Question #78f7f

1 Answer
Stefan V.
Jul 18, 2017

Explanation:

For starters, you should know that phosphorus is located in group 15 of the Periodic Table of Elements, which implies that it needs 3 electrons to complete its octet.

In other words, a neutral phosphorus atom has a total of 5 valence electrons. When a phosphorus atom takes in 3 electrons, it gets a total of 8 electrons in its outermost shell -> it now has 8 valence electrons.

Consequently, a phosphide anion, "P"^(3-) will be formed.

You can thus say that a phosphide anion has a total of 8 valence electrons. Moreover, this anion is isoelectronic, ie. it has the same electron configuration, with argon, "Ar", the noble gas that follows it in the Periodic Table.

Related questions
See all questions in Valence Electrons
Impact of this question
3358 views around the world
You can reuse this answer
Creative Commons License