Syllabus content
1. The particulate nature of matter
2. Experimental techniques
2.1 Measurement
2.2.1 Criteria of purity
2.2.2 Methods of purification
3. Atoms, elements and compounds
3.1 Atomic structure and the Periodic Table
3.2.1 Bonding: the structure of matter
3.2.2 Ions and ionic bonds
3.2.3 Molecules and covalent bonds
3.2.4 Macromolecules
3.2.5 Metallic bonding (Extended candidates
only)
4. Stoichiometry
4.1 Stoichiometry
4.2 The mole concept (Extended candidates
only)
5. Electricity and chemistry
6. Chemical energetic
6.1 Energetics of a reaction
6.2 Energy transfer
7. Chemical reactions
7.1 Physical and chemical changes
7.2 Rate (speed) of reaction
7.3 Reversible reactions
7.4 Redox
8. Acids, bases and salts
8.1 The characteristic properties of acids
and bases
8.2 Types of oxides
8.3 Preparation of salts
8.4 Identification of ions and gases
9. The Periodic Table
9.1 The Periodic Table
9.2 Periodic trends
9.3 Group properties
9.4 Transition elements
9.5 Noble gases
10. Metals
10.1 Properties of metals
10.2 Reactivity series
10.3 Extraction of metals
10.4 Uses of metals
11. Air and water
11.1 Water
11.2 Air
11.3 Nitrogen and fertilizers
11.4 Carbon dioxide and methane
12. Sulfur
13. Carbonates
14. Organic chemistry
14.1 Names of compounds
14.2 Fuels
14.3 Homologous series
14.4 Alkanes
14.5 Alkenes
14.6 Alcohols
14.7 Carboxylic acids
14.8.1 Polymers
14.8.2 Synthetic polymers
14.8.3 Natural polymers
1. The
particulate nature of matter
Core
•
State the distinguishing properties of solids, liquids and gases
•
Describe the structure of solids, liquids and gases in terms of particle
separation, arrangement and types of motion
•
Describe changes of state in terms of melting, boiling, evaporation, freezing,
condensation and sublimation
• Describe qualitatively the pressure and
temperature of a gas in terms of the motion of its particles
• Show an understanding of the random motion
of particles in a suspension (sometimes known as Brownian motion) as evidence
for the kinetic particle (atoms, molecules or ions) model of matter
•
Describe and explain diffusion
Supplement
•
Explain changes of state in terms of the kinetic theory
•
Describe and explain Brownian motion in terms of random molecular bombardment
•
State evidence for Brownian motion
•
Describe and explain dependence of rate of diffusion on molecular mass
2. Experimental techniques
2.1
Measurement
Core
•
Name appropriate apparatus for the measurement of time, temperature, mass and
volume, including burettes, pipettes and measuring cylinders Syllabus content
16 Cambridge IGCSE Chemistry 0620.
2.2.1 Criteria of purity
Core
•
Demonstrate knowledge and understanding of paper chromatography
• Interpret simple chromatograms
•
Identify substances and assess their purity from melting point and boiling
point information
•
Understand the importance of purity in substances in everyday life, e.g.
foodstuffs and drugs
Supplement
• Interpret simple chromatograms, including
the use of Rf values
•
Outline how chromatography techniques can be applied to colourless substances
by exposing chromatograms to substances called locating agents (Knowledge of
specific locating agents is not required.)
2.2.2
Methods of purification
Core
•
Describe and explain methods of purification by the use of a suitable solvent,
filtration, crystallisation and distillation (including use of fractionating
column). (Refer to the fractional distillation of petroleum in section14.2 and
products of fermentation in section 14.6.)
• Suggest suitable purification techniques,
given information about the substances involved
3.
Atoms, elements and compounds
3.1
Atomic structure and the Periodic Table
Core
• State the relative charges and approximate
relative masses of protons, neutrons and electrons
•
Define proton number (atomic number) as the number of protons in the nucleus of
an atom
• Define nucleon number (mass number) as the
total number of protons and neutrons in the nucleus of an atom
•
Use proton number and the simple structure of atoms to explain the basis of the
Periodic Table (see section 9), with special reference to the elements of
proton number 1 to 20
•
Define isotopes as atoms of the same element which have the same proton number
but a different nucleon number
•
State the two types of isotopes as being radioactive and non-radioactive
•
State one medical and one industrial use of radioactive isotopes
•
Describe the build-up of electrons in ‘shells’ and understand the significance
of the noble gas electronic structures and of the outer shell electrons (The
ideas of the distribution of electrons in s and p orbitals and in d block
elements are not required.) Note: a copy of the Periodic Table, as shown in the
Appendix, will be available in Papers 1, 2, 3 and 4.
