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83. Which of the following electron configurations is correct?
A)
Ga: [Kr]4s23d104p1
B)
Mo: [Kr]5s24d5
C)
Ca: [Ar]4s13d10
D)
Br: [Kr]4s23d104p7
E)
Bi: [Xe]6s24f145d106p3
84. 1s22s22p63s23p64s23d2 is the correct electron configuration for which of the following
atoms?
A)
Ca
B)
Ti
C)
Ge
D)
Zr
E)
none of these
85. Which of the following atoms has three electrons in p orbitals in its valence shell?
A)
Ba
B)
Ga
C)
V
D)
Bi
E)
none of these
86. How many of the following electron configurations for the species in their ground state are
correct?
I.
Ca:
1s22s22p63s23p64s2
II.
Mg:
1s22s22p63s1
III.
V:
[Ar]3s23d3
IV.
As:
[Ar]4s23d104p3
V.
P:
1s22s22p63p5
A)
1
B)
2
C)
3
D)
4
E)
5
87. The number of unpaired electrons in the outer subshell of a Cl atom is
A)
0
B)
1
C)
2
D)
3
E)
none of these
88. For which of the following elements does the electron configuration for the lowest energy
state show a partially filled d orbital?
A)
Ti
B)
Rb
C)
Cu
D)
Ga
E)
Kr
89. Which of the following electron configurations is different from that expected?
A)
Ca
B)
Sc
C)
Ti
D)
V
E)
Cr
90. Which of the following have 10 electrons in the d orbitals?
A)
Mn
B)
Fe
C)
Cu
D)
Zn
E)
two of the above
91. Which of the following is the highest energy orbital for a silicon atom?
A)
1s
B)
2s
C)
3s
D)
3p
E)
3d
92. When electron configurations differ from expected, it is because orbitals want to be
half-filled.
93. Copper exhibits the expected electron configuration.
94. Which of the following processes represents the ionization energy of bromine?
A)
Br(s) Br+(g) + e–
B)
Br(l) Br+(g) + e–
C)
Br(g) Br+(g) + e–
D)
Br(s) Br+(s) + e–
E)
Br2(g) Br2+(g) + e–
95. Order the elements S, Cl, and F in terms of increasing ionization energy.
A)
S, Cl, F
B)
Cl, F, S
C)
F, S, Cl
D)
F, Cl, S
E)
S, F, Cl
96. Order the elements S, Cl, and F in terms of increasing atomic radii.
A)
S, Cl, F
B)
Cl, F, S
C)
F, S, Cl
D)
F, Cl, S
E)
S, F, Cl
97. Which of the following atoms would have the largest second ionization energy?
A)
Mg
B)
Cl
C)
S
D)
Ca
E)
Na
98. The first ionization energy of Mg is 735 kJ/mol. The second ionization energy is
A)
735 kJ/mol
B)
less than 735 kJ/mol
C)
greater than 735 kJ/mol
D)
More information is needed to answer this question.
E)
None of these.
99. Which of the following exhibits the correct orders for both atomic radius and ionization
energy, respectively? (smallest to largest)
A)
S, O, F, and F, O, S
B)
F, S, O, and O, S, F
C)
S, F, O, and S, F, O
D)
F, O, S, and S, O, F
E)
none of these
100. Choose the element with the highest ionization energy.
A)
Na
B)
Mg
C)
Al
D)
P
E)
S
101. Which of the following concerning second ionization energies is true?
A)
That of Al is higher than that of Mg because Mg wants to lose the second electron,
so it is easier to take the second electron away.
B)
That of Al is higher than that of Mg because the electrons are taken from the same
energy level, but the Al atom has one more proton.
C)
That of Al is lower than that of Mg because Mg wants to lose the second electron,
thus the energy change is greater.
D)
That of Al is lower than that of Mg because the second electron taken from Al is in
a p orbital, thus it is easier to take.
E)
The second ionization energies are equal for Al and Mg.
102. Consider a planet where the temperature is so high that the ground state of an electron in the
hydrogen atom is n = 4. What is the ratio of ionization energy for hydrogen on this planet
compared to that on Earth?
