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Radiums Lab
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@Fulmen thank you for the safey suggestion. I've worked with the metal before but not its comp.
Water is dangerous if you don't know how to handle it, elemental fluorine (F₂) on the other hand is pretty tame if you know what you are doing.
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Radiums Lab
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I am aware that Hg salts(especially soluable ones) are more toxic than Hg metal.
Water is dangerous if you don't know how to handle it, elemental fluorine (F₂) on the other hand is pretty tame if you know what you are doing.
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Radiums Lab
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I will try to make Ag[HgI4] in the near future. Sorry for 3 posts but my device wont support long...
Water is dangerous if you don't know how to handle it, elemental fluorine (F₂) on the other hand is pretty tame if you know what you are doing.
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Neal
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Quote: Originally posted by Lionel Spanner  | For what it's worth, when I carried out a Jones oxidation of an alcohol to an acid, back in my first year of university (20 years ago) I ended up with
a thermochromic impurity, which was red around 80 °C and green near room temperature.
This was a chromium compound of some kind, for sure - but I don't remember what the alcohol was, so when all's said and done, this post is not
actually very helpful. |
@Lionel Spanner did it have yellow and orange in between from green to red?
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chempyre235
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This seems to confirm that the thermochromism of these salts is related to the specific tetrahedral structure of the anion. Copper, nickel and mercury
all display thermochromism with similar anions, and are in the +4 oxidation state, with the anion being in the -2 state. Additionally, these all bear
four halogen atoms, and the choice of halogen seemingly has a direct impact on the transition temperature of the salt (F > Cl > Br > I).
This leads me to have a few questions:
Have the other metals I mentioned: Mn, Fe, Co, Cd, (which all form tetrahedral complexes in the +4 state) been tested for this property
experimentally?
Is thermochromism of transition metals in this manner limited only to metals that have a tetrahedral +4 state?
Why do different halogens affect transition temperature?
What differences does the choice of cation (e.g., Ag2+, Et2NH2+, etc.) have on the thermochromic
properties?
Is there a way to predict what the colors of these salts will be?
[Edited on 7/22/2025 by chempyre235]
"However beautiful the strategy, you should occasionally look at the results." -Winston Churchill
"I weep at the sight of flaming acetic anhydride." -@Madscientist
"...the elements shall melt with fervent heat..." -2 Peter 3:10
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Radiums Lab
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Halogens have different radi thus differdent EN and more the EN, difficult to go to exited state.
Water is dangerous if you don't know how to handle it, elemental fluorine (F₂) on the other hand is pretty tame if you know what you are doing.
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Lionel Spanner
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| Quote: Originally posted by Neal | | Quote: Originally posted by Lionel Spanner | For what it's worth, when I carried out a Jones oxidation of an alcohol to an acid, back in my first year of university (20 years ago) I ended up with
a thermochromic impurity, which was red around 80 °C and green near room temperature.
This was a chromium compound of some kind, for sure - but I don't remember what the alcohol was, so when all's said and done, this post is not
actually very helpful. |
@Lionel Spanner did it have yellow and orange in between from green to red? |
I seem to remember it did - but as it was so long ago and I've never done a Jones oxidation since them, my memory is not 100% reliable.
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DraconicAcid
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| Quote: Originally posted by chempyre235 | Copper, nickel and mercury all display thermochromism with similar anions, and are in the +4 oxidation state, with the anion being in the -2
state.....
Is thermochromism of transition metals in this manner limited only to metals that have a tetrahedral +4 state?
Why do different halogens affect transition temperature?
What differences does the choice of cation (e.g., Ag2+, Et2NH2+, etc.) have on the thermochromic
properties?
|
The metal is in the +2 oxidation state.
Nickel, at least, generally does thermochromism because it goes from square planar to tetrahedral.
The halogens affect the transition temperature because they have different sizes (larger ones prefer tetrahedral to square planar) and because they
have different splitting effects on the orbital (strong ligands split the orbitals more and favour square planar, which is why the cyanides are all
square planar).
The cations can have an effect because of their size- they pack differently in the solid state.
Please remember: "Filtrate" is not a verb.
Write up your lab reports the way your instructor wants them, not the way your ex-instructor wants them.
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Radiums Lab
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Maybe Ag[HgAt4] is the complex i'm looking for  .
Water is dangerous if you don't know how to handle it, elemental fluorine (F₂) on the other hand is pretty tame if you know what you are doing.
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bnull
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| Quote: | | Maybe Ag[HgAt4] is the complex i'm looking for . |
Well, I happen to have a kilo of astatine fluoride (AtF) left from an old experiment. It is the only reagent that fluorinates photons, glows in the
dark, lots of fun for kids. Free worldwide shipping.
I think this will interest you: Jesse H. Day, Thermochromism of Inorganic Compounds. Chem. Rev. 1968, 68, 6, 649–657, https://doi.org/10.1021/cr60256a001.
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