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Inorganic Chemistry Mock Final Exam
Inorganic Chemistry (De La Salle University)
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KEMINO1 MOCK FINAL EXAM
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7.
A Lewis acid-base adduct results from the interaction
between
a. Acid HOMO and base LUMO
b. Acid LUMO and base HOMO
c. Acid HOMO and base HOMO
d. Acid LUMO and base LUMO
The HSAB theory can be used to predict solubility
trends. Based on the determination of the hardness of
the ions, what happens when AgF and LiI are placed
together into solution?
a. Only AgI precipitates initially, but dissolves
back into solution when Ag+ forms a
complex ion with F- and H2O.
b. Only LiF precipitates
c. Both LiF and AgI precipitate
d. No precipitate is formed
Which of the following trends has a negative
correlation with hardness?
a. Oxidation state
b. Polarizability
c. Electronegativity
d. Charge Density
Determine the cell diagram for the reaction below.
Assume a platinum electrode is used when no other
solid is present
2Fe2+(aq) + Pb4+(aq) -> 2Fe3+(aq) + Pb2+(s)
a. Pt(s) | Fe2+(aq), Fe3+(aq) | | Pb4+(aq), Pb2+(aq)
| Pt(s)
b. Pt(s) | Pb2+(aq), Pb4+(aq)| | Fe2+(aq), Fe3+(aq) |
Pt(s)
c. Pt(s) | Fe3+(aq), Fe2+(aq)| | Pb2+(aq), Pb4+(aq) |
Pt(s)
d. Pt(s) | Pb4+(aq), Pb2+(aq)| | Fe2+(aq), Fe3+(aq) |
Pt(s)
Consider an electrochemical cell constructed from the
following half cells, linked by a KCl salt bridge
-a Fe electrode in 1.0 M FeCl2 solution
-a Sn electrode in 1.0 M Sn(NO3)2 solution
When the cell is running spontaneously, which choice
includes only true statements and no false ones?
a. The tin electrode loses mass and the tin
electrode is the cathode
b. The tine electrode gains mass and the tin
electrode is the cathode
c. The iron electrode gains mass and the iron
electrode is the anode
d. The iron electrode loses mass and the iron
electrode is the cathode
Determine the equilibrium constant, K eq at 25 C for
the reaction [ 2Br-(aq) + I2(s)  Br2(l) + 2I-(aq) ]
a. 5.7 x 10-19
b. 18.30
c. 1.7 x 1054
d. 1.9 x 1018
Calculate G for the electrochemical cell Pb(s) | Pb 2+
(aq) | | Fe3+(aq) | Fe2+(aq) | Pt(s)
a. -1.7 x 102 kJ/mol
b. 1.2 x 102 kJ/mol
c. -8.7 x 101 kJ/mol
d. -3.2 x 105 kJ/mol
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A solution of unknown pH is placed in the hydrogen
compartment of a galvanic cell, with the H 2 pressure
maintained at 1 atm. The other half-cell compartment
consists of a Cu/Cu2+ electrode with [Cu2+] = 1.00M.
If the overall cell potential at 25 C is +0.65 V, which
describes hydrogen electrode?
a. Hydrogen is the anode with a [H+] > 1.0M
b. Hydrogen is the cathode with a [H+] > 1.0M
c. Hydrogen is the anode with a [H+] < 1.0M
d. Hydrogen is the cathode with a [H+] < 1.0M
Predict the products of the electrolysis of aqueous
aluminum bromide AlBr3(aq). Balancing is not
required
a. Al + Br2
b. Al + O2 + H+
c. H2 + OH- + Br2
d. H2 + O2
When an aqueous solution of AgNO3 is electrolyzed,
a gas is observed to form at the anode. The gas is
a. H2
b. O2
c. NO
d. NO2
How many coulombs of charge are required to cause
reduction of 0.20 mole of Cr3+ to Cr?
a. 0.60 C
b. 3.0C
c. 2.9 x 104 C
d. 5.8 x 104 C
List of the number of protons, neutrons, and nucleons
(protons + nucleons), in that order, for an isotope
with the Symbol: 137Cs
a. 137, 55, 192
b. 55, 137, 192
c. 55, 82, 137
d. 82, 55, 137
Beta particles are identical to
a. Protons
b. Helium atoms
c. Helium nuclei
d. Electrons
As a result of alpha emission, the product nucleus is
a. One atomic number lower than the original
element
b. Two atomic numbers higher than the
original element
c. One atomic number higher than the original
element
d. Two atomic numbers lower than the original
element
e. Four atomic numbers lower than the original
element
As a result of beta decay, the product of the nucleus is
a. One atomic number lower than the original
element
b. Two atomic numbers higher than the
original element
c. One atomic number higher than the original
element
d. Two atomic numbers lower than the original
element
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16. What is the missing symbol in this plutonium fission
reaction?
