1. Identification of ions and gases

1. describe the use of aqueous sodium hydroxide and aqueous ammonia to identify the following cations: aluminium, ammonium, calcium, copper(II), iron(II), iron(III), lead(II) and zinc, (Formulae of complex ions are not required.)
2. describe the tests to identify the following anions: carbonate (by reaction with dilute acid and then limewater), chloride (by reaction, under acidic conditions, with aqueous silver nitrate), iodide (by reaction, under acidic conditions, with aqueous lead(II) nitrate), nitrate (by reduction with aluminium to ammonia) and sulphate (by reaction, under acidic conditions, with aqueous barium ions).
3. ammonia (using damp red litmus paper), carbon dioxide (using limewater), chlorine (using damp litmus paper), hydrogen (using lighted splint), oxygen (using glowing splint) and sulphur dioxide (using acidified potassium dichromate(VI).

2. Redox

1. define oxidation and reduction in terms of oxygen/hydrogen gain/loss.
2. define redox in terms of electron transfer and changes in oxidation state.
3. identify redox reactions in terms of oxygen/hydrogen, and/or electron gain/loss.
4. describe the use of aqueous potassium iodide, acidified potassium dichromate(VI) and acidified potassium manganate(VII) in testing for oxidising and reducing agents from the resulting colour changes.

3. The Chemistry and Uses Acids, Bases and Salts

   3.1 The characteristics and properties of acids and bases

1. describe the meanings of the terms acid and alkali in terms of the ions they contain or produce in aqueous solution and their effects on Univeral indicator paper.
2. describe how to test hydrogen ion concentration and hence relative acidity using Universal Indicator paper and the pH scale.
3. describe the characteristic properties of acids as in reactions with metals, bases, alkalis, carbonates.
4. describe qualitatively the difference between strong and weak acids in terms of the extent of ionisation
5. describe neutralisation as a reaction between hydrogen ions and hydroxide ions to produce water:
   H⁺ + OH^- ---> H₂O
6. describe the characteristic properties of bases in reactions with acids and with ammonium salts.
7. classify oxides as either acidic, basic or amphoteric related to metallic/non-metallic character.

   3.2 Preparation of Salts

1. describe the techniques used in the preparation, separation and purification of salts as examples of some of the techniques specific in 'Experimental Techniques' (Methods of preparing salts to illustrate the practical techniques should include the action of acids with metals, insoluble bases and insoluble carbonates.)
2. describe the general rules of solubility for common slats to include nitrates, chlorides (including silver and lead), sulphates (including barium, calcium and lead), carbonates, hydroxides, Group I cations and ammonium salts.

   3.3 Properties and uses of ammonia

   3.4 Sulphuric acid

4. Metals

     4.1 Properties of Metals

1. describe the general physical as solids having high melting and boiling points, malleable, good conductors of heat and electricity in terms of their structure.
2. describe alloys as a mixture of a metal with another element, e.g. brass; stainless steel.
3. identify representations of metals and alloys from diagrams of structures.
4. explain why alloys have different physical properties to their constituent elements.

     4.2 Reactivity Series

1. place in order of reactivity calcium, copper, (hydrogen), iron magnesium, potassium, silver, sodium and zinc by reference to: the reactions, if any, of the metals with: water or steam; dilute hydrochloric acid
2. the reduction, if any, of their oxides with carbon and/or with hydrogen
   1. 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.
   2. describe the order of reactivity from a given set of experimental results.
   3. describe the action of heat on the carbonates of the listed metals and relate thermal stability to the reactivity series.

5. Periodic Table

   5.1 Periodic Trends

1. describe the position of an element in the Periodic Table is related to proton number and electronic structure.
2. describe the relationship between group number and the ionic charge of an element.
3. explain the similarities between group number and the ionic charge of an element.
4. explain the similarities between the elements in the same group of the Periodic Table in terms of their electronic structure.
5. describe the relationship between group number, number of valency electrons and metallic and non-metallic character.
6. Predict the properties of elements in Group I, VII and the transition elements using the Periodic Table.

   5.2 Group Properties

1. 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.
2. 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.

   5.3 Transition Elements

1. describe the central block of elements as transition metals with high melting points, high density, variable oxidation state and forming coloured compounds.
2. state the use of these elements and/or their compounds as catalysts, e.g. iron in the Haber process; vanadium(V) oxide in the Contact Process; nickel in the hydrogenation of alkenes.

6. Energy From Chemicals

1. describe the meaning of enthalphy change in terms of exothermic(DH negative) and endothermic (DH positive) reactions.

7. Organic Chemistry

   7 .1 Alcohols

1. describe the properties of alcohol in terms of combustion and oxidation to carboxylic acids.

   7.2 Carboxylic acids

1. describe the carboxylic acids as weak acids, reacting with carbonates, bases and some metals.
2. describe the formation of ethanoic acid by the oxidation of ethanol by atmospheric oxygen or acidified potassium dichromate(VI).
3. describe the reaction of ethanoic acid with ethanol to form the ester, ethyl ethanoate.

8. Reagents List for 5068/3

(This reagent list is drawn up as a guide concerning the standard reagents that are expected to be generally available for examination purposes. The list is not intended to be exhaustive and the `Instructions to Supervisors' issued several weeks in advance of the examination will give a full list of all the reagents that are required for each practical examination.)