A)
1 : 4
B)
4 : 1
C)
1 : 16
D)
16 : 1
E)
1 : 1
103. Consider the following orderings.
I.
Na+ < Mg2+ < Al3+ < Si4+
II.
Be < Mg < Ca < Sr
III.
I < Br < Cl < F
IV.
Al < Si < P < Cl
Which of these give(s) a correct trend in ionization energy?
A)
III
B)
II, IV
C)
I, IV
D)
I, III, IV
E)
none of them
104. List the following atoms in order of increasing ionization energy: Li, Na, C, O, F.
A)
Li < Na < C < O < F
B)
Na < Li < C < O < F
C)
F < O < C < Li < Na
D)
Na < Li < F < O < C
E)
Na < Li < C < F < O
105. Consider the ionization energy (IE) of the magnesium atom. Which of the following is not
true?
A)
The IE of Mg is lower than that of sodium.
B)
The IE of Mg is lower than that of neon.
C)
The IE of Mg is lower than that of beryllium.
D)
The IE of Mg is higher than that of calcium.
E)
The IE of Mg is lower than that of Mg+.
106. Of the following elements, which has the lowest first ionization energy?
A)
Ba
B)
Ca
C)
Si
D)
P
E)
Cl
107. Of the following elements, which is most likely to form a negative ion with charge 1–?
A)
Ba
B)
Ca
C)
Si
D)
P
E)
Cl
108. Which of the following atoms has the largest ionization energy?
A)
O
B)
Li
C)
Ne
D)
Be
E)
K
109. Which of the following statements is true?
A)
The first ionization potential of H is greater than that of He.
B)
The ionic radius of Fe+ is larger than that of Fe3+.
C)
The ionization energy of S2– is greater than that of Cl–.
D)
The atomic radius of Li is larger than that of Cs.
E)
All are false.
110. Which of the following statements is false?
A)
A sodium atom has a smaller radius than a potassium atom.
B)
A neon atom has a smaller radius than an oxygen atom.
C)
A fluorine atom has a smaller first ionization energy than an oxygen atom.
D)
A cesium atom has a smaller first ionization energy than a lithium atom.
E)
All are true.
111. The statement that the first ionization energy for an oxygen atom is lower than the first
ionization energy for a nitrogen atom is
A)
consistent with the general trend relating changes in ionization energy across a
period from left to right, because it is easier to take an electron from an oxygen
atom than from a nitrogen atom
B)
consistent with the general trend relating changes in ionization energy across a
period from left to right, because it is harder to take an electron from an oxygen
atom than from a nitrogen atom
C)
inconsistent with the general trend relating changes in ionization energy across a
period from left to right, due to the fact that the oxygen atom has two
doubly-occupied 2p orbitals and nitrogen has only one
D)
inconsistent with the general trend relating changes in ionization energy across a
period from left to right, due to the fact that oxygen has one doubly-occupied 2p
orbital and nitrogen does not
E)
incorrect
112. Sodium losing an electron is an ________ process and fluorine losing an electron is an
_______ process.
A)
endothermic, exothermic
B)
exothermic, endothermic
C)
endothermic, endothermic
D)
exothermic, exothermic
E)
more information needed
113. Which of the following statements is true about the ionization energy of Mg+?
A)
It will be equal to the ionization energy of Li.
B)
It will be equal to and opposite in sign to the electron affinity of Mg.
C)
It will be equal to and opposite in sign to the electron affinity of Mg+.
D)
It will be equal to and opposite in sign to the electron affinity of Mg2+.
E)
None of the above.
114. Which of the following statements is true?
A)
The krypton 1s orbital is smaller than the helium 1s orbital because krypton's
nuclear charge draws the electrons closer.
B)
The krypton 1s orbital is larger than the helium 1s orbital because krypton contains
more electrons.
C)
The krypton 1s orbital is smaller than the helium 1s orbital because krypton's p and
d orbitals crowd the s orbitals.
D)
The krypton 1s orbital and helium 1s orbital are the same size because both s
orbitals can only have two electrons.
E)
The krypton 1s orbital is larger than the helium 1s orbital because krypton's
ionization energy is lower, so it's easier to remove electrons.
