2007-05-18 05:55:17 · 4 answers · asked by Random G 3 in Science & Mathematics ➔ Chemistry
Skip to the end for the short version :o)
First things first. We need to know the structure of the molecule/ion. This is because oxidation state is defined as the charge on an atom IF all of the bonds were 100% ionic.
So, without speculating about the structure (which is a common pitfall leading to false assumptions), we can find it at sigmaaldrich.com.
http://www.sigmaaldrich.com/catalog/search/ProductDetail/RIEDEL/60352
As you can see, if the bonds were completely ionic, the oxygen that surrounds the phosphorus would pull the electrons from the phoshorus, causing a single positive charge for each single-bonded oxygen atom, and a double positive charge due to the double-bonded oxygen atom.
Since there are 4 oxygen atoms per phosphorus, and one with a double-bond, the hypothetical positive charge would thus be +5.
SHORT VERSION:
+5 is the oxidation state of each phosphorus atom.
2007-05-18 06:13:51 · answer #1 · answered by Anonymous · 0⤊ 0⤋
+6
2007-05-18 06:11:44 · answer #2 · answered by ag_iitkgp 7 · 0⤊ 1⤋
4 x H(+1) = +4
7 x O(-2) = -14
The two P atoms together must be equal to +10 so that the overall charge is zero. Therefore each P has to be +5.
2007-05-18 05:58:45 · answer #3 · answered by mrfarabaugh 6 · 0⤊ 0⤋
H4p2o7 Structure
2017-01-19 10:31:56 · answer #4 · answered by ? 4 · 0⤊ 0⤋