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why does phosphorus oxides to form phosphorus pentoxide whereas it should be forming diphosphorus troxide?
as far as their valancies r concerned......
4 Answers
- cool nerdLv 41 decade agoFavorite Answer
no, it is always P2O5. because by the law of VSPER.
Source(s): trust me. i am good at CHEM. lol. i won many chem competitions - jorganosLv 61 decade ago
Easy answer: Phosphorous donates 5 electrons to go to the Neon shell.
A bit more complicated: Only elements of the 2nd main quantum number are restricted to 4 electron pairs per atom - hybridization of 1 2s and 3 2p orbitals. Elements of the 3rd and higher main quantum number can (besides using the 3s and 3p orbitals) also use the 3d orbitals (which get filled only after the 4s orbitals if you look at the periodic system). So, phosphorous can have 5 covalent bonds (because it has 5 outer electrons), sulphur can have 6, and chlorine can have 7 bonds (e.g. in perchloric acid).
- 1 decade ago
Phosphorus has multiple oxidation states. The product will depend on the energy present when the oxidation reaction occurs. This might be changed by heating the material greatly or altering the amount of oxygen present.
- 1 decade ago
ACCORDING TO MOLECULAR ARRANGEMENT OF ELECTRONS IN THE ORBIT OF PHOSPHOROUS IT EITHER DONATES FIVE ELECTRONS OR ACCEPTS 3 ELECTRONS WHATEVER IS EASY FOR IT TO ATTAIN STABILITY AND SO IT FORMS PHOSPHOROUS PENTOXIDE