Supplement
• Understand that isotopes have the same
properties because they have the same number of electrons in their outer shell .
3.2.1 Bonding: the structure of matter
Core
• Describe the differences between elements,
mixtures and compounds, and between metals and non-metals
• Describe an alloy, such as brass, as a
mixture of a metal with other elements
3.2.2
Ions and ionic bonds
Core
• Describe the formation of ions by electron
loss or gain
• Describe the formation of ionic bonds
between elements from Groups I and VII
Supplement
• Describe the formation of ionic bonds
between metallic and non-metallic elements
• Describe the lattice structure of ionic
compounds as a regular arrangement of alternating positive and negative ions
3.2.3 Molecules and covalent bonds
Core
•
Describe the formation of single covalent bonds in H2, Cl2, H2O, CH4, NH3 and
HCl as the sharing of pairs of electrons leading to the noble gas configuration
• Describe the differences in volatility,
solubility and electrical conductivity between ionic and covalent compounds
Supplement
•
Describe the electron arrangement in more complex covalent molecules such as
N2, C2H4, CH3OH and CO2
• Explain the differences in melting point and
boiling point of ionic and covalent compounds in terms of attractive forces
3.2.4
Macromolecules
Core
•
Describe the giant covalent structures of graphite and diamond
•
Relate their structures to their uses, e.g. graphite as a lubricant and a
conductor, and diamond in cutting tools
Supplement
•
Describe the macromolecular structure of silicon(IV) oxide (silicon dioxide)
•
Describe the similarity in properties between diamond and silicon(IV) oxide,
related to their structures
3.2.5
Metallic bonding
Supplement
•
Describe metallic bonding as a lattice of positive ions in a ‘sea of electrons’
and use this to describe the electrical conductivity and malleability of metals
Syllabus content 18 Cambridge IGCSE Chemistry 0620.
4. Stoichiometry
4.1
Stoichiometry
Core
• Use the symbols of the elements and write
the formulae of simple compounds
• Deduce the formula of a simple compound from
the relative numbers of atoms present
• Deduce the formula of a simple compound from
a model or a diagrammatic representation
•
Construct word equations and simple balanced chemical equations
• Define relative atomic mass, Ar , as the
average mass of naturally occurring atoms of an element on a scale where the
12C atom has a mass of exactly 12 units
• Define relative molecular mass, Mr , as the
sum of the relative atomic masses (Relative formula mass or Mr will be used for
ionic compounds.) (Calculations involving reacting masses in simple proportions
may be set. Calculations will not involve the mole concept.)
Supplement
• Determine the formula of an ionic compound
from the charges on the ions present
•
Construct equations with state symbols, including ionic equations
• Deduce the balanced equation for a chemical
reaction, given relevant information
4.2 The mole concept
Supplement
• Define the mole and the Avogadro constant
•
Use the molar gas volume, taken as 24dm3 at room temperature and pressure
• Calculate stoichiometric reacting masses,
volumes of gases and solutions, and concentrations of solutions expressed in
g/dm3 and mol/dm3 (Calculations involving the idea of limiting reactants may be
set. Questions on the gas laws and the conversion of gaseous volumes to
different temperatures and pressures will not be set.)
•
Calculate empirical formulae and molecular formulae
•
Calculate percentage yield and percentage purity Syllabus content Cambridge
IGCSE Chemistry 0620.
5. Electricity and chemistry
Core
•
Define electrolysis as the breakdown of an ionic compound, molten or in aqueous
solution, by the passage of electricity
• Describe the electrode products and the
observations made during the electrolysis of: – molten lead(II) bromide –
concentrated hydrochloric acid – concentrated aqueous sodium chloride – dilute
sulfuric acid between inert electrodes (platinum or carbon)
• State the general principle that metals or
hydrogen are formed at the negative electrode (cathode), and that non-metals
(other than hydrogen) are formed at the positive electrode (anode)
Supplement
• Relate the products of electrolysis to the
electrolyte and electrodes used, exemplified by the specific examples in the
Core together with aqueous copper(II) sulfate using carbon electrodes and using
copper electrodes (as used in the refining of copper)
•
Describe electrolysis in terms of the ions present and reactions at the
electrodes in the examples given
•
Predict the products of the electrolysis of a specified binary compound in the
molten state
• Describe the electroplating of metals
• Outline the uses of electroplating
•
Describe the reasons for the use of copper and (steelcored) aluminium in
cables, and why plastics and ceramics are used as insulators
•
Predict the products of electrolysis of a specified halide in dilute or
concentrated aqueous solution
• Construct ionic half-equations for reactions
at the cathode
•
Describe the transfer of charge during electrolysis to include: – the movement
of electrons in the metallic conductor – the removal or addition of electrons
from the external circuit at the electrodes – the movement of ions in the
electrolyte
• Describe the production of electrical energy
from simple cells, i.e. two electrodes in an electrolyte. (This should be
linked with the reactivity series in section 10.2 and redox in section 7.4.)
