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

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

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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 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.

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

Similar Questions

Which one of the following statements is correct?

The ionization constants of $HF$,$HCOOH$,and $HCN$ at $298 \ K$ are $6.8 \times 10^{-4}$,$1.8 \times 10^{-4}$,and $4.8 \times 10^{-9}$ respectively. Calculate the ionization constants of their corresponding conjugate bases.

For the following two acid-base reactions,which statement is True?
$(I) CH_3CH_2^- + CH_3NH_2$ $(pK_a = 35)$ $\rightleftharpoons CH_3CH_3$ $(pK_a = 50)$ $+ CH_3NH^-$
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