symboom - 2-7-2017 at 11:30
I mean why not if lithium and ceasium can be made in an ameture setting.it seems the common method is actually distillation except for lithium and
sodium from lithium chloride and sodium hydroxide
Boiling point 2,426°F
https://m.youtube.com/watch?v=eytU_eY-dfk
Sodium can be made
Boiling point 1,621°F
https://m.youtube.com/watch?v=jCrFFVVcPUI
Potassium metal
Boiling point 1,398°F
https://m.youtube.com/watch?v=PkTaz3UEThY
Rubidium metal
Boiling point 1,270°F
Ceasium metal
Boiling point 1,240°F
https://m.youtube.com/watch?v=rSJGwnERIVU
Next up the alkaline earth metals
Two options exist either electrolysis or single displacement
Beryllium metal
Boiling point 5,378°F
Ok this one I dont think is distilled like magnesium is and just rinsed with water to remove salts from the metal
Pure beryllium may be obtained by electrolysis of molten BeCl2 containing some NaCl. The salt is added since the molten BeCl2 conducts very poorly.
Another method involves the reduction of beryllium fluoride with magnesium at 1300°C.
BeF2 + Mg → MgF2 + Be
Magnesium metal
Boiling point 1,996°F
>Silicothermic Pidgeon process (the reduction of the oxide at high temperatures with silicon, often provided by a ferrosilicon alloy in which the
iron is but a spectator in the reactions) to obtain the metal.
The process can also be carried out with carbon at 2300 °C
>The Dow process uses the electrolysis of molten fused magnesium chloride
A new process, solid oxide membrane technology, involves the electrolytic reduction of MgO. The electrolyte is Yttria-stabilized zirconia (YSZ). A
layer of graphite borders the liquid metal anode. silver is used as the liquid metal anode
Calcium metal isolation from calcium chloride attempt
Boiling point 2,703°F
https://m.youtube.com/watch?v=KGMKlsG9_1o
https://m.youtube.com/watch?v=n4w5hp_dC3w
The problem with making calcium through molten salt electrolysis is it desolves in calcium chloride im not sure how industry prevents this from
happening.
calcium metal is readily available commercially and there is no need to make it in the laboratory. Commercially it can be made by the electrolysis of
molten calcium chloride, CaCl2.
Alternatively, and on small scale, calcium can be made through the reduction of CaO with aluminium or of CaCl2 with sodium metal
6CaO + 2Al→ 3Ca + Ca3Al2O6
CaCl2 + 2Na→ Ca + 2NaCl
Calcium production with lithium chloride
Calcium oxide is reduced in situ by the electrolysis of lithium chloride forming lithium metal which then reduces the calcium oxide
Or a mixture of lithium chloride and calcium chloride
Another possable idea would be to make an alloy with the cathode calcium being absorbed in a metal such as mercury or mercury repacement just as a
lead sodium alloy exists
Strontium metal
Boiling point 2,519°F
strontium metal is available commercially and there is no need to make it in the laboratory. Commercially it is made on small scale by the
electrolysis of molten strontium chloride, SrCl2.
Strontium metal can also be islated from the reduction of strontium oxide, SrO, with aluminium.
6SrO + 2Al → 3Sr + Sr3Al2O6
Barium metal
Boiling point 3,447°F
barium metal is available commercially and there is normally no need to make it in the laboratory. Commercially, it is made on small scale by the
electrolysis of molten barium chloride, BaCl2.
Barium metal can also be islated from the reduction of barium oxide, BaO, with aluminium.
6BaO + 2Al→ 3Ba + Ba3Al2O6
Summary
Various reduction reactions
Phttps://m.youtube.com/watch?v=GRSlGt26uUA
Maybe dioxine may help in desolving the salt and leaving the metal behind such as with sodium production
It seems that distillation is the best option for isolating the metal due to the difficulty single displacement clearly being more feasible in
reactive metals such as isolation of ceasium the alkaline earth metals being obtained in a similar nature.
Since sodium has been done by side production of potassium
Boiling point 1,621°F
And magnesium at Boiling point 1,996°F and calcium Boiling point 2,703°F unless dioxane could be used as it is used in sodium production of course
maybe not the metals can not coglomerate at such a low temperature the melting of the metal under powdered graphite could be used as it is used to
prevent magnesium from catching fire in making magalium (magnesium aluminum alloy)
the only other possible synthysis of alkaline earth metals would be a polar aprotic solution electrolysis in proplene carbonate
______________________________________________________________
Side notes silicon production
Silicon is readily available through the treatment of silica, SiO2, with pure graphite (as coke) in an electric furnace.
SiO2 + 2C → Si + 2CO
Under these conditions, silicon carbide, SiC, can form. However, provided the amount of SiO2 is kept high, silicon carbide may be eliminated.
Also aluminum reduction aka silicon thermite can be used with silicon dioxide
But a booster is needed sulfur is used but this will interfere with
Magnesium production as silicon sulfide
The material is formed by heating silicon and sulfur or by the exchange reaction between SiO2 and Al2S3. So some silicon will be inevitably lost.
_________________________________
Other methods
FFC Cambridge process
https://m.youtube.com/watch?v=97dfa1GoF7w
In which a metal oxide is reduced by electrolysis in molten calcium chloride taking advantage of the fact that calcium metal desolves in calcium
chloride
Considering
Magnesium strontium and barium metal being formed from the metal oxide effectively being reduced by calcium metal
By applying a metal hydroxide and driving off the water the oxide forms and adheres to the electrode thereby making a carbon alkaline metal oxide
cathode
And even aluminum maybe isolated.
Aluminum metal by electrolysis
https://m.youtube.com/watch?v=qkyPvhapxQs
[Edited on 3-7-2017 by symboom]
[Edited on 3-7-2017 by symboom]
[Edited on 3-7-2017 by symboom]
metalresearcher - 19-9-2024 at 09:01
Seven years later I stumbled upon this topic.
Very interesting.
Cody's Lab making aluminum is just a hobby version of the commercial Bayer process followed by the Hall-Héroult process.
And making Calcium with Al powder and CaSO4 ?
I tried this once for just a bright fireworks, but maybe performing this in a confined and enclosed space (e.g. a paint can with a lid on it) might
prevent oxidation.