Question

Which of the following has sp² hybridisation?

• A. BF₃
• B. H₂SO₄
• C. NH₄₊
• D. NH₃

Answer 1

The Correct Option is A

To determine which of the given compounds has \(sp^2\) hybridization, let's consider the hybridization concept and analyze each option individually.

Understanding Hybridization: 

• The hybridization of an atom in a molecule depends on the number of sigma bonds and lone pairs around it.
• \(sp^2\) hybridization corresponds to three regions of electron density around the central atom, compromising of two sigma bonds and one lone pair or three sigma bonds.

Let's examine each option:

1. BF₃ (Boron Trifluoride)
   • Boron (B) is the central atom bonded to three fluorine (F) atoms via three sigma bonds.
   • There are no lone pairs on boron in BF₃.
   • Thus, with three sigma bonds and no lone pairs, the hybridization of Boron in BF₃ is \(sp^2\).
2. H₂SO₄ (Sulfuric Acid)
   • Sulfur (S) is the central atom with bonding to two OH groups and two double-bonded oxygens.
   • Counting all the sigma bonds, sulfur typically undergoes \(sp^3\) hybridization in this molecular structure.
3. NH₄₊ (Ammonium Ion)
   • Nitrogen (N) is the central atom bonded to four Hydrogen (H) atoms.
   • This ion adopts a tetrahedral geometry, leading to an \(sp^3\) hybridization.
4. NH₃ (Ammonia)
   • Nitrogen (N) is the central atom with three H atoms bonded via sigma bonds and one lone pair.
   • This configuration leads to \(sp^3\) hybridization.

Conclusion: Among the given options, only BF₃ has the \(sp^2\) hybridization.