0.175 mol N (g); 2 (iii) 2.55 g NO(g)?

9 Find the amount, in mol,

of solute dissolved in the following solutions: (a) 2 dm3 of a 0.225 mol dm–3 solution; (b) 25 cm3 of a 0.175 mol dm–3 solution.

(c) alkali.

13 Write balanced equa tions

for the following acid reac tions: (a) nitric acid and iron( III) hydroxide. (b) sulfuric acid and copp er(II) carbonate. (c) hydrochloric acid and aluminium.

14 What is the oxida tion

g, in:

7 Determine the mole cular

Oxidation • Loss of electrons • Increase in oxidation number

10 Find the concentra tion,

11 Balance each of the follow

atomic mass, A , to 4 signi r ficant figures, for the following. (a) Lithium containing: 7.42%6Li and 92.58%7 Li. (b) Lead containing: 204 Pb, 1.1%; 206Pb, 24.9%; 207 Pb, 21.7%; 208Pb, 52.3 %.

formula of the compoun d formed when 1.472 g of tungsten reacts with 0.384 g of oxyg en.

Redox

a factor of 10 to , of HX in the was made up.

18 O; 8 64 30 Zn; 79 – 35 Br ;

6 Determine the emp irical

Redox

are the same mple. however, there u would be an AS exam.

(d) (f)

4 Calculate the mas s, in

Acid proton donor

H2SO4 3 ) cm__ V (in___ ___ 1000

(b)

2 Calculate the relat ive

ule 1

ations

11 B; 5 30 14 Si; 23 + 11 Na ; 45 3+ 21 Sc .

Mo

Atoms and

In Exclusive Partnership

following? (a) Cu; (d) MgSO4;

(g) (NH4)3PO4.

state of each species in

(b) I2; (e) PbCO3;

the

(c) CH4; (f) Cr2O7 2–;

15 From the experime ntal

results below, work out the formula of the hydrated salt. Mass of ZnSO ·xH O = 4 8.985 g 2 Mass of ZnSO = 5.047 4 g

16 Lithium carbonat e decompo

ses with heat: Li2CO3(s) }m Li O(s) + CO2(g) 2 What volume of CO , mea sured at RTP, is formed 2 by the decomposition of 5.71 95 g of Li2CO ? 3

17 Calcium carbonat e reac

ts with nitric acid: Na2CO3(s) + 2HNO m 2NaNO3(aq) + H O(l) + 3 CO (g) 2 0.371 g of Na CO reac 2 ts with an excess of HNO 2 3 The final volume of the 3. solution is 25.0 cm3. (a) What volume of CO , mea sured at RTP, is formed? 2 (b) What is the concentra tion, in mol dm–3, of NaN O3 formed?

18 In the redox reac tions

below, use oxidation num bers to find out what has been oxidi sed and what has been reduced. (a) N2 + 3H2 m 2NH 3 (b) 3Mg + 2Fe(NO ) m 3Mg(NO3)2 + 2Fe 33 (c) MnO2 + 4HCl m MnC l2 + Cl2 + 2H2O

M1.indd 34-35

35

Practice exam questions provided at the end of each module. Answers are in the back of the book. 29 7:26 am 10/3/08 11:2

t Don’t forge our A2 resources e coming in th m! Autumn ter

Sample pages from OCR AS Chemistry A Student Book.

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Sample questions and answers to each module with tips on how to improve, examiner tips and advice to students on practical skills.

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This revis ion guide is tailored endorsed to the OCR by specificat examiners OCR for GCE Chem ion and exclu and teach istry A. It ers, givin is written g you: by experiencsively ed complete coverage of the spec content orga ification for nised by the exam specificat s ion and exammodule and unit to follow the s bite-sized structure chun of the revision time ks of informatio n to make it easier to quick-chec organise k your knowledge revision questions so that you easily can test your hints and tips from own examiners lots of pract to help you ice exam-style avoid comm all the answ questions on errors for each unit ers to ques right track tions so that . you can chec k that you’r Titles in this e on the series: OCR AS Chem OCR A2 Chem istry student book OCR AS Chem istry student book and exam café CD-R OM and exam café 978 0 43569 OCR A2 Chem istry Teacher Supp CD-ROM 1 978 0 43569 81 3 OCR AS Chem istry Teacher Supp ort CD-ROM 1 ort CD-ROM 978 0 43569 98 1 OCR A2 Chem istry revision guid 1 e istry revis 978 0 43569 83 7 ion guide 1 978 0 43558 93 6 3 978 0 43558 71 2 3 74 3

