Ionic bonding question about "double" ionic bonds

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Discussion Overview

The discussion revolves around the concept of "double" ionic bonds versus "single" ionic bonds, specifically comparing the bonding in compounds like MgO and NaCl. Participants explore the strength, structure, and feasibility of creating compounds with double ionic bonds in a laboratory setting.

Discussion Character

  • Debate/contested
  • Conceptual clarification
  • Technical explanation

Main Points Raised

  • Some participants suggest that a "double" ionic bond, involving the transfer of two electrons, is stronger than a "single" ionic bond due to the increased ionic charge affecting bond energy.
  • Others argue that ionic bonds primarily rely on Coulomb forces, which can be estimated using a specific formula, implying that the strength of the bond can be quantitatively analyzed.
  • A question is raised about the possibility of creating NaCl with a double ionic bond using Cl+ and Na-, and whether such a compound exists.
  • Some participants assert that it is not feasible to create a double bond from singly charged ions, noting that Na2+ would interact with Cl2- in a specific energetic manner.
  • Further inquiries are made regarding the reaction between Cl2 and Na-, questioning whether Cl would steal an electron from Na or if Na- could bond with both Cl atoms, potentially forming a structure like MgCl2.
  • A participant references external sources to identify compounds that may exist, questioning the structural differences between them.
  • Another participant clarifies that sodium dichloride should be viewed as Na+ combined with two Cl- ions, rather than as Na- and Cl2.

Areas of Agreement / Disagreement

Participants express differing views on the nature and strength of double versus single ionic bonds, as well as the feasibility of creating compounds with double ionic bonds. The discussion remains unresolved regarding the specifics of reactions involving Na- and Cl2.

Contextual Notes

There are limitations in the assumptions made about ionic bonding and the conditions under which certain reactions may occur. The discussion also reflects uncertainty regarding the existence and structural characteristics of specific compounds mentioned.

ProjectFringe
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Is a "double" ionic bond (the transfer of two electrons) like in MgO any stronger (or really any different, structurally etc.) than a "single" ionic bond (the transfer of one electron) like in NaCl?
 
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Yes it is. Doubling the ionic charge nearly quadruples the bond energy.
 
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Ionic bonds are mostly about simple Coulomb forces, these are quite easy to estimate with

F = k\frac{q_1q_2}{r^2}

Just try to put what you wrote into the equation and you will see where @chemisttree answer comes from.
 
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Is it possible then to make NaCl with a double ionic bond by combining in a lab Cl+ and Na-? Does this compound exist and if so what is it called (how to differentiate from normal NaCl)?
 
No, you can't make a double bond out of single charged ions.

And you can't ionize Na nor Cl further - that is, in some exotic conditions you can, but when you combine them the Na2+ will steal an electron from Cl2- and they will live happily ever after in their local energetic optimum.
 
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Got it. Thanks:biggrin:
 
Borek said:
No, you can't make a double bond out of single charged ions.

And you can't ionize Na nor Cl further - that is, in some exotic conditions you can, but when you combine them the Na2+ will steal an electron from Cl2- and they will live happily ever after in their local energetic optimum.
Sorry, one more question. o_O

What reaction would occur between Cl2 and a Na-? Would a Cl atom steal an electron from Na, making Cl- + NaCl? Or would the Na- create an ionic bond with both Cl atoms creating a structure similar to MgCl2?
 
ProjectFringe said:
Sorry, one more question. o_O

What reaction would occur between Cl2 and a Na-? Would a Cl atom steal an electron from Na, making Cl- + NaCl? Or would the Na- create an ionic bond with both Cl atoms creating a structure similar to MgCl2?

Actually, I was able to find both compounds here:

https://pubchem.ncbi.nlm.nih.gov/compound/22590707

https://pubchem.ncbi.nlm.nih.gov/compound/57736105

So, what makes the difference between which of these compound structures is formed, or are they the same thing?
 
Sodium dichloride (assuming it exists) is not Na- + Cl2, if anything, I would treat it as Na+ + 2Cl-.
 
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