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Junior Freshman Annual
Department of Chemistry
Wednesday 19 May
Multiple Choice Test
RDS
Trinity Term, 2004
Chemistry Paper II
Answer All questions
The use of Log Tables is permitted.
14.00 - 16.00
A Periodic Table giving Atomic Weights etc., and a Table of fundamental constants is attached.
INSTRUCTIONS
1. Using a soft pencil (grade B or softer) complete sections A, B, C and D on the
Computer Answer Form. Write your student number in Section D as well as marking the number on the form by filling in the box with a clear thick horizontal line ( not a

, X or 0).
GOOD BAD BAD BAD BAD
2. Answer each question by first marking on the question paper the answer that you think is appropriate. Do not mark more than one answer to each question. In questions with numerical answers, mark the answer closest to yours, if you do not get exactly any of those given.
3. Carefully transfer your answers to the Computer Answer Form. If you make a mistake, rub it out with a CLEAN eraser and enter the correct answer.
Use only a soft pencil and mark your answers with a clear thick horizontal line. Failure to do this could result in the misreading of your form. Do not write comments on the form.
4. When you have finished, make sure your name, student number and seat number are on the Computer Answer Form and hand it up to the invigilator. Do not in any way tear, crumple or deface the form. This form is the only record of your answers.
5.
There will be no negative marking for this exam .

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1. The mass (in grams) of FeSO
4
 7H
2
O required for preparation of 125 mL of
0.90 M solution is:
(a) 16 g
(b) 25 g
(c) 31 g
(d) 13 g
(e) 43 g
Correct Answer (c)
2. Which assignment of oxidation number is incorrect for the underlined element?
(a) K
2
Cr
2
O
7
; +6
(b) SeO
3
2

; +4
(c) H
2
PO
2

; +1
(d) NH
3
; +3
(e) Cu(NO
3
)
2
; +2
Correct Answer (d)
3. What is the standard enthalpy change for the reaction:
2NOCl (g)

N
2
(g) + O
2
(g) + Cl
2
(g).
Given that:
½ N
2
(g) + ½ O
2
(g)

NO (g)

H = +90 kJ
NO (g) + ½ Cl
2

NOCl (g)
(a)

100 kJ
(b)

130 kJ
(c)

50 kJ
(d) +1005 kJ
(e) +170 kJ
Correct Answer (a)

H =

40kJ

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4. Consider two identical flasks containing equal masses of gas: the first contains pure Ar, the second pure He. Unless otherwise indicated assume the temperature is the same for both. Identify which of the following statements are incorrect .
(i) There are equal numbers of molecules in each flask.
(ii) The molecules in the Ar flask have a lower average kinetic energy.
(iii) The molecular mean free path is larger in the Ar flask.
(iv) The pressure is higher in the Ar flask.
(v) The pressure in both flasks can be made equal by heating the Ar flask.
(a) (i) and (ii)
(b) (i), (ii) and (iii)
(c) (i), (ii) and (iv)
(d) (i), (iii) and (v)
(e) (ii), (iii) and (v)
Correct Answer (c)
5. Consider a thermodynamic process in which a drop of water evaporates to form water vapour. Identify which of the following statements are correct .
(i) The entropy of the system has increased.
(ii) The entropy of the surroundings has increased.
(iii) The entropy on the universe has increased.
(iv) Heat was transferred from the surroundings to the system.
(v) The free energy of the system has increased.
(a) (i) and (iii)
(b) (ii) and (iii)
(c) (i), (ii) and (iv)
(d) (i), (iii) and (iv)
(e) (ii), (iii) and (v)
Correct Answer (d)

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6. Deuterons (a deuteron is a nucleus consisting of a proton-neutron pair) in a beam are travelling with a uniform velocity of 990.4 m s

1 .
They have a wavelength of:
(a) 2.00

10

10
m
(b) 4.00

10

12
m
(c) 2.00

10

15
m
(d) 4.00

10

8
m
(e) 2.00

10

6
m
Correct Answer (a)
7. Which combination of answers is correct ?
The Mn
3+
ion:
(i) has a greater number of unpaired electrons than Cr
2+
(ii) has the same number of unpaired electrons as Cr
2+
(iii) has the same number of unpaired electrons as neutral Mn
(iv) can lose an electron to create an ion with a greater spin
(v) can lose an electron to create an ion with the same spin as Co
2+
.
(a) (i) and (iv)
(b) (ii) and (v)
(c) (iv) and (v)
(d) (iii) only
(e) (ii) and (iii)
Correct Answer (b)

