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pages Chapter 1.1 How fast? Rates of chemicalchange
At thestart
I havestudied..
I haverevised
14-1520-2324-2730-31
I can demonstrate an understanding of the termsrate of reaction,
rate equation, order ofreaction, rate constant, half-life,
rate-determining step, activation energy,heterogeneous and
homogeneous catalyst(4.3a)
1 2 3 1 2 3 1 2 3
10-13 I can select and describe a suitable experimentaltechnique
to obtain rate data for a givenreaction, eg colorimetry, mass
change andvolume of gas evolved (4.3b)
1 2 3 1 2 3 1 2 3
20-23 I can investigate reactions which produce datathat can be
used to calculate the rate of the
reaction, its half-life from concentration orvolume against time
graphs, eg a clock reaction(4.3c)
1 2 3 1 2 3 1 2 3
20-23 I can present and interpret the results of
kineticmeasurements in graphical form, includingconcentration-time
and rate-concentrationgraphs (4.3d)
1 2 3 1 2 3 1 2 3
32-33 I can investigate the reaction of iodine withpropanone in
acid to obtain data for the orderwith respect to the reactants and
the hydrogenion and make predictions about molecules/ionsinvolved
in the rate-determining step andpossible mechanism (details of the
actualmechanism can be discussed at a later stage inthis topic)
(4.3e)
1 2 3 1 2 3 1 2 3
16-1920-2328-2930-31
I can deduce from experimental data forreactions with zero,
first and second orderkinetics:i) half-life (the relationship
between half-life andrate constant will be given if required)ii)
order of reactioniii) rate equationiv) rate-determining step
related to reactionmechanismsv) activation energy (by graphical
methods only;
the Arrhenius equation will be given if needed)(4.3f)
1 2 3 1 2 3 1 2 3
28-29 I can investigate the activation energy of areaction, eg
oxidation of iodide ions by iodate(V)(4.3g)
1 2 3 1 2 3 1 2 3
30-31 I can apply a knowledge of the rate equations forthe
hydrolysis of halogenoalkanes to deduce themechanisms for primary
and tertiaryhalogenoalkane hydrolysis and to deduce themechanism
for the reaction between propanoneand iodine (4.3h)
1 2 3 1 2 3 1 2 3
30-31 I can demonstrate that mechanisms proposed forthe
hydrolysis of halogenoalkanes are consistent
with the experimentally determined orders ofreactions, and that
a proposed mechanism for
1 2 3 1 2 3 1 2 3
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the reaction between propanone and iodine isconsistent with the
data from the experiment in4.3e (4.3i)
30-31 I can use kinetic data as evidence for SN1 or
SN2mechanisms in the nucleophiclic substitutionreactions of
halogenoalkanes (4.3j)
1 2 3 1 2 3 1 2 3
pages Chapter 1.2 How far? Entropy At thestart
I havestudied..