239
Pu + 01n -> ____ + 97Sr + 3 01n
a. 0-1
b. 143Xe
c. 140Ba
d. 91Sr
17. The best capable alternative source which can meet
the future energy demand is
a. Thermal power plant
b. Nuclear power plant
c. Hydroelectric power plant
d. Geothermal power plant
18. The isotope with the greatest nuclear binding energy
per nucleon is
a. 56Fe
b. 14C
c. 4He
d. 2H
19. Find the nuclear binding energy of U-234 (atomic
mass = 234.040947 amu) in units of joules per
nucleon.
a. 3.04 x 10-10 J/nucleon
b. 1.30 x 10-12 J/nucleon
c. 1.22 x 10-12 J/nucleon
d. 1.42 x 10-12 J/nucleon
20. Carbon-11 is a radioactive isotope of carbon. Its halflife is 20.3 minutes. What fraction of the initial
number of carbon-11 atoms in a sample will remain
after 81 minutes?
a. 1/16
b. ¼
c. ½
d. 1/32
21. Radioactive nitrogen-13 has a half-life of 10 minutes.
After 40 minutes, how much of this isotope would
remain in a sample that originally contained 96 mg?
a. 6 mg
b. 8 mg
c. 10 mg
d. 12 mg
22. Some metals are found in the uncombined free state
while other metals are found in the combined state.
What is the deciding factor?
a. Metals with negative reduction potentials
can occur in the free state while metals with
positive reduction potentials occur in the
combined state
b. The active metals can occur in the free state
while the less active metals occur in the
combined state
c. Metals with positive reduction potentials can
occur in the free state while metals with
negative reduction potentials can occur in
the combined state
d. There is no way we can predict which
metals will be free or combined
23. Soluble metal compounds tend to be found in the
____, whereas insoluble metal compounds tend to be
found in the _____.
a. Oceans; earth’s crust
b. Bathroom; kitchen
c. Salt beds; oceans
d. Earth’s crust; oceans
e. Rivers; oceans
24. The Hall-Heroult process is used in the production of:
a. Mg
b. Fe
c. Al
d. Au
e. Halls candy
Balance the following redox equation in acidic solution
NO3-(aq) + SO2 (aq) -> NO(aq) + SO42-(aq)
25. The sum of the coefficients is
a. apple
b. 10
c. 12
d. 16
26. The number of moles of electrons transferred in the
reaction above is
a. Pineapple
b. 8
c. 6
d. 4
e. 3
27. The reductant in the reaction is
a. NO3b. SO2
c. COS
d. NO2e. SO3
28. Calculate the standard cell potential for the following
cell: Mg | Mg2+ | | NO-3 (acid soln) | NO(g) | Pt
a. 3.33 V
b. 1.41 V
c. -1.41 V
d. 8.46 V
29. Consider an electrochemical cell based on the
following cell diagram:
Pt | Pu3+(aq), Pu4+(aq) | | Cl2(g), Cl-(aq) | Pt
Given that the standard cell emf is 0.35V and that the
standard reduction potential of chlorine is 1.36V,
what is the standard reduction potential E (Pu4+/Pu3+)
a. 2.37 V
b. 1.01 V
c. -1.71 V
d. -1.01 V
30. Using a table of standard electrode potentials, decide
which of the following statements is completely true
a. Cu2+ can oxidize H2, and Fe can reduce Mn2+
b. Ni2+ can oxidize Cu2+, and Fe2+ can reduce
H+
c. Br2 can oxidize Ni, and H2 can reduce Mn2+
d. H+ can oxidize Fe, Ni can reduce Br2
31. Which one of the following reagents is capable of
oxidizing Cu(s) to Cu2+(1M)
a. I- (1M)
b. Ni(s)
c. Ag+(1M)
d. Al3+(1M)
32. How many grams of Na will be deposited from
molten NaCl by a current of 3.0 amp flowing for 4.0
hours?
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33.
34.
35.
36.
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39.
a. 1.1g
b. 10. g
c. 13 g
d. 22 g
How long will it take to place 0.100 g Cu from a
Cu(NO3)2 solution if a current of 8.0 amp is used?
a. 9.0 s
b. 19 s
c. 38 s
d. 304 s
A galvanic cell is constructed by placing unknown
metal X in a solution of X 2+ and Pb(s) in solution of
Pb2+, and the E cell was found to be +2.24V. After
some time, the mass of the X decreases while the
mass of Pb increases. What is the E red for the half
reaction X2+ + 2e- -> X?
a. 2.37 V
b. 2.11 V
c. -2.11 V
d. -2.37 V
What is the value of G for the following reaction?
