2016 Unit 3 4 Chemistry No Activities

8/19/2019 2016 Unit 3 4 Chemistry No Activities

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2016 Year 12 ChemistryTeaching and Learning Program

UNIT 3 – EQUILI!IU"# $CI% $&E& ' !E%() !E$CTI(N&Learning (*tcomes+By the end of this unit, students:

• understand the characteristics of equilibrium systems, and explain and predict how they are aected by changes to temperature,

concentration and pressure

• understand the dierence between the strength and concentration of acids, and relate this to the principles of chemical equilibrium

• understand how redox reactions, galvanic and electrolytic cells are modelled in terms of electron transfer

• understand how models and theories have developed over time and the ways in which chemical knowledge interacts with social and

economic considerations in a range of contexts

• use science inquiry skills to design, conduct, evaluate and communicate investigations into the properties of acids and bases, redox

reactions and electrochemical cells, including volumetric analysis

• evaluate, with reference to empirical evidence, claims about equilibrium systems and justify evaluations

•

communicate, predict and explain chemical phenomena using qualitative and quantitative representations in appropriate modes andgenres.

UNIT , – (!-$NIC C.E"I&T!Y $N% C.E"IC$L &YNT.E&I&Learning (*tcomes+By the end of this unit, students:

• understand how the presence of functional groups and the molecular structure of organic compounds are related to their properties

• understand addition, condensation and oxidation reactions, and predict the products of these reactions

• understand how knowledge of chemical systems is used to design synthesis processes

• understand how models and theories have developed over time, and the ways in which chemical knowledge interacts with social and

economic considerations in a range of contexts

• use science inquiry skills to design, conduct, evaluate and communicate investigations into reactions to identify organic compounds,

including analysis of secondary data derived from chemical analysis

• evaluate, with reference to empirical evidence, claims about organic synthesis and chemical design, and justify evaluations

• communicate, predict and explain chemical phenomena using qualitative and quantitative representations in appropriate modes and

genres.


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&cience In/*iry &is &I&+ &cience as a .*man Endea4o*r &.E+-enera ca5aiities and

Cross7c*rric*ar 5riorities+Q*estioning and 5redicting

• identify, research, construct and re!ne

questions for investigation" propose

hypotheses" and predict possible outcomes

Panning and cond*cting

• design investigations, including the

procedure#s$ to be followed, the materials

required, and the type and amount of

primary and%or secondary data to becollected" conduct risk assessments" and

consider research ethics

• conduct investigations safely, competently

and methodically for the collection of valid

and reliable data, including properties of

organic compounds containing dierent

functional groups and using chemical

synthesis processes

Processing and anaysing data andin8ormation

• represent data in meaningful and useful

ways, including using appropriate graphic

representations and correct units and

symbols" organise and analyse data to

identify patterns and relationships" identify

and distinguish between random and

systematic errors, and estimate their eect

Chemica e/*iiri*m systems

&evels of carbon dioxide in the atmosphere are

rising and have a signi!cant impact on global

systems, including surface temperatures. 'he

increasing level of carbon dioxide in the

atmosphere causes more carbon dioxide to

dissolve in the ocean producing carbonic acid

and leading to increased ocean acidity. 'his is

predicted to have a range of negative

consequences for marine ecosystems such ascoral reefs. (alci!cation is the process which

results in the formation of calcium carbonate

structures in marine organisms. )cidi!cation

shifts the equilibrium of carbonate chemistry in

seawater, decreasing the rate and amount of

calci!cation among a wide range of marine

organisms. 'he *nited +ations yoto -rotocol

and the ntergovernmental -anel on (limate

(hange aim to secure a global commitment to

reducing greenhouse gas emissions over thenext few decades.

(9idation and red*ction

/pontaneous redox reactions can be used as a

source of electrical energy, including primary,

secondary and fuel cells. 0uel cells are a

potential lower1emission alternative to the

internal combustion engine and are already

-enera ca5aiities+

&iteracy

+umeracy

(' capability

(ritical and creative thinking

-ersonal and social capability

2thical behaviour

ntercultural understanding

Cross7c*rric*ar 5riorities+

• )boriginal and 'orres /traitslander histories and cultures

• /ustainability

For a full description of the above:

htt5+::;ace1


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on measured results" discuss how the

nature of the procedure and the sample

si4e may in5uence uncertainty and

limitations in data" and select, synthesise

and use evidence from a range of sourcesto make and justify conclusions

E4a*ating

• interpret a range of scienti!c and media

texts, and evaluate processes, claims and

conclusions by considering the quality of

available evidence" and use reasoning to

construct scienti!c arguments

Comm*nicating• communicate to speci!c audiences and for

speci!c purposes using appropriate

language, nomenclature, genres and

modes, including scienti!c reports

being used to power various modes of

transport. 6rganisations, including the

nternational -artnership for 7ydrogen and 0uel

(ells in the 2conomy, have been created to

foster global cooperation on research anddevelopment, common codes and standards,

and information sharing on infrastructure

development.

