Problem: NO3- :Molecular geometry?Ideal bond angle?Are polar bonds present?Is there an overall dipole?Octect rule violator and how?

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  • N will appear as our central atom since it is less electronegative than O

  • N will appear to have 3 Os single bonded on it however, each O atom will appear as negatively charged with 3 lone pairs in it

  • One O must have a double bond with N making it neutral while N as positively charged

  • This will give a total charge of -1

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Problem Details

NO3- :

Molecular geometry?

Ideal bond angle?

Are polar bonds present?

Is there an overall dipole?

Octect rule violator and how?

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