July 17, 2024, 07:02:55 AM
Forum Rules: Read This Before Posting

Topic: Why is HgCl_2 more covalent than CaCl2?  (Read 727 times)

0 Members and 1 Guest are viewing this topic.

Offline sd79812

  • Regular Member
  • ***
  • Posts: 36
  • Mole Snacks: +0/-2
Why is HgCl_2 more covalent than CaCl2?
« 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?

Offline JamesMN

  • Very New Member
  • *
  • Posts: 2
  • Mole Snacks: +0/-0
Re: Why is HgCl_2 more covalent than CaCl2?
« Reply #1 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.

Sponsored Links