Aluminum

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Legality: DEA Listed Chemicals

Production of this substance may be illegal in some jurisdictions under certain circumstances.

21CFR1310.02 a & b

In 1995/6, two lists were created "List I" and "List II", for which commercial manufacturers and distributors must register, and for which possession with the intent to manufacture illegal substances (such as methamphetamine, ecstasy, etc) is illegal. On these a few dozen "precursor" compounds commonly used in the manufacture of illegal drugs. <ref>{{

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Bottom line: Do not produce this chemical without checking to make sure that you may do so legally.

 

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Legality: CWC Schedule 3

CONVENTION ON THE PROHIBITION OF THE DEVELOPMENT, PRODUCTION, STOCKPILING AND USE OF CHEMICAL WEAPONS AND ON THEIR DESTRUCTION
ANNEX ON CHEMICALS
A. GUIDELINES FOR SCHEDULES OF CHEMICALS
Guidelines for Schedule 3
The following criteria shall be taken into account in considering whether a toxic chemical or precursor, not listed in other Schedules, should be included in Schedule 3:
(a) It has been produced, stockpiled or used as a chemical weapon;
(b) It poses otherwise a risk to the object and purpose of this Convention because it possesses such lethal or incapacitating toxicity as well as other properties that might enable it to be used as a chemical weapon;
(c) It poses a risk to the object and purpose of this Convention by virtue of its importance in the production of one or more chemicals listed in Schedule 1 or Schedule 2, part B;
(d) It may be produced in large commercial quantities for purposes not prohibited under this Convention.

Production of this substance may be illegal in some jurisdictions under certain circumstances. Bottom line: Do not produce this chemical without checking to make sure that you may do so legally.

 

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Legality: Controlled Substance

USC Title 21<ref>21 USC §812{{
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This substance is currently {{#if
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Production, Possession, or distribution of this substance without permission or defined legal justification may be illegal.

Bottom line: Do not produce this substance without checking to make sure that you may do so legally.

 

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NFPA 704
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Uses

Primary

  • Structural material
  • Aluminothermic reduction of other metals

Secondary

  • Thermite
  • Alloyed with barium ({{#Chem: BaAl4}}) for gas "getter"

Natural Occurrence

Hazards

Character

Production

While aluminum oxide is plentiful on earth, the aluminum-oxygen bonds are extremely strong, thus it is very difficult to reduce to pure aluminum by simple means.

Synthesis

AKA Hall-Heroult process

Direct electrolysis of aluminum oxide is impractical because the melting temperature of aluminum oxide (2072°C) is beyond the range of normal furnaces. Sodium aluminum hexafluoride, however, has a melting point of 1012°C and aluminum oxide will dissolve in molten cryolite. The mixture has a combined melting point of about 1000°C. Electrolysis then cleaves the aluminum from the oxygen. The oxygen combines with the graphite of the anode producing carbon dioxide which exits the system as a gas, and leaves the molten cryolite to absorb additional bauxite.

  1. Melt a fluorinating agent (below) at 1012°C
  2. Repeat
    1. Saturate with pure aluminum oxide
    2. Electrolyze at 3-5V using a carbon electrodes producing liquid aluminum at the cathode and carbon dioxide at the anode:
      {{#Chem: 2Al2O3 + 3C { AlF3 = 1012°C 3-5V } 4Al + 3CO2 }}
    3. Tap off the aluminum from the bottom of the cell (it is denser than the fluoride mixture)
  3. Until all the aluminum oxide is converted

Production of fluorination agents

sodium aluminum hexafluoride

This material, mineralized, is called cryolite. It does occur naturally, but is somewhat rare. It has a melting point near 950°C. It is mainly produced by combining sodium hydroxide and aluminum oxide

{{#Chem: 6 NaOH + Al2O3 + 12 HF → 2 Na3AlF6 + 9 H2O }}

aluminum fluoride

This material, mineralized, is called rosenbergite has a melting point near 1300°C.

theory

Combining hydrofluoric acid and aluminum oxide will produce aluminum trifluoride:

{{#Chem: 2Al2O3 + 6HF = 2AlF3 + 3H2O}}

In practice, it is much easier to do a "one pot" mixture of fluoride minerals, sulfuric acid, and aluminum oxide

practice

We start with with sulfuric acid and fluorine-containing silica minerals, producing hexafluorosilic acid:

Fluorine-bearing minerals and sulfuric acid, generating {{#Chem: F2 or HF}} which combine with silicon dioxide to give rise to {{#Chem: H2SiF6}}
Fluorite: {{#Chem: CaF2 + H2SO4 = CaSO4 + 2HF }}; {{#Chem: HF + SiO2 = H6SiO2F6 }}
Fluorapatite: {{#Chem: Ca5(PO4)3F + 5H2SO4 = 5CaSO4 + 3H3PO4 + HF }}; {{#Chem: HF + SiO2 = H6SiO2F6 }}
Hexafluorosilic acid readily converts to aluminum fluoride in the presence of aluminum oxide
{{#Chem: H2SiF6 + Al2O3 → 2 AlF3 + SiO2 + H2O }}

Purification

Testing

Storage

Disposal

See Also

References

<references/>

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