(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

Easy

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 Questions

Class 11

Chemistry Questions

Chapter

6-2.Equilibrium-II (Ionic Equilibrium)

Subtopic

Acids and Bases

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AP EAMCET 2020 Paper All AP EAMCET years →

Which of the following cannot act as a Bronsted base?

Easy

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The enthalpies of neutralization of $HCN$ and $H_2S$ with a strong base are $12.13 \ kJ \ equi^{-1}$ and $15.9 \ kJ \ equi^{-1}$ respectively. Then:

Medium

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Consider the following data for a series of hydrogen halide Bronsted acids:-

Acid $HF$ $HCl$ $HBr$ $HI$

$K_a$ $7.2 \times 10^{-4}$ $1 \times 10^6$ $1 \times 10^9$ $3 \times 10^{11}$

Which of these Bronsted acids would have the weakest conjugate base?

Medium

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According to the $Br\o nsted-Lowry$ theory,water is a/an:

Easy

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Which one of the following can be classified as a Bronsted base?

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Acid	$HF$	$HCl$	$HBr$	$HI$
$K_a$	$7.2 \times 10^{-4}$	$1 \times 10^6$	$1 \times 10^9$	$3 \times 10^{11}$

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

Similar Questions

Which of the following cannot act as a Bronsted base?

The enthalpies of neutralization of $HCN$ and $H_2S$ with a strong base are $12.13 \ kJ \ equi^{-1}$ and $15.9 \ kJ \ equi^{-1}$ respectively. Then:

Consider the following data for a series of hydrogen halide Bronsted acids:- Acid $HF$ $HCl$ $HBr$ $HI$ $K_a$ $7.2 \times 10^{-4}$ $1 \times 10^6$ $1 \times 10^9$ $3 \times 10^{11}$ Which of these Bronsted acids would have the weakest conjugate base?

According to the $Br\o nsted-Lowry$ theory,water is a/an:

Which one of the following can be classified as a Bronsted base?

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Consider the following data for a series of hydrogen halide Bronsted acids:-

Acid $HF$ $HCl$ $HBr$ $HI$

$K_a$ $7.2 \times 10^{-4}$ $1 \times 10^6$ $1 \times 10^9$ $3 \times 10^{11}$

Which of these Bronsted acids would have the weakest conjugate base?