115. Which of the following statements are false?
I.
It takes less energy to add an electron to nitrogen than to carbon because nitrogen
will be closer to achieving a noble gas configuration.
II.
It takes more energy to add an electron to fluorine than to oxygen because the radius
of fluorine is smaller and more repulsion would occur in the p-orbitals.
III.
It takes more energy to add an electron to nitrogen than to carbon because of the
extra repulsions that would occur in the 2p orbitals.
IV.
Less energy is released in adding an electron to iodine than to chlorine because
the radius of iodine is larger and the electron is added at a distance further
from the nucleus.
A)
II, III
B)
I, II, IV
C)
III only
D)
I, II
E)
All of the above are false statements.
116. The second ionization energy for calcium is smaller than the first ionization energy.
117. Ionization energy increases with an increasing number of electrons.
118. When examining the electromagnetic spectrum, why is it more harmful to be exposed to
x-rays than radio waves over a period of time? In your explanation, include the concepts of
frequency, waves, and energy. Also, draw transverse waves to assist in your explanation.
119. Photogray lenses incorporate small amounts of silver chloride in the glass of the lens. The
following reaction occurs in the light, causing the lenses to darken:
AgCl → Ag + Cl
The enthalpy change for this reaction is 3.10 102 kJ/mol. Assuming all this energy is
supplied by light, what is the maximum wavelength of light that can cause this reaction?
120. Electromagnetic radiation can be viewed as a stream of "particles" called __________.
121. __________ results when light is scattered from a regular array of points or lines.
122. How does the Bohr theory explain the emission and absorption spectra of hydrogen?
123. A specific wave function is called a(n) __________.
124. The __________ quantum number is related to the size and energy of the orbital.
125. Consider the following sets of quantum numbers. Which set(s) represent(s) impossible
combinations?
n
l
ml
Set a
1
0
1
Set b
3
3
0
Set c
2
1
1
Set d
3
2
–2
Set e
3
1
–2
Set f
2
0
0
126. A hydrogen 3s wave function has __________ (how many?) nodal planes and __________
(how many?) radial nodes (not counting r = 0).
127. Areas of zero probability of finding an electron are called _________.
128. The ____________ states that in a given atom no two electrons can have the same set of
four quantum numbers.
129. How many electrons in an atom can have the following quantum numbers?
a) n = 3
b) n = 2, l = 0
c) n = 2, l = 2, ml = 0
d) n = 2, l = 0, ml = 0, ms = 1/2
130. Give the quantum numbers for the last electron in:
a) gold
b) magnesium
c) iodine
d) cadmium
131. [Ar]4s13d5
132. [Ne]3s23p5
133. [Kr]5s24d105p4
134. [Ar]4s13d10
135. [He]2s22p3
136. P
137. Ag
138. S2–
139. I
140. K+
141. The __________ electrons are in the outermost principal quantum level of an atom.
142. In general, the ionization energy and electron affinity involve more energy from
__________ (left to right or right to left) in a period of the periodic table. Why?
143. In general, the ionization energy and electron affinity involve more energy from _________
(top to bottom or bottom to top) in a family of the periodic table. Why?
144. For the set of elements Be, B, C, and N, which element has the smallest ionization energy?
Explain any deviation from the expected pattern.
145. For the set of elements Li, O, Ne, and Na, which element has the largest atomic radius?
Explain any deviation from the expected pattern.
146. Larger first ionization energy, Li or Be
147. Larger first ionization energy, Na or Rb
148. Larger first ionization energy, Be or B
149. Larger first ionization energy, C or N
150. Larger second ionization energy, Na or Mg
151. Larger atomic radius, P or Sb
152. Larger atomic radius, N or O
153. Larger atomic or ionic radius, F or F–
154. Larger atomic or ionic radius, Mg or Mg2+
155. Larger atomic radius, Fe2+ or Fe3+
156. The calcium atom is much larger than the calcium ion, while the fluorine atom is much
smaller than the fluorine ion. Explain this natural occurrence.
Consider the graph below to answer the next two questions:
157. Explain why argon has the highest ionization energy.
158. Explain the ionization energy difference between sodium and potassium.
