CARIBBEAN EXAMINATIONS COUNCIL ADVANCED PROFICIENCYEXAMINATION
SPECIMEN PAPER MULTIPLE CHOICE QUESTIONS FOR CHEMISTRY UNIT 1- Paper 01 90 minutes
READ THE FOLLOWING DIRECTIONS CAREFULLY Each item in this test has four suggested answers lettered (A), (B), (C), (D). Read each item you are about to answer and decide which choice is best. Sample Item Which ofthe following is the highest energy transition in an organic compound? (A) (B) (C) (D)
n to er* n to n•
Sample Answer
cr to a* n to n•
@@•@
The best answer to this item is "cr to cr•", so answer space (C) has been blackened.
Copyright© 2005 Caribbean.ExaminationsCouncil ®. All rights reserved.
021120i0/SPEC2007
-2-
1.
When a Group I metal atom, Q, forms ion Q', the (A)
positive charge on the nucleus
(B) (C)
number of protons increases number of occupied electron shells decreases by one radius of the particle increases
5.
The molar volume of a gas at room temperature and pressure (r.t.p) is 24dm 3 • If 0.032g ofa gas occupies 48cm 3 at r.t.p., what is the molar mass?
increases
(D)
2.
Radioactivity is hazardous because it (A) (B) (C) (D)
(A) (B)
6.
can cause cancer and sterilization in human beings is accumulative and interacts with matter needs to be transported and disposed of properly has particulate as well as high energy
(C)
0.016g 2g 16g
(D)
64g
Propane is a fuel used in lamps. The equation for the combustion of propane is C,H, + 50 2 -+ 3C02 + 4H,0 What volume ofC02 is produced when 8.8g of propane is burnt in oxygen at r.t.p.? (The molar volume of gas at r.t.p.
=
24dm 3 )
emissions
3.
In which of the following compounds will hydrogen bonding NOT be present? (A)
C 2 H 51
(B) (C)
C 2 H5 0H CH 1 NH 2
(DJ 4.
(A) (B) (C) (D)
H,so,
Which of the following species has a structure with a bond angle less than 109° 28'?
7.
Which of the following are redox reactions? I. II. lll. IV.
(B)
NH+4
(C) (D)
CH, BF,
1.44 dm 3 4.8 dm' 14.4 dm 3 72 dm'
(A) (B) (C)
(D)
BaC/ 2 (aq) + H 2 SO.(aq) -+ BaSO.(s) + 2HCI (aq) 2H 20 2 (aq) -+ 2H20 (/) + 0 2 (g) NaOH (aq) + HCI (aq)-+ NaCl (aq) + H,0 (/) Fe 20 3 (s) + 2AI (s) -+ Al, 0 3 (s) + 2 Fe(~)
I and II only II and III only I and IV only II and IV only
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-38.
In the reaction between potassium manganate (VII) .and potassium iodide in acid solution, the following relevant half equations can be written: 2r
~
11.
12 + 2e-
What is the relative molecular mass of the gas?
Mn0; + 8W + se· ~ Mn''+ 4H 20 Which of the following is the overall balanced equation? (A)
Mno;
A mass of 25g of an unknown gas, X, is pumped through an industrial pipeline of volume 60m' at a pressure of 120 kPa and temperature of l 50°C. (Molar gas constant = 8.31 JK·' mol· 1 .)
(A) (B) (C) (D)
+8W+2r~Mn 2 '+4H,O
1.2 x I 0-2 4.3 x 10- 2 4.3 12.2
+ 12 (B)
Mno-4· +8W+2f~Mn 2 '+4HO 2 + 12 + 2e·
(C)
2Mno; + t6H'+ tor ~2Mn'' + ' 8H 20 + 51 2
(D)
2Mno; + 16W + 4f ~ 2Mn 2 ' + 8H 20 + 21 2
9.
12.
The melting points and boiling points of two pure substances, X and Y, are given below: Boiling point/K
273 317
373 400
x y
Which of the following statements about X and Y are correct? Which of the following is NOT true about a dynamic equilibrium?
I.
(A)
IL
(B)
(C) (D)
Macroscopic properties are constant. Microscopic processes are in balance. It is reversible. It cannot be achieved in a closed system.