Pro5erties and str*ct*re o8 organic

materias

'he -rotein 8ata Bank #-8B$ houses an

international repository of structural data of

proteins. 'he information is accessed and

contributed to by scientists worldwide. 'he

function of a protein is closely linked to its

structure.

Chemica synthesis

/cienti!c knowledge can be used to design

alternative chemical synthesis pathways,

taking into account sustainability, local

resources, economics and environmental

impacts #green chemistry$, including the

production of ethanol and biodiesel.

!eso*rces+ 'ext:

2xploring (hemistry 9r 3 1aree Baddock, Bernadine7unneybun, Brenda ;inning. #3' -*B&/72>$

2xploring (hemistry /tage 31 (larke et al. #3


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2xploring (hemistry /tage @1 (larke et al. #3


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changes and chemical reactions and

may be open #which allow matter and

energy to be exchanged with the

surroundings$ or closed #which allow

energy, but not matter, to beexchanged with the surroundings$

diagrams for exothermic andendothermic processes showing thetransition state, activation energy andheat of reaction.

• /tate that the characteristics of

chemical equilibrium in a closedsystem at constant temperature are:

o a constancy of macroscopic properties,in particular that the concentrationsof all species are constant

o a dynamic condition in which the ratesof the forward and reverse reactionsare equal.

• dentify from a qualitative descriptionwhether a particular chemical systemis at equilibrium.

&.E

&evels of carbon dioxide in the atmosphere are rising and have a signi!cant impact onglobal systems, including surface temperatures. 'he increasing level of carbon dioxide inthe atmosphere causes more carbon dioxide to dissolve in the ocean producing carbonicacid and leading to increased ocean acidity. 'his is predicted to have a range of negativeconsequences for marine ecosystems such as coral reefs. (alci!cation is the processwhich results in the formation of calcium carbonate structures in marine organisms.)cidi!cation shifts the equilibrium of carbonate chemistry in seawater, decreasing the rateand amount of calci!cation among a wide range of marine organisms. 'he *nited +ationsyoto -rotocol and the ntergovernmental -anel on (limate (hange aim to secure a globalcommitment to reducing greenhouse gas emissions over the next few decades.

27, EQUILI!IU"

• observable changes in chemical

reactions and physical changes can be

described and explained at an atomic

• ;rite the equilibrium law expressionfor a reaction at equilibrium. +ocalculations are required.

• 2xplain that the equilibrium

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and molecular level

• over time, in a closed system, reversible

physical and chemical changes may

reach a state of dynamic equilibrium,

with the relative concentrations ofproducts and reactants de!ning the

position of equilibrium

• the characteristics of a system in

dynamic equilibrium can be described

and explained in terms of reaction rates

and macroscopic properties

• the reversibility of chemical reactions

can be explained in terms of the

activation energies of the forward andreverse reactions

• the eect of changes of temperature on

chemical systems initially at equilibrium

can be predicted by considering the

enthalpy changes for the forward and

reverse reactions" this can be

represented on energy pro!le diagrams

and explained by the changes in the

rates of the forward and reverse

reactions

• the eects of changes in concentration

of solutions and partial pressures of

gases on chemical systems initially at

equilibrium can be predicted and

explained by applying collision theory to

the forward and reverse reactions

• the eects of changes in temperature,

constant #$ for a chemical reactiono indicates the relative proportions of

products to reactants at equilibrium,o is a constant for that reaction at a

given temperature

o provides no information about therate of a particular reaction.

• -redict the eect on the relativeproportions of products to reactantsat equilibrium of the followingchanges:

o 'emperatureo concentration #or partial

pressure of a gas in themixture$

o volume #or partial pressureof all gases in the mixture$.

