The electron-deficient compound among the following is -

1. ${\mathrm{SiCl}}_4$

2. ${\mathrm{BCl}}_3$

3. ${\mathrm{PCl}}_3$

4. $\mathrm{ICl}$

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 correct statement(s) among the following options is/are:

The correct statement(s) regarding diborane and boric acid is/are-

1. Diborane has two 3c-2e^- bonds.

2. Boric acid has a layered structure.

3. Four 2c-2e^- bonds are present in diborane.

4. All of the above

Assertion: B-X bond length in ${\mathrm{BX}}_3$ is shorter than the expected value.

Reason: $p\mathrm{\pi }-\mathrm{p\pi }$ back bonding occurs between B and X.

1. Both Assertion & Reason are true and the reason is the correct explanation of the assertion.
2. Both Assertion & Reason are true but the reason is not the correct explanation of the assertion.
3. Assertion is a true statement but Reason is false.
4. Both Assertion and Reason are false statements.

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:

A compound X, of boron, reacts with ${\mathrm{NH}}_3$ on heating to give another compound Y which is called inorganic benzene. The compound X can be prepared by treating ${\mathrm{BF}}_3$ with Lithium aluminium hydride. The compounds X and Y are represented by the formulas -

An anion that cannot be formed by Boron is -

1. ${\mathrm{BF}}_6^{3-}$

2. ${\mathrm{BH}}_4^{-}$

3. $\mathrm{B}{\left(\mathrm{OH}\right)}_4^{-}$

4. ${\mathrm{BO}}_2^{-}$

Boric acid is a-

1. Protic acid.

2. Weak monobasic acid.

3. Lewis acid.

4. Both '2' and '3'