314403
Which of the following acts as Lewis acid ?
1 \(\mathrm{Zn}^{2+}\)
2 \(\mathrm{FeCl}_{3}\)
3 \(\mathrm{CO}_{2}\)
4 All the above
Explanation:
Due to empty orbitals in \(\mathrm {\mathrm{Fe}^{3+}}\) and \(\mathrm {\mathrm{Zn}^{2+}}\). Multiple bond containing compounds can behave as Lewis acids.
CHXI07:EQUILIBRIUM
314404
The relative Lewis acid strength of boron trihalide is in the order of
314405
Which of the following is not a Lewis acid?
1 \(\mathrm{SnCl}_{2}\)
2 \(\mathrm{NH}_{4}^{+}\)
3 \(\mathrm{NH}_{3}\)
4 Both \(\mathrm{NH}_{3}\) and \(\mathrm{NH}_{4}^{+}\)
Explanation:
\(\mathrm {\mathrm{NH}_{3}}\) behaves as a Lewis base. \(\mathrm {\mathrm{NH}_{4}^{+}}\)ion is neither a Lewis acid nor a Lewis base.
CHXI07:EQUILIBRIUM
314406
In complex compounds, the central metal atom can act as
1 A Lewis acid
2 A Lewis base
3 A Bronsted acid
4 An Arrhenius acid
Explanation:
Central atom in complex behaves as Lewis acid due to vacant orbitals present in it.
CHXI07:EQUILIBRIUM
314407
Amongst the given options which of the following molecules/ions atcs as a Lewis acid?
1 \(\mathrm{H}_{2} \mathrm{O}\)
2 \(\mathrm{BF}_{3}\)
3 \(\mathrm{OH}^{-}\)
4 \(\mathrm{NH}_{3}\)
Explanation:
Electron pair acceptor is Lewis acid. can not act as Lewis acids because donate a pair of \(\mathrm{e}^{-}\).(Lewis base) \(\mathrm{BF}_{3} \rightarrow\) Central atom Boron has incomplete octect. Thus, accepts a pair of \(\mathrm{e}^{-}\).(Lewis acid).
314403
Which of the following acts as Lewis acid ?
1 \(\mathrm{Zn}^{2+}\)
2 \(\mathrm{FeCl}_{3}\)
3 \(\mathrm{CO}_{2}\)
4 All the above
Explanation:
Due to empty orbitals in \(\mathrm {\mathrm{Fe}^{3+}}\) and \(\mathrm {\mathrm{Zn}^{2+}}\). Multiple bond containing compounds can behave as Lewis acids.
CHXI07:EQUILIBRIUM
314404
The relative Lewis acid strength of boron trihalide is in the order of
314405
Which of the following is not a Lewis acid?
1 \(\mathrm{SnCl}_{2}\)
2 \(\mathrm{NH}_{4}^{+}\)
3 \(\mathrm{NH}_{3}\)
4 Both \(\mathrm{NH}_{3}\) and \(\mathrm{NH}_{4}^{+}\)
Explanation:
\(\mathrm {\mathrm{NH}_{3}}\) behaves as a Lewis base. \(\mathrm {\mathrm{NH}_{4}^{+}}\)ion is neither a Lewis acid nor a Lewis base.
CHXI07:EQUILIBRIUM
314406
In complex compounds, the central metal atom can act as
1 A Lewis acid
2 A Lewis base
3 A Bronsted acid
4 An Arrhenius acid
Explanation:
Central atom in complex behaves as Lewis acid due to vacant orbitals present in it.
CHXI07:EQUILIBRIUM
314407
Amongst the given options which of the following molecules/ions atcs as a Lewis acid?
1 \(\mathrm{H}_{2} \mathrm{O}\)
2 \(\mathrm{BF}_{3}\)
3 \(\mathrm{OH}^{-}\)
4 \(\mathrm{NH}_{3}\)
Explanation:
Electron pair acceptor is Lewis acid. can not act as Lewis acids because donate a pair of \(\mathrm{e}^{-}\).(Lewis base) \(\mathrm{BF}_{3} \rightarrow\) Central atom Boron has incomplete octect. Thus, accepts a pair of \(\mathrm{e}^{-}\).(Lewis acid).
314403
Which of the following acts as Lewis acid ?
1 \(\mathrm{Zn}^{2+}\)
2 \(\mathrm{FeCl}_{3}\)
3 \(\mathrm{CO}_{2}\)
4 All the above
Explanation:
Due to empty orbitals in \(\mathrm {\mathrm{Fe}^{3+}}\) and \(\mathrm {\mathrm{Zn}^{2+}}\). Multiple bond containing compounds can behave as Lewis acids.
CHXI07:EQUILIBRIUM
314404
The relative Lewis acid strength of boron trihalide is in the order of
314405
Which of the following is not a Lewis acid?
1 \(\mathrm{SnCl}_{2}\)
2 \(\mathrm{NH}_{4}^{+}\)
3 \(\mathrm{NH}_{3}\)
4 Both \(\mathrm{NH}_{3}\) and \(\mathrm{NH}_{4}^{+}\)
Explanation:
\(\mathrm {\mathrm{NH}_{3}}\) behaves as a Lewis base. \(\mathrm {\mathrm{NH}_{4}^{+}}\)ion is neither a Lewis acid nor a Lewis base.