• Describe, in outline, the manufacture of: –
aluminium from pure aluminium oxide in molten cryolite (refer to section 10.3)
– chlorine, hydrogen and sodium hydroxide from concentrated aqueous sodium
chloride (Starting materials and essential conditions should be given but not
technical details or diagrams.)
6.
Chemical energetics
6.1 Energetics of a reaction
Core
•
Describe the meaning of exothermic and endothermic reactions
•
Interpret energy level diagrams showing exothermic and endothermic reactions
Supplement
•
Describe bond breaking as an endothermic process and bond forming as an
exothermic process
• Draw and label energy level diagrams for
exothermic and endothermic reactions using data provided
•
Calculate the energy of a reaction using bond energies
6.2
Energy transfer
Core
•
Describe the release of heat energy by burning fuels
•
State the use of hydrogen as a fuel
•
Describe radioactive isotopes, such as 235U, as a source of energy Supplement
•
Describe the use of hydrogen as a fuel reacting with oxygen to generate
electricity in a fuel cell (Details of the construction and operation of a fuel
cell are not required.)
7.
Chemical reactions
7.1
Physical and chemical changes
Core
• Identify physical and chemical changes, and
understand the differences between them
7.2
Rate (speed) of reaction
Core
• Describe and explain the effect of
concentration, particle size, catalysts (including enzymes) and temperature on
the rate of reactions
•
Describe the application of the above factors to the danger of explosive
combustion with fine powders (e.g. flour mills) and gases (e.g. methane in
mines)
•
Demonstrate knowledge and understanding of a practical method for investigating
the rate of a reaction involving gas evolution
•
Interpret data obtained from experiments concerned with rate of reaction Note:
Candidates should be encouraged to use the term rate rather than speed.
Supplement
• Devise and evaluate a suitable method for
investigating the effect of a given variable on the rate of a reaction
•
Describe and explain the effects of temperature and concentration in terms of
collisions between reacting particles (An increase in temperature causes an
increase in collision rate and more of the colliding molecules have sufficient
energy (activation energy) to react whereas an increase in concentration only
causes an increase in collision rate.) cont.
7.2 Rate (speed) of reaction continued
• Describe and explain the role of light in
photochemical reactions and the effect of light on the rate of these reactions
(This should be linked to section 14.4.)
•
Describe the use of silver salts in photography as a process of reduction of
silver ions to silver; and photosynthesis as the reaction between carbon
dioxide and water in the presence of chlorophyll and sunlight (energy) to
produce glucose and oxygen
7.3 Reversible reactions
Core
• Understand that some chemical reactions can
be reversed by changing the reaction conditions (Limited to the effects of heat
and water on hydrated and anhydrous copper(II) sulfate and cobalt(II)
chloride.) (Concept of equilibrium is not required.)
Supplement
• Predict the effect of changing the
conditions (concentration, temperature and pressure) on other reversible
reactions
•
Demonstrate knowledge and understanding of the concept of equilibrium 7.4 Redox
Core
•
Define oxidation and reduction in terms of oxygen loss/gain. (Oxidation state
limited to its use to name ions, e.g. iron(II), iron(III), copper(II),
manganate(VII).)
Supplement
•
Define redox in terms of electron transfer
• Identify redox reactions by changes in
oxidation state and by the colour changes involved when using acidified
potassium manganate(VII), and potassium iodide. (Recall of equations involving
KMnO4 is not required.)
• Define oxidising agent as a substance which
oxidises another substance during a redox reaction. Define reducing agent as a
substance which reduces another substance during a redox reaction.
•
Identify oxidising agents and reducing agents from simple equations Syllabus
content 22 Cambridge IGCSE Chemistry .