I haverevised
40-41 I can demonstrate an understanding that, sinceendothermic
reactions can occur spontaneouslyat room temperature, enthalpy
changes alone donot control whether reactions occur (4.4a)
1 2 3 1 2 3 1 2 3
34-37 I can demonstrate an understanding of entropy interms of
the random dispersal of molecules andof energy quanta between
molecules (4.4b)
1 2 3 1 2 3 1 2 3
34-37 I can demonstrate an understanding that the
entropy of a substance increases withtemperature, that entropy
increases as solid liquid gas and that perfect crystals at
zerokelvin have zero entropy (4.4c)
1 2 3 1 2 3 1 2 3
34-37 I can demonstrate an understanding that thestandard
entropy of a substance depends mainlyon its physical state but also
on its complexity(4.4d)
1 2 3 1 2 3 1 2 3
38-39 I can demonstrate an understanding thatreactions occur due
to chance collisions, and thatone possible ordered arrangement, eg
in acrystalline solid, can be rearranged into manypossible
disordered arrangements, eg in a
solution so that the probability of disorder isgreater than
order (4.4e)
1 2 3 1 2 3 1 2 3
38-39 I can interpret the natural direction of change asbeing in
the direction of increasing total entropy(positive entropy change),
eg gases spreadspontaneously through a room (4.4f)
1 2 3 1 2 3 1 2 3
40-41 I can carry out experiments and relate the resultsto
disorder and enthalpy changes including:i) dissolving a solid, eg
adding ammonium nitratecrystals to waterii) gas evolution, eg
reacting ethanoic acid withammonium carbonateiii) exothermic
reaction producing a solid, eg
burning magnesium ribbon in airiv) endothermic reaction of two
solids, eg mixingsolid barium hydroxide, Ba(OH)2.8H2O with
solidammonium chloride (4.4g)
1 2 3 1 2 3 1 2 3
42-43 I can demonstrate an understanding that theentropy change
in any reaction is made up of theentropy change in the system added
to theentropy change in the surroundings, summarisedby the
expression:
Stotal = Ssystem + Ssurroundings (4.4h)
1 2 3 1 2 3 1 2 3
42-43 I can calculate the entropy change in the system
for a reaction, Ssystem, given entropy data (4.4i)
1 2 3 1 2 3 1 2 3
42-43 I can use the expression Ssurroundings = -H/Ttocalculate
the entropy change in the surroundings
1 2 3 1 2 3 1 2 3
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and hence Stotal (4.4j)
44-47 I can demonstrate an understanding that thefeasibility of
a reaction depends on the balancebetween Ssystem and Ssurroundings,
and that athigher temperatures the magnitude of
Ssurroundingsdecreases and its contribution to Stotal is less.
Reactions can occur as long as Stotal is positiveeven if one of
the other entropy changes isnegative (4.4k)
1 2 3 1 2 3 1 2 3
44-47 I can demonstrate an understanding of anddistinguish
between the concepts ofthermodynamic stability and kinetic
inertness(4.4l)
1 2 3 1 2 3 1 2 3
44-47 I can calculate Ssystem and Ssurroundings for thereactions
in 4.4g to show that endothermicreactions can occur spontaneously
at roomtemperature (4.4m)
1 2 3 1 2 3 1 2 3
48-49 I can define the term enthalpy of hydration of anion and
use it and lattice energy to calculate theenthalpy of solution of
an ionic compound (4.4n)
1 2 3 1 2 3 1 2 3
48-49 I can demonstrate an understanding of thefactors that
affect the values of enthalpy ofhydration and the lattice energy of
an ioniccompound (4.4o)
1 2 3 1 2 3 1 2 3
48-49 I can use entropy and enthalpy of solution valuesto
predict the solubility of ionic compounds(4.4p)
1 2 3 1 2 3 1 2 3
pages Chapter 1.3 Equilibria At the
start
I have
studied..
I have
revised50-54 I can demonstrate an understanding of the term
dynamic equilibrium as applied to states ofmatter, solutions and
chemical reactions (4.5a)
1 2 3 1 2 3 1 2 3
50-54 I can recall that many important industrialreactions are
reversible (4.5b)
1 2 3 1 2 3 1 2 3
50-54 I can use practical data to establish the idea thata
relationship exists between the equilibriumconcentrations of
reactants and products whichproduces the equilibrium constant for a
particularreaction, eg data on the hydrogen-iodineequilibrium
(4.5c)
1 2 3 1 2 3 1 2 3
60-61 I can calculate a value for the equilibriumconstant for a
reaction based on data fromexperiment, eg the reaction of ethanol
andethanoic acid (this can be used as an example ofthe use of ICT
to present and analyse data), theequilibrium Fe2+(aq) + Ag+ (aq)
Fe3+(aq) +Ag(s) or the distribution of ammonia or iodinebetween two
immiscible solvents (4.5d)
1 2 3 1 2 3 1 2 3
50-5455-57
I can construct expressions for Kcand Kp forhomogeneous and
heterogeneous systems, interms of equilibrium concentrations
orequilibrium partial pressures, perform simplecalculations on
Kcand Kp and work out the units
of the equilibrium constants (4.5e)
1 2 3 1 2 3 1 2 3
62-63 I can demonstrate an understanding that when 1 2 3 1 2 3 1
2 3
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Stotalincreases the magnitude of the equilibrium
constant increases since S = RlnK(4.5f)
58-59 I can apply knowledge of the value of equilibriumconstants
to predict the extent to which areaction takes place (4.5g)
1 2 3 1 2 3 1 2 3
62-63
I can relate the effect of a change in temperatureon the value
ofStotal.(4.5h) 1 2 3 1 2 3 1 2 3
pages Chapter 1.4 Application of rates andequilibrium
At thestart
I havestudied..
