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

Which of the following correctly describes the behavior of BCl₃ and CCl₄ towards hydrolysis in water?

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. $\mathrm{ICl}$

The hybridization of carbon in (a) ${\mathrm{CO}}_3^{2-}$ (b) diamond (c) graphite is respectively:

1. ${\mathrm{sp}}^2$, ${\mathrm{sp}}^3$, ${\mathrm{sp}}^2$

2. ${\mathrm{sp}}^2$, ${\mathrm{sp}}^3$, $s{p}^3$

3. ${\mathrm{sp}}^3$, ${\mathrm{sp}}^3$, ${\mathrm{sp}}^2$

4. ${\mathrm{sp}}^3$, ${\mathrm{sp}}^2$, ${\mathrm{sp}}^3$

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:

Why carbon monoxide (CO) is poisonous?