Question

The properties regarding with B2H6 is?

Answer 1

The properties of $\text{B}_2\text{H}_6$ include:

• Structure: Contains two 3-center-2-electron (B-H-B) "banana bonds" and four 2-center-2-electron (B-H) terminal bonds. It is an electron-deficient molecule.
• Physical State: Colorless, highly toxic gas with a sweet smell.
• Reactivity:
  • Undergoes vigorous hydrolysis with water to form boric acid ($\text{H}_3\text{BO}_3$) and hydrogen gas.
  • Highly flammable, burning spontaneously in air to form boron trioxide ($\text{B}_2\text{O}_3$) and water.
  • Acts as a Lewis acid, undergoing cleavage reactions with Lewis bases: symmetrical cleavage with weak bases (e.g., $\text{CO}$, ethers) forming $\text{BH}_3\cdot\text{L}$ adducts, and unsymmetrical cleavage with strong bases (e.g., $\text{NH}_3$) forming ionic compounds like $[\text{BH}_2(\text{NH}_3)_2]^+[\text{BH}_4]^-$.
  • Reacts with ammonia at high temperatures to form borazine ($\text{B}_3\text{N}_3\text{H}_6$).
  • Acts as a powerful reducing agent in organic synthesis (e.g., hydroboration).

Answer 2

Diborane ($\text{B}_2\text{H}_6$) has a unique structure with two 3-center-2-electron (3c-2e) B-H-B bonds (banana bonds) and four 2-center-2-electron (2c-2e) terminal B-H bonds, making it an electron-deficient compound and a Lewis acid. It is a colorless, highly toxic gas. Chemically, it undergoes vigorous hydrolysis with water to form boric acid, burns spontaneously in air, and reacts with Lewis bases via symmetrical or unsymmetrical cleavage. At high temperatures with ammonia, it forms borazine. It is also a significant reducing agent in organic chemistry.