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141. What is the best approximation for the normal boiling point of octane in
Figure 4.3?
(A) 126°C
(B) 100°C
(C) 145°C
(D) 98°C
142. According to Figure 4.4, the alkanes exhibit normal boiling points most
similar to which other group?
(A) Alkynes
(B) Alcohols
(C) Carboxylic acids
(D) Amines
143. Based on the data in Figure 4.4, a 2-carbon alcohol would exhibit a normal
boiling point closest to that of a:
(A) 3-carbon alkane.
(B) 9-carbon alkene.
(C) 4-carbon ketone.
(D) 2-carbon carboxylic acid.
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144. Based on the data in Figure 4.4, which type of bond listed in Table 4.1 is
the weakest?
(A) Dipole–dipole
(B) Double hydrogen
(C) Van der Waals
(D) Single hydrogen
145. Caproic acid is a carboxylic acid with a molecular formula of C6H12O2.
Which of the following temperatures is closest to the normal boiling point
of caproic acid?
(A) 200°C
(B) 250°C
(C) 100°C
(D) 125°C
146. Based on the data in Figure 4.4, which of the following lists the bonds in
Table 4.1 from the highest to the lowest boiling point required to break
them?
(A) Van der Waals, dipole–dipole, single hydrogen, double hydrogen
(B) Double hydrogen, single hydrogen, dipole–dipole, Van der Waals
(C) Single hydrogen, double hydrogen, dipole–dipole, Van der Waals
(D) Dipole–dipole, Van der Waals, single hydrogen, double hydrogen
68 › McGraw Hill 500 ACT Science Questions
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Test 4 ‹ 69
147. Which of the following generalizations about the relationship between an
organic compound’s molecular weight and its boiling point is best supported
by the data in Table 4.2?
(A) The boiling point varies directly with molecular weight.
(B) As molecular weight increases, the boiling point decreases.
(C) As molecular weight decreases, the boiling point increases.
(D) The boiling point is not determined by molecular weight.
148. Based on the data in Figure 4.4, n-Butanol (see Table 4.2) most likely
contains which functional group?
(A) Alcohol
(B) Ester
(C) Amine
(D) Alkyne
149. Based on the information in the passage, which of the following can be
inferred about the type of bonds in an organic compound?
(A) Double hydrogen bonds are easier to break at high temperatures than
single hydrogen bonds.
(B) Dipole–dipole bonds require the highest boiling point to break of all
four types of bonds.
(C) Van der Waals bonds become easier to break as a compound’s vapor
pressure is increased.
(D) At the same vapor pressure, single hydrogen bonds require a higher
boiling point to break than dipole–dipole bonds.
150. Which of the following generalizations is best supported by the data in
Figures 4.3 and 4.4?
(A) Organic compounds containing the same number of carbon atoms
have similar boiling points.
(B) The boiling point increases with the number of carbon atoms among
organic compounds within the same group.
(C) The number of carbon atoms in an organic compound cannot be
used to predict the compound’s relative boiling point.
(D) The greater the number of carbon atoms in an organic compound,
the lower that compound’s boiling point is.
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