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l Written by experienced examiners and tailored to the new specification. l Packed with examiner tips. l Targeted at ensuring understanding with quick-check questions on each topic and end of unit exam-style questions. Provides students with lots of opportunities to see problems worked through and the answers are provided step by step.

Clearly linked to the specification.

valent ssible. In a co nes the far apart as po l atom determi so they are as und the centra el each other aro rep irs irs pa pa on on ctr Electr er of ele mb nu the , ion compound or molecule. shape of the

Key words air v electron-p repulsion d v covalent bon v lone pair

CO2 ble bonds) (in fact two dou

linear

rs 2 electron pai

Module 2

example

Shape

rs

Number of pai

× × × × × ×O

O

+ exaMple J WOrked mple H3O : an ion, for exa

O

C

180
180
Bond angle

trigonal

rs

3 electron pai

× ×

BF3

××

F

×

× ×

× × B× ×× × F × × F× × × × × ×

F 120


B F F 120
Bond angle H

4 electron pai

rs

tetrahedral

CH4 + NH4

H

×

×

C

×

×

H

H 109.5
C

H H

Bond angle

rs 6 electron pai

octahedral

SF6

109.5


F

F

F F

F F

Bond angle

✔Quick che H

×

ck 1

××

N

×

×

H

H

N H H 107
H
Bond angle 107

Sample pages from OCR AS Chemistry Revision Guide.

10

90


electron pairs out how the l us that: s by working s of molecule ion theory tel pe uls sha rep t ir en -pa fer dif es of electron We know the ssible space. The rul po in as es art elv ap ms as far arrange the er so they are ir (BP) repel each oth a bonding pa atoms is called v electron pairs between two lone pair (LP) a red led sha ir cal is pa ) t shared v an electron atom only (no . g pair on one –BP repulsion v a non-bondin ules. repulsion > BP BP LP– ter, H2O, molec > ion , NH3, and wa nia mo v LP–LP repuls am s of the pe sha the lain These rules exp y e up a basicall re these will tak NH3 shared pairs mo electrons, so so it repels the s four pairs of ir, ha pa m The e ato lon 10 en a pair is 9.5° to 7°. 10 on The nitrog m ctr fro ele d e pe. But on gle is decrease tetrahedral sha d the bond an pair would, an pyramidal. than a bonding is described as ule lec mo the final shape of

24

Number of electrons

H

×

××

O

×

× ×

H O

H 104.5


H .5


Bond angle 104

Examiner tip e the Don’t confus molecule shape of the pe the sha the h wit adopt. rs pai electron

H

×

××

O

×


× ×

H

H

✔Quick che

ck 2

3

H

H

atom

shape of To work out the approach this 6 two ways to are Oxygen STep 1 There 3 ens problem. Three hydrog the of m gra dia –1 dot-and-cross e charge either draw a itiv e); Pos sit po e diagram op 8 molecule (se ber the num at s al Tot ctron number of ele or count up the d ge an m. arr central ato t. They will be pairs will adop ctrons. pe the electron ele sha of at irs pa wh r e are fou STep 2 Se because there pair. tetrahedrally Yes, one lone any lone pairs. are re repel the the if see lone pair will the t STep 3 Now tha u er, and the ory tells yo y repel each oth ir repulsion the the -pa n on tha ctr Ele gly stron STep 4 as NH3. a little more d bond angle bonding pairs same shape an uld have the of 107°. molecule sho gle an nd bo e with a ramidal shap + H O has a py