• /tate and apply that changes in themass of a solid, the volume of aliquid and the presence of a catalysthave no eect on the relativeproportions of products to reactantsat equilibrium.

• 2xplain how industrial processes suchas the 7aber process and (ontactprocess often involve a compromiseof rate, equilibrium yield andeconomic considerations.

F


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concentration of species in solution,

partial pressures of gases, total volume

and the addition of a catalyst on

equilibrium systems can be predicted

using &e (hGtelierHs -rinciple• equilibrium law expressions can be

written for homogeneous and

heterogeneous systems" the equilibrium

constant #$, at any given temperature,

indicates the relationship between

product and reactant concentrations at

equilibrium

• the relative amounts of reactants and

products #equilibrium position$ can be

predicted qualitatively using equilibrium

constants # c $

•

&.E

odels and theories are contested and re!ned or replaced when new evidence challengesthem, or when a new model or theory has greater explanatory scope. 8avy initiallyproposed that acids were substances that contained replaceable hydrogen #hydrogen thatcould be partly or totally replaced by metals$ and bases were substances that reacted withacids to form salts and water. 'he )rrhenius model, which includes only soluble acids andbases, identi!ed acids as substances which produce hydrogen ions in solution and bases

as substances which produce hydroxide ions in solution. /ubsequently, the BrInsted1&owrymodel describes acid1base behaviour in terms of proton donors and proton acceptors. 'hisapproach includes a wider range of substances and can be more broadly applied.


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of protons available for donation

• the strength of acids is explained by

the degree of ionisation at equilibrium

in aqueous solution which can be

represented by chemical equations

and acidity constants # a$

• the relationship between acids and

bases in equilibrium systems can be

explained using the BrInsted1&owry

model and represented using chemical

equations that illustrate the transfer of

protons between conjugate acid1base

pairs

• the hydrolysis of salts of weak acids

and weak bases can be represented

using equations" theBrInsted1&owry model can be applied

to explain the acidic, basic and neutral

nature of salts derived from bases and

monoprotic and polyprotic acids

• buer solutions are conjugate in

nature and resist changes in p7 when

small amounts of strong acid or base

are added to the solution" buering

capacity can be explained

qualitatively" &e (hGtelierHs -rinciplecan be applied to predict how buers

respond to the addition of hydrogen

ions and hydroxide ions

• water is a weak electrolyte" the self1

ionisation of water is represented by

w K L7CML671M where w K .< x


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concentration of hydrogen ions or

hydroxide ions in solutions of strong

acids or bases

• the p7 scale is a logarithmic scale and

the p7 of a solution can be calculated

from the concentration of hydrogen

ions using the relationship p7 K 1 log


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an accurately known concentration.• 8escribe how to prepare a standard

solution by:o dissolving a known mass of a

primary standard

in a known volume of solution #e.g.anhydrous sodium carbonate$o standardisation of the solution

#e.g. sodium hydroxide$ bytitration against a standard

solution e.g. hydrochloricacid$.

• 8escribe an indicator as a substancewhich exhibits two p71dependentcolour forms with particular referenceto methyl orange andphenolphthalein.

• 8istinguish between the equivalencepoint and the end point in a titration.

• 2xplain the use of phenolphthaleinindicator in titrations between astrong base and a weak acid andmethyl orange indicator in titrationsbetween a strong acid and a weakbase.

• /tate that either phenolphthalein ormethyl orange could be used as theindicator in titrations between strongacids and strong bases.

• 8escribe how to use a pipette, buretteand volumetric 5ask in volumetricanalysis.

• 8escribe the procedures used involumetric analysis

T2@ 17,

()I%$TI(N $N% !E%UCTI(N 3

• oxidation1reduction #redox$ reactions

involve the transfer of one or more

electrons from one species to another

• dentify the term OredoxH as one whichemphasises the interdependence of

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• oxidation involves the loss of electrons

from a chemical species, and

reduction involves the gain of

electrons by a chemical species" these

processes can be represented using

half1equations and redox equations

#acidic conditions only$

• a range of reactions involve the

oxidation of one species and reduction

of another species, including metal

and halogen displacement reactions,

combustion and corrosion

• the species being oxidised and

reduced in a redox reaction can be

identi!ed using oxidation numbers

• the relative strength of oxidising and

reducing agents can be determined by

comparing standard electrode

potentials, and can be used to predict

reaction tendency

• electrochemical cells, including

galvanic and electrolytic cells, consist

of oxidation and reduction half1

reactions connected via an external

circuit through which electrons move

from the anode #oxidation reaction$ tothe cathode #reduction reaction$

• galvanic cells produce an electric

current from a spontaneous redox

reaction

• the electric potential dierence of a

cell under standard conditions can be

calculated from standard electrode

potentials" these values can be used

oxidation and reduction processes.• )pply the terms Ooxidising agents

#oxidants$H and Oreducing agents#reductants$H in terms of a substancePstendency to accept or donate electrons.

