AP Chemistry
2.7 VSEPR and Hybridization
2.5 Lewis Diagrams
Gaseous boron trifluoride, \(\text{BF}_3\), reacts with ammonia, \(\text{NH}_3\), to form a solid Lewis acid-base adduct according to the equation below.
\[ \text{BF}_3\text{(g)} + \text{NH}_3\text{(g)} \rightarrow \text{F}_3\text{B-NH}_3\text{(s)} \]
During this reaction, the nitrogen atom in \(\text{NH}_3\) donates a lone pair of electrons into the vacant \(2\text{p}\) orbital of the boron atom to form a coordinate covalent bond. Which of the following correctly identifies the hybridization of the boron atom and the approximate \(\text{F}-\text{B}-\text{F}\) bond angle in the resulting \(\text{F}_3\text{B-NH}_3\) adduct?
\[ \text{BF}_3\text{(g)} + \text{NH}_3\text{(g)} \rightarrow \text{F}_3\text{B-NH}_3\text{(s)} \]
During this reaction, the nitrogen atom in \(\text{NH}_3\) donates a lone pair of electrons into the vacant \(2\text{p}\) orbital of the boron atom to form a coordinate covalent bond. Which of the following correctly identifies the hybridization of the boron atom and the approximate \(\text{F}-\text{B}-\text{F}\) bond angle in the resulting \(\text{F}_3\text{B-NH}_3\) adduct?
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