khourygeo77
Hazard to Others
Posts: 114
Registered: 2-1-2017
Member Is Offline
Mood: No Mood
|
|
How to get metal/metal oxides?
So I was trying to make metal/mineral oxides by turning them into salts that supposedly decompose at common kitchen fire. I worked on magnesium for
example, and got its acetate that decomposes at 350 deg. I heated the acetate on that temperature but instead of decomposing and turning into a white
magnesium oxide, it blackened then eventually turned a little grey without becoming pure. There is absolutely no contamination in the process. I have
tried this on zinc acetate, and same thing happened.
Any idea on how to get the real white oxides of zinc or magnesium for example? Unfortunately, I cant get the different kinds of torches here that many
would use in other countries, the ones that would quickly oxidize anything with the high heat
Thanks
|
|
|
Rhodanide
Hazard to Others
Posts: 348
Registered: 23-7-2015
Location: Ｔｈｅ ８０ｓ
Member Is Offline
Mood: That retro aesthetic
|
|
Quote: Originally posted by khourygeo77  | So I was trying to make metal/mineral oxides by turning them into salts that supposedly decompose at common kitchen fire. I worked on magnesium for
example, and got its acetate that decomposes at 350 deg. I heated the acetate on that temperature but instead of decomposing and turning into a white
magnesium oxide, it blackened then eventually turned a little grey without becoming pure. There is absolutely no contamination in the process. I have
tried this on zinc acetate, and same thing happened.
Any idea on how to get the real white oxides of zinc or magnesium for example? Unfortunately, I cant get the different kinds of torches here that many
would use in other countries, the ones that would quickly oxidize anything with the high heat
Thanks |
Good question!
One way is to just burn them in metal form.
Both Zinc and Magnesium metal can be burned by a normal methane burner, you just need to be careful, and have good ventilation so as not to get MFF
(Metal Fume Fever, it's terrible.) from the dusty zinc oxide.
If you only have access to the compounds, then yes- acetates are a good place to start.
However, this is not the best way, for MgO that is. That would go to the hydroxide decomposition method. Combine concentrated solutions of NaOH or
any Alkali OH salt and Magnesium Sulfate, also known as Epsom Salt.
You'll get a gel, most likely. Filter the solution and keep the gel. Dry this however you like. Note this also works just fine for the Carbonate, just
substitute the OH for Sodium Carbonate (DON'T use NaHCO3, I've found it to be quite unreliable. Remember- if you only have NaHCO3 then just heat it up
in a pan for a long time, or until no more gas comes off it. I usually do this for 30-45 minutes) Just heat either the MgCO3 or Mg(OH)2 strongly. I'm
not sure how long, so someone else can pitch in hopefully and give their two cents on how long they heated it. As for the Zinc, I can only assume that
given their similarity, the same process is likely viable for Zinc as well. Don't quote me on that, for I'm not completely sure.
EDIT: It is also likely that it was something wrong with whatever you used to contain the material whilst you heated it.
[Edited on 12-4-2017 by Tetra]
|
|
|
khourygeo77
Hazard to Others
Posts: 114
Registered: 2-1-2017
Member Is Offline
Mood: No Mood
|
|
| Quote: Originally posted by Tetra | | Quote: Originally posted by khourygeo77 | So I was trying to make metal/mineral oxides by turning them into salts that supposedly decompose at common kitchen fire. I worked on magnesium for
example, and got its acetate that decomposes at 350 deg. I heated the acetate on that temperature but instead of decomposing and turning into a white
magnesium oxide, it blackened then eventually turned a little grey without becoming pure. There is absolutely no contamination in the process. I have
tried this on zinc acetate, and same thing happened.
Any idea on how to get the real white oxides of zinc or magnesium for example? Unfortunately, I cant get the different kinds of torches here that many
would use in other countries, the ones that would quickly oxidize anything with the high heat
Thanks |
Good question!
One way is to just burn them in metal form.
Both Zinc and Magnesium metal can be burned by a normal methane burner, you just need to be careful, and have good ventilation so as not to get MFF
(Metal Fume Fever, it's terrible.) from the dusty zinc oxide.
If you only have access to the compounds, then yes- acetates are a good place to start.
However, this is not the best way, for MgO that is. That would go to the hydroxide decomposition method. Combine concentrated solutions of NaOH or
any Alkali OH salt and Magnesium Sulfate, also known as Epsom Salt.
You'll get a gel, most likely. Filter the solution and keep the gel. Dry this however you like. Note this also works just fine for the Carbonate, just
substitute the OH for Sodium Carbonate (DON'T use NaHCO3, I've found it to be quite unreliable. Remember- if you only have NaHCO3 then just heat it up
in a pan for a long time, or until no more gas comes off it. I usually do this for 30-45 minutes) Just heat either the MgCO3 or Mg(OH)2 strongly. I'm
not sure how long, so someone else can pitch in hopefully and give their two cents on how long they heated it. As for the Zinc, I can only assume that
given their similarity, the same process is likely viable for Zinc as well. Don't quote me on that, for I'm not completely sure.
EDIT: It is also likely that it was something wrong with whatever you used to contain the material whilst you heated it.
[Edited on 12-4-2017 by Tetra] |
You were right. I reacted with ammonia, and got magnesium hydroxide, then upon heat, decomposition into oxide was very easy.
Do you think this may be the case for most metals and minerals?
|
|
|
Fulmen
International Hazard
Posts: 1725
Registered: 24-9-2005
Member Is Online
Mood: Bored
|
|
Many useful or otherwise interesting metals can be precipitated as hydroxides or carbonates, both can easily be converted into the oxide by heating.
Be aware that ammonia can dissolve many metals as ammonia complexes, in these instances you can use sodium hydroxide.
We're not banging rocks together here. We know how to put a man back together.
|
|
|
yobbo II
National Hazard
Posts: 764
Registered: 28-3-2016
Member Is Offline
Mood: No Mood
|
|
http://www.sciencemadness.org/talk/viewthread.php?tid=71009
If you can get access to a furnace and steam you can make metal oxides easily. Just add steam to the furnace and place the metals inside in non
contaminating containers (alumina?)
I have tries this with iron, copper, titanium some stainless steels (don't know composition).
Nickle seems to hold up well (no conversion).
I presume the copper and Ti were converted to oxides. What else could the crispy brittle stuff they were converted into, be?
Yob
|
|
|
|
![[*]](images/xpblue/default_icon.gif){kind=icon}