• 8escribe oxidation and reduction in termsof electron donation and acceptance usingsimple displacement reactions betweenmetals and halogen displacementreactions, combustion and corrosion.

• dentify common oxidising agents

#oxidants$ including 63, (l3, n6EN,

(r36J3N

, (l6N, 7

C, conc. sulfuric acid,

conc. nitric acid and common reducingagents #reductants$ including Qn, (, 73,

0e3C, (36E3N.• 8e!ne and assign oxidation numbers

#oxidation states$.• dentify the species oxidised and reduced

from given chemical equations.• Balance oxidation1reduction equations and

half1equations using one of the followingmethods:o the oxidation number methodo the ion1electron method.

• *se appropriate half1equations to

illustrate that hydrogen peroxide canundergo both oxidation and reduction.

• dentify disproportionation reactions suchas the decomposition of hydrogenperoxide

• 8escribe the use of hypochlorite ion inbleaching and in water treatment.

Eectrochemica ces


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to compare the voltages generated by

cells constructed from dierent

materials

• electrochemical cells can be described

in terms of the reactions occurring at

the anode and cathode, the role of the

electrolyte, salt bridge #galvanic cell$,

ion migration, and electron 5ow in the

external circuit

• cell diagrams can be used to

represent electrochemical cells&.E

/pontaneous redox reactions can be usedas a source of electrical energy, includingprimary, secondary and fuel cells. 0uel

cells are a potential lower1emissionalternative to the internal combustionengine and are already being used topower various modes of transport.6rganisations, including the nternational-artnership for 7ydrogen and 0uel (ells inthe 2conomy, have been created to fosterglobal cooperation on research anddevelopment, common codes andstandards, and information sharing oninfrastructure development.• electrolytic cells use an external

electrical potential dierence toprovide the energy to allow a non1

spontaneous redox reaction to occur"

electrolytic cells are used in a range

of industrial situations, including

metal plating and the puri!cation of

copper

• 8escribe an electrochemical cell as asystem for transforming the chemicalpotential energy of an oxidation1reduction reaction to electrical energy.

• 8e!ne the OanodeH as the electrode at

which oxidation occurs and theOcathodeH as the electrode at whichreduction occurs.

• 8escribe the components and operationof an electrochemical cell with regardto:

o anode processeso cathode processeso electrolyteo salt bridge and ion migrationo electron 5ow in the external circuit.

• 8e!ne Oelectromotive force #20$H of acell.

• 8escribe and explain how anelectrochemical cell can be consideredas two half1cells.

• 8e!ne standard reduction potentials forhalf1cells.

• 2xplain the use of the hydrogen half1cellas the standard for determining half1cell reduction potentials.

• /tate that standard reduction potential#2R$ values are measured at solution

concentrations of

o mol &N

at 3?A and gas pressure of


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standard reduction potential #2R$tables.

• 8escribe the construction and operationof the following electrochemical cells:

o the dry cell

o the lead1acid accumulatoro the fuel cell e.g. hydrogen%oxygen fuel

cell.• 8escribe the conditions and reactions

for the corrosion of iron.• ;rite the chemical equations and half1

equations for the corrosion of iron andthe formation of rust.

• 8escribe methods for the prevention ofcorrosion of iron using:

o cathodic protectiono sacri!cial anodes e.g. use of magnesium

or 4inco exclusion of air e.g. painting and

plating.

Eectroysis

• 8escribe electrolysis as a process inwhich electrical energy is used toproduce chemical change.

• 8escribe an electrolytic cell as a systemfor transforming electrical energy to

chemical potential energy.• 8escribe the components and operation

of an electrolytic cell with regard to:o anode processeso cathode processeso electrolyte #aqueous or molten$o ion migrationo electron 5ow in the external circuit.

