vano
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Gallium and mercury compound + photo
I know this reaction is true:
Hg2Cl2 + 2GaCl3 →Hg2[GaCl3]2
I tried it with mercury (I) nitrate dihydrate and gallium (III) nitrate nonanhydrate. I mixed this hydrates and heated.
There are reagents and compounds. I dont know why it is transparent.
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vano
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Bezaleel
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Thanks for showing pictures of some unusual compound 
What are the products in your second post?
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DraconicAcid
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Quote: Originally posted by vano.kavt  | I know this reaction is true:
Hg2Cl2 + 2GaCl3 →Hg2[GaCl3]2
I tried it with mercury (I) nitrate dihydrate and gallium (III) nitrate nonanhydrate. I mixed this hydrates and heated.
There are reagents and compounds. I dont know why it is transparent.
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I suspect that the gelatinous blob that you have obtained is not the product you desire. You would probably need to use anhydrous starting materials
to get the desired product.
ETA: GaCl3 is a Lewis acid because Ga doesn't have a full octet (just like the aluminum and boron analogues). Ga(NO3)3*9H2O will have a gallium
coordinated by plenty of oxygens, and will not abstract any anion from the mercury(I) cation.
[Edited on 6-12-2020 by DraconicAcid]
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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vano
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Yellow is mercury(I) nitrate dihydrate and white is gallium nitrate nonanhydrate. Thanks for your interest.
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vano
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| Quote: Originally posted by DraconicAcid |
I suspect that the gelatinous blob that you have obtained is not the product you desire. You would probably need to use anhydrous starting materials
to get the desired product. |
I dont know exact formula, but i think Hg2[Ga(NO3)4] is imposoble. I have never read Mercury(I) tetranitratogallate. But halogen complexes are
possible. I took hydrates specifically, because they have low melting points. Also this mercury salt isn't stable and produce mercury oxide. First of
all I use it to get it.
[Edited on 6-12-2020 by vano.kavt]
[Edited on 6-12-2020 by vano.kavt]
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vano
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| Quote: Originally posted by DraconicAcid |
ETA: GaCl3 is a Lewis acid because Ga doesn't have a full octet (just like the aluminum and boron analogues). Ga(NO3)3*9H2O will have a gallium
coordinated by plenty of oxygens, and will not abstract any anion from the mercury(I) cation.
[Edited on 6-12-2020 by DraconicAcid] |
Yes, you are right. The final product was waterless. Completely evaporated. I dont know what it is, maybe its only mixture. I will try chloride in
the future.
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DraconicAcid
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| Quote: Originally posted by vano.kavt |
Yes, you are right. The final product was waterless. Completely evaporated. I dont know what it is, maybe its only mixture. I will try chloride in
the future. |
Letting all the solvent evaporate doesn't mean that the compound is anhydrous.
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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vano
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of course. I know hydrates exist, I always point out. But when you heat it to a high temperature it is impossible to be hydrated.
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DraconicAcid
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| Quote: Originally posted by vano.kavt |
of course. I know hydrates exist, I always point out. But when you heat it to a high temperature it is impossible to be hydrated.
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How much did you heat it?
Something like hydrated aluminum nitrate would surely decompose to the oxide or hydroxide instead of becoming anhydrous aluminum nitrate when heated-
I would expect the gallium salt to behave similarly.
ETA: https://link.springer.com/article/10.1007/s10973-005-0909-x
[Edited on 6-12-2020 by DraconicAcid]
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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vano
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Finally I heated it too much with propane torch. Would most likely decompose into oxides, but I do not know why it remained white. mercury oxide is
orange. It also produced nitrogen oxide gas.
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