Vivace

Chem EOY Topics

Date: Friday, October 3, 2008 || Time: 9:08 PM

SEC 3 CHEMISTRY
END-OF-YEAR EXAM 2008

SCHEME OF ASSESSMENT

Section A : MCQ (30 marks)
Section B : Structured questions (40 marks)
Section C : School-based Science Practical Assessment (SPA) (30 marks)

TOPICS TO BE TESTED

Chapters 1 - 12 , 14 and 16

Experimental design

(a) name appropriate apparatus for the measurement of time, temperature, mass and volume, including burettes, pipettes, measuring cylinders and gas syringes

(b) suggest suitable apparatus, given relevant information, for a variety of simple experiments, including collection of gases and measurement of rates of reaction
Methods of purification and analysis

(a) has knowledge of methods of separations and purification for the components of the following types of mixtures:

(i) solid-solid

(ii) solid-liquid

(iii) liquid-liquid (miscible and immiscible)

Techniques to be covered for separations and purification include: i) use of a suitable solvent, filtration and crystallisation or
evaporation

(ii) sublimation

(iii) distillation and fractional distillation

(iv) use of a separating funnel

(v) paper chromatography (b) describe paper chromatography and interpret chromatograms including comparison with ‘known’ samples and the use of Rf values

(c) explain the need to use locating agents in the chromatography of colourless compounds

(d) deduce from the given melting point and boiling point the identities of
substances and their purity

(e) explain that the measurement of purity in substances used in everyday life, e.g. foodstuffs and drugs, is important

Identification of ions and gases

(a) describe the use of aqueous sodium hydroxide and aqueous ammonia to identify the following aqueous cations: aluminium, ammonium, calcium, copper(II), iron(II), iron(III), lead(II) and zinc (formulae of complex ions are not required)

(b) describe tests to identify the following anions: carbonate (by the addition of dilute acid and subsequent use of limewater); chloride (by reaction of an aqueous solution with nitric acid and aqueous silver nitrate); iodide (by reaction of an aqueous solution with nitric acid and aqueous lead(II) nitrate); nitrate (by reduction with aluminium and aqueous sodium hydroxide to ammonia and subsequent use of litmus paper) and sulphate (by reaction of an aqueous solution with nitric acid and aqueous barium nitrate)

(c) describe tests to identify the following gases: ammonia (using damp red litmus paper); carbon dioxide (using limewater); chlorine (using damp litmus paper); hydrogen (using a burning splint); oxygen (using a glowing splint) and sulphur dioxide (using acidified potassium dichromate(VI))

The Particulate Nature of Matter- Kinetic particle theory

(a) describe the solid, liquid and gaseous states of matter and explain their interconversion in terms of the kinetic particle theory and of the energy changes involved

(b) describe and explain evidence for the movement of particles in liquids and gases

(c) explain everyday effects of diffusion in terms of particles, e.g. the spread of perfumes and cooking aromas; tea and coffee grains in water

(d) state qualitatively the effect of molecular mass on the rate of diffusion and explain the dependence of rate of diffusion on temperature

Atomic structure

(a) state the relative charges and approximate relative masses of a proton, a neutron and an electron

(b) describe, with the aid of diagrams, the structure of an atom as containing protons and neutrons (nucleons) in the nucleus and electrons arranged in shells (energy levels)

(c) define proton (atomic) number and nucleon (mass) number

(d) interpret and use symbols such as C126

(e) define the term isotopes

(f) deduce the numbers of protons, neutrons and electrons in atoms and ions given proton and nucleon numbers

Ionic bonding

(a) describe the formation of ions by electron loss/gain in order to obtain the electronic configuration of a noble gas

(b) describe the formation of ionic bonds between metals and non-metals, e.g. NaCl; MgCl2

(c) state that ionic materials contain a giant lattice in which the ions are held by electrostatic attraction, e.g. NaCl (candidates will not be required to draw diagrams of ionic lattices)

(d) deduce the formulae of other ionic compounds from diagrams of their lattice structures, limited to binary compounds

(e) relate the physical properties (including electrical property) of ionic compounds to their lattice structure

Covalent bonding

(a) describe the formation of a covalent bond by the sharing of a pair of electrons in order to gain the electronic configuration of a noble gas

(b) describe, using ‘dot-and-cross’ diagrams, the formation of covalent bonds between non-metallic elements, e.g. H2; O2; H2O; CH4; CO2

(c) deduce the arrangement of electrons in other covalent molecules

(d) relate the physical properties (including electrical property) of covalent substances to their structure and bonding

Metallic bonding

(a) describe metals as a lattice of positive ions in a ‘sea of electrons’

(b) relate the electrical conductivity of metals to the mobility of the electrons in the structure

Formulae, Stoichiometry and the Mole Concept

(a) state the symbols of the elements and formulae of the compounds mentioned in the syllabus

(b) deduce the formulae of simple compounds from the relative numbers of atoms present and vice versa

deduce the formulae of ionic compounds from the charges on the ions present and vice versa

(d) interpret chemical equations with state symbols

(e) construct chemical equations, with state symbols, including ionic equations

(f) define relative atomic mass, Ar

(g) define relative molecular mass, Mr, and calculate relative molecular mass (and relative formula mass) as the sum of relative atomic masses

(h) calculate the percentage mass of an element in a compound when given appropriate information

(i) calculate empirical and molecular formulae from relevant data

(j) calculate stoichiometric reacting masses and volumes of gases (one mole of gas occupies 24 dm3 at room temperature and pressure); calculations involving the idea of limiting reactants may be set (The gas laws and the calculations of gaseous volumes at different temperatures and pressures are not required.)