• 2xplain how electrolysisreactions provide evidence for

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the )tomic 'heory.• -redict the products of simple

electrolysis reactions using, thetable of

• 8escribe the use of electrolysis

in electrolytic re!ning e.g.copper, and electroplating e.g.silver.

E9traction o8 metas

• 8escribe the extraction of metals, using,as examples, the production of:

o iron by carbon reductionoaluminium by electrolytic reductionogold by carbon in pulp

• >elate the method of extraction to theease of reduction of the metalconcerned.

!edo9 titrations

• /tate the characteristics of a primarystandard.

• 8e!ne a Ostandard solutionH as one withan accurately known concentration.

• 8escribe how to prepare a standardsolution by:

o dissolving a known mass of a primarystandard in a known volume of solution

#e.g. ammoniumiron#$sulfatehexahydrate, oxalic aciddihydrate or an oxalate$

• standardisation of the solution bytitration against a standard solution.

• 2xplain why an indicator is not requiredin potassium permanganate titrations.

E


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• 8escribe the use of a pipette, buretteand volumetric 5ask in volumetricanalysis.

• 8escribe the procedures used involumetric analysis with particular

reference to the following redoxtitrations:

o standardisation of potassiumpermanganate solution usingammonium iron#$ sulfate hexahydrateor oxalic acid dihydrate

o analysis of hydrogen peroxide solutionusing standard potassiumpermanganate solution.

< '6

E)$" !EAI&I(N : E)$"&

B710 (!-$NIC C.E"I&T!Y ,• organic molecules have a hydrocarbon

skeleton and can contain functional

groups, including alkenes, alcohols,

aldehydes, ketones, carboxylic acids,

esters, amines and amides" functional

groups are groups of atoms or bonds

within molecules which are responsible

for the moleculeHs characteristic

chemical properties

• structural formulae #condensed or

showing bonds$ can be used to show

the arrangement of atoms and

bonding in organic molecules that

contain the following functional

groups: alkenes, alcohols, aldehydes,

ketones, carboxylic acids, esters,

amines and amides

• >elate the large number of known carboncompounds to the unlimited number ofstable chains, branched chains andrings which can be formed due to:

• strong covalent bonding between carbonatoms and between carbon andhydrogen atoms.

• the high valency #E$ of carbon, whichallows chains to branch and to bebonded to a variety of substituents.

• 8istinguish between alkane and alkenesaccording to the type of carbon1carbonbonding.

• 8escribe the structure of ben4ene andrelate the stability of its structure to thepresence of delocalised electrons.

Nomencat*re and 8orm*ae

• ;rite the *-)( names and structural

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• functional groups within organic

compounds display characteristic

chemical properties and undergo

speci!c reactions" these reactions

include addition reactions of alkenes,redox reactions of alcohols, and acid1

base reactions of carboxylic acids"

these reactions can be used to identify

the functional group present within the

organic compound

• *-)( nomenclature is used to name

organic species, including those with a

parent chain of up to A carbon atoms

with simple branching and one of the

following functional groups: alkenes,

alcohols, aldehydes, ketones,

carboxylic acids, esters, amines and

amides

• isomers are compounds with the same

molecular formulae but dierent

structures" dierent types of

isomerism include chain and position

structural isomerism and cis1trans

isomerism

• all alcohols can undergo complete

combustion" with oxidising agents,including acidi!ed n6E1 or (r36J31

oxidation of primary alcohols produces

aldehydes and carboxylic acids, while

the oxidation of secondary alcohols

produce ketones" these reactions have

characteristic observations and can be

represented with equations

formulae of:o straight and branched chain alkanes #(

to (A$

o simple cycloalkanes #(@ to (F$

o straight and branched chain alkenes #(3

to (A$

o simple cycloalkenes #(@ to (F$

o straight and branched chain alkynes #(3

to (A$

o straight chain alkyl groups #( to (A$

o halogen substituted alkanes #( to (A$

o simple examples of: alcohols, aldehydes,ketones, carboxylic acids, esters andprimary amines.

SNote+ t is not expected that students will be

able to name dienes, diynes, trienes,triynes etc.• 8escribe and identify simple aromatic

compounds as substances containing aben4ene ring.

• dentify and write structural formulae ofstructural isomers having:

• dierent carbon con!gurations#branched chains and cycliccompounds$

• the same carbon chain with the samefunctional group in dierent positions

#e.g. the propanols$• the same carbon chain with dierent

functional groups #e.g. propanal andpropanone$.

