I"m confused because when I draw all of the Os attached with single bonds to P the formal charges don"t make sense. But when I add a double bond to one of the Os the formal charges are -1 to 3 of the oxygens. I"m confused if there should be a double bond or not for the PO4 3- structure.
If we start at the beginning by drawing the Lewis dot structure we start with valence electrons.
You are watching: Lewis dot structure for po4 3
P has 5 ve
each O has 6 ve so that"s a total of 4x6 = 24 ve
We add 3 more for the 3- charge for a total of 32 valence electrons
So, this can be written with P at the center and 4 O atoms attached with single bonds and all O atoms would have 3 lone pairs. This arrangement gives a formal charge of +1 on P and -1 on all O atoms. Not good.
Adding a double bond to one of the O atoms results in a formal charge of zero on P, zero on the O with the double bond, and -1 on the other 3 O atoms. This is fine because the charge on the phosphate anion is 3- and so the -1 on each of 3 oxygens accounts for this. You shouldn"t be confused because you have done it correctly. Also recall that P can have an expanded octet (which it does in the dot structure we just drew).
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