Name: __________________________ Date: _____________



1.
Give, from left to right, the oxidation number of the central metal atom for
the following coordination compounds.

K3[Fe(CN)6],   [Cr(NH3)4Br2]Br,    [Ni(H2O)6]Cl2,    Na2[TaF7]
A.
3, 3, 3, 5
B.
3, 3, 2, 7
C.
–3, 3, 2, 5
D.
–3, 1, 2, 5
E.
3, 3, 2, 5


2.
Which of the following coordination compounds will form a precipitate
when treated with an aqueous solution of AgNO3?
A.
[Cr(NH3)3Cl3]
B.
[Cr(NH3)6]Cl3
C.
None of the compounds in the other choices.
D.
Na3[Cr(CN)6]
E.
Na3[CrCl6]


3.
Which of the following complexes shows geometric isomerism?
A.
[Co(NH3)5Cl]SO4
B.
[Co(NH3)6]Cl3
C.
[Co(NH3)5Cl]Cl2
D.
K[Co(NH3)2Cl4]
E.
none of the complexes given in the other choices


4.
The number of geometric and optical isomers for the complex ion [Co(en)2Cl2]+ is:

     Geometric         Optical
A.
       2                    2
B.
       0                    2
C.
       2                    0
D.
       3                    2
E.
       2                    3


5.
According to crystal field theory, how many unpaired electrons are present in
the complex ion [Fe(H2O)6]3+? The water molecules are weak field ligands.
A.
1
B.
2
C.
3
D.
4
E.
5


6.
What are the respective names of K3[Fe(CN)6] and [Cr(NH3)4Br2]Br ?
(The correct choice has both names given correctly)
A.
Potassium hexacyano iron(III);   Tetraamminedibromochromium(III) bromide
B.
Potassium hexacyano ferrate(III); Triamminedibromochromium(III) bromide
C.
Potassium hexacyano ferrate(I);   Tetraammoniadibromochromium(II) bromide
D.
Hexacyano iron(III) potassium; Tetraammoniumdibromochromium(II) bromide
E.
Potassium hexacyano ferrate(III); Tetraamminedibromochromium(III) bromide


7.
The central atom in Hemoglobin is:
A.
Co3+
B.
Mg2+
C.
Fe2+
D.
Sc3+
E.
Zn2+


8.
Which of the following is paramagnetic?
(NH3 , ethylenenediammine (en) and CN– are all strong-field ligands)
A.
[Zn(H2O)6]2+
B.
[Co(NH3)6]3+
C.
[Fe(CN)6]4–
D.
[Mn(CN)6]2–
E.
[Co(en)3]3+


9.
Which of the following elements produces strong steel when added
to iron in the correct amount?
A.
copper
B.
phosphorous
C.
sulfur
D.
carbon
E.
zinc


10.
Name the following:
A.
n-heptane
B.
2-methyl-2-ethylbutane
C.
3,3-dimethylpentane
D.
2,2-diethylpropane
E.
2-ethyl-2-methylbutane


11.
Which of the following types of compounds must have an
sp2-hybridized carbon center?
A.
ethers
B.
ketones
C.
alcohols
D.
alkanes
E.
amines


12.
Which of the following choices are correct for chloropropene?

     No. of Structural isomers                   No. of Geometric isomers
A.
                   3                                                    2
B.
                   2                                                    3
C.
                   3                                                    0
D.
                   0                                                    4
E.
                   2                                                    1


13.
Which of the following has an optical isomer?
A.

B.

C.

D.

E.
none of the other choices.


14.
Which of the following pairs of substances can form a polyester?
A.
H2C=CHCH3 + HOCH2CH2COOH
B.
HO(CH2)4COOH + HOCH2CH=CHCH3
C.
H2C=CHCN + H2C=CHCH3
D.
HOCH2CH2OH + HOOCCOOH
E.
H2NCH2COOH + H2NCH2CH2COOH


15.
Which is a possible product of the chlorination of butane in the presence of light?
A.
C4H9Cl
B.
C4H8Cl
C.
C4H10Cl2
D.
C4H6Cl2
E.
C4H9Cl2


16.
When C4H8 is treated with water and H2SO4 a tertiary alcohol is produced.
Which of the following structures could represent C4H8 in this reaction?
A.
CH3CH = CHCH3
B.
CH3CH2CH = CH2
C.

