(a) Atoms of four non-metallic elements in the same group of the periodic table are arranged in order of increasing atomic radius as R < T < W < X. Which of the elements

(i) would readily lose electron(s) from the outermost shell;

(ii) is most electronegative;

(iii) would T displace from aqueous solution;

(iv) is at the top of the group?

(b) The following table shows the electronic configuration of two elements Y and Z.

(i) Name the I. group to which Y belongs II. period to which Z belongs.

(ii) What is the number of protons present in an atom of Z?

(iii) How many unpaired electrons are in an atom of Y?

(iv) Write the formula of the compound formed between Y and Z

(c) Name the type of bond(s) that exist(s) in each of the following compounds.

(i) CaCl\(_2\); (ii) NH\(_4\)Cl; CCl\(_4\)

(d) Describe how the conductance of a molar solution of ammonia compares to that of sodium hydroxide solution.

(e) State the type of reaction illustrated by each of the following equations:

(i) CH\(_3\)CH\(_2\)OH\(_{(/)}\) + CH\(_3\)COOH\(_{(aq)}\) \(\rightleftharpoons\) CH\(_3\)COOC\(_2\)H\(_5\)\(_{(/)}\) + H\(_2\)O\(_{(/)}\)

(ii) H+\(_{Y^+_{(aq)}\) + OH\(^+_{(aq)}\) \(\to\) H\(_2\)O

(f) Determine the volume of the residual gas when 20.0cm\(^3\) of hydrogen was sparked with 15.0cm\(^3\) of oxygen and the resulting mixture cooled to room temperature.

 (a)(1) Define each of the following terms: I. deliquescence; II. efflorescence.

(ii) Give one example I substance that undergoes each of the processes in (a)(i).

(b) Outline how three colourless gases suspected to be ethane, ethene and ethyne could be distinguished in the laboratory.

(c)(i) What is water crystallization?

(ii) Hydrated calcium chloride (CaCl\(_2\) = 111, xH\(_2\)O) contains 49.32% water of cystallization. Calm the value of x. [ (CaCl\(_2\) = 111, H\(_2\)O = 18 ]

(d) Name one calcium compound used (i) in the manufactur cement; (ii) as a dessicant; (iii) in the production of plaster of Paris (POP);

(iv) to neutralise acidic soils

(e) A concentrated solution of sodium chloride was electrolysed using graphite electrodes.

(i) State the ions present in the solution

(ii) Name the products at the I. anode, II. cathode.

(iii) Give the by-product of the electrolysis.

(a) State Gay Lussac's Law.

(b) Carbon (II) oxide reacted with oxygen to form carbon (IV) oxide in a see tube.

(i) Write a balanced equation for the reaction.

(ii) If 40 cm\(^3\) of the carbon (II) oxide were mixed with cm\(^3\) of oxygen,

I. calculate the volume of carbon (IV) oxide produced

II. which reactant is in excess and how much?

III. what was the total volume of the gaseous mixture at the end of the reaction?

(c) Consider the following oxides: CaO, SiO\(_2\), CO, NO\(_2\) and ZnO. Which of the oxide(s) 

(i) is an acidic oxide that is insoluble in water?

(ii) reacts with water to give alkaline solution?

(iii) is amphoteric?

(iv) is neutral?

(v) is/are gaseous at room temperature?

(d) Explain why

(i) colourless concentrated trioxonitrate (V) acid turns yellow,

(ii) dilute trioxonitrate (V) acid does not liberate hydrogen when it reacts with magnesium.

(e) Write a chemical equation for the thermal decomposition of (i) Cu(NO\(_3\))\(_{2(g)}\)

(ii) NH\(_4\)NO\(_{3(g)}\)

 (a) State (i) Pauli's Excusion principle;

(ii) Hund's rule of maximum multiplicity.

(b)(i) Write the electronic configuration of each of the following ions of copper: I. Cu\(_+\) II. Cu\(_{(2+)}\) [\(_{29}Cu\)]

(ii) Give the number of unpaired-electrons in each of the ions in (b)(i) above.

(iii) State the type of reaction represented by the following equation:

2Cu\(^+_{(aq)}\) \(\to\) Cu\(^{2+}_{(aq)}\)  + Cu\(_{(s)}\)

(iv) Write the formula of one compound of Cu+.

(c)(i) Name the type  of radiation that will I. penetrate lead block; II. be stopped by thin paper

(ii) Give the charge on each of the radiations mentioned in I(c)(i) above.

(iii) What term is used to describe each of the following nuclear processes?

I. Combination of two lighter nuclei to form a heavy nucleus II. Splitting of a heavy nucleus into two or more lighter nuclei

III. Time required for one-half of the atoms of a radioactive substance to decay.

(d) Arrange the following ions in order of increasing size. Give a reason for your answer in each case. I. Li\(^{+}\), K\(^{+}\), Na\(^{+}\); II. O\(^{2-}\), F\(^{-}\), N\(^{3-}\)

(e) Determine the percentage composition of phosphorus and oxygen in phosphorus (V) oxide [ P = 31, O = 16 ]

(a)(i) Define in terms of electron transfer I. oxidizing agent; II. reducing agent.

(ii) Write a balanced equation to show that carbon in a reducing agent.

(iii) State the change in oxidation number of the specie that reacted with carbon in (a)((ii).

(b) A gas X has a vapour density of 32. It reacts with sodium hydroxide solution to form salt and water only. It decolourizes acidified potassium tetraoxomanganate (VII) solution and reacts with H\(_2\)S to form sulphur. Using the information provided:

(i) identify gas X; (ii) state two properties exhibited by X;

(iii) give two uses of X.

(c) Consider the following substances: sodium; lead (II) iodide; hydrogen; magnesium; oxygen. Which of the substances

(i) conducts electricity?

(ii) is produced at the cathode during electrolysis of H\(_2\)SO\(_{4(aq)}\)?

(iii) corresponds to the molecular formula A\(_2\)?

(iv) is an alkaline earth metal?

d)(i) Define the term salt.

(ii) Mention two types of salt

(iii) Give an example of each of the salts mentioned in (d)(ii) above.

(e) In a neutralization reaction, dilute tetraoxosulphate (VI) acid completely reacted with sodium hydroxide solution.

(i) Write a balanced equation for the reaction

(ii) How many moles of sodium hydroxide would be required for the complete neutralization of 0.50 moles of tetraoxosulphate (VI) acid?