Phosphorus can be bi-, tri-, penta- and hexavalent.
Phosphorus typically forms a -3 charge when it becomes an ion by gaining three electrons.
The charge of a phosphorus (P) ion can vary depending on its oxidation state. For example, in the common phosphate ion (PO4)3-, phosphorus has a charge of +5.
A phosphorus ion is called a phosphate ion, which has a charge of -3.
The most common charge of phosphorus is -5.
Phosphorus typically forms the phosphate ion, which has a charge of -3. This is the most common stable ion of phosphorus found in nature.
The phosphide ion, meaning phosphorous by itself not bound up in a poly-atomic ion, has a charge of -3 in ionic compounds.
This ion would be an atom of phosphorus with a +3 charge, as phosphorus typically has 15 electrons and 15 protons (which gives it a neutral charge). The number of neutrons doesn't affect the charge of the ion, so it would still be considered a phosphorus ion with a +3 charge.
Most commonly, it will have a 3- charge.
Phosphorus forms a -3 ion called phosphide.
Phosphorus generally forms phosphide ion (P3- ion).
Phosphorus (P) typically forms an ion with a charge of -3, known as the phosphate ion (PO4)^3-. The outer electron configuration of phosphorus allows it to gain three electrons to achieve a stable electron configuration, resulting in a -3 charge.
When phosphorus forms its ion, it gains three electrons to become the phosphide ion with a 3- charge. This allows phosphorus to complete its valence shell and achieve a stable electronic configuration.