Which of the following compounds is electron-deficient?

1. ${\mathrm{SiCl}}_4$

2. ${\mathrm{BCl}}_3$

3. ${\mathrm{PCl}}_3$

4. $\mathrm{ICl}$

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

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: The B–X bond lengths in boron trihalides (BX₃) are shorter than those expected for
                   pure B–X single bonds.

Reason: $\mathrm{p\pi –p\pi \; back-bonding\; occurs\; between\; the\; halogen\; atoms\; and\; the\; boron\; atom\; in\; BX₃.}$

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.

Why is BCl₃ more stable than TlCl₃?

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 -

Find the anion that cannot be formed by boron.
1. [BF₆]³⁻
2. BH₄⁻
3. B(OH)₄⁻
4. BO₂⁻

Find the correct nature of boric acid, H₃BO₃:

1. Protic acid.

2. Weak monobasic acid.

3. Lewis acid.

4. Both '2' and '3'

Which of the following Group 13 elements cannot form the hexafluoro complex ion [MF₆]³⁻?