Version: A
___________________________________________________________
1. Energy is released when nitrogen gas combines with hydrogen gas to form
ammonia according to the equation:
N2 (g) + 3 H2 (g) → 2 NH3 (g)
Which of the following is responsible for the release of energy?
A.
B.
C.
D.
E.
2. The standard enthalpy of formation of atomic oxygen is:
A.
B.
C.
D.
E.
3. Breaking nitrogen bonds
Breaking hydrogen bonds
Forming nitrogen-hydrogen bonds
Breaking both nitrogen and hydrogen bonds.
All of these release energy
Negative, since all spontaneous reactions are exothermic Zero, since oxygen is an element Positive, since breaking of bonds is always endothermic Negative, zero, or positive depending on the temperature Zero, since oxygen is an element and Positive, since breaking of
bonds is always endothermic Given the following standard enthalpies of formation:
Compound
CH4(g)
CO2(g)
H2O(g)
ΔHf (kJ/mol)
-75
-394
-242
What is the standard enthalpy change for the combustion of methane:
CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)
A.
B.
C.
D.
E.
+561 kJ
-561 kJ
+803 kJ
-803 kJ
-711 kJ
1 4. The standard enthalpy of formation for H2O(l) is ΔH = - 285 kJ/mol.
Beginning with H2O (l), which of the following physical and/or chemical changes
is/are exothermic?
A.
B.
C.
D.
E.
5. only i
i, ii & iii
ii & iv
only ii
only iv
Which of the following are NOT correctly written as a standard enthalpy of
formation reactions?
i) Mg(s) + O2(g) + H2(g) → Mg(OH)2 (s)
ii) H2(g) + ½ O2(g) → H2O(l)
iii) Mg(s) + 2H2O(l) → Mg2+ (aq) + 2 OH- (aq) + H2(g)
iv) H+ (aq) + OH- (aq) → H2O (l)
A.
B.
C.
D.
E.
i & ii
iii & iv
ii, iii & iv
i & iv
all are correct
2 ΔH = -924.7 kJ/mol
ΔH = -285.8 kJ/mol
ΔH = -704.7 kJ/mol
ΔH = -124.1 kJ/mol
6. 100 mL of water, 100 mL of alcohol, and 200 mL of an unknown liquid, all at 25°C,
are heated at the same rate under identical conditions. After 3 minutes the
temperature of the alcohol is 50°C. It took 5 minutes for the water to reach 50°C. It
took 6 minutes for the unknown liquid to reach 50°C.
Which statement is TRUE regarding the specific heat, Cs?
A.
B.
C.
D.
7. Cs (water) = Cs (alcohol)
Cs (water) > Cs (alcohol)
Cs (water) < Cs (unknown)
Cs (alcohol) > Cs (unknown)
What amount of heat energy, kJ, is released in the combustion of 16.0 g of C3H6?
2 C3H6(g) + 9 O2(g) → 6 CO2(g) + 6 H2O(l)
A.
B.
C.
D.
E.
8. 581
783
504
624
725
Which of these will lead to the greatest increase in temperature when added to
100.0 mL of water at 25°C?
A.
B.
C.
D.
ΔH° = -4120 kJ
94 g of gold at 150°C, specific heat = 0.128 J/g K.
50 g of iron at 110°C, specific heat = 0.452 J/g K.
66 g of silver at 124°C, specific heat = 0.234 J/g K.
70 g of copper at 150°C, specific heat = 0.385 J/g K.
3 9. Given the following equations and ΔH° values, determine the heat of reaction (kJ)
at 298 K for the reaction:
2 NF3(g) + Cu(s) → N2F4(g) + CuF2(s)
2 NF3(g) + 2 NO(g) → N2 F4(g) + 2 NOF(g)
NO(g) + ½F2(g) → NOF(g)
Cu(s) + F2(g) → CuF2(g)
A.
B.
C.
D.
E.
ΔH° (kJ)
-82.9
-156.9
-531.0
+770.8
-605.0
-300.1
+291.2
-291.6
10. A volume of 50.0 mL of 0.400 M NaOH(aq) was added to 20.0 mL of 0.500 M
H2SO4(aq) in a calorimeter of heat capacity 39.0 JK-1. The temperature of the
resulting solution rose by 3.60°C. What is the total heat produced (in kJ) in this
neutralization? Assume that the specific heat capacity of the neutralized solution is
4.18 J.K-1g-1.
H2SO4(aq) + 2 NaOH(aq) → 2 Na2SO4(aq) + H2O(l)
A.
B.
C.
D.
E.
-102
-111
-119
-126
-132
4 11. In the introduction to Chapter 6 I played several clips from the hit TV show “The
Big Bang Theory” in class. In this episode, Dr. Sheldon Cooper is trying to
visualize the behavior of electrons traveling through a graphene sheet. Which of the
following statements is/are true regarding his findings?
i) Sheldon’s model of the behavior of electrons failed with lima beans, peas, and
marbles, but he was able to come up with an accurate model with balls from a ball
pit after he determined the proper size ratio with bigger carbon atoms.
ii) Just like Dalton, Thompson, and Bohr, it was relatively easy for Sheldon to
develop an accurate model of the behavior of an electron.
iii) Sheldon’s model of the behavior of electrons failed with lima beans, peas, and
marbles, but he was able to come up with an accurate model after recognizing the
electron behaved as both a particle and a wave.
A.
B.
C.
D.
E.
ii only iii only
i & ii
i & iii
ii & iii
12. What is the energy of the photons emitted from the He-Ne laser, wavelength = 655
nm?
A.
B.
C.
D.
E.
2.27 10-19 J
4.34 10-40 J
3.03 10-19 J
1.01 10-27 J
5.29 10-18 J
13. Which emission line in the hydrogen spectrum occurs at highest frequency?
A.
B.
C.
D.
E.
n = 3 to n = 1
n = 1 to n =3
n = 4 to n = 2
n = 2 to n = 4
n = 5 to n = 7
5 14. Suppose a certain atom has four energy levels, and assume all transitions between
levels are possible. Which statement is TRUE?
A.
B.
C.
D.
E.
The lowest energy light is emitted for n=3 → n = 1
The longest wavelength light is emitted for n = 4 → n = 2
The potential energy is greatest when the electron is at the n=1
There are a total of 6 spectral emission lines.
There are a total of 4 spectral emission lines.
level.
