(a) What are nucleons?

(b) State Graham's law of diffusion.

(c) Explain briefly why aluminium does not corrode easily.

(d) State three examples of periodic properties.

(e) State two reasons why real gases deviate from ideal gas behaviour.

(f) List three uses of fractional distillation in industry.

(g) What factors determine the selective discharge of ions at the electrodes during electrolysis?

(h) State the type of reaction represented by each of the following equations:

(i) C\(_2\)H\(_6\) + Br\(_2\) ---> C\(_2\)H\(_5\)Br + HBr;

(ii) C\(_2\)H\(_4\) + .Br\(_2\) ---> CH\(_4\)Br\(_2\)

(i) Name the products formed when butane burns in limited supply of air.

(j) List three methods of separating a solid from a liquid.

(a) Consider the following atoms: \(^R_T\)X; \(^S_T\)X.

(i) State the phenomenon exhibited by the two atoms.

(ii) What is the difference between the atoms?

(iii) Give two examples of elements that exhibit the phenomenon stated in (ai)

(iv) lf T is 17, write the electron configuration of the element

(b)(i) State two differences between metals and-non-metals with respect to their:

I. physical properties;

2. chemical properties.

(ii) Give one example of each for the following compounds:

I. an amphoteric oxide;

II. a hydride which evolves hydrogen when reacted with water;

Ill. a trioxocarbonate (IV) salt which is readily decomposed on heating;

IV. a chloride salt which is readily hydrolyzed in water.

(c)(i) State three characteristic properties of transition metals. 

(ii) Write the electron configuration of \(_{30}Zn\)

(iii.) Explain briefly why zinc is not considered as a typical transition element.

(d) Consider the reaction represented by the following equation:- Na\(_2\)CO\(_{3(aq)}\) + MgCl\(_{2(aq)}\) ----> 2NaCl\(_{(aq)}\) + MgCO\(_{3(aq)}\). Calculate the mass of sodium trioxocarbonate (IV) needed to produce 3.36 of magnesium trioxocarbonate (IV). [C = 12.0, O = 16.0, Na = 23.0, Mg = 24:0 ]

(a) (i) Draw the structures of the isomers of the alkene with molecular formurat C\(_4\)H\(_8\)

(ii) State the class of alkanols to which each of the following compounds belongs:

I. CH\(_3\)C(CH\(_3\))\(_2\)OH;

II. CH\(_3\)CH(CH\(_3\))CH\(_2\)OH;

III. CH\(_3\)CH\(_2\)CH(CH\(_3\))OH.

(b) (i) Write the formulae of the products formed in the following reactions:
I. CH\(_3\)CH\(_2\)COOH \(\frac{K_{(s)}}{}\)

II. CH\(_3\)CH\(_2\)COOH. \(\frac{C_4H_6OH, heat}{Conc.H_2SO_4}\)

III. CH\(_3\)CH\(_2\)CH\(_2\)CH\(_2\)OH \(\frac{H^+/KMnO_4}{(excess)}\)

(ii) Name the major product(s) of each of the reactions in (b)(i).

(c) A gaseous hydrocarbon R of mass 7.0 g occupies a volume of 2.24 dm\(^3\) at s. t.p. If the percentage composition by mass of hydrogen is 14.3, determine its:

(i) empirical formula;

(ii) molecular formula. [ H = 1.00, C = 12.0, Molar volume of gas at s.t.p, = 22.4 dm\(^3\) ]

(d) Define structural isomerism.

(a)(i) Name a suitable drying agent for the preparation of carbon (IV) oxide in the laboratory.

(ii) Using one chemical test, distinguish between carbon (II) oxide and carbon (IV) oxide.

(b)(i) Describe briefly how oxygen and nitrogen could be obtained separately from air on an industrial scale

(ii) State how a lighted splint can be used to distinguish between samples of oxygen and nitrogen.

(c)(i) Give one reason why bauxite is usually preferred as the ore for the extraction of aluminium.

(ii). List two main impurities. usually present in bauxite.

(iii) State the function of sodium hydroxide solution in the extraction of aluminium from its ore.

(iv) Explain briefly why it is difficult to extract aluminium by chemical reduction of aluminium oxide

(v) Write an equation for the reaction of aluminium oxide with aqueous sodium hydroxide.

(d) (i) The melting and boiling points of sodium chloride are 801 °C and 141.3 °C respectively. Explain briefly why sodium chloride does not conduct electricity at 25°C but does so between 801 °C and 1413 °C.

(ii) State the reason why sodium metal is stored under paraffin oil in the laboratory.

(e)(i) State what would be observed when aqueous sodium trioxocarbonate(IV) is added to a solution containing iron (III) ions

(ii) Write a balanced equation for the reaction in (e)(i).

(a)(i) Determine the oxidation number of sulphur in Na\(_2\)S\(_2\)O\(_3\)

(ii) Name the allotropes of sulphur.

(iii) State two ways in which the structure of graphite and diamond are similar.

(b)(i) Name two green-house gases.

(ii) State one effect of an increased level of green-house gases on the environment.

(iii) State one source from which nitrogen (I) oxide is released into the environment.

(iv) Write a chemical equation to show the effect of heat on each of the following compounds: I. KNO\(_{3(s)}\) II. AgNO\(_{3(s)}\)

(C)(i)Describe briefly how pure crystals of calcium chloride could be obtained from a solution of calcium chloride

ii) Explain briefly each of the following observations:

I. ammonia gas is highly soluble in water;

II. boiling ploint of chlorine is lower than that of iodine

(d) Consider the reaction represented by the following equation:- 2NaCl + H\(_2\)SO\(_{4(s)}\)  \(\to\) Na\(_2\)SO\(_{4(s)}\) + 2HCl\(_{(g)}\)

Calculate the volume of HCl gas that can be obtained at s.t.p. from 5.85 g of sodium. chloride. [ Na = 23.0, Cl = 35.5, Molar volume of gas at s.t.p. = 22.4 dm\(^3\)]