Question:
Which of the following behaves as a Lewis acid?
Which of the following behaves as a Lewis acid?
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Electron-deficient molecules like \(BF_3\), \(BCl_3\), and \(AlCl_3\) behave as Lewis acids because they can accept electron pairs.
Updated On: Jun 26, 2026
- \(PH_3\)
- \(BF_3\)
- \(NMe_3\)
- \(CO\)
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The Correct Option is B
Solution and Explanation
Step 1: Recall the definition of Lewis acid.
A Lewis acid is a species that can accept an electron pair.
A Lewis base is a species that can donate an electron pair.
Step 2: Analyze \(BF_3\).
In \(BF_3\), boron has only six electrons in its valence shell.
Thus, boron is electron deficient and can accept an electron pair from a Lewis base.
Therefore, \[ BF_3 \] acts as a Lewis acid.
Step 3: Analyze the other options.
\(PH_3\) has a lone pair on phosphorus and generally behaves as a Lewis base.
\(NMe_3\) has a lone pair on nitrogen and behaves as a Lewis base.
\(CO\) can donate an electron pair through carbon and often behaves as a ligand or Lewis base.
Hence, these are not the best Lewis acids among the given options.
Step 4: Final conclusion.
Therefore, the species that behaves as a Lewis acid is \[ \boxed{BF_3} \] Hence, the correct option is \[ \boxed{(2)} \]
A Lewis acid is a species that can accept an electron pair.
A Lewis base is a species that can donate an electron pair.
Step 2: Analyze \(BF_3\).
In \(BF_3\), boron has only six electrons in its valence shell.
Thus, boron is electron deficient and can accept an electron pair from a Lewis base.
Therefore, \[ BF_3 \] acts as a Lewis acid.
Step 3: Analyze the other options.
\(PH_3\) has a lone pair on phosphorus and generally behaves as a Lewis base.
\(NMe_3\) has a lone pair on nitrogen and behaves as a Lewis base.
\(CO\) can donate an electron pair through carbon and often behaves as a ligand or Lewis base.
Hence, these are not the best Lewis acids among the given options.
Step 4: Final conclusion.
Therefore, the species that behaves as a Lewis acid is \[ \boxed{BF_3} \] Hence, the correct option is \[ \boxed{(2)} \]
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