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jamit
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Experiments with Cesium chloride?
i just received some cesium chloride from a friend... the problem is I don't know what experiment I can do with it?
I don't think I want to make cesium... too dangerous!
There's isn't much info on what to do with it on the web, although there are lots of info on cesium chloride.
Anybody done any useful with cesium chloride? I'd appreciate any suggestion or leads I can research. thanks.
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weiming1998
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Maybe make some CsOH with it. As it is extremely soluble (300g/100ml), it will actually precipate the NaCl or KCl if you poured a NaOH or KOH
solution in it. But be careful with that stuff; it's the strongest non-super-base alkaline available. It would be interesting to perform experiments
on it.
[Edited on 30-1-2012 by weiming1998]
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strontiumred
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Hi Jamit,
Try this one - It worked well for me:
http://woelen.homescience.net/science/chem/exps/CsCuCl3/inde...
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AirCowPeaCock
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Aren't Cs compounds important catalysts?
BOLD
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jamit
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@strontiumred
Thanks for the link. I'll give that a try.
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woelen
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There are more interesting things you can do with it:
- Make Cs2CoCl4 (a blue compound, similar to the experiment as linked above).
- Prepare Cs2Cr2O7 (this compound is almost insoluble in cold water)
- Prepare cesium polyholide compounds, e.g. CsICl4 (if you have conc. HCl and an iodate) or CsBrCl2 from Br2 and CsCl.
Cs also perfectly make nearly insoluble CsClO3. You could make CsClO3 directly from CsCl by means of electrolysis or use NaClO3 and CsCl to make this.
This compound makes nice blue flames when mixed with sulphur and ignited (be careful though with chlorate/sulphur mixes!). I also did a similar
experiment with CsBrO3 (can easily be made from KBrO3 and CsCl, KBrO3 can easily be made from KBr, see my website).
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jamit
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Thanks woelen. Are the synthesis of these compounds on your website? I didn't see all of them. Again thanks.
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alkalimetals
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Hello! I'm new, I don't speak english very well... Sorry
I've found this interesting discussions in Home Chemistry Forum (italian forum) which talk about Cs+ and his compounds and complexes. I hope these
articles will be interesting
Caesium Tetrachlorocobaltate (II) Cs2[CoCl]4
http://homechemistry.gratisforum.tv/viewtopic.php?f=3&t=...
Caesium Tetrachlorocuprate (II) Cs2[CuCl]4
http://homechemistry.gratisforum.tv/viewtopic.php?f=3&t=...
Caesium Dichloroiodide CsICl2
http://homechemistry.gratisforum.tv/viewtopic.php?f=3&t=...
Caesium Tetrachloroiodide CsICl4
http://homechemistry.gratisforum.tv/viewtopic.php?f=3&t=...
Caesium Tribromide CsBr3
http://homechemistry.gratisforum.tv/viewtopic.php?f=3&t=...
Caesium Tetraiodomercurate (II) Cs2[HgI4]
http://homechemistry.gratisforum.tv/viewtopic.php?f=3&t=...
Caesium Dichlorobromide CsBrCl2
http://homechemistry.gratisforum.tv/viewtopic.php?f=3&t=...
Dicaesium Octaiodide Cs2I8
http://homechemistry.gratisforum.tv/viewtopic.php?f=3&t=...
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blogfast25
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Make your own Cs metal:
http://www.sciencemadness.org/talk/viewthread.php?tid=6981&a...
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alkalimetals
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I've got 100 grams of caesium chloride, I had bought to try to synthesize cesium metal, but after reading the patent, I realized it could not make
this because I'll never get a vacuum of at least 0.01 mm Hg...
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Adas
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Quote: Originally posted by alkalimetals  | | I've got 100 grams of caesium chloride, I had bought to try to synthesize cesium metal, but after reading the patent, I realized it could not make
this because I'll never get a vacuum of at least 0.01 mm Hg... |
I think there's no need for vacuum, use pure argon. I think it should not be extremely hard to get, neither very expensive.
Rest In Pieces!
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alkalimetals
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The patent US3164461 contains a tabel which talk about the conditions of reaction... If you work at 760 mmHg the yield is about 50% and the purity is
unknow; and you have to keep the temperature between 675 and 760 °C... this is not very easy!
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blogfast25
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High vacuum not only eliminates oxygen (to which Cs is very sensitive), it also lowers its boiling point a lot)
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AndersHoveland
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| Quote: Originally posted by Adas | ... to try to synthesize cesium metal, but after reading the patent, I realized it could not make this because I'll never get a vacuum of at least
0.01 mm Hg
I think there's no need for vacuum, use pure argon. |
Nitrogen would probably work. Despite being considered so "reactive", elemental caesium is actually completely unreactive towards nitrogen gas.
Lithium is the only alkali metal that can burn in nitrogen. (caesium nitride, Cs3N, is actually unstable, and it has probably never been prepared,
although some of the older literature refers to caesium azide, CsN3, as "caesium nitride")
[Edited on 27-4-2012 by AndersHoveland]
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Eddygp
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@AndersHoveland However, a vacuum is needed or something to keep the temperature at more than 1000K...
there may be bugs in gfind
[ˌɛdidʒiˈpiː] IPA pronunciation for my Username |
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AndersHoveland
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A vacuum is not absolutely needed, but it would certainly help. Without a vacuum, the distillation will have to reach caesium's standard boiling
point, at 671°C. This temperature is going to be fairly difficult to reach, and one would need an iron retort, as glass would melt and fuse into the
alkali metals.
