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$ceSO4^2-$ is a polyatomic ion as well as a nonpolar covalent compound. How deserve to it it is in ionic and also covalent in ~ the same time?Same applies to sulfite $ceSO3^2-$. It"s a polyatomic ion as well as a polar covalent bond. How?


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These two types have bonds in ~ them, and also (non)polar covalency describes those interior bonds. The varieties as a totality can it is in an ion, and yet not have net polarity on its bonds.Sulfate is tetrahedral, so each individual dipole vector would be opposed and also cancelled, making the overall molecule non-polar (in the same method that this question and also answer around $ceCO2$ details).Sulfate has negative charges which could make a Lewis dot structure show up to have a net dipole, over there is resonance that distributes that charge throughout the molecule, it is negative the net effect.

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Sulfite, top top the various other hand, is trigonal pyramidal. In this geometry, not every bond is opposed and also thus over there is a polarity within these covalently-bonded atoms the constitute the ion.

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Polyatomic ions, usually negatively charged, are groupings of atoms bound with each other by covalent bonds. This groupings can carry extra electrons, offering them a an unfavorable charge, or have fewer electrons than the merged valence count of the atoms present, offering them a positive charge. Thus, despite its charge, a polyatomic ion is still written of covalent bonds. As in uncharged molecules, those covalent bonds deserve to be one of two people polar or nonpolar, and the ion, as a whole, deserve to be either polar or nonpolar, relying on the spatial species of the bonds. Therefore, the is feasible for a charged ion, such as sulfate, to it is in both ionic, and also nonpolar covalent - definition the electron arrangements among the covalent bonds are equally and symmetrically distributed.


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