8. Acids, bases and salts
8.1 The characteristic properties of acids
and bases
Core
•
Describe the characteristic properties of acids as reactions with metals,
bases, carbonates and effect on litmus and methyl orange
•
Describe the characteristic properties of bases as reactions with acids and
with ammonium salts and effect on litmus and methyl orange
• Describe neutrality and relative acidity and
alkalinity in terms of pH measured using Universal Indicator paper (whole
numbers only)
• Describe and explain the importance of
controlling acidity in soil Supplement
• Define acids and bases in terms of proton
transfer, limited to aqueous solutions
• Describe
the meaning of weak and strong acids and bases
8.2
Types of oxides
Core
• Classify oxides as either acidic or basic,
related to metallic and non-metallic character
Supplement
•
Further classify other oxides as neutral or amphoteric
8.3
Preparation of salts
Core
•
Demonstrate knowledge and understanding of preparation, separation and
purification of salts as examples of some of the techniques specified in
section 2.2.2 and the reactions specified in section 8.1 .
Supplement
• Demonstrating knowledge and understanding of
the preparation of insoluble salts by precipitation
•
Suggest a method of making a given salt from a suitable starting material,
given appropriate information Syllabus content Cambridge IGCSE Chemistry 0620.
8.4 Identification of ions and gases
Core
• Describe the following tests to identify:
aqueous cations: aluminium, ammonium, calcium, chromium(III), copper(II),
iron(II), iron(III) and zinc (using aqueous sodium hydroxide and aqueous
ammonia as appropriate) (Formulae of complex ions are not required.) cations:
use of the flame test to identify lithium, sodium, potassium and copper(II)
anions: carbonate (by reaction with dilute acid and then limewater), chloride,
bromide and iodide (by reaction under acidic conditions with aqueous silver
nitrate), nitrate (by reduction with aluminium), sulfate (by reaction under
acidic conditions with aqueous barium ions) and sulfite (by reaction with
dilute acids and then aqueous potassium manganate(VII)) gases: ammonia (using
damp red litmus paper), carbon dioxide (using limewater), chlorine (using damp
litmus paper), hydrogen (using lighted splint), oxygen (using a glowing
splint), and sulfur dioxide (using aqueous potassium manganate(VII))
9. The Periodic Table
9.1
The Periodic Table
Core
•
Describe the Periodic Table as a method of classifying elements and its use to
predict properties of elements
9.2 Periodic trends
Core
• Describe the change from metallic to
non-metallic character across a period Supplement
•
Describe and explain the relationship between Group number, number of outer
shell electrons and metallic/nonmetallic character
9.3 Group properties
Core
•
Describe lithium, sodium and potassium in Group I as a collection of
relatively soft metals showing a trend in melting point, density and reaction
with water
•
Predict the properties of other elements in Group I, given data, where
appropriate
• Describe the halogens, chlorine, bromine and
iodine in Group VII, as a collection of diatomic non-metals showing a trend in
colour and density and state their reaction with other halide ions
• Predict the properties of other elements in
Group VII, given data where appropriate Supplement
• Identify trends in Groups, given information
about the elements concerned 9.4
Transition elements
Core
• Describe the transition elements as a
collection of metals having high densities, high melting points and forming coloured
compounds, and which, as elements and compounds, often act as catalysts.
Supplement
• Know that transition elements have variable
oxidation states .
9.5 Noble gases
Core
•
Describe the noble gases, in Group VIII or 0, as being unreactive, monoatomic
gases and explain this in terms of electronic structure
•
State the uses of the noble gases in providing an inert atmosphere, i.e. argon
in lamps, helium for filling balloons .
10. Metals
10.1
Properties of metals
Core
• List the general physical properties of
metals
• Describe the general chemical properties of
metals e.g. reaction with dilute acids and reaction with oxygen
• Explain in terms of their properties why
alloys are used instead of pure metals
• Identify representations of alloys from
diagrams of structure
10.2 Reactivity series
Core
• Place in order of reactivity: potassium,
sodium, calcium, magnesium, zinc, iron, (hydrogen) and copper, by reference to
the reactions, if any, of the metals with: – water or steam – dilute
hydrochloric acid and the reduction of their oxides with carbon
•
Deduce an order of reactivity from a given set of experimental results Supplement
•
Describe the reactivity series as related to the tendency of a metal to form
its positive ion, illustrated by its reaction, if any, with: – the aqueous
ions – the oxides of the other listed metals
•
Describe and explain the action of heat on the hydroxides, carbonates and
nitrates of the listed metals
• Account for the apparent unreactivity of
aluminium in terms of the oxide layer which adheres to the metal
10.3 Extraction of metals
Core
•
Describe the ease in obtaining metals from their ores by relating the elements
to the reactivity series
• Describe and state the essential reactions
in the extraction of iron from hematite
• Describe the conversion of iron into steel
using basic oxides and oxygen
• Know that aluminium is extracted from the
ore bauxite by electrolysis
• Discuss the advantages and disadvantages of
recycling metals, limited to iron/steel and aluminium
Supplement
• Describe in outline, the extraction of zinc
from zinc blende
• Describe in outline, the extraction of
aluminium from bauxite including the role of cryolite and the reactions at the
electrodes Syllabus content 26 Cambridge IGCSE Chemistry 0620.
