---
title: "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?"
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url: "https://nerd-notes.com/ubq/123518/"
date_modified: "2026-09-28T12:00:00+00:00"
---

# 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?

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?

- **A.** Hybridization: \(\text{sp}^2\) ; Bond angle: \(120^\circ\)
- **B.** Hybridization: \(\text{sp}^3\) ; Bond angle: \(109.5^\circ\)
- **C.** Hybridization: \(\text{sp}^3\) ; Bond angle: \(120^\circ\)
- **D.** Hybridization: \(\text{sp}^2\) ; Bond angle: \(109.5^\circ\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/123518/*