III.
Item 10 refers to the following equation:
Y. At 380 K, the particles of Y are not mobile.
(A)
I and II only I and III only II and III only II and IV only
(C) (D)
c,H,NH,(g) + HNO,(aq) H 20(/) + N 2(g)
~
At 298 K, the particles of X can occupy the volume of its container. At 298 K, the particles of Y are in fixed positions. At 380 K, the particles of X have more energy than the particles of
IV.
(B)
10.
Melting point/K
C,H,OH(l) +
The volume ofnitrogen gas collected at r.t.p. when O.Olmol of ethylamine completely reacts with an excess of nitrous acid is (A) (B)
(C) (D)
0.224 dm 3 0.24 dm' 2.24 dm 3 2.40 dm 3
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02112010/SPEC2007
..
-4Items 13 and 14 refer to the following options. (A) (B) ( C) (D)
Enthalpy of formation Lattice energy Enthalpy of solution Enthalpy of hydration
Match EACH item below with one of the options above, each of which may be used once, more than once or not at all.
13.
Y(s) + O,(g)--+ Y0 2(g)
14.
XY(s) +water--+ XY(aq)
Item 15 refers to the diagram below which shows a Born-Haber Cycle for NaCl.
Na'{g) + Cl(g) + e·
-3 49 kJ mor 1
+436 kJ mo r1 Na+(g) + cr(g),, N a(g) + C l(g)
+122 kJ mor 1 Na(g) + y, Cl,(g)
+107 kJ mo r1 Na(s) + y, Cl,(g) -4llkJm 01· 1 Na+ Cr(s)
15.
•
What is the lattice energy of sodium chloride? (A) (B) (C) (D)
-727 kJ mol- 1 -95 kJ mol• 1 +663 kJ mol- 1 +727 kJ mol 1
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02112010/SPEC2007
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16.
The gen.eral form of a rate equation is given by: Rate= k [A]'[B]b
Item 18 refers to the following data for the rea~tion between propanone, iodine and hydrogen ions.
The rate constant, k, is defined as the rate of reaction when the concentration of each reactant (in mol dm·') is (A)
(B)
CH,COCH, + H+ + 12 --> ICH 2 COCH 3 + 2W + 12
0
Experiment number
I 2 3 4
2
(C) (D)
2
Item 17 refers to the data in the table, obtained for the reaction between molecules X and Y 111 500 K. The stoichiometric equation for the reaction is 2X(g) + Y 2{g)--> X 2 Y, (g) Experiment number
Initial concentration/ mol dm-
17.
Initial rate/ mol dm"3s· 1
Concentration/ mol dm-"
Reaction
Rate/ mol
CH 3 COCH 3
H+
I,
dm- 3 s" 1
0.1 0.2
0.1 0.1
0.1 0.1
0.2 0.2
0.1 0.1 0.1
0.04 0.08 0.08 0.08
0.2
The rate of reaction is given by Rate = k[CH 3COCH 3] ' [H+]' [12 ] ' 18.
The values of x, y and z are (A) (B) (C) (D)
x=l,y=l,z=l x=O,y= l,z= I x=l,y=l,z=O x = 0, y = 0, z = 1
3
x
y
I
0.01
0.02
2.4x 10·0
2
0.02
0.02
4.Sx 10·
3
0.01
0.01
1.2 x IO"
0
The correct orders of reaction with respect to X and Y are
x (A) (B)
y
0
2
2
0 0
(C) (D)
'
"'
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Item 19 refers to the graph which shows the Boltzmann distribution of kinetic energies in a gas.
Item 21 refers to the data in the table below.
No. of molecules with a given energy
21.
Gas
Equilibrium partial
N, H, NH3
a b c
pressure
What is the expression for Kp for the equilibruim N 2(g) + 3H,(g)
Energy
19.
(A)
Which statements are correct for the Boltzmann distribution?
(B)
Increasing temperature I.
II. Ill.
IV.
(A) (B) (C)
(D) 20.
(C)
causes the maximum of the curve to move to the right causes the maximum of the curve to move to the left increases the number of molecules with energy greater than the activation energy increases the number of molecules present in the gas
22.