15. Sodium metal requires a photon with a minimum energy of 4.41 x 10-19 J to emit
electrons. Suppose you have two lasers, one emitting light with a wavelength of
210 nm and the other emitting light with a wavelength of 335 nm. Each laser
produces 10,000 photons/sec.
Which statement is true regarding the removal of electrons from the metal’s
surface?
A.
B.
C.
D.
E.
Both lasers eject electrons from the metal surface at the same rate.
Both lasers eject electrons from the metal surface, but the weaker laser
needs to operate for a longer period of time.
Only the laser with photons of 335 nm ejects electrons.
Only the laser with photons of 210 nm ejects electrons.
Neither laser will eject electrons.
6 16. Which of the following statements best describes a 4dxz atomic orbital?
A.
B.
C.
D.
E.
The 4dxz orbital has the same number of radial and angular nodes. The 4dxz orbital has more radial nodes than angular nodes.
The 4dxz orbital has more angular nodes than radial nodes.
The 4dxz orbital does not have any radial nodes.
The 4dxz orbital does not have any angular nodes.
17. Which of the following electron configurations is correct for mercury (Hg)?
A.
B.
C.
D.
E.
[Kr] 6s26f146d10
[Xe] 4s25f146d10
[Xe] 6s24f146d10
[Xe] 6s25d10
[Xe] 6s24f145d10
18. How many electrons in a zinc atom have the quantum number ml = 0 ?
A.
B.
C.
D.
E.
6
8
10
14
30
19. Which response correctly fills in the blanks?
The atom _________________ has _________ core electrons, __________ valence
electrons, and _____________unpaired electrons.
A.
B.
C.
D.
E.
oxygen, 2, 6, 4
chlorine, 12, 5, 2
nitrogen, 2, 5, 3
neon, 2, 8, 6
fluorine, 2, 7, 5
20. Which of the following sets of quantum numbers could describe one of the valence
electrons in a sulfur atom in the ground state?
A.
B.
C.
D.
E.
n= 1
n= 2
n= 3
n= 3
n= 4
l=0
l=1
l=1
l=3
l=0
ml = 0 ms = +½
ml = -1 ms = -½
ml = 0 ms = +½
ml = -2 ms = +½
ml = -1 ms = +½
7 21. The attraction of the nucleus on the outermost electron in an atom tends to:
A.
B.
C.
D.
E.
decrease moving from left to right and top to bottom on the periodic table. decrease moving from right to left and top to bottom on the periodic table.
decrease moving from left to right and bottom to top on the periodic table.
decrease moving from right to left and bottom to top of the periodic table.
the attraction of the nucleus to the outermost electron remains constant for
each element on the periodic table.
22. Lithium’s first and second ionization energies are 519 kJ/mol and 7300 kJ/mol,
respectively. Element X has a first ionization energy of 590 kJ/mol and a second
ionization energy of 1150 kJ/mol. Element X is most likely to be:
A.
B.
C.
D.
E.
Oxygen
Sodium
Calcium
Xenon
Fluorine
23. Which of the following is correctly ordered in terms of atomic radius, from smallest
to largest?
A.
B.
C.
D.
E.
Mg2+ < Na+ < FMg2+ < F-< Na+
F- < Na+ < Mg2+
F- < Mg2+ < Na+
Na+ < F- < Mg2+
24. Arrange the following in order of increasing electron affinity: Cl, P, S, Ar.
A.
B.
C.
D.
E.
Most positive EA
Most positive EA
Most positive EA
Most positive EA
Most positive EA
Cl < S < P < Ar
Ar < Cl < S < P
P < S < Cl < Ar
Ar < P < S < Cl
Cl < Ar < P < S
Most negative EA Most negative EA
Most negative EA
Most negative EA
Most negative EA
25. Which of the following statements is TRUE?
A.
B.
C.
D.
E.
The first ionization potential of H is greater than that of He.
The ionic radius of Fe+ is larger than that of Fe3+.
The electron affinity of C is greater than that of Cl.
The atomic radius of Li is larger than that of Cs.
All are false.
8 Version: B
___________________________________________________________
1. Energy is released when nitrogen gas combines with hydrogen gas to form
ammonia according to the equation:
N2 (g) + 3 H2 (g) → 2 NH3 (g)
Which of the following is responsible for the release of energy?
A.
B.
C.
D.
E.
2. The standard enthalpy of formation of atomic oxygen is:
A.
B.
C.
D.
E.
3. Forming nitrogen-hydrogen bonds
All of these release energy
Breaking nitrogen bonds
Breaking both nitrogen and hydrogen bonds.
Breaking hydrogen bonds
Positive, since breaking of bonds is always endothermic Negative, zero, or positive depending on the temperature Zero, since oxygen is an element and Positive, since breaking of
bonds is always endothermic Zero, since oxygen is an element Negative, since all spontaneous reactions are exothermic Given the following standard enthalpies of formation:
Compound
CH4(g)
CO2(g)
H2O(g)
ΔHf (kJ/mol)
-75
-394
-242
What is the standard enthalpy change for the combustion of methane:
CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)
A.
B.
C.
D.
E.
+803 kJ
+561 kJ
-561 kJ
-803 kJ
-711 kJ
1 4. The standard enthalpy of formation for H2O(l) is ΔH = - 285 kJ/mol.
Beginning with H2O (l), which of the following physical and/or chemical changes
is/are exothermic?
A.
B.
C.
D.
E.
5. ii & iv
only i
only iv
only ii
i, ii & iii
Which of the following are NOT correctly written as a standard enthalpy of
formation reactions?
i) Mg(s) + O2(g) + H2(g) → Mg(OH)2 (s)
ii) H2(g) + ½ O2(g) → H2O(l)
iii) Mg(s) + 2H2O(l) → Mg2+ (aq) + 2 OH- (aq) + H2(g)
iv) H+ (aq) + OH- (aq) → H2O (l)
A.
B.
C.
D.
E.
ii, iii & iv
iii & iv
i & ii
i & iv
all are correct
2 ΔH = -924.7 kJ/mol
ΔH = -285.8 kJ/mol
ΔH = -704.7 kJ/mol
ΔH = -124.1 kJ/mol
6. 100 mL of water, 100 mL of alcohol, and 200 mL of an unknown liquid, all at 25°C,
are heated at the same rate under identical conditions. After 3 minutes the
temperature of the alcohol is 50°C. It took 5 minutes for the water to reach 50°C. It
took 6 minutes for the unknown liquid to reach 50°C.
Which statement is TRUE regarding the specific heat, Cs?
A.
B.
C.
D.
