How many lone pairs of electrons are represented in the Lewis structure of a phosphate ion (PO43-)?

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Hey P has 5 valence electrons O has 6 valence electrons (each for 4 oxygen) And finally, for every negative charge, there is an additional valence electron We should add these all up = 5 + 24 + 3 = 32 valence electrons With this, we can be guided to illustrate the lewis structure as P as central atom and the 3 oxygen each with a single bond with P and 1 oxygen with a double bond with P. We place the valence electrons until octet rule is satisfied, we will be left with 12 lone pairs for phosphate ion. Hoped I Helped

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