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8. Which one of the following statements about the carbon dioxide molecule is true ?
(a) the electron pair lobes on the central atom are tetrahedral, resulting in a bond angle of about 109°
(b) the electron pair lobes on the central atom are trigonal, resulting in a bond angle of about 120°
(c) the structure is stabilized by resonance between single and double
CO bonds
(d) the molecular structure is linear
(e) the central atom has an expanded octet.
Correct Answer (d)
9. The molecular orbital description of F
2
+
shows that the molecular ion:
(i) is paramagnetic
(ii) could lose an electron to produce a half-filled molecular orbital
(iii) could lose an electron to produce an ion whose total spin is the same as that of a N
2
molecule
(iv) has a bond order which is greater than that of F
2
(v) has a bond order which is less than that of O
2
.
(a) (i) only
(b) (i) and (ii)
(c) (iii) and (iv)
(d) (v) only
(e) (i), (ii), (iv) and (v)
Correct Answer (e)

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10. For the salt AgCl the lattice enthalpy is

916 kJ mol

1 and the sum of the hydration enthalpies of the ions is

832 kJ mol

1 . Which of the following statements are correct.
(i)

H for solution = + 84 kJ mol
-1
(ii)

H for solution = –1748 kJ mol
-1
(iii) the solubility of AgCl in water decreases with temperature
(iv) AgCl is only sparingly soluble.
(a) all
(b) (i) and (iv) only
(c) (ii) and (iv) only
(d) (ii) and (iii) only
(e) None
Correct Answer (b)
11. For the reaction
2NO + 2H
2
→ N
2
+ 2H
2
O the following data was obtained:
[NO]
(mol dm

3
[H
2
]
) (mol dm

3
Rate
) (mol dm

3
s

1
)
5 x 10

3 2 x 10

3
10 x 10

3
5 x 10

3
2 x 10
4 x 10

3

3
2.4 x 10

5
9.6 x 10
4.8 x 10

5

5
10 x 10

3
4 x 10

3
19.2 x 10

5
The rate (mol dm

3 s

1 ) of reaction is:
(a) 24 [NO][H
2
]
(b) 480 [NO] 2 [H
2
]
(c) 240 [NO][H
2
]
(d) 48 [NO] 2 [H
2
] 2
(e) 2400 [NO]
Correct Answer (b)

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12. The rate of the reaction:
A+B
2
→ AB + B is directly proportional to the concentration of B
2
but independent of A.
Which of the following statements is correct ?
(a) The reaction obeys second order kinetics
(b) The mechanism involves a single bimolecular reaction step
(c) The mechanism may be
B
2
→ 2B slow
B + A → AB fast
(d) The mechanism may be
A + B
2
→ AB
2
slow
AB
2
→ AB + B fast
CH1S002
Correct Answer (c)
13. Which of the following statement(s) is /are incorrect ?
(i) If two liquids A and B undergo ideal mixing
∆
H mixing
= 0
(ii) In the above case,
∆
G mixing
=

T∆S mixing
(iii) The vapour pressure above an ideal solution of two liquids A and B will be equal to x
A
P
A o
+ x
B
P
B o
, where x
A
and x
B
are the mole fractions of A and B and P
A o
and P
B o
are their standard vapour pressures
(iv) All solutions exhibit ideal behaviour if sufficiently dilute
(a) all
(b) (i) and (iii) only
(c) (iii) and (iv) only
(d) (ii) only
(e) (iv) only
Error in question

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14.
Electrophilic addition of bromine to cyclohexene yields:
(a)
(b) cis cis
-1,2-dibromocyclohexane
-1,1-dibromocyclohexane
(c)
(d)
(e) trans trans trans
-1,2-dibromocyclohexane
-1,1-dibromocyclohexane
-1,3-dibromocyclohexane
Correct Answer (c)
15.
The reaction of 2-chloropropane with cyanide ion is:
(a) first order
(b) second order
(c) an S
N
1 reaction
(d)
(e) a free-radical reaction none of the above
Correct Answer (b)
16.
Which of the following is the strongest acid?
(a) ethanoic acid
(b) 4-methylbenzoic acid
(c) 2-chloroethanoic acid
(d) 2,2-dichloroethanoic acid
(e) carbonic acid
Correct Answer (d)
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17.
Alkoxide ions react with alkyl halides to give:
(a)
(b) ethers esters
(c) acetals
(d) alcohols
(e) alkanes
Correct Answer (a)
18.
The reaction of but-1-yne with aqueous acid in the presence of Hg
2+
ions gives:
(a) but-1-ene
(b) butan-2-ol
(c) butyric acid
(d) butan-2-one
(e) butanal
Correct Answer (d)
19.
A nucleophile should possess:
(a) an overall positive charge
(b) an unpaired electron and a positive charge
(c) an unpaired single electron
(d) a lone pair of electrons
(e) no charge
Correct Answer (d)

