2 Lewis acids : \(\mathrm{HO}^{-}, \mathrm{H}^{+}\); Lewis bases : \(\mathrm{F}^{-}, \mathrm{BCl}_{3}\)
3 Lewis acids : \(\mathrm{H}^{+}, \mathrm{BCl}_{3}\); Lewis bases : \(\mathrm{HO}^{-}, \mathrm{F}^{-}\)
4 Lewis acids : \(\mathrm{HO}^{-}, \mathrm{F}^{-}\); Lewis bases : \(\mathrm{H}^{+}, \mathrm{BCl}_{3}\)
Explanation:
Hydroxyl ion is a Lewis base as it can donate an electron lone pair \(\mathrm {\left(: \mathrm{OH}^{-}\right)}\). Flouride ion acts as a Lewis base as it can donate any one of its four electron lone pairs. A proton is a Lewis acid as it can accept a lone pair of electrons from bases like hydroxyl ion and fluoride ion. \(\mathrm {\mathrm{BCl}_{3}}\) acts as a Lewis acid as it can accept a lone pair of electrons from species like ammonia or amine molecules.
CHXI07:EQUILIBRIUM
314396
Assertion : \(\mathrm{BF}_{3}\) is a Lewis acid but not a Bronsted acid. Reason : \(\mathrm{BF}_{3}\) is \(\mathrm{sp}^{2}\) hybridised and has trigonal planar structure.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
Lewis acid is the one which can accept a pair of electrons. Bronsted acid is the one which can release a proton. \(\mathrm{BF}_{3}\) can accept a pair of electrons but cannot yield a proton, hence it is a Lewis acid. So option (2) is correct.
CHXI07:EQUILIBRIUM
314397
Which of the following is wrong?
1 All Bronsted bases are Lewis bases
2 All Lewis acids are Bronsted acids
3 All Arrhenius acids are Bronsted acids
4 All Arrhenius bases are Bronsted bases
Explanation:
All Arrhenius bases are Bronsted bases but all Bronsted bases are not Arrhenius bases
CHXI07:EQUILIBRIUM
314398
Acidity of \(\mathrm{BF}_{3}\) can be explained on which of the following concepts?
1 Arrhenius concept
2 Bronsted Lowry concept
3 Lewis concept
4 Bronsted Lowry as well as Lewis concept
Explanation:
According to Lewis concept, acid can accept a pair of electrons and base can donate a pair of electrons. Thus, as \(\mathrm {\mathrm{BF}_{3}}\) has six electrons in its valence shell, so it can accept an electrons pair and acts as Lewis acid.
2 Lewis acids : \(\mathrm{HO}^{-}, \mathrm{H}^{+}\); Lewis bases : \(\mathrm{F}^{-}, \mathrm{BCl}_{3}\)
3 Lewis acids : \(\mathrm{H}^{+}, \mathrm{BCl}_{3}\); Lewis bases : \(\mathrm{HO}^{-}, \mathrm{F}^{-}\)
4 Lewis acids : \(\mathrm{HO}^{-}, \mathrm{F}^{-}\); Lewis bases : \(\mathrm{H}^{+}, \mathrm{BCl}_{3}\)
Explanation:
Hydroxyl ion is a Lewis base as it can donate an electron lone pair \(\mathrm {\left(: \mathrm{OH}^{-}\right)}\). Flouride ion acts as a Lewis base as it can donate any one of its four electron lone pairs. A proton is a Lewis acid as it can accept a lone pair of electrons from bases like hydroxyl ion and fluoride ion. \(\mathrm {\mathrm{BCl}_{3}}\) acts as a Lewis acid as it can accept a lone pair of electrons from species like ammonia or amine molecules.
CHXI07:EQUILIBRIUM
314396
Assertion : \(\mathrm{BF}_{3}\) is a Lewis acid but not a Bronsted acid. Reason : \(\mathrm{BF}_{3}\) is \(\mathrm{sp}^{2}\) hybridised and has trigonal planar structure.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
Lewis acid is the one which can accept a pair of electrons. Bronsted acid is the one which can release a proton. \(\mathrm{BF}_{3}\) can accept a pair of electrons but cannot yield a proton, hence it is a Lewis acid. So option (2) is correct.
CHXI07:EQUILIBRIUM
314397
Which of the following is wrong?
1 All Bronsted bases are Lewis bases
2 All Lewis acids are Bronsted acids
3 All Arrhenius acids are Bronsted acids
4 All Arrhenius bases are Bronsted bases
Explanation:
All Arrhenius bases are Bronsted bases but all Bronsted bases are not Arrhenius bases
CHXI07:EQUILIBRIUM
314398
Acidity of \(\mathrm{BF}_{3}\) can be explained on which of the following concepts?
1 Arrhenius concept
2 Bronsted Lowry concept
3 Lewis concept
4 Bronsted Lowry as well as Lewis concept
Explanation:
According to Lewis concept, acid can accept a pair of electrons and base can donate a pair of electrons. Thus, as \(\mathrm {\mathrm{BF}_{3}}\) has six electrons in its valence shell, so it can accept an electrons pair and acts as Lewis acid.