10.4 Uses of metals
Core
•
Name the uses of aluminium: – in the manufacture of aircraft because of its
strength and low density – in food containers because of its resistance to
corrosion
• Name the uses of copper related to its
properties (electrical wiring and in cooking utensils)
•
Name the uses of mild steel (car bodies and machinery) and stainless steel
(chemical plant and cutlery)
Supplement
•
Explain the uses of zinc for galvanising and for making brass
•
Describe the idea of changing the properties of iron by the controlled use of
additives to form steel alloys
11. Air and water
11.1 Water
Core
• Describe chemical tests for water using
cobalt(II) chloride and copper(II) sulfate
• Describe, in outline, the treatment of the
water supply in terms of filtration and chlorination
•
Name some of the uses of water in industry and in the home
Supplement
•
Discuss the implications of an inadequate supply of water, limited to safe
water for drinking and water for irrigating crops
11.2 Air
Core
• State the composition of clean, dry air as
being approximately 78% nitrogen, 21% oxygen and the remainder as being a
mixture of noble gases and carbon dioxide
• Name the common pollutants in the air as
being carbon monoxide, sulfur dioxide, oxides of nitrogen and lead compounds
• State the source of each of these
pollutants: – carbon monoxide from the incomplete combustion of
carbon-containing substances – sulfur dioxide from the combustion of fossil
fuels which contain sulfur compounds (leading to ‘acid rain’) – oxides of
nitrogen from car engines – lead compounds from leaded petrol
•
State the adverse effect of these common pollutants on buildings and on health
and discuss why these pollutants are of global concern
• State the conditions required for the
rusting of iron
• Describe and explain methods of rust
prevention, specifically paint and other coatings to exclude oxygen
Supplement
•
Describe the separation of oxygen and nitrogen from liquid air by fractional
distillation
• Describe and explain the presence of oxides
of nitrogen in car engines and their catalytic removal
•
Describe
and explain sacrificial protection in terms of
the reactivity series of metals and galvanising as a method of rust prevention .
11.3 Nitrogen and fertilizers
Core
•
Describe the need for nitrogen-, phosphorus- and potassium-containing fertilizers
• Describe the displacement of ammonia from
its salts
Supplement
•
Describe and explain the essential conditions for the manufacture of ammonia by
the Haber process including the sources of the hydrogen and nitrogen, i.e.
hydrocarbons or steam and air
11.4 Carbon dioxide and methane
Core
•
State that carbon dioxide and methane are greenhouse gases and explain how they
may contribute to climate change
•
State the formation of carbon dioxide: – as a product of complete combustion of
carboncontaining substances – as a product of respiration – as a product of the
reaction between an acid and a carbonate – from the thermal decomposition of a
carbonate
• State the sources of methane, including
decomposition of vegetation and waste gases from digestion in animals
Supplement
• Describe the carbon cycle, in simple terms,
to include the processes of combustion, respiration and photosynthesis
12.
Sulfur
Core
•
Name some sources of sulfur
•
Name the use of sulfur in the manufacture of sulfuric acid
• State the uses of sulfur dioxide as a bleach
in the manufacture of wood pulp for paper and as a food preservative (by
killing bacteria)
Supplement
•
Describe the manufacture of sulfuric acid by the Contact process, including
essential conditions and reactions
• Describe the properties and uses of dilute
and concentrated sulfuric acid 13.
Carbonates
Core
• Describe the manufacture of lime (calcium
oxide) from calcium carbonate (limestone) in terms of thermal decomposition
• Name some uses of lime and slaked lime such
as in treating acidic soil and neutralising acidic industrial waste products,
e.g. flue gas desulfurisation
•
Name the uses of calcium carbonate in the manufacture of iron and cement.