× ×× × O× ×

C

on theory n-pair repulsi

Module 2

1

ctro lecules – ele

rahedral a basically tet se will take up repelled more H2O ctrons, so the shared pairs are four pairs of ele the s so ha m irs, pa gle ato e an is The oxygen on pairs are lon The final bond than in NH3. o of the electr in H2O is less shape. But tw ar. gle ine an n-l nd no bo as and the scribed than in NH3, molecule is de al shape of the 104.5°. The fin

lecules – Shapes of mo epulsion theory r electron-pair

UNIT

Shapes of mo

s? all located multiple bond ctron pairs are s the bonding ele ir of electron triple) bonds, e bonding pa on (or le as d ub un do s co ha ore they ref the If a molecule d an bonding atoms shape. between the working out the tral atom for around the cen e table). The is O=C=O (se , so the final t the bonding CO2 ch as possible CO2 shows tha mu of as m er gra oth dia oss l repel each A dot-and-cr uble bonds wil do the in irs e electron pa ear. is sulfur dioxid molecule is lin good example shape of the uble bonds? A lecule with do mo ar ine n-l no What about a 3). eck question (see quick ch

What about

k QUeSTION QUICk CHeC

S

molecules: the following bond angles in and predict the OCl2 pes b sha the 1 Sketch d CCl4 up 6) a PCl3 s: that Se is in Gro following ion c SeF6 (note d angles in the– bon the t dic PCl6 pes and pre b sha the tch + 2 Ske + d NH4 a PCl4 te. – diagram opposi c NH2 shown in the SO 2 is for m gra nd-cross dia ? t-a ule do lec The mo 3 shape of the a What is the d angle. roximate bon b Give the app

Enables students to check their knowledge and understanding. Answers are provided at the back of the book.

?

✔Quick che

ck 3

Hints and tips help students avoid common errors.

25

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AS

Exclusively endorsed by OCR for GCE Chemistry A

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Summary of contents

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Dave Gent and Rob Ritchie Series Editor: Rob Ritchie In Exclusive Partnership

endorsed by

OCR for GCE

A2 Chemistry A

Dave Gent and Rob Ritchie Series Editor: Rob Ritchie

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Contents 76 78 searching 1 The Periodic Table: 80 nd beyo and deleev 2 The Periodic Table: Men 82 Table 3 The modern Periodic gies and atomic 2 eriodicity: ionisation ener 4 P 84 4 radii 85 ts 6 5 Periodicity: boiling poin 88 x reactions 8 6 Group 2 elements: redo 90 ions react ds: 10 poun com 2 p 7 Grou 92 12 ents: redox reactions p 7 elem vi8 GrouMod 94 ule 3 The Peri halidTab e tests 14 le 7 elements: uses andodic 76 9 Grou1p The Periodic Table: searching 16 for order 96 questions 78 ticeTable 2 The pracdic andPerio mary Sum : Mendele 98 ev 18 and beyo tions nd ques on 80 3 odul e exam mod ern inati Periodic Table 2 End-of-mThe 20 82 4 Periodicity: ionisation 4 enerand gies and atomic 22 rgy ene ins, radii Cha 2 24 6 UNIT 84 5 Periodicit (F322) 26 8 resources y: boiling points 85 6 Group 2 elem tsxand entscep c con : redo reactions 28 10 Module 1 Basi 100 88 7 Grou p 2 s pounds: reactions 30 12 hydrocarboncom 102 90 8 Group 7 elements nic chemistry 32 14 1 9Introduction to orga: redox reactions 104 92 Group 7 elem ents bons : uses and halide tests 16 ocar hydr 2 Naming 34 94 l tiona ds with func Sum 18 poun mary com g and amin prac N 3 tice 36 questions 106 96 End20 of-m ps odule examination ques grou 108 98 compoundstions 22 4 Formulae of organic 110 3824 skeletal formulae and ins, IT tural 2 Cha Struc 5UN ene 112 rgy ps and 4026 grou l tiona ulae and func form(F3 res ourtalces 6 Skele 22) 114 42 28 7 Isom Mod 115 uleerism 1 Basic con 44 tsreact their andions 30 ents andcep reag nic 8 Orga hyd 118 rocarbons 46 32 from crude oil bons ocar Hydr 100 9 1 Introduction to orga 120 48 nic chemistry 34 ocarbons as fuels Hydring 102 10 2 122 Nam hydrocarfuels 50 e bons futur the of and 36 il fuels 104 11 3 NFoss 124 amin g compounds 52 es l with of alkan functiona ions react on tituti Subs 12groups 126 54 nes Alke 106 13 4 128 3856 Formulae of organic com tions of alkenes pounds Reac 108 514Struc 130 4058 tural and skeletal form of alkenes ions ulae react tion addi er Furth 110132 615Skele 42 60 tal formulae andine brom functional groups and nes Alke 112 16 7 Isomerism 134 44 62 es strial importance of alken Indu 114136 8 17 46 64 Orga nic reagents and their reactions er chemistry 115138 48 66 9 18 HydrPolym ocarbons from crudwith e wast ers – dealing e oilour 118 140 19 Polym 50 68 10 Hydr ocarbons as fuels mer waste r uses of poly 120 20 ilOthe 52 70 11 Foss fuels and fuels of the futur 142 e 122 tice questions prac 54 72 12 Subs maryonand Sumtituti react ions of alkanes tions 144 ques 124 56 74 13 Alke nes of-module examination End126 14 Reactions of alken 58 es 128 15 Further addition react 60 ions of alkenes 130 16 Alkenes and brom 62 ine 132 17 Industrial importanc 64 e of alkenes 18Samples 66 Polymer chemistry pages from OCR 134 136 19 Polymers – dealing 68 with A our Student AS Chemistry Book. waste 138 20 Other uses of poly 70 mer waste 140 72 Summary and practice questions 142 74 End-of-module examinati on questions 144