7. Cs (alcohol) > Cs (unknown)
Cs (water) < Cs (unknown)
Cs (water) > Cs (alcohol)
Cs (water) = Cs (alcohol)
What amount of heat energy, kJ, is released in the combustion of 16.0 g of C3H6?
2 C3H6(g) + 9 O2(g) → 6 CO2(g) + 6 H2O(l)
A.
B.
C.
D.
E.
8. 783
624
725
504
581
Which of these will lead to the greatest increase in temperature when added to
100.0 mL of water at 25°C?
A.
B.
C.
D.
ΔH° = -4120 kJ
66 g of silver at 124°C, specific heat = 0.234 J/g K.
94 g of gold at 150°C, specific heat = 0.128 J/g K.
50 g of iron at 110°C, specific heat = 0.452 J/g K.
70 g of copper at 150°C, specific heat = 0.385 J/g K.
3 9. Given the following equations and ΔH° values, determine the heat of reaction (kJ)
at 298 K for the reaction:
2 NF3(g) + Cu(s) → N2F4(g) + CuF2(s)
2 NF3(g) + 2 NO(g) → N2 F4(g) + 2 NOF(g)
NO(g) + ½F2(g) → NOF(g)
Cu(s) + F2(g) → CuF2(g)
A.
B.
C.
D.
E.
ΔH° (kJ)
-82.9
-156.9
-531.0
-291.6
-300.1
+291.2
-605.0
+770.8
10. A volume of 50.0 mL of 0.400 M NaOH(aq) was added to 20.0 mL of 0.500 M
H2SO4(aq) in a calorimeter of heat capacity 39.0 JK-1. The temperature of the
resulting solution rose by 3.60°C. What is the total heat produced (in kJ) in this
neutralization? Assume that the specific heat capacity of the neutralized solution is
4.18 J.K-1g-1.
H2SO4(aq) + 2 NaOH(aq) → 2 Na2SO4(aq) + H2O(l)
A.
B.
C.
D.
E.
-111
-126
-119
-102
-132
4 11. In the introduction to Chapter 6 I played several clips from the hit TV show “The
Big Bang Theory” in class. In this episode, Dr. Sheldon Cooper is trying to
visualize the behavior of electrons traveling through a graphene sheet. Which of the
following statements is/are true regarding his findings?
i) Sheldon’s model of the behavior of electrons failed with lima beans, peas, and
marbles, but he was able to come up with an accurate model with balls from a ball
pit after he determined the proper size ratio with bigger carbon atoms.
ii) Just like Dalton, Thompson, and Bohr, it was relatively easy for Sheldon to
develop an accurate model of the behavior of an electron.
iii) Sheldon’s model of the behavior of electrons failed with lima beans, peas, and
marbles, but he was able to come up with an accurate model after recognizing the
electron behaved as both a particle and a wave.
A.
B.
C.
D.
E.
i & iii
i & ii
iii only
ii only ii & iii
12. What is the energy of the photons emitted from the He-Ne laser, wavelength = 655
nm?
A.
B.
C.
D.
E.
4.34 10-40 J
2.27 10-19 J
3.03 10-19 J
1.01 10-27 J
5.29 10-18 J
13. Which emission line in the hydrogen spectrum occurs at highest frequency?
A.
B.
C.
D.
E.
n = 1 to n =3
n = 4 to n = 2
n = 3 to n = 1
n = 2 to n = 4
n = 5 to n = 7
5 14. Suppose a certain atom has four energy levels, and assume all transitions between
levels are possible. Which statement is TRUE?
A.
B.
C.
D.
E.
The longest wavelength light is emitted for n = 4 → n = 2
The potential energy is greatest when the electron is at the n=1
level.
The lowest energy light is emitted for n=3 → n = 1
There are a total of 6 spectral emission lines.
There are a total of 4 spectral emission lines.
15. Sodium metal requires a photon with a minimum energy of 4.41 x 10-19 J to emit
electrons. Suppose you have two lasers, one emitting light with a wavelength of
210 nm and the other emitting light with a wavelength of 335 nm. Each laser
produces 10,000 photons/sec.
Which statement is true regarding the removal of electrons from the metal’s
surface?
A.
B.
C.
D.
E.
Only the laser with photons of 335 nm ejects electrons.
Only the laser with photons of 210 nm ejects electrons.
Both lasers eject electrons from the metal surface, but the weaker
laser needs to operate for a longer period of time.
Both lasers eject electrons from the metal surface at the same rate.
Neither laser will eject electrons.
6 16. Which of the following statements best describes a 4dxz atomic orbital?
A.
B.
C.
D.
E.
The 4dxz orbital has more radial nodes than angular nodes.
The 4dxz orbital does not have any angular nodes.
The 4dxz orbital has more angular nodes than radial nodes.
The 4dxz orbital does not have any radial nodes.
The 4dxz orbital has the same number of radial and angular nodes. 17. Which of the following electron configurations is correct for mercury (Hg)?
A.
B.
C.
D.
E.
[Xe] 4s25f146d10
[Xe] 6s24f146d10
[Xe] 6s25d10
[Kr] 6s26f146d10
[Xe] 6s24f145d10
18. How many electrons in a zinc atom have the quantum number ml = 0 ?
A.
B.
C.
D.
E.
10
6
30
14
8
19. Which response correctly fills in the blanks?
The atom _________________ has _________ core electrons, __________ valence
electrons, and _____________unpaired electrons.
A.
B.
C.
D.
E.
nitrogen, 2, 5, 3
oxygen, 2, 6, 4
chlorine, 12, 5, 2
neon, 2, 8, 6
fluorine, 2, 7, 5
20. Which of the following sets of quantum numbers could describe one of the valence
electrons in a sulfur atom in the ground state?
A.
B.
C.
D.
E.
n= 3
n= 4
n= 2
n= 3
n= 1
l=1
l=0
l=1
l=3
l=0
ml = 0 ms = +½
ml = -1 ms = +½
ml = -1 ms = -½
ml = -2 ms = +½
ml = 0 ms = +½
7 21. The attraction of the nucleus on the outermost electron in an atom tends to:
A.
B.
C.
D.
E.
decrease moving from left to right and bottom to top on the periodic table.
decrease moving from right to left and top to bottom on the periodic table.
decrease moving from left to right and top to bottom on the periodic table. decrease moving from right to left and bottom to top of the periodic table.
the attraction of the nucleus to the outermost electron remains constant for
each element on the periodic table.