D.
CH3CH2CH2CH3
E.
none of the other choices


17.
Name the following compound:

             
A.
2-chloro-3-ethyl-1-isopropylbutanone
B.
isopropyl-chloro,methylbutyl ketone
C.
2-butyl,chloro,isobutanoyl methane
D.
4-chloro-2,5-dimethyl-3-heptanone
E.
3-methyl-4-chloro-1-isopropylpentanone


18.
Oxidation of 2-propanol will produce
A.
an aldehyde.
B.
an amine.
C.
an alkene.
D.
a ketone.
E.
a carboxylic acid.


19.
Which of the following oxides is amphoteric?
A.
BeO
B.
MgO
C.
CaO
D.
SrO
E.
BaO


20.
The hydride formed when a transition metal crystal is treated with hydrogen gas is:
A.
A covalent hydride
B.
An interstitial hydride
C.
An active hydride
D.
A saltlike hydride
E.
An ionic hydride


21.
Which, among the following elements, is most metallic?
A.
N
B.
P
C.
As
D.
Sb
E.
Bi


22.
Which Group 5A element cannot form molecules with five covalent bonds?
A.
N
B.
P
C.
As
D.
Sb
E.
Bi


23.
Which of the following statements is not correct?
A.
The molecule is paramagnetic.
B.
The bond energy of is greater than the bond energy of .
C.
The oxidation state of the sulfur atom in is .
D.
The bond strength of is greater than that of .
E.
is a weaker acid than .


24.
The initial rate data given below have been determined at a certain temperature
for the reaction

2NO (g)   + 2H2 (g)    →   N2 (g)   +   2H2O (g)
[NO]0
[H2]0
Initial Rate (M/s)
0.10
0.20
0.0150
0.10
0.30
0.0225
0.20
0.20
0.0600

The rate constant (in the appropriate unit) is:
A.
7.5
B.
3.0 × 10–3
C.
380
D.
0.75
E.
3.0 × 10–4


25.
The reaction
 
2A + B → C
has the following proposed mechanism:
 
 
 
 
 
Step 1:     A + B D (fast equilibrium)
 
 
Step 2:     D + B → E                                        
 
 
 
 
Step 3:     E + A → C + B
     
If step 2 is the rate-determining step, then the rate of formation of C should equal:
A.
k[A]
B.
k[A]2[B]
C.
k[A]2[B]2
D.
k[A][B]
E.
k[A][B]2


26.
Given the following potential energy diagram for the reaction ,



which of the following statements is correct?
A.
A is the enthalpy change for the reaction.
B.
The reaction is endothermic.
C.
B is the activation energy.
D.
B is the enthalpy change for the reaction.
E.
C is the enthalpy change for the reaction.


27.
The autoionization of water

H2O (liq)     ⇌      H+ (aq)     +     OH- (aq)

is endothermic.   Which of the following is correct for water
heated to above 25 ?
A.
Kw = 1 x 10 -14
B.
[H +] > [OH -]
C.
[OH -] > [H +]
D.
Kw > 1 x 10 -14
E.
Kw < 1 x 10 -14


28.
Which of the following changes will shift the following chemical equilibrium
N2(g) + 3H2(g) 2NH3(g)        ;         ,
to the right?
I.
 
increasing the temperature
II.
 
decreasing the temperature
III.
 
increasing the volume
IV.
 
decreasing the volume
V.
 
removing some NH3
VI.
 
adding some NH3
VII.
 
removing some N2
VIII.
 
adding some N2
 
A.
I, IV, VI, VII
B.
II, III, V, VIII
C.
I, VI, VIII
D.
I, III, V, VII
E.
II, IV, V, VIII


29.
The equilibrium constant for the reaction

2A (g) 2B (g)   + C (g)

is 1.33 × 10–6. If Initially 3 moles of A are placed in a 1.5-L flask
the concentration of C at equilibrium.would be :
A.
0.011 M
B.
0.022 M
C.
0.033 M
D.
0.014 M
E.
0.0069 M


30.
Acetic acid, (HC2H3O2) is a weak acid (Ka = 1.8 10-5). Calculate the pH
of a 17.0 M HC2H3O2 solution.
A.
1.25
B.
3.49
C.
1.76
D.
1.25
E.
12.5


31.
Calculate the pH of the following aqueous solution:

   0.2 M NH4Cl (pKb for NH3 = 4.74)
A.
9.02
B.
4.98
C.
9.96
D.
4.04
E.
2.37


32.
The Ksp of Al(OH)3 is 2 10-32. At what pH will a 0.9 M Al3+ solution begin
to show precipitation of Al(OH)3?
A.
3.4
B.
10.6
C.
1.0
D.
5.9
E.
2.5


33.
A certain indicator HIn has a pKa of 9.00 and a color change becomes visible
when 7.00 % of it is In. At what pH is this color change visible?
A.
10.2
B.
3.88
C.
6.15
D.
7.85
E.
7.05


34.
Consider the dissociation of hydrogen:

              H2(g) 2H(g)

One would expect that this reaction:
A.
will be spontaneous at any temperature.
B.
will be spontaneous at high temperatures.
C.
will be spontaneous at low temperatures.
D.
will not be spontaneous at any temperature.
E.
will never happen.


