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molecular geometry for Phosphorus triiodide
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Step 1
: Identify the number of atoms in the molecule and determine its electron group geometry.

Phosphorus triiodide (PI3) has one phosphorus atom and three iodine atoms. Phosphorus has 5 valence electrons, and each iodine has 7 valence electrons. In the PI^3 molecule, phosphorus shares one electron with each iodine atom, forming three P-I bonds. There are also five lone pairs of electrons around the central phosphorus atom (two from phosphorus and one from each iodine). The electron group geometry of PI^3 is octahedral because there are six electron groups around the central phosphorus atom (three bonds and three lone pairs).

Step 2
: Determine the molecular geometry using the AXE method.

In the AXE method, A represents the central atom, X represents the number of atoms bonded to the central atom, and E represents the number of lone pairs on the central atom. For PI^3, A = P, X = 3 (three iodine atoms), and E = 3 (three lone pairs). Since E (lone pairs) is greater than zero, the molecular geometry will be different from the electron group geometry. To find the molecular geometry, we need to consider how the lone pairs are arranged around the central atom.

Final Answer

The molecular geometry of Phosphorus triiodide (PI3) is trigonal bipyramidal.

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