Observe the following species:(i) NH_3(ii) Al | vedclass

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(C) Lewis acid is an electron-pair acceptor.$(i)$ $NH_3$: Has a lone pair on $N$,acts as a Lewis base.$(ii)$ $AlCl_3$: $Al$ has an incomplete octet ($

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$4$

Vedclass · Answer

(C) Lewis acid is an electron-pair acceptor.$(i)$ $NH_3$: Has a lone pair on $N$,acts as a Lewis base.$(ii)$ $AlCl_3$: $Al$ has an incomplete octet ($6$ electrons),acts as a Lewis acid.$(iii)$ $SnCl_4$: $Sn$ has vacant $d$-orbitals and can expand its octet,acts as a Lewis acid.$(iv)$ $CO_2$: The $C$ atom is electron-deficient due to the high electronegativity of oxygen atoms,acts as a Lewis acid.$(v)$ $Ag^{+}$: $A$ metal cation with vacant orbitals,acts as a Lewis acid.$(vi)$ $HSO_4^{-}$: Can act as a Lewis base (due to lone pairs on $O$) or a Brønsted-Lowry acid,but is not typically classified as a Lewis acid in this context.Therefore,$AlCl_3$,$SnCl_4$,$CO_2$,and $Ag^{+}$ act as Lewis acids.The total count is $4$.

List-$I$	List-$II$
$(1)$ Kossel and Lewis	$(A)$ $VSEPR$
$(2)$ Langmuir	$(B)$ Molecular Orbital Theory
$(3)$ Sidgwick and Powell	$(C)$ Covalent Bond
$(4)$ Heitler and London	$(D)$ Octet Rule
$(5)$ $F$. Hund and Mulliken	$(E)$ Valence Bond Theory

Observe the following species:
$(i)$ $NH_3$
$(ii)$ $AlCl_3$
$(iii)$ $SnCl_4$
$(iv)$ $CO_2$
$(v)$ $Ag^{+}$
$(vi)$ $HSO_4^{-}$
How many of the above species act as Lewis acids?

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Observe the following species:$(i)$ $NH_3$$(ii)$ $AlCl_3$$(iii)$ $SnCl_4$$(iv)$ $CO_2$$(v)$ $Ag^{+}$$(vi)$ $HSO_4^{-}$How many of the above species act as Lewis acids?