Bonding and the Periodic Table Discussion

Bonding and the Periodic Table Discussion
84. How does the atomic radius of potassium relate to the atomic radius
of arsenic?
(A) Potassium is smaller because the effective nuclear charge is smaller.
(B) Potassium is larger because the effective nuclear charge is larger.
(C) Potassium is larger because the effective nuclear charge is smaller.
(D) Potassium is smaller because the effective nuclear charge is larger.
85. In the Lewis structure of MgCl2, how many electrons are shared?
(A) 0
(B) 1
(C) 2
(D) 8
Bonding and the Periodic Table Discussion
86. How does the third ionization energy of Ca compare with the third
ionization energy of Sc?
(A) The value for Ca is much higher.
(B) The value for Ca is much lower.
(C) The values are the same.
(D) Unrelated because Sc is a transition element and Ca is not.
87. Which of the following is the correct Lewis structure for O2?
(A) O O
(B) O O
(C) O O
(D) O O
CHAPTER 3
20 ❯ McGraw-Hill’s 500 MCAT General Chemistry Questions
88. An excited-state potassium atom emits light of characteristic wavelengths.
These emitted wavelengths are due to
(A) excited-state electrons moving to higher energy levels
(B) excited-state electrons dropping to lower energy levels
(C) transitions within the potassium nucleus
(D) excited-state potassium atoms interacting with ground-state
potassium atoms
89. Ethyl alcohol has a normal boiling point of 78∘C. The normal boiling
point is determined at
(A) a pressure of 760 torr
(B) a pressure below 760 torr
(C) a pressure above 760 torr
(D) all pressures
90. The radius of a nitrogen atom is about 75 pm. The addition of electrons
to a nitrogen atom results in an increase in the radius. Each added electron
increases the radius by about 20%. What is the approximate radius of
a nitride ion?
(A) 138 pm
(B) 110 pm
(C) 90 pm
(D) 60 pm
91. The rate of the passive diffusion of ions across a cell membrane is inversely
proportional to the radius of the ion. Which of the following ions has
the slowest rate of passive diffusion?
(A) F−
(B) K
(C) Ba²
(D) Mg²
92. Many properties of the elements show a general periodic trend.
What is the general trend in the ionization energies of the elements?
(A) Increases to the left and downward
(B) Decreases to the left and downward
(C) Decreases to the left and increases downward
(D) Increases to the left and decreases downward
Bonding and the Periodic Table ❮ 21
93. Why is the second electron affinity of an atom significantly greater
than the first electron affinity?
(A) This makes an electron capture process more likely.
(B) This completes the stable electron configuration.
(C) The second electron is held more tightly than the first.
(D) There is repulsion of like charges.
Bonding and the Periodic Table Discussion
94. Why is the ionization energy of sodium lower than that of chlorine?
(A) The valence electron of sodium is closer to the nucleus and
experiences a lower effective nuclear charge.
(B) The valence electron of sodium is farther from the nucleus and
experiences a lower effective nuclear charge.
(C) The valence electron of sodium is farther from the nucleus and
experiences a higher effective nuclear charge.
(D) The valence electron of sodium is closer to the nucleus and
experiences a higher effective nuclear charge.
95. Oxygen molecules will bind to the iron in hemoglobin. When this occurs,
the oxygen molecule is acting as
(A) an oxidizing agent
(B) a Lewis acid
(C) a Lewis base
(D) a reducing agent
96. The BEST way of describing the binding of oxygen to the iron
in hemoglobin is the formation of
(A) a dipole-dipole interaction
(B) an ionic bond
(C) a metallic bond
(D) a coordinate covalent bond
97. The following is a Lewis structure for nitrous acid:
H O N O
What is the correct sequence (left to right) of the formal charges?
(A) 1, −2, 3, −2
(B) 0, 0, 0, 0
(C) 1, −1, 2, −2
(D) −1, −2, 5, −2

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