22. Lithium’s first and second ionization energies are 519 kJ/mol and 7300 kJ/mol,
respectively. Element X has a first ionization energy of 590 kJ/mol and a second
ionization energy of 1150 kJ/mol. Element X is most likely to be:
A.
B.
C.
D.
E.
Xenon
Fluorine
Calcium
Oxygen
Sodium
23. Which of the following is correctly ordered in terms of atomic radius, from smallest
to largest?
A.
B.
C.
D.
E.
F- < Mg2+ < Na+
Mg2+ < F-< Na+
F- < Na+ < Mg2+
Mg2+ < Na+ < FNa+ < F- < Mg2+
24. Arrange the following in order of increasing electron affinity: Cl, P, S, Ar.
A.
B.
C.
D.
E.
Most positive EA
Most positive EA
Most positive EA
Most positive EA
Most positive EA
Ar < Cl < S < P
Cl < S < P < Ar
P < S < Cl < Ar
Ar < P < S < Cl
Cl < Ar < P < S
Most negative EA
Most negative EA Most negative EA
Most negative EA
Most negative EA
25. Which of the following statements is TRUE?
A.
B.
C.
D.
E.
The atomic radius of Li is larger than that of Cs.
The electron affinity of C is greater than that of Cl.
The ionic radius of Fe+ is larger than that of Fe3+.
The first ionization potential of H is greater than that of He.
All are false.
8 Version: C
___________________________________________________________
1. Energy is released when nitrogen gas combines with hydrogen gas to form
ammonia according to the equation:
N2 (g) + 3 H2 (g) → 2 NH3 (g)
Which of the following is responsible for the release of energy?
A.
B.
C.
D.
E.
2. The standard enthalpy of formation of atomic oxygen is:
A.
B.
C.
D.
E.
3. Forming nitrogen-hydrogen bonds
Breaking hydrogen bonds
Breaking nitrogen bonds
Breaking both nitrogen and hydrogen bonds.
All of these release energy
Zero, since oxygen is an element and Positive, since breaking of
bonds is always endothermic Positive, since breaking of bonds is always endothermic Zero, since oxygen is an element Negative, zero, or positive depending on the temperature Negative, since all spontaneous reactions are exothermic Given the following standard enthalpies of formation:
Compound
CH4(g)
CO2(g)
H2O(g)
ΔHf (kJ/mol)
-75
-394
-242
What is the standard enthalpy change for the combustion of methane:
CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)
A.
B.
C.
D.
E.
-561 kJ
+561 kJ
+803 kJ
-711 kJ
-803 kJ
1 4. The standard enthalpy of formation for H2O(l) is ΔH = - 285 kJ/mol.
Beginning with H2O (l), which of the following physical and/or chemical changes
is/are exothermic?
A.
B.
C.
D.
E.
5. i, ii & iii
only ii
ii & iv
only i
only iv
Which of the following are NOT correctly written as a standard enthalpy of
formation reactions?
i) Mg(s) + O2(g) + H2(g) → Mg(OH)2 (s)
ii) H2(g) + ½ O2(g) → H2O(l)
iii) Mg(s) + 2H2O(l) → Mg2+ (aq) + 2 OH- (aq) + H2(g)
iv) H+ (aq) + OH- (aq) → H2O (l)
A.
B.
C.
D.
E.
iii & iv
i & iv
i & ii
ii, iii & iv
all are correct
2 ΔH = -924.7 kJ/mol
ΔH = -285.8 kJ/mol
ΔH = -704.7 kJ/mol
ΔH = -124.1 kJ/mol
6. 100 mL of water, 100 mL of alcohol, and 200 mL of an unknown liquid, all at 25°C,
are heated at the same rate under identical conditions. After 3 minutes the
temperature of the alcohol is 50°C. It took 5 minutes for the water to reach 50°C. It
took 6 minutes for the unknown liquid to reach 50°C.
Which statement is TRUE regarding the specific heat, Cs?
A.
B.
C.
D.
7. Cs (water) > Cs (alcohol)
Cs (alcohol) > Cs (unknown)
Cs (water) < Cs (unknown)
Cs (water) = Cs (alcohol)
What amount of heat energy, kJ, is released in the combustion of 16.0 g of C3H6?
2 C3H6(g) + 9 O2(g) → 6 CO2(g) + 6 H2O(l)
A.
B.
C.
D.
E.
8. 504
624
725
581
783
Which of these will lead to the greatest increase in temperature when added to
100.0 mL of water at 25°C?
A.
B.
C.
D.
ΔH° = -4120 kJ
66 g of silver at 124°C, specific heat = 0.234 J/g K.
50 g of iron at 110°C, specific heat = 0.452 J/g K.
94 g of gold at 150°C, specific heat = 0.128 J/g K.
70 g of copper at 150°C, specific heat = 0.385 J/g K.
3 9. Given the following equations and ΔH° values, determine the heat of reaction (kJ)
at 298 K for the reaction:
2 NF3(g) + Cu(s) → N2F4(g) + CuF2(s)
2 NF3(g) + 2 NO(g) → N2 F4(g) + 2 NOF(g)
NO(g) + ½F2(g) → NOF(g)
Cu(s) + F2(g) → CuF2(g)
A.
B.
C.
D.
E.
ΔH° (kJ)
-82.9
-156.9
-531.0
-300.1
+770.8
-605.0
+291.2
-291.6
10. A volume of 50.0 mL of 0.400 M NaOH(aq) was added to 20.0 mL of 0.500 M
H2SO4(aq) in a calorimeter of heat capacity 39.0 JK-1. The temperature of the
resulting solution rose by 3.60°C. What is the total heat produced (in kJ) in this
neutralization? Assume that the specific heat capacity of the neutralized solution is
4.18 J.K-1g-1.
H2SO4(aq) + 2 NaOH(aq) → 2 Na2SO4(aq) + H2O(l)
A.
B.
C.
D.
E.
-119
-111
-102
-126
-132
4 11. In the introduction to Chapter 6 I played several clips from the hit TV show “The
Big Bang Theory” in class. In this episode, Dr. Sheldon Cooper is trying to
visualize the behavior of electrons traveling through a graphene sheet. Which of the
following statements is/are true regarding his findings?
i) Sheldon’s model of the behavior of electrons failed with lima beans, peas, and
marbles, but he was able to come up with an accurate model with balls from a ball
pit after he determined the proper size ratio with bigger carbon atoms.
ii) Just like Dalton, Thompson, and Bohr, it was relatively easy for Sheldon to
develop an accurate model of the behavior of an electron.
iii) Sheldon’s model of the behavior of electrons failed with lima beans, peas, and
marbles, but he was able to come up with an accurate model after recognizing the
electron behaved as both a particle and a wave.
