Which of the following equilibria represents | vedclass

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(D) $Lewis$ acid-base reaction involves the donation of a lone pair of electrons from a $Lewis$ base to a $Lewis$ acid to form a coordinate covalent b

Vedclass · Accepted Answer

$Cu^{2+} + 4NH_3 \rightleftharpoons [Cu(NH_3)_4]^{2+}$

Vedclass · Answer

(D) $Lewis$ acid-base reaction involves the donation of a lone pair of electrons from a $Lewis$ base to a $Lewis$ acid to form a coordinate covalent bond.In the reaction $Cu^{2+} + 4NH_3 \rightleftharpoons [Cu(NH_3)_4]^{2+}$,the $Cu^{2+}$ ion acts as a $Lewis$ acid (electron pair acceptor) and $NH_3$ acts as a $Lewis$ base (electron pair donor).This reaction does not involve the transfer of a proton $(H^+)$,which is the defining characteristic of a $Br\o nsted$ acid-base reaction. Therefore,it is a $Lewis$ acid-base reaction but not a $Br\o nsted$ acid-base reaction.

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 equilibria represents a $Lewis$ acid-base reaction but not a $Br\o nsted$ acid-base reaction?

Similar Questions

Four species are listed below:
$i. \, HCO_3^-$
$ii. \, H_3O^{+}$
$iii. \, HSO_4^-$
$iv. \, HSO_3F$
Which one of the following is the correct sequence of their acid strength?

In the following ionic equilibrium,the conjugate acid of $H_2O_2$ is ........
$H_2O_2 + H_2O \rightleftharpoons H_3O^+ + HO_2^-$

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} $

Ammonia is a Lewis base because it is

Which of the following statements is $NOT$ correct?

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