I haverevised
64-67 I can demonstrate an understanding of how, if atall, and
why a change in temperature, pressureor the presence of a catalyst
affects theequilibrium constant and the equilibriumcomposition and
recall the effects of changes oftemperature and pressure on rate,
eg thethermal decomposition of ammonium chloride, orthe effect of
temperature and pressure changesin the system 2NO2 N2O4 (4.6a)
1 2 3 1 2 3 1 2 3
68-69 I can use information on enthalpy change andentropy to
justify the conditions used to obtaineconomic yields in industrial
processes, andunderstand that in reality industrial processescannot
be in equilibrium since the products areremoved, eg in the Haber
process temperatureaffects the equilibrium yield and rate
whereaspressure affects only the equilibrium yield(knowledge of
industrial conditions are not
required) (4.6b)
1 2 3 1 2 3 1 2 3
70-71 I can demonstrate an understanding of the stepstaken in
industry to maximise the atom economyof the process, eg recycling
unreacted reagentsor using an alternative reaction (4.6c)
1 2 3 1 2 3 1 2 3
70-71 I can demonstrate an understanding of theimportance of
being able to control reactions,through knowledge of equilibrium
constants andentropy changes, the importance of
controllingreactions to produce adequate yields under
safe,economically viable conditions and why somereactions go and
some will never occur (4.6d)
1 2 3 1 2 3 1 2 3
pages Chapter 1.5 Acid/base equilibria At thestart
I havestudied..
I haverevised
72-75 I can demonstrate an understanding that thetheory about
acidity developed in the 19th and20th centuries from a substance
with a sour tasteto a substance which produces an excess ofhydrogen
ions in solution (Arrhenius theory) tothe Brnsted-Lowry theory
(4.7a)
1 2 3 1 2 3 1 2 3
72-75 I can demonstrate an understanding that aBrnstedLowry acid
is a proton donor and abase a proton acceptor and that
acid-base
equilibria involve transfer of protons (4.7b)
1 2 3 1 2 3 1 2 3
72-75 I can demonstrate understanding of theBrnstedLowry theory
of acid-base behaviour,
1 2 3 1 2 3 1 2 3
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and use it to identify conjugate acid-base pairs(4.7c)
76-79 I can define the terms pH, Ka and Kw, pKa and pKw,and be
able to carry out calculations relating thepH of strong acids and
bases to theirconcentrations in mol dm-3(4.7d)
1 2 3 1 2 3 1 2 3
80-83 I can demonstrate an understanding that weakacids and
bases are only slightly dissociated inaqueous solution, and apply
the equilibrium lawto deduce the expressions for the
equilibriumconstants Ka and Kw(4.7e)
1 2 3 1 2 3 1 2 3
76-79 I can analyse the results obtained from thefollowing
experiments:I )measuring the pH of a variety of substances,eg
equimolar solutions of strong and weak acids,strong and weak bases
and saltsii) comparing the pH of a strong acid and a weakacid after
dilution 10, 100 and 1000 times (4.7f)
1 2 3 1 2 3 1 2 3
84-85 I can analyse and evaluate the results obtainedfrom
experiments to determine Ka for a weakacid by measuring the pH of a
solution containinga known mass of acid, and discuss theassumptions
made in this calculation (4.7g)
1 2 3 1 2 3 1 2 3
80-83 I can calculate the pH of a solution of a weak acidbased
on data for concentration and Ka, anddiscuss the assumptions made
in this calculation(4.7h)
1 2 3 1 2 3 1 2 3
86-87 I can measure the pH change during titrationsand draw
titration curves using differentcombinations of strong and weak
monobasicacids and bases (4.7i)
