Question:
Which of the following can act as Lewis acids?
[i.] \( {CCl}_4 \)
[ii.] \( {GeCl}_4 \)
[iii.] \( {SiF}_4 \)
Which of the following can act as Lewis acids?
[i.] \( {CCl}_4 \)
[ii.] \( {GeCl}_4 \)
[iii.] \( {SiF}_4 \)
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In assessing Lewis acidity, focus on the electronic structure and the availability of vacant orbitals that can accommodate additional electron pairs.
Updated On: Mar 25, 2025
- \({CCl}_4\), \({SiF}_4\) only
- \({SiF}_4\) only
- \({SiF}_4\), \({GeCl}_4\) only
- \({CCl}_4\), \({GeCl}_4\), \({SiF}_4\)
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The Correct Option is C
Solution and Explanation
Lewis acids are defined as compounds that can accept a pair of electrons. Among the given compounds:
- \({CCl}_4\) does not have any vacant orbitals available to accept electrons, thus it does not typically act as a Lewis acid.
- \({GeCl}_4\) and \({SiF}_4\) can act as Lewis acids as they have vacant d-orbitals that can accept electron pairs.
Thus, \({SiF}_4\) and \({GeCl}_4\) are the correct choices, capable of acting as Lewis acids by accepting electron pairs.
- \({CCl}_4\) does not have any vacant orbitals available to accept electrons, thus it does not typically act as a Lewis acid.
- \({GeCl}_4\) and \({SiF}_4\) can act as Lewis acids as they have vacant d-orbitals that can accept electron pairs.
Thus, \({SiF}_4\) and \({GeCl}_4\) are the correct choices, capable of acting as Lewis acids by accepting electron pairs.
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