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20. Which one of the following compounds contains the greatest number of sp
2 hybridised carbon atoms?
(a) phenylethene
(b) phenylethyne
(c) cyclohexanone
(d) cyclohexanol
(e) ethane
Correct Answer (a)
21.
The correct IUPAC name for the following compound is:
(a) 4,5,5-trimethylpent-1-ene
(b) 4-methyl-4-isopropylbut-1-ene
(c) 3,5-dimethylhex-1-ene
(d) 2,4-dimethylhex-5-ene
(e) 4-isopropyl-4-methylbut-1-ene
Correct Answer (d)
22.
The dominant product from the reaction between propene and HCl is:
(a) 1-chloropropane
(b) 2-chloropropane
(c) 1,2-dichloropropane
(d) 1-chloropropane and 2-chloropropane are formed in equal amounts
(e) propyne
Correct Answer (b)

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23.
Hydrolysis of a carboxylic ester using aqueous sodium hydroxide gives:
(a) a sodium carboxylate and an alcohol
(b) a carboxylic acid and a sodium alkoxide
(c) a carboxylic acid and an alcohol
(d) a carboxylic ether
(e) a carbocyclic triol
Correct Answer (a)
24.
Reaction of a primary aliphatic amine with aqueous nitrous acid gives:
(a)
(b) an amide a nitro compound
(c) an amidic acid
(d) an alcohol
(e) a nitrile
Correct Answer (d)
25. For a solution labelled 0.2 M barium hydroxide, which of the following is correct ?
(a) [OH
-
] = 0.4 M ; [Ba
2+
] = 0.2 M
(b) [OH
-
] = 0.2 M ; [Ba
2+
] = 0.1 M
(c) [OH
-
] = 0.2 M ; [Ba
2+
] = 0.4 M
(d) [OH
-
] = 0.4 M ; [Ba
2+
] = 0.4 M
(e) [OH
-
] = 0.2 M ; [Ba
2+
] = 0.2 M.
Correct Answer (a)

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26. A buffer solution contains 0.5 M acetic acid (K a
= 1.8 x 10
–5
) and 0.5
M sodium acetate. The pH of the solution is :
(a) 4.74
(b) 1.00
(c) –0.3
(d) 3.74
(e) There is not enough information provided to solve the problem.
Correct Answer (a)
27. The standard potential of the cell Pb(s) Pb
2

(aq) Cl

(aq) AgCl(s) Ag(s) is 0.35 V at 298 K. If the standard potential of the Pb, Pb
2+
couple is – 0.13 V, calculate the standard potential of the Ag/AgCl, Cl
–
couple.
(a)
– 0.22 V
(b) 0.48 V
(c) – 0.48 V
(d) 0.22 V
(e) – 0.35 V.
Correct Answer (d)
28. Given :
Ag

(aq)
 e
 
Ag(s)
Fe 3

(aq)
 e
 
Fe 2

(aq)
Cu
2

(aq)

2e
 
Cu(s)
E
0 
0.80
V
E
E 0
0 

0.77
V
0.34
V
Which is the strongest reducing agent ?
(a) Cu
(b) Fe
2+
(c) Ag
+
(d) Ag
(e) Cu 2+ .
Correct Answer (e)

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29. From the description below, what is the most probable identity of E ?
‘The element E is a monoatomic gas which reacts with O
2
and F
2
only. The formation of EF
2
(linear), EF
4
(square planar) and EF
6
occurs on reaction of F
2 with E under different conditions.’
E is :
(a) Hydrogen
(b) Helium
(c) Nitrogen
(d) Sulfur
(e) Xenon
Correct Answer (e)
30. The mineral corundum is aluminium oxide Al
2
O
3
. Corundum gemstones can have different colours because of:
(a) the presence of organic impurities
(b) the presence of silicate ions
(c) the presence of transition metal ions
(d) the presence of water of crystallization
(e) particulate matter trapped in the oxide
Correct Answer (c)
31. These two elements have a diagonal relationship. They exhibit the electrical properties of semiconductors. The elements and their oxoanions occur in extended covalent networks. Both elements form acidic hydroxides. These elements are:
(a) silicon and boron
(b) lithium and magnesium
(c) beryllium and aluminium
(d) iron and copper
(e) carbon and sulfur
Correct Answer (a)

