Polar or Nonpolar: CO3(2-) Carbonate Ion Help

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The discussion centers on the polarity of the carbonate ion, CO3(2-). It is established that the ion has a trigonal planar geometry and features delocalized double bonds through resonance contributors. This delocalization results in all three bonds having an effective bond order of 1.3333, rather than a mix of bond orders. The symmetrical arrangement of the bonds leads to the conclusion that the carbonate ion is nonpolar, as the charge distribution is uniform across the molecule.
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Is the CO3(2-) carbonate ion polar or nonpolar? I know its a triagonal planar but it also has the double bond. please help.
 
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The double bond is delocalized through its three resonance contributors, so I presume the molecule is nonpolar; the charge central is identical with the weight central (I don't know how to say these in English).

If there is an error, I'll correct though.
 
I believe you are correct. All three bonds are actually of order 1.3333, rather than one bond being of order 2 and the others of order 1. This makes it a symetrical planar molecule, meaning it's nonpolar.
 

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