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# ${ P }_{ 2 }{ I }_{ 4 }$ Hybridization and Bond Angles

CHEM-QF4PUR

Sketch a good Lewis structure of diphosphorus tetraiodide and use it to determine which of the following statements are true.

Note in this symmetrical molecule that there is a phosphorus-phosphorus bond and each phosphorus atom has trigonal pyramidal molecular geometry.

Select ALL that apply.

A

The electron pair geometry around each phosphorus atom is trigonal bipyramidal and the phosphorus-phosphorus double bond is formed by ${ sp }^{ 3 }-{ sp }^{ 3 }d$ and $p-p$ overlap. The P-P-I bond angle is close to 120${ }^{ \circ }$.

B

The electron pair geometry around each phosphorus atom is tetrahedral and the phosphorus-phosphorus bond is formed by ${ sp }^{ 3 }-{ sp }^{ 3 }$ overlap. The P-P-I bond angle is less than 109${ }^{ \circ }$.

C

The phosphorus-iodine bond is formed by ${ sp }^{ 3 }-{ sp }^{ 3 }$ overlap. All of the non-bonding electrons in the molecule are in ${ sp }^{ 3 }$ hybridized orbitals. If iodine is more electronegative than phosphorus then the oxidation state of phosphorus is +2 and its formal charge is 0.

D

The formal charge of each iodine is -1 and each phosphorus is +2 making the molecule have no overall charge. Two of the phosphorus-iodine bonds are double bonds and the other two are single bonds.