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. (a) Do you think there are any unshared pairs of electrons in the P4 molecule? (b) How many bonds are there in the molecule? (c) Can you draw a Lewis structure for a linear P4 molecule that satisfies the octet rule? (d) Using formal charges, what can you say about the stability of the linear molecule versus that of the tetrahedral molecule?
Chapter 2: Atoms, Ions, and Molecules: The Building Blocks of Matter Key: Calculate: Calc Number: # negative: neg + moles: mol (s) proton: p isotopes: iso 0 Average: avg molecules: molec neutron: n With: w/ electrons: e Chemical: chem positive: pos Learning Objectives