Among the following statements, which is true about boron compounds ?

Options

A. `BF_(3)rArr` least acidic among the boron halides
B. `BF_(3)rArr` does not hydrolyses
C. `B_(2)H_(6)rArr` does not have banana bond
D. All are incorrect

Answer

To determine which statement about boron compounds is true, we will analyze each statement provided.

**Step 1: Analyze the first statement.**
- The first statement claims that BF3 is the least acidic among boron halides (BF3, BCl3, BBr3, and BI3).
- Boron halides are Lewis acids, meaning they can accept electron pairs. The acidity of these compounds generally increases with decreasing electronegativity of the halogen.
- The order of acidity is: BF3 < BCl3 < BBr3 < BI3.
- BF3 is less acidic than the others due to back bonding, where the lone pair of electrons on fluorine can be donated back to the empty p-orbital of boron. This stabilizes BF3 and reduces its acidity.

**Conclusion for Step 1:** The first statement is true.

**Step 2: Analyze the second statement.**
- The second statement claims that BF3 does not hydrolyze.
- In reality, BF3 does hydrolyze when it reacts with water, forming boric acid (B(OH)3) and hydrofluoric acid (HF).
- Therefore, this statement is incorrect.

**Conclusion for Step 2:** The second statement is false.

**Step 3: Analyze the third statement.**
- The third statement claims that B2H6 does not have banana bonds.
- B2H6 (diborane) actually has banana bonds, which are formed by the bridging hydrogen atoms. These bonds involve the overlap of orbitals from the boron atoms and the hydrogen atoms, creating a three-center two-electron bond.
- Therefore, this statement is also incorrect.

**Conclusion for Step 3:** The third statement is false.

**Final Conclusion:**
- The only true statement among the options is the first one: "BF3 is least acidic among boron halides."

**Answer: The first statement is true.**

---