Name: __________________________ Date: _____________
1. A microwave oven operating at 1.22  108 nm is used to heat 150 mL of water from
20ºC to 100ºC. What is the number of photons needed if all the microwave energy is
converted to thermal energy of water? [Density of water = 1.00 g/mL]
A)
B)
C)
D)
E)
3.08  1028
4.07  1027
1.63  1028
5.46  1027
5.02  1027
2. What is the wavelength of light required to remove an electron from a sample of
potassium (K) metal, if the binding energy for an electron in potassium is 1.76 103
kJ/mol?
A)
B)
C)
D)
E)
68.0 nm
18.8 nm
147 nm
113 nm
885 nm
3. Which one of the following sets of quantum numbers can correctly represent a 3p
orbital?
i
n=3
l=1
ml = 2
A)
B)
C)
D)
E)
ii
n=1
l=3
ml = 3
iii
n=3
l=2
ml = 1
iv
v
i
ii
iii
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iv
n=3
l=1
ml = –1
v
n=3
l=0
ml = 1
4. A proton is accelerated to one-tenth the velocity of light, and this velocity can be
measured with a precision of 1 %. What is the uncertainty in the positionof this
proton? [The mass of the proton is 1.673 x 10-27 kg]
A)
B)
C)
D)
E)
1 x 10-13 m
5 x 10-13 m
5 x 10-11 m
1 x 10-14 m
1 x 10-15 m
5. The speed of an electromagnetic wave
A)
B)
C)
D)
E)
depends on the type of the wave and the nature of the medium.
always constant and equals to 3.00  108 km/s.
depends on the frequency of the wave.
depends on the nature of the medium only.
depends on the amplitude of the wave.
6. Arrange the following in order of increasing first ionization energy: F, K, P, Ca, and S.
The order of increasing first ionization energy (lowest to highest) is:
A)
B)
C)
D)
E)
K < Ca < S < P < F
S < Ca < P < F < K
S < F < P < Ca < K
S < K < P < F < Ca
K < Ca < P < S < F
7. An M2+ ion derived from a metal that has four electrons in the 3d subshell. What
element might M be?
A)
B)
C)
D)
E)
Chromium (Cr)
Manganese (Mn)
Scandium (Sc)
Titanium (Ti)
Iron (Fe)
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8. Of the following, which element does not match its designation?
In (Atomic number 49) / representative nonmetal
Sr (Atomic number 38) / representative metal
Si (Atomic number 14)/ metalloid
Mo (Atomic number 42) / d-transition metal
U (Atomic number 92) / f-block (transition) metal
A)
B)
C)
D)
E)
9. Which of the following statement(s) is/are false?
I.
Electrons in inner shells screen or shield electrons in outer shells from the full effect of
the nuclear charge.
II. The effective nuclear charge experienced by an electron in an outer shell is more than the
actual nuclear charge.
III. The atomic radii of representative elements increase from left to right across a period
(i.e., horizontal row in the periodic table)
A)
B)
C)
D)
E)
II and III only
I and II only
all of them
I only
III only
10. Which one of the following species is not isoelectronic with neon (Ne)?
A)
B)
C)
D)
E)
Si2Al3+
Na+
O2Mg2+
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11. Use the following data to calculate ΔH°f for barium bromide.
Lattice energy
First ionization energy of Ba
Second ionization energy of Ba
Enthalpy of electron affinity of Br
Bond energy of Br2
Enthalpy of sublimation of Ba
A)
B)
C)
D)
E)
+1985 kJ/mol
+503 kJ/mol
+965 kJ/mol
-325 kJ/mol
+193 kJ/mol
+178 kJ/mol
-796 kJ/mol
-146 kJ/mol
-603 kJ/mol
-618 kJ/mol
-554 kJ/mol
12. Which of the following compounds has/have expanded octet Lewis structure(s)?
A)
B)
C)
D)
E)
XeF2
XeF4
SF4
I
II
III
I, II and III
II and III only
I and II only
II only
III only
Use the given bond energies to estimate H for the following reaction:
13.
HCN(g)
+
2H2(g)

CH3NH2(g)
Bond Energies (kJ/mol):
H–C : 413;
A)
B)
C)
D)
E)
C–N : 305;
C=N : 615;
-158 kJ
-590 kJ
+590 kJ
+214 kJ
-434 kJ
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C≡N : 891;
H–H : 432;
N–H: 391.
14. Which set of elements is arranged in order of increasing electronegativity (lowest to
highest)?
In, O, S, As
A)
B)
C)
D)
E)
In < As < S < O
O < S < As < In
S < O < As < In
As < O < In < S
S < In < O < As
15. Choose the correct statement about the compound SO2.
A) The S atom has an unshared electron pair.
B) The S-O bonds are 100 % ionic in character.
C) The two S-O bonds have different lengths since one is a single bond and the other
is a double bond.
D) The molecule has a linear structure.
E) The O atoms have no unshared electron pairs.
16. The heat of solution (heat of dissolving) of an ionic solid in water is +20.3 kJ/mol. If
enough quantity of ionic solid is added to water at 23.5 °C in a Styrofoam cup to
produce 150.0 mL of 2.50 M solution, what will be the final temperature ? (Assume
the solution has a density of 1.88 g/mL and a specific heat of 2.70 J/g · °C).
A)
B)
C)
D)
E)
13.5 °C
10.0 °C
30.6 °C
37.0 °C
33.5 °C
17. Which one of the following statements is INCORRECT?
A)
B)
C)
D)
E)
Kinetic energy is the energy that results from an object’s position.
Energy is the capacity to do work.
Energy is neither created nor destroyed in chemical reactions.
Exothermic processes transfer heat from the system to the surroundings.
Increasing the thermal energy of a gas increases the motion of its atoms.
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18. How many moles of methanol (CH3OH) are needed to produce 944.5 kJ of energy,
according to the following data:
2CH3OH(l) + 3O2(g)
→ 2CO2(g) + 4H2O(l)
ΔH°f (H2O) = -285.8 kJ/mol
ΔH°f (CO2)= -393.5 kJ/mol
ΔH°f (CH3OH) = -238.7 kJ/mol
A)
B)
C)
D)
E)
1.300 mol
2.599 mol
1.233 x 10-3 mol
3.123 x 10-3 mol
2.332 x 10-3 mol
19. The expansion of a gas in volume from 45.0 mL to 200.0 mL against vacuum absorbs a
heat of 3.0 J. Calculate the change in energy associated with this process.
A)
B)
C)
D)
E)
+3.0 J
-3.0 J
+155 J
-155 J
-152 J
20. Calculate the ratio of heat required to increase the temperature from 280. K to 300. K of
a water sample to that of aluminum, when the same quantities of them are heated. The
specific heats of water and aluminum are 4.184 and 0.900 J/g · °C, respectively.
A)
B)
C)
D)
E)
4.65
0.215
0.430
9.30
2.15
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Answer Key
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
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