(k) apply the concept of solution concentration (in mol/dm3 or g/dm3) to process the results of volumetric experiments and to solve simple problems

(l) calculate % yield and % purity

Acids and bases

(a) describe the meanings of the terms acid and alkali in terms of the ions they produce in aqueous solution and their effects on Universal Indicator

(b) describe how to test hydrogen ion concentration and hence relative acidity using Universal Indicator and the pH scale

(c) describe qualitatively the difference between strong and weak acids in terms of the extent of ionisation

(d) describe the characteristic properties of acids as in reactions with metals, bases and carbonates

(e) state the uses of sulphuric acid in the manufacture of detergents and fertilisers; and as a battery acid

(f) describe the reaction between hydrogen ions and hydroxide ions to produce water,
H+ + OH- → H2O, as neutralisation

(g) describe the importance of controlling the pH in soils and how excess acidity can be treated using calcium hydroxide

(h) describe the characteristic properties of bases in reactions with acids and with ammonium salts

(i) classify oxides as acidic, basic, amphoteric or neutral based on metallic/non-metallic character

(j) classify sulphur dioxide as an acidic oxide and state its uses as a bleach, in the manufacture of wood pulp for paper and as a food preservative (by killing bacteria)

Salts

(a) describe the techniques used in the preparation, separation and purification of
(methods for preparation should include precipitation and titration together with reactions of acids with metals, insoluble bases and insoluble carbonates)

(b) describe the general rules of solubility for common salts to include nitrates, chlorides (including silver and lead), sulphates (including barium, calcium and lead), carbonates, hydroxides, Group I cations and ammonium salts

(c) suggest a method of preparing a given salt from suitable starting materials, given appropriate information

Properties of metals

(a) describe the general physical properties of metals as solids having high melting and boiling points, malleable, good conductors of heat and electricity in terms of their structure

(b) describe alloys as a mixture of a metal with another element, e.g. brass; stainless steel

(c) identify representations of metals and alloys from diagrams of structures

(d) explain why alloys have different physical properties to their constituent elements

Reactivity series

(a) place in order of reactivity calcium, copper, (hydrogen), iron, lead, magnesium, potassium, silver, sodium and zinc by reference to
(i) the reactions, if any, of the metals with water, steam and dilute hydrochloric acid,
(ii) the reduction, if any, of their oxides by carbon and/or by hydrogen

(b) describe the reactivity series as related to the tendency of a metal to form its positive ion, illustrated by its reaction with
(i) the aqueous ions of the other listed metals
(ii) the oxides of the other listed metals

(c) deduce the order of reactivity from a given set of experimental results

(d) describe the action of heat on the carbonates of the listed metals and relate thermal stability to the reactivity series

Extraction of metals

(a) describe the ease of obtaining metals from their ores by relating the elements to their positions in the reactivity series

Recycling of metals

(a) describe metal ores as a finite resource and hence the need to recycle metals, e.g. recycling of iron

(b) discuss the social, economic and environmental issues of recycling metals

Iron

(a) describe and explain the essential reactions in the extraction of iron using haematite, limestone and coke in the blast furnace

(b) describe steels as alloys which are a mixture of iron with carbon or other metals and how controlled use of these additives changes the properties of the iron, e.g. high carbon steels are strong but brittle whereas low carbon steels are softer and more easily shaped

(c) state the uses of mild steel, e.g. car bodies; machinery, and stainless steel, e.g. chemical plants; cutlery; surgical instruments

(d) describe the essential conditions for the corrosion (rusting) of iron as the presence of oxygen and water; prevention of rusting can be achieved by placing a barrier around the metal, e.g. painting; greasing; plastic coating; galvanising

(e) describe the sacrificial protection of iron by a more reactive metal in terms of the reactivity series where the more reactive metal corrodes preferentially, e.g. underwater pipes have a piece of magnesium attached to them

The Periodic Table- Periodic trends

(a) describe the Periodic Table as an arrangement of the elements in the order of increasing proton (atomic) number

(b) describe how the position of an element in the Periodic Table is related to proton number and electronic structure

(c) describe the relationship between group number and the ionic charge of an element

(d) explain the similarities between the elements in the same group of the Periodic Table in terms of their electronic structure

(e) describe the change from metallic to non-metallic character from left to right across a period of the Period Table

(f) describe the relationship between group number, number of valency electrons and metallic/non-metallic character

(g) predict the properties of elements in Group I and VII using the Periodic Table

Group properties

(a) describe lithium, sodium and potassium in Group I (the alkali metals) as a collection of relatively soft, low density metals showing a trend in melting point and in their reaction with water

(b) describe chlorine, bromine and iodine in Group VII (the halogens) as a collection of diatomic non-metals showing a trend in colour, state and their displacement reactions with solutions of other halide ions

(c) describe the elements in Group 0 (the noble gases) as a collection of monatomic elements that are chemically unreactive and hence important in providing an inert atmosphere, e.g. argon and neon in light bulbs; helium in balloons; argon in the manufacture of steel

(d) describe the lack of reactivity of the noble gases in terms of their electronic structures

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