To determine the hybridization of the phosphorus (P) atom in phosphorus pentafluoride (PF5), we start by analyzing the electron configuration and geometry of the molecule.
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Electron Configuration of Phosphorus:
- The electron configuration of phosphorus (atomic number 15) is: \[ 1s^2 2s^2 2p^6 3s^2 3p^3 \]
- The 3s and 3p orbitals are involved in bonding.
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Bonding in PF5:
- In PF5, phosphorus forms five equivalent bonds with five fluorine atoms. To accommodate these five bonds, phosphorus undergoes hybridization.
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Hybridization:
- The hybridization can be explained as follows:
- The 3s orbital and three 3p orbitals mix to form five equivalent sp³d hybrid orbitals.
- The electron configuration changes as phosphorus promotes one of its 3s electrons to the 3d orbital, allowing the P atom to form five bonds.
- The hybridization can be explained as follows:
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Geometry of PF5:
- The molecular shape of PF5 is trigonal bipyramidal:
- Three of the sp³d hybrid orbitals lie in a plane (equatorial), and two of them are positioned above and below this plane (axial).
- The molecular shape of PF5 is trigonal bipyramidal:
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Visualization:
- While I cannot provide pictures directly, I can describe how to sketch the arrangement:
- Draw a central phosphorus atom.
- From the phosphorus atom, draw five lines radiating outward to represent the bonds with the five fluorine atoms.
- Position three bonds in a horizontal plane (equatorial positions) like a triangle.
- Position the remaining two bonds above and below this plane (axial positions).
- While I cannot provide pictures directly, I can describe how to sketch the arrangement:
In summary, the orbitals involved in the hybridization of the phosphorus atom in PF5 are one 3s orbital and three 3p orbitals, leading to the formation of five sp³d hybrid orbitals, resulting in a trigonal bipyramidal molecular geometry.
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