(C) $BF_3$ is electron-deficient,meaning it acts as a lone-pair of electrons acceptor (Lewis acid).In $BF_3$,the central $B$ atom is $sp^2$ hybridized

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(C) $BF_3$ is electron-deficient,meaning it acts as a lone-pair of electrons acceptor (Lewis acid).In $BF_3$,the central $B$ atom is $sp^2$ hybridized and does not satisfy the octet rule because it has only $6$ bonded electrons in its valence shell.

Class 11 Chemistry 6-2.Equilibrium-II (Ionic Equilibrium)Acids and Bases

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Acidity of $BF_3$ can be explained on the basis of which of the following concepts?

AP EAMCET 2020 All AP EAMCET

A
Arrhenius concept
B
Bronsted-Lowry concept
C
Lewis concept
D
Bronsted-Lowry as well as Lewis concept

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Class 11

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6-2.Equilibrium-II (Ionic Equilibrium)

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Acids and Bases

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According to the Bronsted-Lowry theory,the acids in the following reaction are:
$ClO_4^{-} + HCO_3^{-} \rightarrow HClO_4 + CO_3^{2-}$

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The ammonium ion $(NH_4^+)$ is:

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Which of the following compounds can act as both a $Br\o nsted$ acid and a $Br\o nsted$ base?

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On dissolving $1 \ mole$ of each of the following acids in $1 \ L$ of water,the acid which does not give a solution of strength $1 \ N$ is:

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The dissociation constants $(K_a)$ of four acids are given below. Which of these is the strongest acid?

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Acidity of $BF_3$ can be explained on the basis of which of the following concepts?

Similar Questions

According to the Bronsted-Lowry theory,the acids in the following reaction are:$ClO_4^{-} + HCO_3^{-} \rightarrow HClO_4 + CO_3^{2-}$

The ammonium ion $(NH_4^+)$ is:

Which of the following compounds can act as both a $Br\o nsted$ acid and a $Br\o nsted$ base?

On dissolving $1 \ mole$ of each of the following acids in $1 \ L$ of water,the acid which does not give a solution of strength $1 \ N$ is:

The dissociation constants $(K_a)$ of four acids are given below. Which of these is the strongest acid?

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According to the Bronsted-Lowry theory,the acids in the following reaction are:
$ClO_4^{-} + HCO_3^{-} \rightarrow HClO_4 + CO_3^{2-}$