Problem: Why does NO3- have a molecular geometry shape of trigonal planar?? Isn't it true that in order to be  trigonal planar there should be 4 bonded pairs and 0 lone pairs?

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Why does NO3- have a molecular geometry shape of trigonal planar?? Isn't it true that in order to be  trigonal planar there should be 4 bonded pairs and 0 lone pairs?

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Our tutors have indicated that to solve this problem you will need to apply the Molecular vs Electron Geometry concept. You can view video lessons to learn Molecular vs Electron Geometry. Or if you need more Molecular vs Electron Geometry practice, you can also practice Molecular vs Electron Geometry practice problems.

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Based on our data, we think this problem is relevant for Professor Zhang's class at USF.