• dentify and write structural formulae forcis%trans geometric isomers.

• 2xplain and apply the terms OempiricalformulaH, Omolecular formulaH andOstructural formulaH.

F


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• alcohols can react with carboxylic

acids in a condensation reaction to

produce esters and can be

represented with equations

•

• -erform calculations to determine theempirical formula of an unknownsubstance given one of the following:

o its elemental composition by masso its elemental percentage composition

o information concerning the quantities ofproducts #e.g. masses and gasvolumes$ obtained from its combustionor other speci!ed reactions.

• 8etermine the molar mass of asubstance from the volume of a knownmass of its vapour.

• 8etermine the formula of a substancefrom its molecular weight and itsempirical formula.

• 8raw possible structural formulae of anunknown organic compound given its

molecular formula.

?*nctiona gro*5s

• 8escribe the importance of thefunctional groups present in an organiccompound in determining its chemicalbehaviour.

• ;rite the structures for, and identifyfunctional groups in the followingcompounds: alkenes, alkynes, alcohols,

aldehydes, ketones, carboxylic acids,esters, haloalkanes and primaryamines.

• 8istinguish between the structure ofprimary, secondary and tertiaryalcohols as exempli!ed by alcohols withthe formula (E7?67.

• 8escribe, by stating observations andwriting equations, the reactions ofalcohols, in particular ethanol, with the

J


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following substances:osodiumoacidi!ed solutions of the oxidising agents

n6EN#aq$ and (r36J

3N#aq$

ocarboxylic acids.

• 8ierentiate between the reactions ofprimary, secondary and tertiaryalcohols.

• dentify and write equations for thesubstitution reactions of alkanes withhalogens.

• dentify and write equations for theaddition reactions of alkenes andalkynes with hydrogen and halogens.

• ;rite chemical equations to illustrate thefollowing reactions:

o the formation of aldehydes by theoxidation of primary alcohols

o the formation of ketones by the oxidationof secondary alcohols

o the formation of carboxylic acids by theoxidation of primary alcohols oraldehydes

o the formation of esters by the reaction ofcarboxylic acids with alcohols

T3

@ 173

• organic compounds display

characteristic physical properties,including boiling point and solubility in

water and organic solvents" these

properties can be explained in terms

of intermolecular forces #dispersion

forces, dipole1dipole interactions and

hydrogen bonds$ which are in5uenced

by the nature of the functional groups

• empirical and molecular formulae can

• nn

•

T1amino acids can be represented usinga generalised structure

• the characteristic properties of 1amino

acids include the formation of 4witterions

and the ability to react to form amide

#peptide$ bonds through condensation

reactions

• 1amino acids undergo condensation

reactions to form polypeptides #proteins$

A


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be determined by calculation and the

structure of an organic compound

established from the chemical

reactions they undergo, and other

analytical data

• addition reactions can be used to

produce polymers, including

polyethene and polytetra5uoroethene

• the structure of an addition polymer

can be predicted from its monomer

and the structure of an addition

polymer can be used to predict the

monomer from which it was derived

• condensation reactions can be used to

produce polymers, including

polyamides and polyesters• the structure of a condensation

polymer can be predicted and drawn

from its monomer#s$ and the structure

of a condensation polymer can be

used to predict the monomer#s$ from

which it was derived

• T1amino acids can be represented

using a generalised structure

• the characteristic properties of 1

amino acids include the formation of4witterions and the ability to react to

form amide #peptide$ bonds through

condensation reactions

• 1amino acids undergo condensation

reactions to form polypeptides

#proteins$ in which the T1amino acid

monomers are joined by peptide

bonds

in which the T1amino acid monomers are

joined by peptide bonds

• the sequence of T1amino acids in a

protein is called its primary structure

• secondary structures of proteins, # 1

helix and 1pleated sheets$ result from

hydrogen bonding between amide and

carbonyl functional groups" hydrogen

bonding between amide and carbonyl

functional groups within a peptide chain

leads to 1helix structures while

hydrogen bonding between adjacent

polypeptide chains leads to 1pleated

sheets.

