2. Section A consists of THREE stilldured questions, one from each Module. Section B consists of THREE 'xll'nded response questions, one from each Module.
3. For Section A, write your answel'I<ill the spaces provided in this booklet. For Section B, write your answers inIII-answer booklet provided.
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(b) Intermolecular forces ofattraction influencl.'III ph kill prop 'I,ties orsubstances, such as, their melting points, boiling points, and Illuh
lit
II POIIlI lInd non-polar solvents. Consider the structure of the following Nuh tllIl •follow.
o
II H3C-C-CH3 H II I I HC-C-(' II 3 I I H Oil (B) I-propullill II Ii H H I I I I II C- -C-C-H I I I I II Ii H H (C') butane(i) Plac~ substances A,Band C in order onlll" (IIrein"hoiling point (lowest boiling
point first).
(ii) Identify the intermolecular attra<.:liVl'fill'l' (hundill !\!\CII of the substances
(iii) Describe the origin of TW(IIll'the intermolecular attractive fore'N 11t1l11~·tlIII (b)(ii).
(c) Complete Table 1 by indicating wllt·tlt 'I'EACH of the substances, potassium bromide, acetone and solid iodine are solubl'Ill insoluble in the two solvents, water (polarsolvent) and toluene (non-polar solvent).
Substance Water (Polar) Toluene (Non-polar)
0
Potassium bromide
Acetone Soluble
Describe, IIsing FI Y I,l' fl'lIl illIsleps, an ex Iwrltl) \111wllkh t'lll1be Llsed to determine the
solubility rrodu ,( III ('11( )11)) al room kl11lwrlltlll .
(b) The solubility product, K,p' at 25°C for cuklllln IlthonIt ( u 03) was found to be
(c) Calculate the solubility ofcalciul11lllrhonate (!<.p=5.0 x10-9moP dm--6at2
"
e)
in(i) pure water
[3 marks]
(d) What is responsible for the differen~' between the solubilities in (c) (i) and (c) (ii)above?
[1 mark] Total 15 marks
(b) A student was provid 'd with three test tubtN. JlA< '1ll'Olltlltnillg one hydrogen halide.
A red hot wirl.:(l:xcl.:(,;dingJOO0c) was qllidd pllll"d Illln cuch test tube in turn. The
observations Wl.:rc1'l:(;()I'(kd in Table 2.
Test Thbe Ilydrogcn Halide I Ilydrogcl1 chloride
-II Ilydrogl.:n bromide SIII Ilydrogen iodide (
(iii) Using the rl.:levant information provid d illIII•dutu booklet, explain the trend in the observations recorded inTable _.
(c) Concentrated sulphuric acid was car·f\.lIlyadded to test tubes containing sodiumchlorid
and sodium bromide respectively.
(d) The products of the reaction in(c) (i) above were passed into water and the resultant
MODULE 1 FlINDAMENTALS IN ('IU.I\1!,·TI~ ' State TH REE filctOIHwhit'll 1Ifleet the first 10111 IIIhill 11'1 01Ih I m nts.
13
marks] (i) Cu (ii) 02 (iii) Mn2' (iv) Fell (v) Ca(c) Explain how ionization energy data provitk I IIIH Inl II II "ml lib'hells.
[3 marks]
(d) Study Figure I which shows the logarithm III III 1111 III II tl 1I'ccssive ionisation energies of an elcmcnt and answer the qUQ IOil \ hhIIII
!low
,
;;., 4 b1l I. Q) C Q) c .$2
.
•..
c<l '"'i::
.$2 <:> 3..
.
b1l .£ 2 3 4 5 6 7 8 9 10 II 11 l:l 14 15 16 17 18 19Number ofthr IUIIIHIIIIIIII
(i) Write the electronic configullItiol1 of the element represented in Figurl; I.
II murk
I
(iii) Write a balanced equation tn Illustrate the first ionisation of the element.
12 ma.·ksl
MOI)l)LJ~ 2
KINETICS AND l';QUILIBRIA
Copy and complete Table. 10 show the type of equilibrium for the selected equilibrium systems.
System
Number Equilibrium System Type of Equilibrium
Saturated solution
or
a salt at I room temperatureThe vertical balalll'ing of a ruler 2 on a flat surface
3 Heating of limestolle at 800°C
(ii) State TWO characteristics (If the equilibrium represented by System I in
Table 3. L2marks]
Substances A,-B, X and Y form an quilibrium mixture represented by the equation below.
(ii) What deduction can be made when the equilibrium constant is much greater
(c) When sol id bislllut Ii (III) chloride, BiClj i ulld d III 1111'1, II hit prt;cipitate BiOCI is
produced. Thl.:s· '\lI11pnullds form an cqullilll hllllllil 1111 1 pl' ~·1l1I.:dby the equation
(i) Explain wll tile wllile precipitate. UI()('I,tli IIPI III tilt Ih IIddilion ofaqueous Helto the ·qllllihrilll11 mixture. 12 mnrksl
(ii) Explain wllot would he observed if'II lllf/1C olllfn 01WlIl I Wll, lidded to the
cquilibrilllll I\\I:-.t\ll\:.
13
mllrksl(d) Phosphorus(V) ellIllI'i(!l',1'('I,. decomposl.:s iiI (I" IIIHllortllflun ·quilibrium mixture represented by Ill, (1'101\(111
One equilibrium Inixturc III this temperutul' 'ontnin PCI~und PCIJ at concentrations
of 0.20 mol dm Itlnd(J.() I() mol dm-J rcsp cli 1. Given Kc at 250 fI('
mixture.
0.19 mol dm 1, cllh:lIIUI' III 'oncentration ofCl2 in the
(i) State the general trend inIIlomicradii in moving from left to right II On) N
Period 3 (from sodium to al' \Ill). 11 murk
I
(b) Each element in Period 3 exhibits \III1of three structures: simple molecular, gillut metallic or giant molecular.
(c) Study Figure 2 which shows the vlIl'llItionin melting points across the elements in Period 3 and answer the question thai follows.
With reference to structure and bonJing, account for the variation in melting points
Sketch tl sitwlUI dillHllllll to Figurt' #c II •'11ill Cl (I') IIIillustrate the variation in
th' clcclrkul CllllUUl'tivity of the t'l'llH III hi I' I lid.L [2 marks]
With r'("fell' 10 'tl"Uclure, exrlll 11III (d) (i)ab()Vt',
huwn on your sketch in
13marks]
Describe lh' ICUrllllll which ocellI.
gas.
hIII 1111I1'11 11111i heuted in dry chlorine
