Which of the following molecules can show Lew | vedclass

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(B) Lewis acid is a substance that can accept an electron pair.$(I)$ $CO_2$: The carbon atom is electron-deficient due to the electronegative oxygen a

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$I, II, III$

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(B) Lewis acid is a substance that can accept an electron pair.$(I)$ $CO_2$: The carbon atom is electron-deficient due to the electronegative oxygen atoms,allowing it to accept electron pairs.$(II)$ $Br_2$: The $Br-Br$ bond can undergo polarization,and the $Br$ atom can accept an electron pair in its vacant $d$-orbitals.$(III)$ $SnCl_2$: The $Sn$ atom has an incomplete octet (only $6$ electrons),making it a strong Lewis acid.$(IV)$ $HF$: Acts primarily as a Brønsted acid,not a Lewis acid.$(V)$ $NMe_3$: The nitrogen atom has a lone pair,making it a Lewis base.Therefore,$(I)$,$(II)$,and $(III)$ show Lewis acidity.

Which of the following molecules can show Lewis acidity?
$(I)$ $CO_2$ $(II)$ $Br_2$ $(III)$ $SnCl_2$ $(IV)$ $HF$ $(V)$ $NMe_3$

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Which of the following molecules can show Lewis acidity?$(I)$ $CO_2$ $(II)$ $Br_2$ $(III)$ $SnCl_2$ $(IV)$ $HF$ $(V)$ $NMe_3$