BCl3 has higher stability than , because -
1. | The +2 oxidation state of Tl is more stable than the +2 oxidation state of B |
2. | The +2 oxidation state of B is more stable than the +2 oxidation state of Tl |
3. | The +3 oxidation state of B is more stable than the +3 oxidation state of Tl |
4. | The +3 oxidation state of Tl is more stable than the +3 oxidation state of B |
Boron trifluoride behaves as a Lewis acid because -
1. Boron trifluoride is electron-rich.
2. Boron trifluoride is electron-deficient.
3. Boron trifluoride is highly stable.
4. None of these.
Boric acid is a-
1. Protic acid.
2. Weak monobasic acid.
3. Lewis acid.
4. Both '2' and '3'
The effect of heating Boric acid at 370 K or above is -
1. Orthoboric acid changes to metaboric acid.
2. Metaboric acid changes to boric oxide.
3. Both '1' and '2'
4. Neither '1' nor '2'
The electron-deficient compound among the following is -
1.
2.
3.
4.
The B–F bond lengths in (130 pm) and (143 pm) differ because of-
1. Presence of triple bond character in
2. Resonance in
3. Presence of a double bond character in
4. Presence of a double bond character in
Despite the dipole moment in the B–Cl bond, the BCl3 molecule as a whole has no dipole moment because:
1. | The respective dipole-moments of the B–Cl bond add with each other |
2. | The respective dipole moments of the B–Cl bond cancel each other |
3. | BCl3 is tetrahedral in shape |
4. | None of the above |
Amphoteric oxides are:
1. Tl2O3, SiO2
2. ,
3. ,
4. Al2O3 , PbO2
An aqueous solution of Borax is-
1. | Neutral | 2. | Amphoteric |
3. | Basic | 4. | Acidic |
Boric acid is polymeric due to-
1. Its acidic nature.
2. The presence of hydrogen bonds.
3. Its monobasic nature.
4. Its geometry.