Which of the following species are only Lewis | vedclass

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(A) Lewis acid is an electron pair acceptor,while a Bronsted acid is a proton $(H^{+})$ donor.$1$. $CO_{2}$: It has no $H$ atom to donate,so it is not

Vedclass · Accepted Answer

$CO_{2}, BCl_{3}, NO_{2}^{+}$

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(A) Lewis acid is an electron pair acceptor,while a Bronsted acid is a proton $(H^{+})$ donor.$1$. $CO_{2}$: It has no $H$ atom to donate,so it is not a Bronsted acid. It acts as a Lewis acid by accepting electron pairs from bases like $OH^{-}$.$2$. $BCl_{3}$: It has an incomplete octet (electron deficient),acting as a Lewis acid. It has no $H$ atom,so it is not a Bronsted acid.$3$. $NO_{2}^{+}$: It is electron deficient (positive charge),acting as a Lewis acid. It has no $H$ atom,so it is not a Bronsted acid.$4$. $NH_{3}$ and $CH_{3}NH_{2}$: These are Bronsted bases (proton acceptors) and Lewis bases (electron pair donors).$5$. $C_{6}H_{5}NH_{3}^{+}$: This is a Bronsted acid as it can donate a proton.Therefore,the species that are only Lewis acids but not Bronsted acids are $CO_{2}, BCl_{3}$,and $NO_{2}^{+}$.

Species	Conjugate acid
$ (a) NH_{3} $	$ (i) H_{2}CO_{3} $
$ (b) HCO_{3}^{-} $	$ (ii) H_{3}O^{+} $
$ (c) H_{2}O $	$ (iii) NH_{4}^{+} $
$ (d) HSO_{4}^{-} $	$ (iv) H_{2}SO_{4} $

Which of the following species are only Lewis acids but not Bronsted acids from $CO_{2}$,$BCl_{3}$,$NH_{3}$,$CH_{3}NH_{2}$,$NO_{2}^{+}$,and $C_{6}H_{5}NH_{3}^{+}$?

Similar Questions

Which activity from the following is exhibited by a $Lewis$ base according to its definition?

The acid that results when a base accepts a proton is called

The strongest Bronsted base among the following anions is

Match the following species with their respective conjugate acids:

Species Conjugate acid

$ (a) NH_{3} $ $ (i) H_{2}CO_{3} $

$ (b) HCO_{3}^{-} $ $ (ii) H_{3}O^{+} $

$ (c) H_{2}O $ $ (iii) NH_{4}^{+} $

$ (d) HSO_{4}^{-} $ $ (iv) H_{2}SO_{4} $

Which of the following is a set of amphiprotic species?

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