CHXI07:EQUILIBRIUM
314406
In complex compounds, the central metal atom can act as
1 A Lewis acid
2 A Lewis base
3 A Bronsted acid
4 An Arrhenius acid
Explanation:
Central atom in complex behaves as Lewis acid due to vacant orbitals present in it.
CHXI07:EQUILIBRIUM
314407
Amongst the given options which of the following molecules/ions atcs as a Lewis acid?
1 \(\mathrm{H}_{2} \mathrm{O}\)
2 \(\mathrm{BF}_{3}\)
3 \(\mathrm{OH}^{-}\)
4 \(\mathrm{NH}_{3}\)
Explanation:
Electron pair acceptor is Lewis acid. can not act as Lewis acids because donate a pair of \(\mathrm{e}^{-}\).(Lewis base) \(\mathrm{BF}_{3} \rightarrow\) Central atom Boron has incomplete octect. Thus, accepts a pair of \(\mathrm{e}^{-}\).(Lewis acid).
314403
Which of the following acts as Lewis acid ?
1 \(\mathrm{Zn}^{2+}\)
2 \(\mathrm{FeCl}_{3}\)
3 \(\mathrm{CO}_{2}\)
4 All the above
Explanation:
Due to empty orbitals in \(\mathrm {\mathrm{Fe}^{3+}}\) and \(\mathrm {\mathrm{Zn}^{2+}}\). Multiple bond containing compounds can behave as Lewis acids.
CHXI07:EQUILIBRIUM
314404
The relative Lewis acid strength of boron trihalide is in the order of
314405
Which of the following is not a Lewis acid?
1 \(\mathrm{SnCl}_{2}\)
2 \(\mathrm{NH}_{4}^{+}\)
3 \(\mathrm{NH}_{3}\)
4 Both \(\mathrm{NH}_{3}\) and \(\mathrm{NH}_{4}^{+}\)
Explanation:
\(\mathrm {\mathrm{NH}_{3}}\) behaves as a Lewis base. \(\mathrm {\mathrm{NH}_{4}^{+}}\)ion is neither a Lewis acid nor a Lewis base.
CHXI07:EQUILIBRIUM
314406
In complex compounds, the central metal atom can act as
1 A Lewis acid
2 A Lewis base
3 A Bronsted acid
4 An Arrhenius acid
Explanation:
Central atom in complex behaves as Lewis acid due to vacant orbitals present in it.
CHXI07:EQUILIBRIUM
314407
Amongst the given options which of the following molecules/ions atcs as a Lewis acid?
1 \(\mathrm{H}_{2} \mathrm{O}\)
2 \(\mathrm{BF}_{3}\)
3 \(\mathrm{OH}^{-}\)
4 \(\mathrm{NH}_{3}\)
Explanation:
Electron pair acceptor is Lewis acid. can not act as Lewis acids because donate a pair of \(\mathrm{e}^{-}\).(Lewis base) \(\mathrm{BF}_{3} \rightarrow\) Central atom Boron has incomplete octect. Thus, accepts a pair of \(\mathrm{e}^{-}\).(Lewis acid).
314403
Which of the following acts as Lewis acid ?
1 \(\mathrm{Zn}^{2+}\)
2 \(\mathrm{FeCl}_{3}\)
3 \(\mathrm{CO}_{2}\)
4 All the above
Explanation:
Due to empty orbitals in \(\mathrm {\mathrm{Fe}^{3+}}\) and \(\mathrm {\mathrm{Zn}^{2+}}\). Multiple bond containing compounds can behave as Lewis acids.
CHXI07:EQUILIBRIUM
314404
The relative Lewis acid strength of boron trihalide is in the order of
314405
Which of the following is not a Lewis acid?
1 \(\mathrm{SnCl}_{2}\)
2 \(\mathrm{NH}_{4}^{+}\)
3 \(\mathrm{NH}_{3}\)
4 Both \(\mathrm{NH}_{3}\) and \(\mathrm{NH}_{4}^{+}\)
Explanation:
\(\mathrm {\mathrm{NH}_{3}}\) behaves as a Lewis base. \(\mathrm {\mathrm{NH}_{4}^{+}}\)ion is neither a Lewis acid nor a Lewis base.
CHXI07:EQUILIBRIUM
314406
In complex compounds, the central metal atom can act as
1 A Lewis acid
2 A Lewis base
3 A Bronsted acid
4 An Arrhenius acid
Explanation:
Central atom in complex behaves as Lewis acid due to vacant orbitals present in it.
CHXI07:EQUILIBRIUM
314407
Amongst the given options which of the following molecules/ions atcs as a Lewis acid?
1 \(\mathrm{H}_{2} \mathrm{O}\)
2 \(\mathrm{BF}_{3}\)
3 \(\mathrm{OH}^{-}\)
4 \(\mathrm{NH}_{3}\)
Explanation:
Electron pair acceptor is Lewis acid. can not act as Lewis acids because donate a pair of \(\mathrm{e}^{-}\).(Lewis base) \(\mathrm{BF}_{3} \rightarrow\) Central atom Boron has incomplete octect. Thus, accepts a pair of \(\mathrm{e}^{-}\).(Lewis acid).
