Why is CuCl easier or harder to separate than CuCl2?

[JasonRox]

I started reading a book about the basic foundations of chemistry, and I came up across a simple question.

To answer this question you should understand that there are variable valencies, which is what this question consists of.

If you look at the cuprous chloride compound CuCl, copper has a valency of one.

Chlorine will "take" an electron from the Copper atom, which forms a covalent bond. When taking the electron the overall magnetic charge of the chlorine atom is negative (let's say -1), and Copper is now overall positive (+1).

If we look at a slightly different compound cupric chloride CuCl(2), copper has a valency of 2.

Chlorine 1 and 2 will now take each an electron, so you have two with an overall charge of -1. Copper now gives two away, on its own, and now has an overall charge of +2.

My question is...

Is one bond stronger than the other because of magnetic charge?

In other words, would Chlorine be easier to isolate from the CuCl compound than the CuCl(2) compound, or molecule?

Thanks, for any answers.

 

[JasonRox]

Anyone?

This is a simple question in which I am pondering.

 

[thunderfvck]

I'm not sure because I'm no expert but I think that the Cu-Cl bond is identical regardless of how many bonds there are. So it'd require just as much energy to break any Cu-Cl bond.

 

[xie]

chemistry always contains of mystery...

 

[chemisttree]

I started reading a book about the basic foundations of chemistry, and I came up across a simple question.

To answer this question you should understand that there are variable valencies, which is what this question consists of.

If you look at the cuprous chloride compound CuCl, copper has a valency of one.

Chlorine will "take" an electron from the Copper atom, which forms a covalent bond. When taking the electron the overall magnetic charge of the chlorine atom is negative (let's say -1), and Copper is now overall positive (+1).

You are referring to an electric charge... not magnetic.

If we look at a slightly different compound cupric chloride CuCl(2), copper has a valency of 2.

Chlorine 1 and 2 will now take each an electron, so you have two with an overall charge of -1. Copper now gives two away, on its own, and now has an overall charge of +2.

My question is...

Is one bond stronger than the other because of magnetic (electric) charge?

In other words, would Chlorine be easier to isolate from the CuCl compound than the CuCl(2) compound, or molecule?

Thanks, for any answers.

Let's look at trends in the transition metal halide series


Bond Bond dissociation energy (kJmol^-1)
Ti-Cl (TiCl4) 429.3
Ti-Cl (TiCl3) 460.2
Ti-Cl (TiCl2) 504.6
Fe-F (FeF3) ~456
Fe-F (FeF2) 481
Fe-Cl (FeCl3) 341.4
Fe-Cl (FeCl2) 400.0
Fe-Br (FeBr3) 291.2
Fe-Br (FeBr2) 339.7
Fe-I (FeI3) 233.5
Fe-I (FeI2) 279.1
Cu-Cl (CuCl2) 293.7
Cu-Cl (CuCl) 360.7
Cu-Br (CuBr2) ~259
Cu-Br (CuBr) 330.1
Cu-I (CuI2) ~192
Cu-I (CuI) ~142

Clearly the trend is that the higher the oxidation state, the easier it is to remove the first halide in transition metals.

 

[Borek]

Necrophilia

 

[Renge Ishyo]

A thread dig from 2004? That was long before I was even a member here

 

[chemisttree]

Opps! I keep forgetting to check that...