314399
Which of the following pair behaves as strong and weak base hydride respectively\(\mathrm{NH}_{3}, \mathrm{PH}_{3}, \mathrm{AsH}_{3}, \mathrm{SbH}_{3}, \mathrm{BiH}_{3}\)
1 \(\mathrm{NH}_{3}, \mathrm{PH}_{3}\)
2 \(\mathrm{NH}_{3}, \mathrm{BiH}_{3}\)
3 \(\mathrm{PH}_{3}, \mathrm{BiH}_{3}\)
4 \(\mathrm{BiH}_{3}, \mathrm{AsH}_{3}\)
Explanation:
The basic strength of given hydrides decreases in the order as follows \(\mathrm{NH}_{3}>\mathrm{PH}_{3}>\mathrm{AsH}_{3}>\mathrm{SbH}_{3}>\mathrm{BiH}_{3}\) This is due to the decrease in the availability of the lone pair of electrons which depends on the size of central atom that increase from \(\mathrm{N}\) to Bi. Therefore, \(\mathrm{NH}_{3}\) and \(\mathrm{BiH}_{3}\) acts as a strong and weak base hydride respectively.
CHXI07:EQUILIBRIUM
314400
Which of the following are Lewis acids ?
1 \(\mathrm{AlCl}_{3}\) and \({\text{AlC}}{{\text{l}}_4}^ - \)
2 \(\mathrm{PH}_{3}\) and \(\mathrm{SiCl}_{4}\)
3 \(\mathrm{BCl}_{3}\) and \(\mathrm{AlCl}_{3}\)
4 \(\mathrm{PH}_{3}\) and \(\mathrm{BCl}_{3}\)
Explanation:
\(\rm {{\text{BC}}{{\text{l}}_{\text{3}}}{\text{ and AlC}}{{\text{l}}_{\text{3}}}}\) both have vacant p-orbital. So they act as Lewis acid.
CHXI07:EQUILIBRIUM
314401
Which of the following acts as a Lewis acid in the following reaction \(\mathrm{SnCl}_{4}+2 \mathrm{Cl}^{-} \rightarrow\left[\mathrm{SnCl}_{6}\right]^{2-}\)
1 \(\mathrm{Cl}^{-}\)
2 \(\left[\mathrm{SnCl}_{6}\right]^{2-}\)
3 \(\mathrm{SnCl}_{4}\)
4 \(2 \mathrm{Cl}^{-}\)
Explanation:
Due to vacant d-orbital.
CHXI07:EQUILIBRIUM
314402
Which of the following is neither a Lewis acid nor a Lewis base?
1 \(\mathrm{HSO}_{4}^{-}\)
2 \(\mathrm{ZnCl}_{2}\)
3 \(\mathrm{NH}_{4}^{+}\)
4 \(\mathrm{CH}_{3}^{+}\)
Explanation:
\(\mathrm {\mathrm{NH}_{4}^{+}}\)ion is neither a Lewis acid nor a Lewis base.
314399
Which of the following pair behaves as strong and weak base hydride respectively\(\mathrm{NH}_{3}, \mathrm{PH}_{3}, \mathrm{AsH}_{3}, \mathrm{SbH}_{3}, \mathrm{BiH}_{3}\)
1 \(\mathrm{NH}_{3}, \mathrm{PH}_{3}\)
2 \(\mathrm{NH}_{3}, \mathrm{BiH}_{3}\)
3 \(\mathrm{PH}_{3}, \mathrm{BiH}_{3}\)
4 \(\mathrm{BiH}_{3}, \mathrm{AsH}_{3}\)
Explanation:
The basic strength of given hydrides decreases in the order as follows \(\mathrm{NH}_{3}>\mathrm{PH}_{3}>\mathrm{AsH}_{3}>\mathrm{SbH}_{3}>\mathrm{BiH}_{3}\) This is due to the decrease in the availability of the lone pair of electrons which depends on the size of central atom that increase from \(\mathrm{N}\) to Bi. Therefore, \(\mathrm{NH}_{3}\) and \(\mathrm{BiH}_{3}\) acts as a strong and weak base hydride respectively.
