Formation of hydrates from ionic compounds

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SUMMARY

The discussion centers on the formation of hydrates from ionic compounds, specifically comparing aluminum fluoride and sodium fluoride. Aluminum ions, due to their +3 charge and smaller ionic radius, exhibit a strong Coulombic attraction to water molecules, resulting in the formation of aluminum hydrate with six water molecules attached. In contrast, sodium ions, which possess a +1 charge and a larger ionic radius, do not form hydrates and remain as free ions in solution. This highlights the role of ionic charge and size in hydrate formation.

PREREQUISITES
  • Understanding of ionic compounds and their properties
  • Knowledge of Coulombic attraction and its implications
  • Familiarity with the concept of ligands in coordination chemistry
  • Basic principles of solvation and hydration in chemistry
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  • Research the role of ionic charge in solvation dynamics
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  • Study the properties of aluminum hydrates and their formation mechanisms
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Homework Statement



Not really much of a problem - just a general question and some speculation on its answer.

Why do some ionic compounds such as aluminum fluoride form hydrates while other ionic compounds such as sodium fluoride don't form hydrates upon being dissolved in solution?

Homework Equations



Water is a polar molecule.
Coulombic attraction. Attraction (q) is inversely proportional to the distance between the radii of the two charged particles.

The Attempt at a Solution



I'm guessing this is due to the fact that sodium is a much bigger molecule than aluminium and sodium has only a +1 charge while aluminium has a +3 charge. These two factors cause aluminum ions in solution to form aluminium hydrate (aluminium with 6 water molecules attached) while sodium doesn't do anything in solution; it stays as an ion.
 
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This is more about water creating complexes (being a ligand).
 

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