A.
B.
C.
D.
E.
i & ii
ii only ii & iii
i & iii
iii only
12. What is the energy of the photons emitted from the He-Ne laser, wavelength = 655
nm?
A.
B.
C.
D.
E.
4.34 10-40 J
1.01 10-27 J
3.03 10-19 J
2.27 10-19 J
5.29 10-18 J
13. Which emission line in the hydrogen spectrum occurs at highest frequency?
A.
B.
C.
D.
E.
n = 2 to n = 4
n = 3 to n = 1
n = 4 to n = 2
n = 1 to n =3
n = 5 to n = 7
5 14. Suppose a certain atom has four energy levels, and assume all transitions between
levels are possible. Which statement is TRUE?
A.
B.
C.
D.
E.
The longest wavelength light is emitted for n = 4 → n = 2
The lowest energy light is emitted for n=3 → n = 1
The potential energy is greatest when the electron is at the n=1 level.
There are a total of 6 spectral emission lines.
There are a total of 4 spectral emission lines.
15. Sodium metal requires a photon with a minimum energy of 4.41 x 10-19 J to emit
electrons. Suppose you have two lasers, one emitting light with a wavelength of
210 nm and the other emitting light with a wavelength of 335 nm. Each laser
produces 10,000 photons/sec.
Which statement is true regarding the removal of electrons from the metal’s
surface?
A.
B.
C.
D.
E.
Only the laser with photons of 210 nm ejects electrons.
Only the laser with photons of 335 nm ejects electrons.
Both lasers eject electrons from the metal surface, but the weaker
laser needs to operate for a longer period of time.
Both lasers eject electrons from the metal surface at the same rate.
Neither laser will eject electrons.
6 16. Which of the following statements best describes a 4dxz atomic orbital?
A.
B.
C.
D.
E.
The 4dxz orbital has more angular nodes than radial nodes.
The 4dxz orbital has the same number of radial and angular nodes. The 4dxz orbital does not have any radial nodes.
The 4dxz orbital does not have any angular nodes.
The 4dxz orbital has more radial nodes than angular nodes.
17. Which of the following electron configurations is correct for mercury (Hg)?
A.
B.
C.
D.
E.
[Xe] 6s24f146d10
[Xe] 6s25d10
[Xe] 4s25f146d10
[Kr] 6s26f146d10
[Xe] 6s24f145d10
18. How many electrons in a zinc atom have the quantum number ml = 0 ?
A.
B.
C.
D.
E.
30
6
10
14
8
19. Which response correctly fills in the blanks?
The atom _________________ has _________ core electrons, __________ valence
electrons, and _____________unpaired electrons.
A.
B.
C.
D.
E.
chlorine, 12, 5, 2
fluorine, 2, 7, 5
neon, 2, 8, 6
nitrogen, 2, 5, 3
oxygen, 2, 6, 4
20. Which of the following sets of quantum numbers could describe one of the valence
electrons in a sulfur atom in the ground state?
A.
B.
C.
D.
E.
n= 2
n= 1
n= 3
n= 3
n= 4
l=1
l=0
l=1
l=3
l=0
ml = -1 ms = -½
ml = 0 ms = +½
ml = 0 ms = +½
ml = -2 ms = +½
ml = -1 ms = +½
7 21. The attraction of the nucleus on the outermost electron in an atom tends to:
A.
B.
C.
D.
E.
decrease moving from right to left and top to bottom on the periodic table.
the attraction of the nucleus to the outermost electron remains constant for
each element on the periodic table.
decrease moving from left to right and bottom to top on the periodic table.
decrease moving from right to left and bottom to top of the periodic table.
decrease moving from left to right and top to bottom on the periodic table. 22. Lithium’s first and second ionization energies are 519 kJ/mol and 7300 kJ/mol,
respectively. Element X has a first ionization energy of 590 kJ/mol and a second
ionization energy of 1150 kJ/mol. Element X is most likely to be:
A.
B.
C.
D.
E.
Sodium
Calcium
Oxygen
Xenon
Fluorine
23. Which of the following is correctly ordered in terms of atomic radius, from smallest
to largest?
A.
B.
C.
D.
E.
Mg2+ < F-< Na+
Mg2+ < Na+ < FF- < Na+ < Mg2+
F- < Mg2+ < Na+
Na+ < F- < Mg2+
24. Arrange the following in order of increasing electron affinity: Cl, P, S, Ar.
A.
B.
C.
D.
E.
Most positive EA
Most positive EA
Most positive EA
Most positive EA
Most positive EA
Ar < Cl < S < P
P < S < Cl < Ar
Cl < S < P < Ar
Ar < P < S < Cl
Cl < Ar < P < S
Most negative EA
Most negative EA
Most negative EA Most negative EA
Most negative EA
25. Which of the following statements is TRUE?
A.
B.
C.
D.
E.
The electron affinity of C is greater than that of Cl.
The first ionization potential of H is greater than that of He.
The atomic radius of Li is larger than that of Cs.
The ionic radius of Fe+ is larger than that of Fe3+.
All are false.
8 Version: D
___________________________________________________________
1. Energy is released when nitrogen gas combines with hydrogen gas to form
ammonia according to the equation:
N2 (g) + 3 H2 (g) → 2 NH3 (g)
Which of the following is responsible for the release of energy?
A.
B.
C.
D.
E.
2. The standard enthalpy of formation of atomic oxygen is:
A.
B.
C.
D.
E.
3. Breaking hydrogen bonds
Forming nitrogen-hydrogen bonds
Breaking nitrogen bonds
Breaking both nitrogen and hydrogen bonds.
All of these release energy
Negative, zero, or positive depending on the temperature Zero, since oxygen is an element Negative, since all spontaneous reactions are exothermic Zero, since oxygen is an element and Positive, since breaking of
bonds is always endothermic Positive, since breaking of bonds is always endothermic Given the following standard enthalpies of formation:
Compound
CH4(g)
CO2(g)
H2O(g)
ΔHf (kJ/mol)
-75
-394
-242
What is the standard enthalpy change for the combustion of methane:
CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)
A.
B.
C.
D.
E.
-803 kJ
-561 kJ
+561 kJ
+803 kJ
-711 kJ
1 4. The standard enthalpy of formation for H2O(l) is ΔH = - 285 kJ/mol.
