Final answer:
The Lewis structures of PCl4+ and PCl6- are not typically correct because phosphorus does not form stable compounds with four or six chlorine atoms. The signs (+/-) indicate the ionic charge due to loss or gain of electrons.
Step-by-step explanation:
The question pertains to the drawing of the Lewis structures for PCl4+ and PCl6-. However, these structures are hypothetically incorrect because they do not exist under normal conditions. The sign in PCl4+ refers to a cation with a positive charge, indicating a loss of an electron, while in PCl6-, it refers to an anion with a negative charge, indicating a gain of an electron. Phosphorus can indeed form five bonds, as in the case of PCl5, because it can promote an electron from the 3s to an empty 3d orbital during the bonding process. However, phosphorus does not commonly form compounds with six chlorine atoms due to its inability to accommodate more than five bonds in a stable configuration. Therefore, PCl4+ and PCl6- are not typically encountered in chemical literature.