Based on Le Chatelier's principle, which combination ofobervations is NOT true? Temperature change
Effect on
Effect on
K,,
reactants
(A)
Pndothermic
decrease
decrease
iocrease
(B)
Pndothermic
increase
increase
decrease
(C)
Exothermic
increase
increase
decrease
(D)
Exothermic
decrease
increase
decrease
2NH,(g)?
c' a 3b a3 b
7 ab
3
7 c'
(D)
I and III only I and IV only II and III only II and IV only
Type of reaction
i
Which of the following are Bronsted-Lowry acids? I. II. Ill. IV.
NH; cH,cooC,H,OH PH,
(A) (B) (C)
I and III only I and IV only II and III only II and IV only
(D)
23.
a b3
What is the K. value of 2.0 mol dm" NaOH(aq) at 298K? (A) (B) (C) (D)
2.0 1.0 1.0 4.0·
x 1.0 x I 0- 14 x I 0- 14/2.0 x I 0- 14 x I 0- 14
• ;
''
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24.
Which of the following indicators would be suitable for use in titrating a strong acid against a weak base?
27.
Indicator
pH range
(A)
L IL llL
8romophenol blue Methyl red Alizarin yellow
2.8 - 4.6 4.2 - 6.3 10.I - 13.0
(8)
(A) (8) (C)
I only I and II only II and Ill only I, II and Ill
(D)
(C) (D)
28.
25.
When solid silver chloride is added to a solution of potassium iodide, a yellow precipitate of 'silver iodide forms because
A buffer solution consists of ethanoic acid and sodiull'I ethanoate solution.
w
L
CH,coo· +
IL
CH, coo· + NH/--> CH,COONO,
IIL
CH,COOH + HCO,· --> CH,coo· + H20 + C0 2
IV
CH,COOH + OH' --> CH,coo- +
H,0 (A) (8)
(C) (D)
(8) (C)
--> CH,COOH
I and Ill only I and IV only II and Ill only II and IV only
(D) 29.
,,
Which of the following is NOT a standard condition for measurement of electrode potentials? (A)
Which equations show how the buffer maintains constant pH in solution?
chlorine is more electronegative than iodine potassium chloride and potassium iodide are both soluble silver chloride has a lower K value than silver iodide silver iodide has a lower K ,, value than silver chloride
Solutions have a concentration of I mol dm·'. Gases have a pressure of I atmosphere. Temperature is 25"C. Metal alloys are used as electrodes.
Which pair of half cell potentials would produce an E0 N of 1.1 when combined to form a cell? (A) (B)
(C) (D)
Cu2 '(aq)/Cu(s) and Fe 1'(aq)/Fe 2'(aq) Cu 2 '(aq)/Cu(s) and Zn 2 '(aq)/Zn(s) A/3'( aq)/ Ai( s) and Zn''( aq)/Zn(s) Ag'/Ag(s) and Cu 2 '(aq)/Cu(s)
Item 26 refers to the following reaction: CH,COOH(aq) ~ H'"(aq) +CH, C009 (aq) [sodium ethanoate] = 0.5 mol dm·' and [ethanoic acid] = 03 mo! dm·' 26.
Given that K, = LS x IO-', what is the pH of the buffer solution? (A) (8)
~·
(C) (D)
•'•
3.25 4.97 6.50 9.94
02112010/SPEC2007
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•
30.
-8The standard electrode potentials for dichromate and iodide are:
Items 31 and 32 refer to the graphs below which show trends displayed by elements in Period 3.
1/2 Cr,O/ (aq) + 7H+(aq) + 3e-i Cr'+(aq)
+ 7/2 H 20 I,(aq) + 2e·
(A)
+ 1.33 V
t
2I·(aq)
+ 0.54 V
From this it can be deduced that (A) (B)
( C) (D)
acidified dichromate ions would oxidise iodide ions to iodine electrons would flow from the dichromate half cell to the iodine half cell if the two are connected iodine would oxidise chromium (III) ions to dichromate combining both half cells would produce a cell potential of I. 87 V
Na Mg Al
Si
P
S
Cl
Na Mg Al
Si
P
S
Cl
Na Mg Al
Si
P
S
Cl
Na Mg Al
Si
P
S
Cl
(B)
(C)
(D)
In answering Items 31 - 32, makh each item with one of the graphs above. Each graph may be used once, more than once or not at
all.