Beginning with H2O (l), which of the following physical and/or chemical changes
is/are exothermic?
A.
B.
C.
D.
E.
5. i, ii & iii
ii & iv
only ii
only i
only iv
Which of the following are NOT correctly written as a standard enthalpy of
formation reactions?
i) Mg(s) + O2(g) + H2(g) → Mg(OH)2 (s)
ii) H2(g) + ½ O2(g) → H2O(l)
iii) Mg(s) + 2H2O(l) → Mg2+ (aq) + 2 OH- (aq) + H2(g)
iv) H+ (aq) + OH- (aq) → H2O (l)
A.
B.
C.
D.
E.
ii, iii & iv
i & iv
i & ii
iii & iv
all are correct
2 ΔH = -924.7 kJ/mol
ΔH = -285.8 kJ/mol
ΔH = -704.7 kJ/mol
ΔH = -124.1 kJ/mol
6. 100 mL of water, 100 mL of alcohol, and 200 mL of an unknown liquid, all at 25°C,
are heated at the same rate under identical conditions. After 3 minutes the
temperature of the alcohol is 50°C. It took 5 minutes for the water to reach 50°C. It
took 6 minutes for the unknown liquid to reach 50°C.
Which statement is TRUE regarding the specific heat, Cs?
A.
B.
C.
D.
7. Cs (water) > Cs (alcohol)
Cs (water) < Cs (unknown)
Cs (water) = Cs (alcohol)
Cs (alcohol) > Cs (unknown)
What amount of heat energy, kJ, is released in the combustion of 16.0 g of C3H6?
2 C3H6(g) + 9 O2(g) → 6 CO2(g) + 6 H2O(l)
A.
B.
C.
D.
E.
8. 783
504
624
581
725
Which of these will lead to the greatest increase in temperature when added to
100.0 mL of water at 25°C?
A.
B.
C.
D.
ΔH° = -4120 kJ
94 g of gold at 150°C, specific heat = 0.128 J/g K.
70 g of copper at 150°C, specific heat = 0.385 J/g K.
50 g of iron at 110°C, specific heat = 0.452 J/g K.
66 g of silver at 124°C, specific heat = 0.234 J/g K.
3 9. Given the following equations and ΔH° values, determine the heat of reaction (kJ)
at 298 K for the reaction:
2 NF3(g) + Cu(s) → N2F4(g) + CuF2(s)
2 NF3(g) + 2 NO(g) → N2 F4(g) + 2 NOF(g)
NO(g) + ½F2(g) → NOF(g)
Cu(s) + F2(g) → CuF2(g)
A.
B.
C.
D.
E.
ΔH° (kJ)
-82.9
-156.9
-531.0
-605.0
-300.1
+770.8
+291.2
-291.6
10. A volume of 50.0 mL of 0.400 M NaOH(aq) was added to 20.0 mL of 0.500 M
H2SO4(aq) in a calorimeter of heat capacity 39.0 JK-1. The temperature of the
resulting solution rose by 3.60°C. What is the total heat produced (in kJ) in this
neutralization? Assume that the specific heat capacity of the neutralized solution is
4.18 J.K-1g-1.
H2SO4(aq) + 2 NaOH(aq) → 2 Na2SO4(aq) + H2O(l)
A.
B.
C.
D.
E.
-111
-119
-126
-102
-132
4 11. In the introduction to Chapter 6 I played several clips from the hit TV show “The
Big Bang Theory” in class. In this episode, Dr. Sheldon Cooper is trying to
visualize the behavior of electrons traveling through a graphene sheet. Which of the
following statements is/are true regarding his findings?
i) Sheldon’s model of the behavior of electrons failed with lima beans, peas, and
marbles, but he was able to come up with an accurate model with balls from a ball
pit after he determined the proper size ratio with bigger carbon atoms.
ii) Just like Dalton, Thompson, and Bohr, it was relatively easy for Sheldon to
develop an accurate model of the behavior of an electron.
iii) Sheldon’s model of the behavior of electrons failed with lima beans, peas, and
marbles, but he was able to come up with an accurate model after recognizing the
electron behaved as both a particle and a wave.
A.
B.
C.
D.
E.
iii only
i & ii
ii only i & iii
ii & iii
12. What is the energy of the photons emitted from the He-Ne laser, wavelength = 655
nm?
A.
B.
C.
D.
E.
4.34 10-40 J
1.01 10-27 J
2.27 10-19 J
3.03 10-19 J
5.29 10-18 J
13. Which emission line in the hydrogen spectrum occurs at highest frequency?
A.
B.
C.
D.
E.
n = 1 to n =3
n = 3 to n = 1
n = 4 to n = 2
n = 2 to n = 4
n = 5 to n = 7
5 14. Suppose a certain atom has four energy levels, and assume all transitions between
levels are possible. Which statement is TRUE?
A.
B.
C.
D.
E.
The potential energy is greatest when the electron is at the n=1 level.
The lowest energy light is emitted for n=3 → n = 1
The longest wavelength light is emitted for n = 4 → n = 2
There are a total of 6 spectral emission lines.
There are a total of 4 spectral emission lines.
15. Sodium metal requires a photon with a minimum energy of 4.41 x 10-19 J to emit
electrons. Suppose you have two lasers, one emitting light with a wavelength of
210 nm and the other emitting light with a wavelength of 335 nm. Each laser
produces 10,000 photons/sec.
Which statement is true regarding the removal of electrons from the metal’s
surface?
A.
B.
C.
D.
E.
Only the laser with photons of 335 nm ejects electrons.
Neither laser will eject electrons.
Only the laser with photons of 210 nm ejects electrons.
Both lasers eject electrons from the metal surface at the same rate.
Both lasers eject electrons from the metal surface, but the weaker
laser needs to operate for a longer period of time.
6 16. Which of the following statements best describes a 4dxz atomic orbital?
A.
B.
C.
D.
E.
The 4dxz orbital has more angular nodes than radial nodes.
The 4dxz orbital has more radial nodes than angular nodes.
The 4dxz orbital has the same number of radial and angular nodes. The 4dxz orbital does not have any radial nodes.
The 4dxz orbital does not have any angular nodes.
17. Which of the following electron configurations is correct for mercury (Hg)?
A.
B.
C.
D.
E.
[Xe] 4s25f146d10
[Xe] 6s24f146d10
[Kr] 6s26f146d10
[Xe] 6s25d10
[Xe] 6s24f145d10
18. How many electrons in a zinc atom have the quantum number ml = 0 ?
A.
B.
C.
D.