1 2 3 1 2 3 1 2 3
88-89 I can use data about indicators, together withtitration
curves, to select a suitable indicator andthe use of titrations in
analysis (4.7j)
1 2 3 1 2 3 1 2 3
92-95 I can explain the action of buffer solutions andcarry out
calculations on the pH of buffersolutions, eg making buffer
solutions andcomparing the effect of adding acid or alkali onthe pH
of the buffer (4.7k)
1 2 3 1 2 3 1 2 3
90-9192-95
I can use titration curves to show the bufferaction and to
determine Ka from the pH at thepoint where half the acid is
neutralised (4.7l)
1 2 3 1 2 3 1 2 3
96-97 I can explain the importance of buffer solutions
inbiological environments, eg buffers in cells and in
blood (H2CO3/HCO3) and in foods to preventdeterioration due to
pH change (caused bybacterial or fungal activity) (4.7m)
1 2 3 1 2 3 1 2 3
pages Chapter 1.6 Further organic chemistry At thestart
I havestudied..
I haverevised
1 Chirality
98-99 I can recall the meaning of structural and E-Zisomerism
(geometric/cis-trans isomerism)(4.8.1a)
1 2 3 1 2 3 1 2 3
98-99 I can demonstrate an understanding of the
existence of optical isomerism resulting fromchiral centre(s) in
a molecule with asymmetric
1 2 3 1 2 3 1 2 3
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carbon atom(s) and understand optical isomersas object and
non-superimposable mirror images(4.8.1b)
100-101 I can recall optical activity as the ability of asingle
optical isomer to rotate the plane ofpolarization of
plane-polarized monochromatic
light in molecules containing a single chiralcentre and
understand the nature of a racemicmixture (4.8.1c)
1 2 3 1 2 3 1 2 3
102-103 I can use data on optical activity of reactants
andproducts as evidence for proposed mechanisms,as in SN1 and SN2
and addition to carbonylcompounds (4.8.1d)
1 2 3 1 2 3 1 2 3
2 Carbonyl compounds
104-107 I can give examples of molecules that contain
thealdehyde or ketone functional group (4.8.2a)
1 2 3 1 2 3 1 2 3
104-107 I can explain the physical properties of aldehydes
and ketones relating this to the lack of hydrogenbonding between
molecules and their solubility inwater in terms of hydrogen bonding
with thewater (4.8.2b)
1 2 3 1 2 3 1 2 3
108-109110-113
I can describe and carry out, where appropriate,the reactions of
carbonyl compounds. This will belimited to:i) oxidation with
Fehlings or Benedicts solution,Tollens reagent and acidified
dichromate(VI) ionsii) reduction with lithium
tetrahydridoaluminate(lithium aluminium hydride) in dry etheriii)
nucleophilic addition of HCN in the presenceof KCN, using curly
arrows, relevant lone pairs,
dipoles and evidence of optical activity to showthe mechanismiv)
the reaction with 2.4-dinitrophenylhydrazineand its use to detect
the presence of a carbonylgroup and to identify a carbonyl compound
givendata of the melting temperatures of derivativesv) iodine in
the presence of alkali (4.8.2c)
1 2 3 1 2 3 1 2 3
3 Carboxylic acids
114-115 I can give some examples of molecules thatcontain the
carboxylic acid functional group(4.8.3a)
1 2 3 1 2 3 1 2 3
114-115 I can explain the physical properties of carboxylicacids
in relation to their boiling temperatures andsolubility due to
hydrogen bonding (4.8.3b)
1 2 3 1 2 3 1 2 3
114-115 I can describe the preparation of carboxylic acidsto
include oxidation of alcohols and carbonylcompounds and the
hydrolysis of nitriles(4.8.3c)
1 2 3 1 2 3 1 2 3
116-118119-121
I can describe and carry out, where appropriate,the reactions of
