Indicate the hybridization of the central atom BCl3 AlCl4 – CS2 KrF2 PF6 –
The Correct Answer and Explanation is :
Here’s a breakdown of the hybridization for the central atoms of the compounds:
- BCl₃ (Boron Trichloride):
- The central atom is boron (B).
- Boron in BCl₃ forms three covalent bonds with three chlorine (Cl) atoms.
- Since boron has three valence electrons, it uses three orbitals (one from the 2s and two from the 2p orbitals) to form bonds with chlorine.
- Therefore, the hybridization of the boron atom in BCl₃ is sp². This is because boron forms three sigma bonds in a trigonal planar geometry, and there are no lone pairs on the boron atom.
- AlCl₄⁻ (Tetrachoridoaluminate ion):
- The central atom is aluminum (Al).
- In AlCl₄⁻, aluminum is surrounded by four chloride ions (Cl⁻), forming a tetrahedral shape.
- Aluminum has three valence electrons and receives an extra electron from the negative charge, making a total of four valence electrons.
- To accommodate four bonding pairs, aluminum undergoes sp³ hybridization. This creates four equivalent orbitals that overlap with the chlorine atoms to form four sigma bonds.
- CS₂ (Carbon Disulfide):
- The central atom is carbon (C).
- Carbon in CS₂ forms two double bonds with sulfur (S) atoms.
- Carbon has four valence electrons and forms two sigma bonds and two pi bonds, one with each sulfur atom.
- Since carbon forms two sigma bonds and two pi bonds, it uses two sp hybridized orbitals for bonding, leaving two unhybridized p orbitals for pi bonding.
- Therefore, the hybridization of carbon in CS₂ is sp.
- KrF₂ (Krypton Difluoride):
- The central atom is krypton (Kr).
- Krypton is a noble gas and has 8 valence electrons. In KrF₂, it forms two bonds with two fluorine (F) atoms, leaving three lone pairs of electrons.
- Given the presence of lone pairs, krypton in KrF₂ undergoes sp³d hybridization to accommodate five electron pairs (two bonding pairs and three lone pairs) in a linear geometry.
- PF₆⁻ (Hexafluorophosphate ion):
- The central atom is phosphorus (P).
- Phosphorus in PF₆⁻ is surrounded by six fluorine (F) atoms, and it carries a negative charge.
- Phosphorus has five valence electrons, and the negative charge adds one more electron, making a total of six valence electrons.
- To form six bonds with fluorine atoms, phosphorus undergoes sp³d² hybridization, resulting in an octahedral geometry.
Image:
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Here is the diagram showing the hybridization and geometry of the molecules you asked about: BCl₃, AlCl₄⁻, CS₂, KrF₂, and PF₆⁻. Each molecule is labeled with its corresponding hybridization type and molecular geometry. Let me know if you’d like more details or explanations!