35.
Consider the reaction

   

at 25oC for which the following data are relevant:
 
11.29 kJ/mol
355.29 J/K mol
33.15 kJ/mol
239.90 J/K mol
?
204.80 J/K mol

The reaction is allowed to proceed until all substances involved have reached their equilibrium concentrations. Under those conditions, what is for the reaction?
A.
- 1.35 x 105 kJ
B.
98.7 kJ
C.
- 25.2 kJ
D.
135 kJ
E.
0


36.
Calculate E at 25 for the galvanic cell

Cr(s) | Cr3+(0.2 M) || Br2(0.5 M), Br-(0.1 M) |Pt(s)

given the standard reduction potentials,

                   = -0.727 V

               = +1.090 V
A.
1.753 V
B.
1.817 V
C.
1.831 V
D.
1.881 V
E.
1.201 V


37.
The reaction,

takes place in a car battery. To start the car a current of 125 amperes is
drawn for 20.5 seconds. How many grams of Pb would be consumed in
this process. (The atomic mass of Pb is 207.19)
A.
5.50              g
B.
2.75              g
C.
6.55 x 10 -3   g
D.
1.76 x 10 -4   g
E.
1.33 x 10-2    g


38.
What is the nuclear binding energy in joules/ nucleon in a nucleus
given the data below,
species
nucleus
proton ()    
neutron ()
 
mass in amu
 
24.985839
 
1.007825
 
1.008665

and given that 1 amu = 1.660577881 x 10 -27 kg ?
A.
0.22076        J/nucleon
B.
3.30 × 10–11 J/nucleon
C.
1.32 × 10–12 J/nucleon
D.
0.999            J/nucleon
E.
2.75 × 10–12 J/nucleon


39.
The half-life of 90Sr is 29 years. What fraction of the atoms in a sample of 90Sr would remain 175 years later?
A.
0.17
B.
0.12
C.
0.062
D.
0.015
E.
0.50


40.
Neutron capture by U followed by two successive beta decays gives:
A.
Pu
B.
Ra
C.
U
D.
Pu
E.
Np


                                     

KING FAHD UNIVERSITY OF PETROLEUM AND MINERALS
CHEMISTRY DEPARTMENT
CHEM-102-071-FINAL EXAM


TEST CODE NUMBER 000

STUDENT NUMBER:    _____________________________
NAME :                          _____________________________
SECTION NUMBER:    _____________________________

INSTRUCTIONS
1.
Write your student number, name, and section number on the EXAM COVER page.
2.
Write your student number, section number, and your name on your EXAM ANSWER FORM.
3.
Bubble in pencil your student number and your section number on the EXAM ANSWER FORM.
4.
Bubble in pencil on your EXAM ANSWER FORM the correct answer to each of the questions. .
You must not give more than ONE answer per question.
5.
At the end of the exam return the EXAM ANSWER FORM to the proctor.
6.
The exam contains 40 multiple choice questions and the time allowed is 160 min (2 hrs and 20 min). Time will be announced after 80 minutes and again 10 minutes before the end of the exam.

Important constants
Gas Constant (R)
= 0.0821
= 8.31
= 8.31 x 107
L.atm/(mol.K)
J/(mol.K)
g.cm2/(sec2.mol.K)
Planck’s Constant (h)
= 6.626 x 10-34
= 6.626 x 10-34
J.sec/particle kg.m2/(sec.particle)
Velocity of light (c)
= 2.998 x 108
m/sec
Avogadro’s number (N)
= 6.022 x 1023
particles/mole
Bohr’s Constant (RH)
= 2.179 x 10-18
J/particle
Faraday (F)
= 96485
Coulombs
Specific heat of H2O
= 4.18
J/(g.oC)




STOP This is the end of the test. When you have completed all the questions and reviewed your answers, press the button below to grade the test.