carboxylic acids. This will belimited to:i) reduction with lithium
tetrahydridoaluminate(lithium aluminium hydride) in dry
ether(ethoxyethane)
ii) neutralization to produce salts, eg todetermine the amount
of citric acid in fruit
1 2 3 1 2 3 1 2 3
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iii) phosphorus(V) chloride (phosphoruspentachloride)iv)
reactions with alcohols in the presence of anacid catalyst, eg the
preparation of ethylethanoate as a solvent or as pineapple
flavouring(4.8.3d)
4 Carboxylic acid derivatives
122-124127-129
I can demonstrate an understanding that theseinclude acyl
chlorides and esters and recognisetheir respective functional
groups, givingexamples of molecules containing thesefunctional
groups (4.8.4a)
1 2 3 1 2 3 1 2 3
127-129 I can describe and carry out, where appropriate,the
reactions of acyl chlorides limited to theirreaction with:i)
waterii) alcoholsiii) concentrated ammoniaiv) amines (4.8.4b)
1 2 3 1 2 3 1 2 3
122-124 I can describe and carry out, where appropriate,the
reactions of esters. This will be limited to:i) their hydrolysis
with an acidii) their hydrolysis with a base, eg to form soapsiii)
their reaction with alcohols and acids toexplain the process of
trans-esterification andrecall how it is applied to the manufacture
of bio-diesel (as a potentially greener fuel) and low-fatspreads
(replacing the hydrogenation ofvegetable oils to produce margarine)
(4.8.4c)
1 2 3 1 2 3 1 2 3
125-126 I can demonstrate an understanding of the
importance of the formation of polyesters anddescribe their
formation by condensationpolymerization of ethane-1,2-diol and
benzene-1,4-dicarboxylic acid (4.8.4d)
1 2 3 1 2 3 1 2 3
Pages Chapter 1.7 Spectroscopy andchromatography
At thestart
I havestudied..
I haverevised
130-132 I can explain the effect of different types ofradiation
on molecules and how the principles ofthis are used in chemical
analysis and inreactions, limited to:
i) infrared in analysisii) microwaves for heatingiii) radio
waves in nmriv) ultraviolet in initiation of reactions (4.9a)
1 2 3 1 2 3 1 2 3
133-136 I can explain the use of high resolution nmrspectra to
identify the structure of a molecule:i) based on the different
types of proton presentfrom chemical shift valuesii) by using the
spin-spin coupling pattern toidentify the number of protons
adjacent to agiven protoniii) the effect of radio waves on proton
spin innmr, limited to 1H nucleiiv) the use of magnetic resonance
imaging as anon-invasive technique, eg scanning for brain
1 2 3 1 2 3 1 2 3
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disorders, or the use of nmr to check the purityof a compound in
the pharmaceutical industry(4.9b)
130-132 I can demonstrate an understanding of the use ofIR
spectra to follow the progress of a reactioninvolving change of
functional groups, eg in the
chemical industry to determine the extent of thereaction
(4.9c)
1 2 3 1 2 3 1 2 3
137-139 I can interpret simple mass spectra to suggestpossible
structures of a simple compound fromthe m/e of the molecular ion
and fragmentationpatterns (4.9d)
1 2 3 1 2 3 1 2 3
140-143 I can describe the principles of gaschromatography and
HPLC as used as methodsof separation of mixtures, prior to
furtheranalysis (theory of Rfvalues not required), andalso to
determine if substances are present inindustrial chemical processes
(4.9e)
1 2 3 1 2 3 1 2 3
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Pearson Education Ltd 2009 Edexcel A2 Chemistry ActiveBook