vi

Introduction

and UNIT 1 Atoms, bonds groups (F321) s tion

Table Module 3 The Periodic for order

Module 1 Atoms and reac Contents 1 The changing atom 2 Atomic structure 3 Atomic masses Introduction e and the mole 4 Amount of substanc UN s ofITform 1 ula 5 Type Atoms, bonds and volumes gas(F3 s and gro 6 Mole ups 21) ions s and 7 Mole Mod ulesolut 1 Atoms and reaction s tions equa ical 8 Chem 1 The changing atom ions and react 9 Mole 2 sAtom ic structure s base and ic 10 Acid 3 sAtom masses 11 Salts 4 Amount of substanc allisation e and the mole r of cryst 12 Wate 5 Type s of formula tionss and 13 Titra 6 Mole gas volumes number ation 14 Oxid 7 Mole s and solutions ions x react 15 Redo 8 Chem ical equations tice questions prac and Mole s and Sum9mary reactions ination questions e exam 10of-m Acidodul s and Endbases 11 ule Salts2 Electrons, bonding and Mod 12 Wateer of crystallisa tion structur 13 Titrations 1 Evidence for shells 14 Oxidsation numals ber 2 Shell and orbit 15 Redoshell s and ionsenergy levels 3 Sub- x react Periodic Table Sum maryrons andand practhe 4 Elect tice questions chemical bonding ion to Endduct of-m intro odul e exam 5 An ination questions ing Mod 6 Ionic ule 2bond Electrons, bonding and Ionseand the Periodic Table 7 ctur stru lent bonding Cova 1 8Evide nce for shells er covalent bonding Furth 2 9Shell s and orbitals es of molecules and ions Shap 310 Subshell s and energy level s rity pola ronegativity and Elect 4 11 Elect rons and the Periodic cular forces Table 5 12 An Inter intromole duction to chemical bond ing ogen bonding 6 13 IonicHydr bond ing llic bonding and structure 14 Meta 7 Ions and the Periodic Table pounds com ionic of ture Struc 15 lent bonding 8 Cova ds tures of covalent compoun 16 Struc 9 Furth er cova lent bonding practice questions and cules 10 Shap mary Sumes of mole and ions e examination questions odul 11 Elect of-m rone Endgativ ity and polarity 12 Intermolecular force s 13 Hydr iv ogen bonding 14 Metallic bonding and structure 4-5 chemistry.prelims.indd 935 15 Structure of ionic com pounds 16 Structures of cova lent compounds Summary and practice questions End-of-module examinati on questions

