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#Post#: 1604--------------------------------------------------
Properties of Elemental Sodium
DIR By: Shiva
Date: December 17, 2012, 2:05 am
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HTML http://www.youtube.com/watch?v=2bIUMBhh3K8
#Post#: 1609--------------------------------------------------
Re: Properties of Elemental Sodium
DIR By: Michel
Date: December 17, 2012, 7:19 pm
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Interesting...any chance we can see a 'preparation of elemental
sodium' video? :D
#Post#: 1617--------------------------------------------------
Re: Properties of Elemental Sodium
DIR By: Shiva
Date: December 18, 2012, 12:59 am
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Sure will do when I've proper equipments for it :-) Also, I
would love to extract Strontium :-)
Shiva
#Post#: 1618--------------------------------------------------
Re: Properties of Elemental Sodium
DIR By: Michel
Date: December 18, 2012, 1:04 am
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--- Quote from: Shiva link ---
>
> Sure will do when I've proper equipments for it :-) Also, I
would love to extract Strontium :-)
>
> Shiva
>
--- End Quote ---
What processes are involved? Electrolysis of molten NaOH?
#Post#: 1619--------------------------------------------------
Re: Properties of Elemental Sodium
DIR By: Shiva
Date: December 18, 2012, 1:20 am
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Yeah, Sodium can be extracted via two well known routes. One by
electrolyzing Sodium hydroxide (Castner's process), there we
need Iron as cathode and Nickel as anode which resists
oxidation. Another route is electrolyzing molten Sodium chloride
(Down's process). Industries are currently extracting Sodium by
Down's route. Here we are using Iron as cathode and carbon as
anode. As pure Sodium chloride melts only around 1070k, we can
add little potassium chloride and fluoride to lower the melting
point to 870k.
Shiva
#Post#: 1620--------------------------------------------------
Re: Properties of Elemental Sodium
DIR By: Michel
Date: December 18, 2012, 2:59 am
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--- Quote from: Shiva link ---
>
> Yeah, Sodium can be extracted via two well known routes. One
by electrolyzing Sodium hydroxide (Castner's process), there we
need Iron as cathode and Nickel as anode which resists
oxidation. Another route is electrolyzing molten Sodium chloride
(Down's process). Industries are currently extracting Sodium by
Down's route. Here we are using Iron as cathode and carbon as
anode. As pure Sodium chloride melts only around 1070k, we can
add little potassium chloride and fluoride to lower the melting
point to 870k.
>
> Shiva
>
--- End Quote ---
I think for home preparation, using NaOH is better. You can melt
NaOH with a blowtorch around 400'C
#Post#: 1623--------------------------------------------------
Re: Properties of Elemental Sodium
DIR By: Shiva
Date: December 18, 2012, 5:37 am
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Yes, it is quite easy to melt Sodium hydroxide. But, the set up
is bit expensive. We need Nickel anode in this process which is
used to prevent oxidation in this reaction. Also, it does not
react with alkalis even in the fused state. Actually, extracting
Potassium is more easier than extracting Sodium at home.
However, if you got a perfect set up, You can extract Sodium
quite easily and as much as you want. Remember the Nurdrage
video that I showed you (Extraction of Potassium)? If we find
such a method for extracting Sodium (without electrolysis), I
would make some daily lol :-)
Shiva
#Post#: 1627--------------------------------------------------
Re: Properties of Elemental Sodium
DIR By: Michel
Date: December 19, 2012, 7:14 am
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Isn't it possible to use graphite instead of Nickel?
--- Quote from: Shiva link ---
>
> If we find such a method for extracting Sodium (without
electrolysis), I would make some daily lol :-)
>
> Shiva
>
--- End Quote ---
Hahaha
#Post#: 1628--------------------------------------------------
Re: Properties of Elemental Sodium
DIR By: Shiva
Date: December 19, 2012, 8:25 am
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Nope, we can't as graphite readily reacts with molten alkali
metals and produce lamellar compounds. Here alkali metals
invaded through each layer and bonded to each carbon atom (sp2
hybrid bonds and the fourth electron forms pi bond). Because of
the delocalized nature of pi electrons, graphite conducts
electricity. Some of these lamellar compounds have higher
electrical conductivity than Graphite itself and some are non
conducting. But, the reason why we should not use graphite as an
anode is, the lamellar alkali compounds (alkali graphitides) are
very reactive, pyrophoric and react violently with water.
Shiva
#Post#: 1630--------------------------------------------------
Re: Properties of Elemental Sodium
DIR By: Michel
Date: December 19, 2012, 12:07 pm
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--- Quote from: Shiva link ---
>
> Nope, we can't as graphite readily reacts with molten alkali
metals and produce lamellar compounds. Here alkali metals
invaded through each layer and bonded to each carbon atom (sp2
hybrid bonds and the fourth electron forms pi bond). Because of
the delocalized nature of pi electrons, graphite conducts
electricity. Some of these lamellar compounds have higher
electrical conductivity than Graphite itself and some are non
conducting. But, the reason why we should not use graphite as an
anode is, the lamellar alkali compounds (alkali graphitides) are
very reactive, pyrophoric and react violently with water.
>
> Shiva
>
--- End Quote ---
Thanks! Added to my knowledge :D
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