The approximate boiling points for hydrogen compounds of some elements in the nitrogen family are $$\(\left(\mathrm{SbH}_{3}-15^{\circ} \mathrm{C}\right),\left(\mathrm{AsH}_{3}-\right.\)$$ $$\(\left.62^{\circ} \mathrm{C}\right),\left(\mathrm{PH}_{3}-87^{\circ} \mathrm{C}\right)\)$$, and $$\(\left(\mathrm{NH}_{3}-33^{\circ} \mathrm{C}\right)\)$$. Which of the following is the best explanation for the fact that $$\(\mathrm{NH}_{3}\)$$ does NOT follow the trend of the other hydrogen compounds?
A.
\(\mathrm{NH}_{3}\) is the only one to exhibit hydrogen bonding.
B.
\(\mathrm{NH}_{3}\) is the only one that is water soluble.
C.
\(\mathrm{NH}_{3}\) is the only one that is nearly ideal in the gas phase.
D.
\(\mathrm{NH}_{3}\) is the only one that is a base.
Exam No：AP Chemistry Practice Test Year：2024 Question No：8
Answer:
A
Knowledge points:
3.10 Solubility
Solution:
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