What is the correct order of Lewis acidic str | vedclass

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(A) $(I)$ The Lewis acidity of boron trihalides is governed by the extent of $p\pi-p\pi$ back-bonding between the halogen atom and the boron atom.$(II

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$BF_3 < BCl_3 < BBr_3 < BI_3$

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(A) $(I)$ The Lewis acidity of boron trihalides is governed by the extent of $p\pi-p\pi$ back-bonding between the halogen atom and the boron atom.$(II)$ In $BF_3$,the small size of the fluorine atom allows for effective $2p-2p$ back-bonding,which significantly reduces the electron deficiency of the boron atom.$(III)$ As the size of the halogen atom increases from $F$ to $I$,the effectiveness of back-bonding decreases,making the boron atom more electron-deficient and thus more acidic.$(IV)$ Therefore,the correct order of Lewis acidic strength is $BF_3 < BCl_3 < BBr_3 < BI_3$.

What is the correct order of Lewis acidic strength for boron trihalides?

Similar Questions

Identify the correct statements from the following:
$(i)$ The atomic radius of $Al$ is lower than the atomic radius of $Ga$.
$(ii)$ Boron exists in many allotropic forms.
$(iii)$ The melting point of $Ga$ is lowest among the group $13$ elements.

In the reactions $I$ and $II$,the covalencies of $Be$ and $Al$ in $X$ and $Y$ are respectively:
$I$ $Be(OH)_2 + NaOH \text{ (excess)} \rightarrow X$
$II$ $Al(OH)_3 + NaOH \text{ (excess)} \rightarrow Y$

The correct Lewis acidity order of $BX_3$ is:

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$\underline{B}_2O_3 + 3H_2O \longrightarrow 2H_3BO_3$

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