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Chapter 16: Problem 79

Classify each of these following species as a Lewis acid or a Lewis base: \((\mathrm{a}) \mathrm{CO}_{2},(\mathrm{~b}) \mathrm{H}_{2} \mathrm{O},(\mathrm{c}) \mathrm{I}^{-},(\mathrm{d}) \mathrm{SO}_{2}\) (e) \(\mathrm{NH}_{3},\) (f) \(\mathrm{OH}^{-}\) \((\mathrm{g}) \mathrm{H}^{+},(\mathrm{h}) \mathrm{BCl}_{3}\).

Short Answer

Expert verified
CO2, SO2, H+, and BCl3 are Lewis acids while H2O, I-, NH3, and OH- are Lewis bases.

Step by step solution

01

Classifying CO2

Since CO2 doesn't have a lone pair of electrons to donate, it can accept a pair of electrons. Therefore, CO2 is a Lewis acid.
02

Classifying H2O

H2O is capable of donating a pair of electrons due to the presence of two lone pairs on the oxygen atom. Therefore, H2O is a Lewis base.
03

Classifying I-

I- has a lone pair of electrons, which makes it capable of donating a pair of electrons. Therefore, I- is a Lewis base.
04

Classifying SO2

SO2 can potentially accept a pair of electrons due to its electron-deficient sulfur atom. Therefore, SO2 is a Lewis acid.
05

Classifying NH3

NH3 is capable of donating a pair of electrons due to the presence of a lone pair on the nitrogen atom. Therefore, NH3 is a Lewis base.
06

Classifying OH-

OH- has a lone pair of electrons and can therefore donate a pair of electrons. Therefore, OH- is a Lewis base.
07

Classifying H+

H+ is in need of two electrons to fill its outermost electron shell, so it can accept a pair of electrons. Therefore, H+ is a Lewis acid.
08

Classifying BCl3

BCl3 has an incomplete octet around the central B atom, which makes it capable of accepting a pair of electrons. Therefore, BCl3 is a Lewis acid.

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