E.
10
8
6
14
30
19. Which response correctly fills in the blanks?
The atom _________________ has _________ core electrons, __________ valence
electrons, and _____________unpaired electrons.
A.
B.
C.
D.
E.
neon, 2, 8, 6
chlorine, 12, 5, 2
nitrogen, 2, 5, 3
oxygen, 2, 6, 4
fluorine, 2, 7, 5
20. Which of the following sets of quantum numbers could describe one of the valence
electrons in a sulfur atom in the ground state?
A.
B.
C.
D.
E.
n= 3
n= 3
n= 2
n= 1
n= 4
l=3
l=1
l=1
l=0
l=0
ml = -2 ms = +½
ml = 0 ms = +½
ml = -1 ms = -½
ml = 0 ms = +½
ml = -1 ms = +½
7 21. The attraction of the nucleus on the outermost electron in an atom tends to:
A.
B.
C.
D.
E.
decrease moving from right to left and top to bottom on the periodic table.
decrease moving from right to left and bottom to top of the periodic table.
decrease moving from left to right and bottom to top on the periodic table.
decrease moving from left to right and top to bottom on the periodic table. the attraction of the nucleus to the outermost electron remains constant for
each element on the periodic table.
22. Lithium’s first and second ionization energies are 519 kJ/mol and 7300 kJ/mol,
respectively. Element X has a first ionization energy of 590 kJ/mol and a second
ionization energy of 1150 kJ/mol. Element X is most likely to be:
A.
B.
C.
D.
E.
Sodium
Calcium
Xenon
Oxygen
Fluorine
23. Which of the following is correctly ordered in terms of atomic radius, from smallest
to largest?
A.
B.
C.
D.
E.
F- < Na+ < Mg2+
Mg2+ < F-< Na+
F- < Mg2+ < Na+
Mg2+ < Na+ < FNa+ < F- < Mg2+
24. Arrange the following in order of increasing electron affinity: Cl, P, S, Ar.
A.
B.
C.
D.
E.
Most positive EA
Most positive EA
Most positive EA
Most positive EA
Most positive EA
Ar < P < S < Cl
Ar < Cl < S < P
P < S < Cl < Ar
Cl < Ar < P < S
Cl < S < P < Ar
Most negative EA
Most negative EA
Most negative EA
Most negative EA
Most negative EA 25. Which of the following statements is TRUE?
A.
B.
C.
D.
E.
The ionic radius of Fe+ is larger than that of Fe3+.
The atomic radius of Li is larger than that of Cs.
The first ionization potential of H is greater than that of He.
The electron affinity of C is greater than that of Cl.
All are false.
8 Version: E
___________________________________________________________
1. Energy is released when nitrogen gas combines with hydrogen gas to form
ammonia according to the equation:
N2 (g) + 3 H2 (g) → 2 NH3 (g)
Which of the following is responsible for the release of energy?
A.
B.
C.
D.
E.
2. The standard enthalpy of formation of atomic oxygen is:
A.
B.
C.
D.
E.
3. Breaking hydrogen bonds
Breaking both nitrogen and hydrogen bonds.
All of these release energy
Forming nitrogen-hydrogen bonds
Breaking nitrogen bonds
Zero, since oxygen is an element Positive, since breaking of bonds is always endothermic Negative, zero, or positive depending on the temperature Negative, since all spontaneous reactions are exothermic Zero, since oxygen is an element and Positive, since breaking of
bonds is always endothermic Given the following standard enthalpies of formation:
Compound
CH4(g)
CO2(g)
H2O(g)
ΔHf (kJ/mol)
-75
-394
-242
What is the standard enthalpy change for the combustion of methane:
CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)
A.
B.
C.
D.
E.
+803 kJ
+561 kJ
-561 kJ
-803 kJ
-711 kJ
1 4. The standard enthalpy of formation for H2O(l) is ΔH = - 285 kJ/mol.
Beginning with H2O (l), which of the following physical and/or chemical changes
is/are exothermic?
A.
B.
C.
D.
E.
5. ii & iv
only i
only iv
only ii
i, ii & iii
Which of the following are NOT correctly written as a standard enthalpy of
formation reactions?
i) Mg(s) + O2(g) + H2(g) → Mg(OH)2 (s)
ii) H2(g) + ½ O2(g) → H2O(l)
iii) Mg(s) + 2H2O(l) → Mg2+ (aq) + 2 OH- (aq) + H2(g)
iv) H+ (aq) + OH- (aq) → H2O (l)
A.
B.
C.
D.
E.
ii, iii & iv
i & ii
i & iv
iii & iv
all are correct
2 ΔH = -924.7 kJ/mol
ΔH = -285.8 kJ/mol
ΔH = -704.7 kJ/mol
ΔH = -124.1 kJ/mol
6. 100 mL of water, 100 mL of alcohol, and 200 mL of an unknown liquid, all at 25°C,
are heated at the same rate under identical conditions. After 3 minutes the
temperature of the alcohol is 50°C. It took 5 minutes for the water to reach 50°C. It
took 6 minutes for the unknown liquid to reach 50°C.
Which statement is TRUE regarding the specific heat, Cs?
A.
B.
C.
D.
7. Cs (water) = Cs (alcohol)
Cs (water) < Cs (unknown)
Cs (water) > Cs (alcohol)
Cs (alcohol) > Cs (unknown)
What amount of heat energy, kJ, is released in the combustion of 16.0 g of C3H6?
2 C3H6(g) + 9 O2(g) → 6 CO2(g) + 6 H2O(l)
A.
B.
C.
D.
E.
8. 624
783
504
581
725
Which of these will lead to the greatest increase in temperature when added to
100.0 mL of water at 25°C?
A.
B.
C.
D.
ΔH° = -4120 kJ
70 g of copper at 150°C, specific heat = 0.385 J/g K.
50 g of iron at 110°C, specific heat = 0.452 J/g K.
94 g of gold at 150°C, specific heat = 0.128 J/g K.
66 g of silver at 124°C, specific heat = 0.234 J/g K.
3 9. Given the following equations and ΔH° values, determine the heat of reaction (kJ)
at 298 K for the reaction:
2 NF3(g) + Cu(s) → N2F4(g) + CuF2(s)
2 NF3(g) + 2 NO(g) → N2 F4(g) + 2 NOF(g)
NO(g) + ½F2(g) → NOF(g)
Cu(s) + F2(g) → CuF2(g)
A.
B.
C.
D.
E.
