Question

BF₃ is planar and electron-deficient compound. Hybridization and the number of electrons around the central atom, respectively are

• A. sp² and 8
• B. sp³ and 4
• C. sp³ and 6
• D. sp² and 6

Answer 1

The Correct Option is D

To solve this question, we need to determine the hybridization of BF₃ and the number of electrons around the central atom (Boron).

1. The molecular formula for Boron trifluoride (BF₃) shows that Boron is the central atom bonded to three fluorine atoms.
2. To find the hybridization of Boron in BF₃, let's consider the number of valence electrons and bonded pairs:
   1. Boron (B) belongs to group 13 of the periodic table and has 3 valence electrons.
   2. Each Boron-fluorine bond uses one valence electron from Boron to bond with a fluorine atom.
   3. This results in Boron forming three single covalent bonds with fluorine atoms using its three valence electrons.
3. To understand the hybridization, count the number of electron domains around the central atom:
   1. Each of the three B-F bonds represents one electron domain.
   2. No lone pairs are present on Boron in BF₃.
   3. Therefore, there are three electron domains, implying a sp² hybridization.
4. Next, we need to find the number of electrons around the central atom in the molecule:
   1. Boron initially has 3 valence electrons.
   2. With three bonds to Fluorine, the electrons shared in bonding can be considered.
   3. Each B-F bond shares 2 electrons (1 from Boron and 1 from Fluorine), so the total number of electrons involved around Boron is 6.

Thus, BF₃ is an electron-deficient compound with a trigonal planar shape and sp² hybridization. The number of electrons around the Boron atom is 6. Hence, the hybridization and the number of electrons around the central atom, respectively, are sp² and 6.