CHXI07:EQUILIBRIUM
314400
Which of the following are Lewis acids ?
1 \(\mathrm{AlCl}_{3}\) and \({\text{AlC}}{{\text{l}}_4}^ - \)
2 \(\mathrm{PH}_{3}\) and \(\mathrm{SiCl}_{4}\)
3 \(\mathrm{BCl}_{3}\) and \(\mathrm{AlCl}_{3}\)
4 \(\mathrm{PH}_{3}\) and \(\mathrm{BCl}_{3}\)
Explanation:
\(\rm {{\text{BC}}{{\text{l}}_{\text{3}}}{\text{ and AlC}}{{\text{l}}_{\text{3}}}}\) both have vacant p-orbital. So they act as Lewis acid.
CHXI07:EQUILIBRIUM
314401
Which of the following acts as a Lewis acid in the following reaction \(\mathrm{SnCl}_{4}+2 \mathrm{Cl}^{-} \rightarrow\left[\mathrm{SnCl}_{6}\right]^{2-}\)
1 \(\mathrm{Cl}^{-}\)
2 \(\left[\mathrm{SnCl}_{6}\right]^{2-}\)
3 \(\mathrm{SnCl}_{4}\)
4 \(2 \mathrm{Cl}^{-}\)
Explanation:
Due to vacant d-orbital.
CHXI07:EQUILIBRIUM
314402
Which of the following is neither a Lewis acid nor a Lewis base?
1 \(\mathrm{HSO}_{4}^{-}\)
2 \(\mathrm{ZnCl}_{2}\)
3 \(\mathrm{NH}_{4}^{+}\)
4 \(\mathrm{CH}_{3}^{+}\)
Explanation:
\(\mathrm {\mathrm{NH}_{4}^{+}}\)ion is neither a Lewis acid nor a Lewis base.
314399
Which of the following pair behaves as strong and weak base hydride respectively\(\mathrm{NH}_{3}, \mathrm{PH}_{3}, \mathrm{AsH}_{3}, \mathrm{SbH}_{3}, \mathrm{BiH}_{3}\)
1 \(\mathrm{NH}_{3}, \mathrm{PH}_{3}\)
2 \(\mathrm{NH}_{3}, \mathrm{BiH}_{3}\)
3 \(\mathrm{PH}_{3}, \mathrm{BiH}_{3}\)
4 \(\mathrm{BiH}_{3}, \mathrm{AsH}_{3}\)
Explanation:
The basic strength of given hydrides decreases in the order as follows \(\mathrm{NH}_{3}>\mathrm{PH}_{3}>\mathrm{AsH}_{3}>\mathrm{SbH}_{3}>\mathrm{BiH}_{3}\) This is due to the decrease in the availability of the lone pair of electrons which depends on the size of central atom that increase from \(\mathrm{N}\) to Bi. Therefore, \(\mathrm{NH}_{3}\) and \(\mathrm{BiH}_{3}\) acts as a strong and weak base hydride respectively.
CHXI07:EQUILIBRIUM
314400
Which of the following are Lewis acids ?
1 \(\mathrm{AlCl}_{3}\) and \({\text{AlC}}{{\text{l}}_4}^ - \)
2 \(\mathrm{PH}_{3}\) and \(\mathrm{SiCl}_{4}\)
3 \(\mathrm{BCl}_{3}\) and \(\mathrm{AlCl}_{3}\)
4 \(\mathrm{PH}_{3}\) and \(\mathrm{BCl}_{3}\)
Explanation:
\(\rm {{\text{BC}}{{\text{l}}_{\text{3}}}{\text{ and AlC}}{{\text{l}}_{\text{3}}}}\) both have vacant p-orbital. So they act as Lewis acid.
