Problem: A common form of elemental phosphorus is the tetrahedral P4 molecule, where all four phosphorus atoms are equivalent: At room temperature phosphorus is a solid. How many P - P bonds are there in the molecule?

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The Lewis structure for P4 is:

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A common form of elemental phosphorus is the tetrahedral P4 molecule, where all four phosphorus atoms are equivalent:

 A diagram shows P4 as four atoms arranged in a pyramid shape, each single bonded to the other three atoms.

At room temperature phosphorus is a solid. How many P - P bonds are there in the molecule?

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Lewis Dot Structures: Neutral Compounds concept. You can view video lessons to learn Lewis Dot Structures: Neutral Compounds. Or if you need more Lewis Dot Structures: Neutral Compounds practice, you can also practice Lewis Dot Structures: Neutral Compounds practice problems.

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Based on our data, we think this problem is relevant for Professor Han's class at UNLV.