Is Nitrate Polar or Non-Polar? Understanding Molecular Properties and Solubility

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SUMMARY

Nitrate (NO3-) is a polar molecule despite its trigonal planar shape and resonance structures that distribute negative charge across the oxygen atoms. The molecule's solubility in water is attributed to its ionic nature and the ability to form hydrogen bonds, which contribute to the Gibbs free energy favoring dissolution. The discussion clarifies that while nitrate exhibits symmetry, its charge distribution and interactions with water make it polar and soluble.

PREREQUISITES
  • Understanding of molecular geometry, specifically trigonal planar shape.
  • Knowledge of resonance structures and their impact on molecular properties.
  • Familiarity with solubility principles, including ionic interactions in solvents.
  • Basic grasp of thermodynamics, particularly Gibbs free energy and its role in dissolution.
NEXT STEPS
  • Research the impact of molecular geometry on polarity and solubility.
  • Study the principles of resonance and charge distribution in molecules.
  • Explore the role of hydrogen bonding in solubility of ionic compounds.
  • Investigate thermodynamic principles related to Gibbs free energy in chemical processes.
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Chemistry students, molecular biologists, and professionals in environmental science who seek to understand the properties of nitrate and its behavior in aqueous solutions.

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Is nitrate a polar or non-polar molecule? I understand that it has a trigonal planer shape (and therefore it has symmetry) but should we also consider the double bond (do multiple bonds destroy symmetry)? I assume it would be polar because it is SOLUBLE in WATER, however, after viewing many links online, many people say it is non-polar
 
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Resonance distributes the negative charge, so it's not constrained to any oxygen in particular. This makes the entire outside negative, so there's no polarity.
 
Solubility

Oh okay, but why is it soluble in water?
 
It's not polar, but it's still charged. Why are singular ions soluble in water? Na+ on its own isn't polar, but it's very soluble.
 
hydrogen bonding and entropy effects contribute to the Gibbs free energy of the process of dissolution. Its thermodynamically favorable for it to dissolve, and there is also a kinetic pathway available. What more could one want ? :)
 

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