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Chemistry Forums for Students => High School Chemistry Forum => Topic started by: constant thinker on May 03, 2007, 09:18:36 PM

Title: Ammonium Chloride, Ionic or Molecular?
Post by: constant thinker on May 03, 2007, 09:18:36 PM

Is ammonium chloride (NH₄Cl in case someone reads this and doesn't know the chemical formula) an ionic or molecular compound?

I'm leaning towards it being molecular because the difference in the electronegativity values of nitrogen and chlorine is .12.

The reason for me to questions this is the ammonium ion would be fairly electron dense. That simple thought makes wonder if an electron is completely transferred.

Thoughts anyone?

Title: Re: Ammonium Chloride, Ionic or Molecular?
Post by: enahs on May 03, 2007, 09:37:44 PM

It is Ionic.

Most ammonium salts (such as ammonium chloride in this case) tend to resemble the salts of potassium and rubidium in structure as well as solubility, due to comparable ion radii.

Salts of the strong acids are fully ionized and the solutions are slightly acidic.

NH₄Cl  <-> NH₄⁺ Cl^-     K~infinity
NH₄⁺ + H₂O  <->  NH³ + H₃O⁺     K=5.5x10^-10

Title: Re: Ammonium Chloride, Ionic or Molecular?
Post by: constant thinker on May 05, 2007, 05:26:59 PM

Ok thanks enahs. I understand why.