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

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The CO3(2-) carbonate ion is classified as a nonpolar molecule due to its symmetrical trigonal planar geometry and the delocalization of electrons across its three resonance structures. Each of the carbon-oxygen bonds in the carbonate ion has a bond order of approximately 1.3333, which contributes to the overall symmetry and nonpolarity of the ion. The charge distribution is uniform, confirming that there is no net dipole moment in 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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