2 Lewis acids : \(\mathrm{HO}^{-}, \mathrm{H}^{+}\); Lewis bases : \(\mathrm{F}^{-}, \mathrm{BCl}_{3}\)
3 Lewis acids : \(\mathrm{H}^{+}, \mathrm{BCl}_{3}\); Lewis bases : \(\mathrm{HO}^{-}, \mathrm{F}^{-}\)
4 Lewis acids : \(\mathrm{HO}^{-}, \mathrm{F}^{-}\); Lewis bases : \(\mathrm{H}^{+}, \mathrm{BCl}_{3}\)
Explanation:
Hydroxyl ion is a Lewis base as it can donate an electron lone pair \(\mathrm {\left(: \mathrm{OH}^{-}\right)}\). Flouride ion acts as a Lewis base as it can donate any one of its four electron lone pairs. A proton is a Lewis acid as it can accept a lone pair of electrons from bases like hydroxyl ion and fluoride ion. \(\mathrm {\mathrm{BCl}_{3}}\) acts as a Lewis acid as it can accept a lone pair of electrons from species like ammonia or amine molecules.
CHXI07:EQUILIBRIUM
314396
Assertion : \(\mathrm{BF}_{3}\) is a Lewis acid but not a Bronsted acid. Reason : \(\mathrm{BF}_{3}\) is \(\mathrm{sp}^{2}\) hybridised and has trigonal planar structure.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
Lewis acid is the one which can accept a pair of electrons. Bronsted acid is the one which can release a proton. \(\mathrm{BF}_{3}\) can accept a pair of electrons but cannot yield a proton, hence it is a Lewis acid. So option (2) is correct.
CHXI07:EQUILIBRIUM
314397
Which of the following is wrong?
1 All Bronsted bases are Lewis bases
2 All Lewis acids are Bronsted acids
3 All Arrhenius acids are Bronsted acids
4 All Arrhenius bases are Bronsted bases
Explanation:
All Arrhenius bases are Bronsted bases but all Bronsted bases are not Arrhenius bases
CHXI07:EQUILIBRIUM
314398
Acidity of \(\mathrm{BF}_{3}\) can be explained on which of the following concepts?
1 Arrhenius concept
2 Bronsted Lowry concept
3 Lewis concept
4 Bronsted Lowry as well as Lewis concept
Explanation:
According to Lewis concept, acid can accept a pair of electrons and base can donate a pair of electrons. Thus, as \(\mathrm {\mathrm{BF}_{3}}\) has six electrons in its valence shell, so it can accept an electrons pair and acts as Lewis acid.
2 Lewis acids : \(\mathrm{HO}^{-}, \mathrm{H}^{+}\); Lewis bases : \(\mathrm{F}^{-}, \mathrm{BCl}_{3}\)
3 Lewis acids : \(\mathrm{H}^{+}, \mathrm{BCl}_{3}\); Lewis bases : \(\mathrm{HO}^{-}, \mathrm{F}^{-}\)
4 Lewis acids : \(\mathrm{HO}^{-}, \mathrm{F}^{-}\); Lewis bases : \(\mathrm{H}^{+}, \mathrm{BCl}_{3}\)
Explanation:
Hydroxyl ion is a Lewis base as it can donate an electron lone pair \(\mathrm {\left(: \mathrm{OH}^{-}\right)}\). Flouride ion acts as a Lewis base as it can donate any one of its four electron lone pairs. A proton is a Lewis acid as it can accept a lone pair of electrons from bases like hydroxyl ion and fluoride ion. \(\mathrm {\mathrm{BCl}_{3}}\) acts as a Lewis acid as it can accept a lone pair of electrons from species like ammonia or amine molecules.
CHXI07:EQUILIBRIUM
314396
Assertion : \(\mathrm{BF}_{3}\) is a Lewis acid but not a Bronsted acid. Reason : \(\mathrm{BF}_{3}\) is \(\mathrm{sp}^{2}\) hybridised and has trigonal planar structure.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
Lewis acid is the one which can accept a pair of electrons. Bronsted acid is the one which can release a proton. \(\mathrm{BF}_{3}\) can accept a pair of electrons but cannot yield a proton, hence it is a Lewis acid. So option (2) is correct.
CHXI07:EQUILIBRIUM
314397
Which of the following is wrong?
1 All Bronsted bases are Lewis bases
2 All Lewis acids are Bronsted acids
3 All Arrhenius acids are Bronsted acids
4 All Arrhenius bases are Bronsted bases
Explanation:
All Arrhenius bases are Bronsted bases but all Bronsted bases are not Arrhenius bases
CHXI07:EQUILIBRIUM
314398
Acidity of \(\mathrm{BF}_{3}\) can be explained on which of the following concepts?
1 Arrhenius concept
2 Bronsted Lowry concept
3 Lewis concept
4 Bronsted Lowry as well as Lewis concept
Explanation:
According to Lewis concept, acid can accept a pair of electrons and base can donate a pair of electrons. Thus, as \(\mathrm {\mathrm{BF}_{3}}\) has six electrons in its valence shell, so it can accept an electrons pair and acts as Lewis acid.
