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.

The electron-deficient compound among the following is -

1. ${\mathrm{SiCl}}_4$

2. ${\mathrm{BCl}}_3$

3. ${\mathrm{PCl}}_3$

4. $\mathrm{ICl}$

CO is a poisonous gas because :

BCl₃  has higher stability than ${\mathrm{TlCl}}_3$, because -

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

Boric acid is a-

1. Protic acid.

2. Weak monobasic acid.

3. Lewis acid.

4. Both '2' and '3'

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

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 correct statement among the following regarding behavior of ${\mathrm{BCI}}_3$ $\mathrm{and}$ ${\mathrm{CCI}}_4$ in water is -

The B–F bond lengths in ${\mathrm{BF}}_3$ (130 pm) and $\mathrm{B}{{\mathrm{F}}_4}^{-}$(143 pm) differ because of:

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 $\mathrm{B}{{\mathrm{F}}_4}^{-}$