Draw a single lewis structure for the phosphate ion (po43-), assuming that the phosphorus atom can expand its octet such that the formal charge on each of the atoms is minimized. include all formal charges and lone-pair electrons.

Question

Marlon Ashley

Chemistry

7 August, 05:25

Draw a single lewis structure for the phosphate ion (po43-), assuming that the phosphorus atom can expand its octet such that the formal charge on each of the atoms is minimized. include all formal charges and lone-pair electrons.

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Emilia Choi · Answer 1

The Lewis diagram with single bonds, and all the oxygens have 3 lone pairs. PO4^3 - has 5+4x6+3 = 32 e-

... O

... |

O-P-O

... |

... O

The only purpose that you might want to contain a double bond is for the reason that of an excessively strict adherence to formal charges. By creating one of the bonds a double bond you decrease the formal charge on P from + 2 to + 1 and one of the oxygens from - 1 to 0.

The detail is that all four bonds are undistinguishable. If one of the bonds was a double bond then one bond would have a superior energy that the others. That is why you could use resonance, to make all the bonds equal.