CHXI07:EQUILIBRIUM
314401
Which of the following acts as a Lewis acid in the following reaction \(\mathrm{SnCl}_{4}+2 \mathrm{Cl}^{-} \rightarrow\left[\mathrm{SnCl}_{6}\right]^{2-}\)
1 \(\mathrm{Cl}^{-}\)
2 \(\left[\mathrm{SnCl}_{6}\right]^{2-}\)
3 \(\mathrm{SnCl}_{4}\)
4 \(2 \mathrm{Cl}^{-}\)
Explanation:
Due to vacant d-orbital.
CHXI07:EQUILIBRIUM
314402
Which of the following is neither a Lewis acid nor a Lewis base?
1 \(\mathrm{HSO}_{4}^{-}\)
2 \(\mathrm{ZnCl}_{2}\)
3 \(\mathrm{NH}_{4}^{+}\)
4 \(\mathrm{CH}_{3}^{+}\)
Explanation:
\(\mathrm {\mathrm{NH}_{4}^{+}}\)ion is neither a Lewis acid nor a Lewis base.
314399
Which of the following pair behaves as strong and weak base hydride respectively\(\mathrm{NH}_{3}, \mathrm{PH}_{3}, \mathrm{AsH}_{3}, \mathrm{SbH}_{3}, \mathrm{BiH}_{3}\)
1 \(\mathrm{NH}_{3}, \mathrm{PH}_{3}\)
2 \(\mathrm{NH}_{3}, \mathrm{BiH}_{3}\)
3 \(\mathrm{PH}_{3}, \mathrm{BiH}_{3}\)
4 \(\mathrm{BiH}_{3}, \mathrm{AsH}_{3}\)
Explanation:
The basic strength of given hydrides decreases in the order as follows \(\mathrm{NH}_{3}>\mathrm{PH}_{3}>\mathrm{AsH}_{3}>\mathrm{SbH}_{3}>\mathrm{BiH}_{3}\) This is due to the decrease in the availability of the lone pair of electrons which depends on the size of central atom that increase from \(\mathrm{N}\) to Bi. Therefore, \(\mathrm{NH}_{3}\) and \(\mathrm{BiH}_{3}\) acts as a strong and weak base hydride respectively.
CHXI07:EQUILIBRIUM
314400
Which of the following are Lewis acids ?
1 \(\mathrm{AlCl}_{3}\) and \({\text{AlC}}{{\text{l}}_4}^ - \)
2 \(\mathrm{PH}_{3}\) and \(\mathrm{SiCl}_{4}\)
3 \(\mathrm{BCl}_{3}\) and \(\mathrm{AlCl}_{3}\)
4 \(\mathrm{PH}_{3}\) and \(\mathrm{BCl}_{3}\)
Explanation:
\(\rm {{\text{BC}}{{\text{l}}_{\text{3}}}{\text{ and AlC}}{{\text{l}}_{\text{3}}}}\) both have vacant p-orbital. So they act as Lewis acid.
CHXI07:EQUILIBRIUM
314401
Which of the following acts as a Lewis acid in the following reaction \(\mathrm{SnCl}_{4}+2 \mathrm{Cl}^{-} \rightarrow\left[\mathrm{SnCl}_{6}\right]^{2-}\)
1 \(\mathrm{Cl}^{-}\)
2 \(\left[\mathrm{SnCl}_{6}\right]^{2-}\)
3 \(\mathrm{SnCl}_{4}\)
4 \(2 \mathrm{Cl}^{-}\)
Explanation:
Due to vacant d-orbital.
CHXI07:EQUILIBRIUM
314402
Which of the following is neither a Lewis acid nor a Lewis base?
1 \(\mathrm{HSO}_{4}^{-}\)
2 \(\mathrm{ZnCl}_{2}\)
3 \(\mathrm{NH}_{4}^{+}\)
4 \(\mathrm{CH}_{3}^{+}\)
Explanation:
\(\mathrm {\mathrm{NH}_{4}^{+}}\)ion is neither a Lewis acid nor a Lewis base.