ΔH° (kJ)
-82.9
-156.9
-531.0
-605.0
-291.6
-300.1
+291.2
+770.8
10. A volume of 50.0 mL of 0.400 M NaOH(aq) was added to 20.0 mL of 0.500 M
H2SO4(aq) in a calorimeter of heat capacity 39.0 JK-1. The temperature of the
resulting solution rose by 3.60°C. What is the total heat produced (in kJ) in this
neutralization? Assume that the specific heat capacity of the neutralized solution is
4.18 J.K-1g-1.
H2SO4(aq) + 2 NaOH(aq) → 2 Na2SO4(aq) + H2O(l)
A.
B.
C.
D.
E.
-126
-119
-102
-111
-132
4 11. In the introduction to Chapter 6 I played several clips from the hit TV show “The
Big Bang Theory” in class. In this episode, Dr. Sheldon Cooper is trying to
visualize the behavior of electrons traveling through a graphene sheet. Which of the
following statements is/are true regarding his findings?
i) Sheldon’s model of the behavior of electrons failed with lima beans, peas, and
marbles, but he was able to come up with an accurate model with balls from a ball
pit after he determined the proper size ratio with bigger carbon atoms.
ii) Just like Dalton, Thompson, and Bohr, it was relatively easy for Sheldon to
develop an accurate model of the behavior of an electron.
iii) Sheldon’s model of the behavior of electrons failed with lima beans, peas, and
marbles, but he was able to come up with an accurate model after recognizing the
electron behaved as both a particle and a wave.
A.
B.
C.
D.
E.
iii only
ii & iii
i & ii
i & iii
ii only 12. What is the energy of the photons emitted from the He-Ne laser, wavelength = 655
nm?
A.
B.
C.
D.
E.
3.03 10-19 J
4.34 10-40 J
5.29 10-18 J
2.27 10-19 J
1.01 10-27 J
13. Which emission line in the hydrogen spectrum occurs at highest frequency?
A.
B.
C.
D.
E.
n = 5 to n = 7
n = 4 to n = 2
n = 2 to n = 4
n = 1 to n =3
n = 3 to n = 1
5 14. Suppose a certain atom has four energy levels, and assume all transitions between
levels are possible. Which statement is TRUE?
A.
B.
C.
D.
E.
The longest wavelength light is emitted for n = 4 → n = 2
There are a total of 6 spectral emission lines.
The potential energy is greatest when the electron is at the n=1 level.
The lowest energy light is emitted for n=3 → n = 1
There are a total of 4 spectral emission lines.
15. Sodium metal requires a photon with a minimum energy of 4.41 x 10-19 J to emit
electrons. Suppose you have two lasers, one emitting light with a wavelength of
210 nm and the other emitting light with a wavelength of 335 nm. Each laser
produces 10,000 photons/sec.
Which statement is true regarding the removal of electrons from the metal’s
surface?
A.
B.
C.
D.
E.
Both lasers eject electrons from the metal surface, but the weaker
laser needs to operate for a longer period of time.
Both lasers eject electrons from the metal surface at the same rate.
Only the laser with photons of 335 nm ejects electrons.
Only the laser with photons of 210 nm ejects electrons.
Neither laser will eject electrons.
6 16. Which of the following statements best describes a 4dxz atomic orbital?
A.
B.
C.
D.
E.
The 4dxz orbital has more radial nodes than angular nodes.
The 4dxz orbital has more angular nodes than radial nodes.
The 4dxz orbital has the same number of radial and angular nodes. The 4dxz orbital does not have any radial nodes.
The 4dxz orbital does not have any angular nodes.
17. Which of the following electron configurations is correct for mercury (Hg)?
A.
B.
C.
D.
E.
[Xe] 4s25f146d10
[Kr] 6s26f146d10
[Xe] 6s24f146d10
[Xe] 6s25d10
[Xe] 6s24f145d10
18. How many electrons in a zinc atom have the quantum number ml = 0 ?
A.
B.
C.
D.
E.
10
14
6
8
30
19. Which response correctly fills in the blanks?
The atom _________________ has _________ core electrons, __________ valence
electrons, and _____________unpaired electrons.
A.
B.
C.
D.
E.
nitrogen, 2, 5, 3
neon, 2, 8, 6
oxygen, 2, 6, 4
chlorine, 12, 5, 2
fluorine, 2, 7, 5
20. Which of the following sets of quantum numbers could describe one of the valence
electrons in a sulfur atom in the ground state?
A.
B.
C.
D.
E.
n= 3
n= 4
n= 2
n= 3
n= 1
l=1
l=0
l=1
l=3
l=0
ml = 0 ms = +½
ml = -1 ms = +½
ml = -1 ms = -½
ml = -2 ms = +½
ml = 0 ms = +½
7 21. The attraction of the nucleus on the outermost electron in an atom tends to:
A.
B.
C.
D.
E.
decrease moving from left to right and bottom to top on the periodic table.
decrease moving from right to left and bottom to top of the periodic table.
decrease moving from left to right and top to bottom on the periodic table. decrease moving from right to left and top to bottom on the periodic table.
the attraction of the nucleus to the outermost electron remains constant for
each element on the periodic table.
22. Lithium’s first and second ionization energies are 519 kJ/mol and 7300 kJ/mol,
respectively. Element X has a first ionization energy of 590 kJ/mol and a second
ionization energy of 1150 kJ/mol. Element X is most likely to be:
A.
B.
C.
D.
E.
Calcium
Sodium
Oxygen
Xenon
Fluorine
23. Which of the following is correctly ordered in terms of atomic radius, from smallest
to largest?
A.
B.
C.
D.
E.
F- < Mg2+ < Na+
F- < Na+ < Mg2+
Mg2+ < F-< Na+
Mg2+ < Na+ < FNa+ < F- < Mg2+
24. Arrange the following in order of increasing electron affinity: Cl, P, S, Ar.
A.
B.
C.
D.
E.
Most positive EA
Most positive EA
Most positive EA
Most positive EA
Most positive EA
Ar < Cl < S < P
Cl < S < P < Ar
P < S < Cl < Ar
Ar < P < S < Cl
Cl < Ar < P < S
Most negative EA
Most negative EA Most negative EA
Most negative EA
Most negative EA
25. Which of the following statements is TRUE?
A.
B.
C.
D.
E.
The electron affinity of C is greater than that of Cl.
The first ionization potential of H is greater than that of He.
The atomic radius of Li is larger than that of Cs.
The ionic radius of Fe+ is larger than that of Fe3+.
All are false.
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