iv

198 $H i 8 Enthalpy changes from ci 200 $H 9 Enthalpy changes from f 202 146 ry theo s of reaction – collision Rate 10 204 148 ol lysts Cata 11 206 1 Making and using alcoh 150 e of catalysts 12 Economic importanc 208 2 Properties of alcohols 152 ibution of alcohols distr n ation man oxid Boltz and The ion 13 210 3 Combust 154 dration of alcohols equilibrium dehy ical and ion Chem 14 ificat Ester 212 4 156 stry genoalkanes 15 Equilibrium and indu 5 Introduction to halo 158 214 alkanes practice questions 6 Reactions of halogeno and mary 160 Sum 216 the environment on questions 7 Halogenoalkanes and 162 End-of-module examinati 8 Percentage yield Contents 218 164 s urce Module 4 Reso 9 Atom economy 220 166 t – global warming 1 The greenhouse effec 10 Infrared spectroscopy 222 168 ps grou l Module Alco func, tiona opy:hols halogenoalkanes170 2 Climate change 11 Infrared spec2trosc 224 se effect i 8 Enth and ana etry the gree channhou lysis to alpy trom ges from $H 12 Mass spec 226 198 172 1463 Solutions istry chem nic 9 Enthalpy changes from ci orga in 1 Maki etry ng and using alcohol 4 The ozone layer $Hf 13 Mass spectrom 228 200 174 rns patte 148 entation 10e Rate fragm 2 s Prop of etry: react etion ertie trom ion depl s of spec – alcoh collis ass Ozon ols ion theory 14 M 230 202 176 150 5 11 Cata air pollution 3 Commec sms oxid busthani ion and 6 Controllinglysts 15 Reaction ation of alcohols 232 204 178 152 12 nEcon 4 Esterification and omic istryimportance of catalysts chem tions Gree dehy ques 7 tice drati 234 206 prac on of and alcoh ols 180 154 Summary 13 ur The 5 Introduction to halo savio Boltz and man n tions n villai distr – quesalkanes ibution 8 CO2 odule examinationgeno End-of-m 236 208 156 14 Chemical equilibriu tions 6 Reactions of halogeno m ques tice alkanes and prac mary 182158 Sum15 238210 Equilibrium and indu 7 Halogenoalkanes and questions on stry inati rgy the exam e Ene envir 3 odul onm ent Mod8ule 212 184160 End-of-m Percentage yield Summary and practice 240 alpy ques 1 Enth tions 186162 9 Atom economy 214 ic reactions Ends odule examination of-m wer Ans hermic and endotherm 210Exot ques tions 188 164 258 Infrared specletrosc 216 rams alpy profi diagopy 311Enth sary Glos 190 166 Mod Infrared specalpy ule 4 Resources opy:ges 262 functional groups dard enth troscchan 412Stan Sheet 192 168 218 ata le/D 1 Mass spectrom Tab The ges gree odic chan nhou Peri alpy se effect – global warm enth rmination ofetry 5 Dete ing 264 194 170 220 13 2 Climate change Mass spectrom ion bust of com in orga nic alpy changeetry chemistry x Inde 6 Enth 196 172 222 14 3 Solutions to the gree Mass spectromsetry: fragm nhou alpie enta se enth effec tion t patterns 174 7 Bond 224 15 4 The ozone layer Reaction mechanisms 176 226 5 Ozone depletion Summary and practice questions 228 6 Controlling air pollu 178 End-of-module examinati tion on questions 230 7 Gree n chemistry 180 232 8 CO2 – villain and savio Module 3 Energy ur 234 182 1 Enthalpy Summary and practice questions 184 236 2 Exothermic and endo End-of-module examinati thermic reactions on questions 186 238 3 Enthalpy profile diag rams Answers 188 4 Standard enthalpy chan ges 240 190 5 Determination of enth Glossary alpy changes 192 6 Enthalpy change of 258 combustion Periodic Table/Data She 194 7 Bond enthalpies et 262 196 Index 264 v

anes

genoalk Module 2 Alcohols, halo and analysis

10/3/08 11:23:32 am

935 chemistry.prelim

s.indd 4-5

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