14. Organic chemistry
14.1
Names of compounds
Core
•
Name and draw the structures of methane, ethane, ethene, ethanol, ethanoic acid
and the products of the reactions stated in sections 14.4–14.6
•
State the type of compound present, given a chemical name ending in ‑ane, ‑ene,
‑ol, or ‑oic acid or a molecular structure
Supplement
•
Name and draw the structures of the unbranched alkanes, alkenes (not cistrans),
alcohols and acids containing up to four carbon atoms per molecule
• Name and draw the structural formulae of the
esters which can be made from unbranched alcohols and carboxylic acids, each
containing up to four carbon atoms
14.2 Fuels
Core
• Name the fuels: coal, natural gas and
petroleum
•
Name methane as the main constituent of natural gas
• Describe petroleum as a mixture of
hydrocarbons and its separation into useful fractions by fractional
distillation
• Describe the properties of molecules within
a fraction
•
Name the uses of the fractions as: – refinery gas for bottled gas for heating
and cooking – gasoline fraction for fuel (petrol) in cars – naphtha fraction
for making chemicals – kerosene/paraffin fraction for jet fuel – diesel oil/gas
oil for fuel in diesel engines – fuel oil fraction for fuel for ships and home
heating systems – lubricating fraction for lubricants, waxes and polishes –
bitumen for making roads
14.3 Homologous series
Core
•
Describe the concept of homologous series as a ‘family’ of similar compounds
with similar chemical properties due to the presence of the same functional
group
Supplement
• Describe the general characteristics of an
homologous series
• Recall that the compounds in a homologous
series have the same general formula
•
Describe and identify structural isomerism
14.4 Alkanes
Core
•
Describe the properties of alkanes (exemplified by methane) as being generally
unreactive, except in terms of burning
•
Describe the bonding in alkanes
Supplement
• Describe substitution reactions of alkanes
with chlorine .
14.5 Alkenes
Core
•
Describe the manufacture of alkenes and of hydrogen by cracking
• Distinguish between saturated and
unsaturated hydrocarbons: – from molecular structures – by reaction with
aqueous bromine
•
Describe the formation of poly(ethene) as an example of addition polymerisation
of monomer units
Supplement
• Describe the properties of alkenes in terms
of addition reactions with bromine, hydrogen and steam
14.6 Alcohols
Core
•
Describe the manufacture of ethanol by fermentation and by the catalytic
addition of steam to ethane
• Describe the properties of ethanol in terms
of burning
•
Name the uses of ethanol as a solvent and as a fuel
Supplement
•
Outline the advantages and disadvantages of these two methods of manufacturing
ethanol
14.7 Carboxylic acids
Core
• Describe the properties of aqueous ethanoic
acid
Supplement
• Describe the formation of ethanoic acid by
the oxidation of ethanol by fermentation and with acidified potassium
manganate(VII)
•
Describe ethanoic acid as a typical weak acid
•
Describe the reaction of a carboxylic acid with an alcohol in the presence of a
catalyst to give an ester
14.8.1
Polymers
Core
•
Define polymers as large molecules built up from small units (monomers) Supplement
• Understand that different polymers have
different units and/or different linkages.
14.8.2 Synthetic polymers
Core
• Name some typical uses of plastics and of
man-made fibres such as nylon and Terylene
• Describe the pollution problems caused by
nonbiodegradable plastics Supplement
• Explain the differences between condensation
and addition polymerisation • Deduce the structure of the polymer product from
a given alkene and vice versa
• Describe the formation of nylon (a
polyamide) and Terylene (a polyester) by condensation polymerisation, the
structure of nylon being represented as: C O C O C C O O N H N H N H N H C O
and the structure of Terylene as: C O C O C C O O O O O O (Details of
manufacture and mechanisms of these polymerisations are not required.)
14.8.3 Natural polymers
Core
• Name proteins and carbohydrates as
constituents of food
Supplement
• Describe proteins as possessing the same
(amide) linkages as nylon but with different units
• Describe the structure of proteins as: N H C
O N H C O N H C O • Describe the hydrolysis of proteins to amino acids
(Structures and names are not required.)
•
Describe complex carbohydrates in terms of a large number of sugar units,
considered as HO OH, joined together by condensation polymerisation, e.g.
O O O O
• Describe the hydrolysis of complex
carbohydrates (e.g. starch), by acids or enzymes to give simple sugars
• Describe the fermentation of simple sugars
to produce ethanol (and carbon dioxide) (Candidates will not be expected to
give the molecular formulae of sugars.)
• Describe, in outline, the usefulness of
chromatography in separating and identifying the products of hydrolysis of
carbohydrates and proteins
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