Why is BCl₃ more stable than TlCl₃?

Why does BF₃ act as a Lewis acid?

1. Boron trifluoride is electron-rich.

2. Boron trifluoride is electron-deficient.

3. Boron trifluoride is highly stable.

4. None of the above

Find the correct nature of boric acid, H₃BO₃:

1. Protic acid.

2. Weak monobasic acid.

3. Lewis acid.

4. Both '2' and '3'

What is the effect of heating H₃BO₃ at 370 K and above?

1. Orthoboric acid changes to metaboric acid.

2. Metaboric acid changes to boric oxide.

3. Both '1' and '2'

4. Neither '1' nor '2'

Which of the following compounds is electron-deficient?

1. ${\mathrm{SiCl}}_4$

2. ${\mathrm{BCl}}_3$

3. ${\mathrm{PCl}}_3$

4. $\mathrm{ICl}$

Why is the B–F bond length in BF₃ (130 pm) shorter than that in BF₄⁻ (143 pm)?

1. Presence of triple-bond character in ${\mathrm{BF}}_3$

2. Resonance in $\mathrm{B}{{\mathrm{F}}_4}^{-}$

3. Presence of a double-bond character in ${\mathrm{BF}}_3$

4. Presence of a double bond character in $\mathrm{B}{{\mathrm{F}}_4}^{-}$

Despite the dipole moment in the B–Cl bond, the BCl₃ molecule as a whole has no dipole moment because:

Identify the pair in which both oxides are amphoteric in nature.
 

1. Tl₂O₃ and SiO₂

2. CO₂ and B₂O₃

3. B₂O₃ and SiO₂

4. Al₂O₃ and PbO₂

Which of the following correctly describes the nature of an aqueous solution of borax?

Which of the following is primarily responsible for the formation of a layered
polymeric structure in solid boric acid (H₃BO₃)?

1. Its acidic nature.

2. The presence of hydrogen bonds.

3. Its monobasic nature.

4. Its trigonal planar geometry.