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32. Salts of this metal element are present in seawater and have an important biological role. The metal ion is involved in phosphate metabolism and is present in chlorophyll. Salts of this metal are used in the treatment of indigestion and constipation.
The identity of the metal element is:
(a) copper
(b) magnesium
(c) sodium
(d) lithium
(e) barium
Correct Answer (b)
© University of Dublin 2004

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Use the following values for fundamental constants, conversion factors, atomic masses and other data for examination purposes:
Constants
Gas Constant
Boltzmann’s Constant
Planck’s Constant
Velocity of light
Charge of electron
Rest mass of electron
Rest mass of proton
Vacuum permittivity
Vacuum permeability
Bohr magneton
Nuclear magneton
Rydberg constant
Avogadro’s constant
Faraday constant
Bohr radius
Molar volume at S.T.P.
R = 8.314 J K

1 mol

1
(R = 8.206

10

2
L atm K

1
mol

1
) k
B
= 1.381

10

23
J K

1 h = 6.626

10

34
J s
 = h/2

= 1.055

10

34 J s c = 2.998

10 8 m s

1 e =

1.602

10

19 C m e
= 9.109

10

31 kg m p
= 1.673

10

27 kg
 o
= 8.854

10

12
J

1
C
2
m

1
 o
= 4
 
10

7
J s
2
C

2
m

1

= 9.274

10

24
J T

1
 n
= 5.051

10

27
J T

1
R  = 2.178

10

18
J = 1.097

10
5
cm

1
N
A
= 6.022

10
23
mol

1
F = N
A e = 9.648

10
4
C mol

1 a o
= 5.292

10

11 m
M v
= 22.414 dm 3 mol

1
Conversion factors etc.
1 eV = 1.602

10

19
J = 9.648

10
4
J mol

1
1 cm

1
= 1.986

10

23
J = 11.96 J mol

1
= 1.240

10

4 eV
1 Å = 0.1 nm = 10 
10
m
1 standard atmosphere = 1.013

10
5
N m

2
(Pa) = 760 torr = 1013 mbar
1 L = 1 dm
3
= 10

3 m
3
1 Debye (D) = 3.336

10

30
C m
1 calorie = 4.184 J
1 L atm = 101.34 J

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1
1
3
2
1.0079
4
11
6.941 9.01218
12
3 4
22.98977 24.305 3d, 4d, 5d
19 20 21 22
( ) mass numbers of most stable isotope
5 6
The Periodic Table of the Elements
7 8 9 10 11 12
5
13 14 15 16 17
6 7 8 9
18
2
4.0026
10
13
10.81 12.011 14.0067 15.9994 18.9984 20.179
14 15 16 17 18
26.9815 28.0855 30.9738 32.06 35.453 39.948
31 32 33 34 35 36 23 24 25 26 27 28 29 30
39.0983 40.08 44.9559 47.88 50.9415 51.996 54.938 55.847 58.9332 58.69 63.546 65.38 69.72 72.59 74.9216 78.96 79.904 83.80
37 28 29 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54
85.4678 87.62 88.9059 91.22 92.9064 95.94 (97.9) 101.07 102.9055 106.42 107.868 112.41 114.82 118.69 121.75 127.60 126.9045 131.29
55 56 57 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86
#
132.9054 137.33 138.9055 178.49 180.9479 183.85 186.207 190.2 192.22 195.08 196.9665 200.59 204.383 207.2 208.9804 (209) (210) (222)
87 88 89
(223) 226.0254 227.0278
#
LANTHANUM SERIES
58 59 60
* ACTINIUM SERIES
61 62 63 64 65 66 67 68 69 70 71
140.12 140.9077 144.24 (145) 150.36 151.96 157.25 158.9254 162.50 164.9304 167.26 168.9342 173.04 174.967
90 91 92 93 94 95 96 97 98 99 100 101 102 103
232.0381 231.0359 238.0389 237.0482 (244) (243) (247) (247) (242.1) (254) (257) (258.1) (259.1) (260)