One method that might be considered is igniting a "thermite" mixture of CsOH and Mg in a closed metal pot. (the formation of CsH would not be
problematic, as this compound decomposes at around 170 °C )
2 CsOH + Mg --> MgO + 2 Cs + H2
(but remember that caesium is still considered the most "reactive" element on the periodic table, it can reduce the chloride salts of all of the other
metallic elements)
MgCl2 + 2 Cs --> 2 CsCl + Mg
[Edited on 27-4-2012 by AndersHoveland]
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Eddygp
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Not an easy isolation, that one of elemental Cs 
Maybe some electrolysis, in a solution of a cesium salt?
there may be bugs in gfind
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blogfast25
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Is there anything you actually DO KNOW??? Any misinformation
you're NOT willing to cackle away about???
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elementcollector1
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Whoa there, blogfast, even if I don't know about the vacuum part, the rest of his post holds up to scrutiny.
As for Eddygp, that would only result in cesium hydroxide, as cesium reacts with water. This is the common industrial method of producing alkali
hydroxides from other alkali compounds.
Elements Collected:52/87
Latest Acquired: Cl
Next in Line: Nd
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Eddygp
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And calcinating an hydroxide would only bring up an oxide, I believe. Moreover, caesium isn't considered the most reactive -element-. Maybe it is the
most reactive metal or alkali metal, but fluorine and other halogens are much more reactive.
┼┼┼Eddygp┼┼┼
[Edited on 28-4-2012 by Eddygp]
there may be bugs in gfind
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weiming1998
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What, now there are copycat bots now?
Spam reported.
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Eddygp
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The bond between Cs and oxygen might be quite complicated to break. After all, it will turn rapidly to cesium hydroxide in presence of water. The
problem is that many ions will attach to Cs instead of other metal, because of its properties. Therefore, the vacuum would be the best way, or the
only possible one with acceptable yield...
there may be bugs in gfind
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blogfast25
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No, it bloody well doesn't!
'Thermiting' alkali hydroxides with Mg at best leaves a dangerous mess (especially in the case of Cs) from which any metal formed cannot be recovered.
And in closed chamber, the hydride will form when the assembly cools down, at least assuming its formation is exothermic.
Cs and Rb are best prepared by reducing with Li or Ca. Vacuum is needed to:
a. eliminate oxygen
b. remove the Cs as vapour, thereby driving the equilibrium MCl(s) + Li(l) < === > M(g) + LiCl(s) to the right (Le Chatelier).
AH loves talking through his *rse. He's got previouses the length of the Golden Gate Bridge.
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blogfast25
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| Quote: Originally posted by Eddygp | | The bond between Cs and oxygen might be quite complicated to break. After all, it will turn rapidly to cesium hydroxide in presence of water. The
problem is that many ions will attach to Cs instead of other metal, because of its properties. Therefore, the vacuum would be the best way, or the
only possible one with acceptable yield... |
Oxides and hydroxides of alkali metals are ionic compounds par excellence. There are no bonds other than M<sup>+</sup> (M a
generic alkali metal) ions forming an ionic lattice M<sup>+</sup> A<sup>-</sup> (A<sup>-</sup> a generic anion)
with the anions. Much (but not all) of the Standard Heat of Formation of such compounds in the solid form is released when the lattice is formed, when
Coulombic attraction between the cation-anion ‘pairs’ is converted to lattice energy (heat).
In the case of the reduction of a Ceasium or Rubidium salt (usually the chloride) the reduction of the metal can be effectuated by means of the
equilibrium CsCl (s) + Li (l) < === > Cs(g) + LiCl (l) at quite high temperature. But even in those conditions the equilibrium point is still
too far to the left to yield much metal. To remediate that, high vacuum is pulled so the Cs vapour distils off. This, following Le Chatelier,
’pulls’ the equilibrium to the right and the yield of Cs metal is near quantitative.
[Edited on 28-4-2012 by blogfast25]
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AndersHoveland
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| Quote: Originally posted by blogfast25 |
'Thermiting' alkali hydroxides with Mg at best leaves a dangerous mess (especially in the case of Cs) from which any metal formed cannot be recovered.
|
If I remember correctly, one of the members on this forum isolated potassium from this method, but was unable to isolate sodium. It was speculated
that this was either because of potassium's higher volatility, or because the sodium had a higher affinity for hydrogen, and that NaH was forming
instead of sodium.
This is not likely to happen, as the decomposition temperature of CsH (160°C) is much lower than the boiling point of caesium (671°C). The hydrogen
may not have enough surface area to react with the caesium rapidly enough before it cools.
| Quote: Originally posted by blogfast25 |
Vacuum is needed to:
a. eliminate oxygen
b. remove the Cs as vapour, thereby driving the equilibrium to the right (Le Chatelier).
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As I previously mentioned, a vacuum would certainly help drive the equilibrium, but may not absolutely be required. There are other inert gases that
could potentially be used instead of a vacuum. Nitrogen would be suitable if metallic sodium was being used to distill caesium vapor out from a
caesium salt. Li, Mg, and Ca can all burn in N2 however, so if using these elements, it would necessitate using argon or a vacuum instead.
[Edited on 28-4-2012 by AndersHoveland]
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