Molecular Shape of BrF3 - P-Block Elements - Chemistry Class 12 | Summary and Q&A

TL;DR

The molecule structure of BRF3 is trigonal bipyramidal, with the central atom undergoing sp3 hybridization.

Key Insights

• ❓ The electronic configuration of bromine in BRF3 is 1s2 2s2 2p6 3s2 3p6 4s2 4p5.
• ❓ Bromine undergoes sp3 hybridization in BRF3 to acquire three unpaired electrons for bonding.
• 💠 The molecular shape of BRF3 is trigonal bipyramidal.
• 🫀 The equatorial position in BRF3 is occupied by one fluorine atom, while the axial position is occupied by the other two fluorine atoms.
• 🥺 There is repulsion between the two lone pairs of electrons, leading to their positioning in the equatorial positions.
• 🙂 Electronegativity causes the fluorine atoms to distort the structure slightly.
• ❓ BRF3 is considered to be a trigonal bipyramidal molecule due to its molecular structure.

Transcript

Read and summarize the transcript of this video on Glasp Reader (beta).

Questions & Answers

Q: What is the electronic configuration of the central atom in BRF3?

The electronic configuration of the central atom, bromine, in BRF3 is 1s2 2s2 2p6 3s2 3p6 4s2 4p5.

Q: How many unpaired electrons does bromine have in the ground state?

In the ground state, bromine has one unpaired electron.

Q: Why does bromine undergo sp3 hybridization in BRF3?

Bromine undergoes sp3 hybridization in BRF3 to acquire three unpaired electrons, which are necessary for bonding with the three fluorine atoms.

Q: What is the molecular shape of BRF3?

The molecular shape of BRF3 is trigonal bipyramidal.

Summary & Key Takeaways

• BRF3 is a molecule with a central atom of bromine and three fluorine atoms.

• The electronic configuration of bromine in its ground state is 1s2 2s2 2p6 3s2 3p6 4s2 4p5.

• In the excited state, the bromine atom undergoes sp3 hybridization, resulting in a trigonal bipyramidal structure.