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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$4$

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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 ($6$ 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 $4$.

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?