• 'he tertiary structure of a protein #the

overall three1dimensional shape$ is aresult of folding due to interactions

between the side chains of the 1amino

acid in the polypeptide, including

disul!de bridges, hydrogen bonding,

dipole1dipole interactions, dispersion

forces and ionic interactions

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20/23


&.E

'he -rotein 8ata Bank #-8B$ houses an

international repository of structural data

of proteins. 'he information is accessed

and contributed to by scientists

worldwide. 'he function of a protein is

closely linked to its structure.

• the sequence of T1amino acids in a

protein is called its primary structure

• secondary structures of proteins, # 1

helix and 1pleated sheets$ result

from hydrogen bonding between

amide and carbonyl functional groups"

hydrogen bonding between amide and

carbonyl functional groups within a

peptide chain leads to 1helix

structures while hydrogen bonding

between adjacent polypeptide chains

leads to 1pleated sheets

the tertiary structure of a protein #the

overall three1dimensional shape$ is a

result of folding due to interactions

between the side chains of the 1amino

acid in the polypeptide, including disul!de

bridges, hydrogen bonding, dipole1dipole

interactions, dispersion forces and ionic

interactions

,7B C.E"IC$L &YNT.E&I&• chemical synthesis to form products

with speci!c properties may require

the construction of reaction sequences

with more than one chemical reaction

and involves the selection of particular

• -erform multistage equation calculations.

3<


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reagents and reaction conditions in

order to optimise the rate and yield of

the product

• quantities of products in a chemical

synthesis reaction can be calculated

by comparing stoichiometric quantities

with actual quantities and by

determining the limiting reagent

• the percentage yield of a chemical

synthesis reaction can be calculated

by comparing theoretical versus actual

product quantities

• reagents and reaction conditions are

chosen to optimise yield and rate for

chemical synthesis processes,

including in the production ofammonia #7aber process$, sulfuric

acid #(ontact process$ and biodiesel

#base1catalysed and lipase1catalysed

methods$

&.E

/cienti!c knowledge can be used to

design alternative chemical synthesis

pathways, taking into account

sustainability, local resources, economics

and environmental impacts #greenchemistry$, including the production of

ethanol and biodiesel.

• en4ymes are protein molecules which

are biological catalysts and can be

used on an industrial scale to produce

chemicals that would otherwise

require high pressure or temperature

• -erform limiting reagent calculations.

• -erform percentage yield calculations.

• 2xplain the production of sulfuric acid,ammonia and biodiesel.

• 2xplain the importance and howcatalysts work in industrial processes.

3


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conditions to achieve an economically

viable rate, including fermentation to

produce ethanol versus hydrolysis of

ethene

• chemical synthesis processes may

involve the construction of reaction

sequences with more than one

chemical reaction, including the

hydrolysis of ethene to form ethanol

and the subsequent reaction of

ethanol with acetic #ethanoic$ acid to

produce ethyl ethanoate

industry produces a vast range of

plastics, including addition polymers

#polyethene, polytetra5uoroethene$

and condensation polymers #nylon andpolyethylene terephthalate L-2'M$

which have dierent properties and

uses

• 8e!ne the terms OmonomerH andOpolymerH.

• 8escribe the formation of poly#ethene$and poly#vinyl chloride$ #additionpolymers$ and polyesters#condensation polymers$ and writeequations for their formation.

B7 C.E"IC$L &YNT.E&I&• the base hydrolysis #saponi!cation$ of

fats #triglycerides$ produces glycerol

and the salt of a long chain fatty acid

#soap$

• the structure of soaps contains a non1

polar hydrocarbon chain and a

carboxylate group" the structure of the

anionic detergents derived from

•

8raw structural formulae to exemplifya simple soap and a sulfonate

detergent.

• 8escribe the action of soaps and

sulfonate detergents in terms of the

interaction of the polar and non1polar

parts of the molecule with water and

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dodecylben4ene contains a non1polar

hydrocarbon chain and a sulfonate

group

• the cleaning action of soaps and

detergents can be explained in terms

of their non1polar hydrocarbon chainand charged group" the properties of

soaps and detergents in hard water

can be explained in terms of the

solubilities of their calcium salts

greases, etc.

• 8escribe the preparation of a simple

soap and write a simple equation for

the reaction #ester hydrolysis$.• 8escribe with examples the use of

organic liquids as solvents, e.g. petrol,

kerosene, chloroform, acetone, esters,

mineral turpentine and methylated

spirits.

10 E)$" !EAI&I(N

3@

Documents

2016 Unit 3 4 Chemistry No Activities