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Chemistry Forums for Students => High School Chemistry Forum => Topic started by: sd79812 on June 07, 2024, 06:02:33 PM

Title: Why is HgCl_2 more covalent than CaCl2?
Post by: sd79812 on June 07, 2024, 06:02:33 PM

Hg2+ has more shells of p-orbitals and s-orbitals than the Ca2+ in CaCl2. Do those extra p and s shells in Hg2+ shield the two Chlorines in HgCl2 from the effect of Hg2+ nucleus attraction or leave the Hg2+ valence electrons attracted to the chlorine electron cloud in HgCl2?

Title: Re: Why is HgCl_2 more covalent than CaCl2?
Post by: JamesMN on June 21, 2024, 05:19:08 PM

I don't know to what depth you're looking for an answer, I certainly wouldn't be looking at it as you seem to be given what you're addressing in your question.

Me? What's the electronegativity difference? Ca: 1.0, Hg: 1.9, and Cl: 3.0.

I know there's no "fixed" difference that sets an ionic over a covalent bond, but let's go with if the difference is > or equal to 1.7 it's ionic, < 1.7 it's covalent.

Now why is the electronegativity what it is? Definitely tied to the size of the atom, with > size resulting in lower EN values, which  certainly fits here. But for a high school forum? Heck, an EN explanation works for me.