31.
Atomic radius
J2.
Firit ionmtion ener&Y
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•
-9Items 33 and 34 refer to the following oxidation states. (A) (B) (C) (D)
37.
+I +3
Group IV elements show an increaseing tendency towards metallic character as atomic number incFeases. Which of the following may account for this? I.
+6 +7
II.
Match each element below with one of the options above, each of which may be used more than once, once or not at all
i
I
III.
(A) (B) (C) (D)
33. 34.
Na,o
35.
Which of the following has a simple molecular s!ructure? (A)
(B) (Cl
(D) 36.
Sodium oxide Magnesium chloride Aluminium chloride Silicon (IV) oxide
In descending Group II of the periodic table, the first ionization energy value of the elements decreases. This is due to which two of the following? I.
ll.
m. IV.
(A) (B) (C) (D)
38.
39.
The electronegativity of the atoms decreases. I and [[ only I and Ill only II and Ill only II and IV only
(A) (B) (C)
co,
(D)
Si02
40.
Sn02 PbO
The decrease in volatility going down Group Vll can be described by all of the following statements EXCEPT
(B) (C) (D)
ionic radius decreases. Each succeeding atom has one more quantum shell than the other.
I only II only Ill only II and Ill only
Which of the following oxides of elements in Group IV is the LEAST acidic in character?
(A)
Atomic radius increases down the group. Electrons are more delocalised as
The +2 state becomes more stable than the +4 state. The +4 state becomes more stable than the +2 state. The valence electrons in the +4 state do not take part in bonding.
strength of van der Waals forces increases electropositivity increases size of atoms increases molecular mass increases
A student tests an unknown sample with a few cm' of AgNO/aq) followed by a few cm' of dilute NH/aq). Which of the following observations would confirm that the sample contains the Br- ion?
Precipitate with A2No3 Dissolves in dilute NH,
(A)
(B)
(C)
(D)
white
white
off-white
sparingly
readily
sparingly
offwhite readily
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•
- 10 -
Transition metal complexes contain a central metal atom or ion surrounded by ligands. Which of the following does NOT explain why these complexes are formed?
41.
(A) (B) (C) (D)
Vacant d-orbitals on the metal atom orion The presence of lone pairs of electrons on ligands The formation of covalent bonds between the metal and ligands The complex ion formed is stable with respect to its constituents
Item 44 refers to the following information: An unknown salt sample, FA!, is subjected to analysis and the results are shown in the· table. · ·· Reaction Kl(aq) +FA! (aq) NH 3 (aq) + FAl(aq)
44.
Which of the following represents the electronic configuration of Mn'+?
No visible reaction White precipitate, insoluble in excess NH 3(aol
It can be deduced that the cation is MOST likely (A)
42.
Results
(B)
(C) (D)
AP+ Zn 2 + Na+ Pb 2 +
'Note: [Ar]= ls', 2s 2 2p6 , 3s 2 3p6 3d (A)
[Ar]
(B)
[Ar]
4s
It It It It It I 3d
4s
It It It It I 3d
[Ar]
(C)
It It It I 3d
[Ar]
(D)
43.
It It I
[ill
I
I
D4s D4s
[ill
Transition metals can exhibit more than one oxidation state because they (A) (B) (C)
(D)
have more than one free electron exist in different colours have similar energy levels for 3d and 4s have incomplete d-orbitals
0211201QISl>EC2007
45.
When silver nitrate solution followed by dilute ammonia is added to a solution containing chloride ions, which of the following is the formula for the complex formed? (A) (B) (C) (D)
Ag(NHJ AgNH 2 [Ag(NH 3) 2]' [Ag(NH),]'+
• CHEMISTRY Specimen Paper 2007 UNIT I Paper 01 Item Number I
Key
2 3 4 5 6 7 8 9
D A A
JO
11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30
'
c c c
D
c
D
B D
c A
c A
c
D
c A
c D A
c B B B D D
B A
Item Number
31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 55 56 57 58 59 60
Key
c
A
B A
c B A
B B
c
D
B
c A
c