Mn2+ + 2 Fe2+ -> Mn(s) + 2Fe3+
a. -79 kJ/mol
b. 69 kJ/mol
c. 376 kJ/mol
d. 525 kJ/mol
In a Ag/Cu galvanic cell, Ag(s) and Cu(s) electrodes
were placed in a solution with 0.50M Ag + and 0.50M
Cu2+. What can be concluded about the cell potential?
a. The cell potential is less than the standard
cell potential
b. The cell potential is the same as the standard
cell potential
c. The cell potential is greater than the standard
cell potential
d. Nothing can be concluded about the
potential of this cell.
What is the nuclear binding energy per nucleon, in
joules, for 25Mg (atomic mass 24.985839)? [Data: 1H
atomic mass = 1.007825 amu; 01n mass = 1.008665; 1
kg = 6.022 x 1026 amu; c = 3.00 x 108 m/s]
a. 1.32 x 10-12 J/nucleon
b. 0.22076 J/nucleon
c. 3.30 x 10-11 J/nucleon
d. 0.999 J/nucleon
What happens to the mass number and the atomic
number of an element when it emits alpha radiation?
a. The mass number remains unchanged while
the atomic number decreases by one
b. The mass number decreases by four and the
atomic number decreases by two
c. The mass number increases by four and the
atomic number increases by two
d. The mass number remains unchanged while
the atomic number increases by one
If 12% of a certain radioisotope decays in 5.2 years,
what is the half-life of this isotope?
a. 0.59 yr
b. 1.7 yr
c. 22 yr
d. 28 yr
40. How old is a bottle of wine if the tritium (3H) content
is 25% of a new wine? The half-life of tritium is 12.5
years
a. 0.25 yr
b. 3.1 yr
c. 25 yr
d. 38 yr
41. List the different types of nuclear radiation (alpha,
beta, gamma) in order of increasing penetrating
power.
a. Alpha < beta < gamma
b. Beta < alpha < gamma
c. Gamma < alpha < beta
d. Gamma < beta < alpha
42. A sample of a radioisotope shows an activity of 999
disintegrations per minute due to beta decay. If after
1.10 years the activity is 952 disintegrations per
minute, what is the half-life of this radioisotope?
a. 4.38 x 10-2 yr
b. 11.4 yr
c. 0.25 yr
d. 15. 8 yr
43. Decay of lutetium-167 by electron capture yiels
a. Ytterbium-167
b. Lutetium-166
c. Thulium-163
d. Tantalum-171
44. Decay of silicon-27 by positron emission yields
a. Sulfur-31
b. Phosphorus-27
c. Silicon-26
d. Aluminum-27
45. Which statement is true?
a. The electrical conductivity of a metal
increase with temperature
b. The
electrical
conductivity
of
a
semiconductor increases with temperature
c. The resistivity of a semiconductor increases
with temperature
d. Metals and semiconductors have similar
electrical conducting properties
46. The behavior of metals and semiconductors is usually
discussed in terms of band theory. Which statement is
not true?
a. A partially filled band is characteristic of a
metal
b. Doping Si with As enhances its
semiconducting properties
c. Band
gaps
vary
among
different
semiconductors but are always relatively
large
d. Band gaps of insulators are large
47. The energy gap in a semiconductor
a. Increases with temperature
b. Does not change with temperature
c. Decreases with temperature
d. Is zero
48. In an n-type semiconductor, the position of the fermi
level
a. Is lower than the center of the energy gap
b. Is at the center of the energy gap
c. Is higher than the center of the energy gap
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d. Can be anywhere
49. At room temperature, a semiconducting material is a
a. Perfect insulator
b. Conductor
c. Slightly conducting
d. Any of the above
50. Which metal can be found as a free element?
a. Na
b. Mn
c. Fe
d. Cr
e. Pt
45.
46.
47.
48.
49.
50.
B
C
C
C
C
E
ANSWER KEYS
1. B
2. C
3. B
4. A
5. B
6. A
7. A
8. C
9. C
10. B
11. D
12. C
13. D
14. D
15. C
16. C
17. B
18. A
19. C
20. A
21. A
22. C
23. A
24. C
25. D
26. C
27. B
28. A
29. B
30. D
31. C
32. B
33. C
34. D
35. C
36. A
37. A
38. B
39. D
40. C
41. A
42. D
43. A
44. D
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