Get Lithium Metal from an Energizer Battery

video Get Lithium Metal from an Energizer Battery

We show you how to get Lithium Metal from an Energizer Ultimate Lithium battery.

There are a great many types of lithium batteries and the particular chemistry of interest is "lithium iron disulfide" batteries which contain pure lithium metal and less toxic electrolyte than other batteries. Lithium ion batteries do not contain lithium metal (just lithium ions) and other pure metal lithium batteries often contain incredibly toxic electrolyte that make them too dangerous for the average person to safely open.

It just so happens that the popular Energizer Ultimate Lithium batteries are based on lithium iron disulfide chemistry making them the ideal choice for the home chemist to obtain lithium.

The rolled lithium core is protected by a mini-fortress of steel that you have to cut through. The danger is accidentally shorting the battery and causing the internal materials to fuse. The video shows you what you have to go through and what to expect when opening an energizer ultimate lithium battery.

Lithium is a powerful chemical reducing agent, it's also used for lithiation reactions in organic synthesis, batteries, unusual pyrotechnic formulations and some types of nuclear technologies.

It's in the same category as the alkali metals which include the ever so popular sodium, potassium and cesium.

if you like this video, please visit our channel at http://www.youtube.com/NurdRage

poikilotherm says: Apr 21, 2013. 5:45 PM

So, I tried this (three times.) The first time, it worked perfectly. The second time, it also worked perfectly. The third time, the battery started burning - not only that, but after I threw it away from me, it took off, shot around the room I was in, caused a large amount of general panic, and what's more, scared the daylights out of some guests. Everyone was no worse for the occasion, fortunately, though.

poikilotherm in reply to poikilothermApr 22, 2013. 5:17 AM

Oh yes - the battery was a laptop battery, not an energizer one...was that an incredibly stupid thing to do or what?
Anyways, I think I found out what happened. The "incredibly toxic electrolyte" was ignited by the sparks produced by the battery terminals touching...
Regardless, my battery-opening days are over.

YoungPyro19 says: Jun 4, 2010. 7:49 PM

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NurdRage (author) in reply to YoungPyro19Jun 4, 2010. 7:53 PM

I could... but why would you want it?

YoungPyro19 in reply to NurdRageJun 5, 2010. 6:11 PM

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NurdRage (author) in reply to YoungPyro19Jun 5, 2010. 6:33 PM

the pure form is dangerously unstable. For most uses, salt forms are preferable and much safer to handle. But to make a video on a particular salt form i need to know what you're going to use it for so i know what salt would be best.

YoungPyro19 in reply to NurdRageJun 5, 2010. 6:50 PM

(removed by author or community request)

OCPik4chu in reply to YoungPyro19Oct 8, 2012. 12:35 PM

@younPyro19: From the ATF: Binary explosives are pre-packaged products consisting of two separate components—usually an oxidizer like ammoni¬um nitrate and a fuel such as aluminum or another metal. These components typically are not listed separately on the List of Explosive Materials and do not meet the definition of "Explosives" in 27 CFR 555.11. Therefore, ATF does not regulate the sale and distribution of these component chemicals, even when sold together in binary "kits." However, when the binary components are combined, the resulting mixture is an explosive material subject to the regulatory requirements found in 27 CFR, Part 555

Please learn before you hurt yourself, or worse, someone else. Explosives are not toys.

finniano says: Apr 16, 2011. 4:09 PM

can you do the same thing with energizer lithium photo batteries? it is 3 volts. it doesnt say that its ultimate lithium, but the packaging is blue and silver just like the ultimate lithium ones.

ginbot86 in reply to finnianoNov 21, 2011. 8:52 PM

Yes, Energizer lithium photo batteries will work as they are lithium-manganese dioxide batteries. The lithium might be more difficult to obtain cleanly, but don't quote me on it as I haven't taken one of those apart.

docm8trx says: Mar 20, 2011. 5:12 PM

dont tell that kid how to make anhydrous....if AFTER reading this particular ible, he wants to make the other, he probably wants to make a certain substance that will remove the enamel from his teeth. also, its easier to remove the strips if you first soak the cells in acetone then pull off the pos terminal withdiagonal cutters...beeeeeeeeeeeeeeee carrrrrrrrrrefulllllllllll.....

furlow says: Mar 20, 2011. 2:28 PM

You have increase the sales of lithium AA batteries I think all battery companies will be happy! Since most products now include their own batteries.

kiko2704 says: Mar 20, 2011. 12:11 PM

NurdRage can I use dead/used batteries?

omnibot says: Mar 19, 2011. 2:53 PM

Oooohhh, I have got to get me some of those batteries!!

bignerd says: Apr 12, 2010. 4:13 PM

is there an easier way?
also, when i was doing it and the pliers hit the edge it makes a spark
does that mean its shorted out?

hintss in reply to bignerdDec 21, 2010. 12:01 AM

yes.

for a short time, probably not bad, but yes...

Saturn V says: Jun 21, 2010. 1:40 PM

Why would you want lithium? What practical uses does it have?

hintss in reply to Saturn VDec 20, 2010. 11:59 PM

it burns on contact with air. some type of igniter that lights on impact?

funke75 says: Oct 23, 2010. 1:57 PM

I remember from highschool chemistry that some metals can be stored in mineral oil to prevent there oxidation. I believe my teacher had sodium stored this way because of its volitile reaction. would this be a viable way to store the lithium? and if so, would we be able to save the lithium from oxidizing even more if we did your unwraping process under mineral oil so that it never even touchs the air?

hintss in reply to funke75Dec 20, 2010. 11:55 PM

I believe if you buy lithium, it is shipped that way, so yes.

jessmt says: Dec 14, 2010. 11:55 PM

NurdRage... Please tell us about yourself; or is that forbidden? Why the voice disguise? Afriad of all the teen guys here hitting on you, or up to no good?
Anyway, I like your videos... very interesting, here's a pointer for your Nitric Acid Mfg:
Sulfuric Acid (drain opener), Potassium or sodium nitrate like in the last way you show but with much better results if you pull a vacuum during distillation. Less decomp and it comes out crystal clear.
I bet all the Al-Qaeda wanna-be's love you! Oh no... the FBI!
Have fun!

Oh! By the way... What is the electrolyte on the CR123 (3v) lithium batteries? They reek of ether so I assume that is one of the things in there.

redlizard5 says: Sep 25, 2010. 8:23 PM

Could you put the lithium into a zip lock bag for storage

Ivraine says: Aug 30, 2010. 5:46 AM

I read somewhere that pyrite is used to create sulfur dioxide, which is used to make sulfuric acid. Can the iron disulphide in the batteries be used like pyrite? Or am I just confusing two separate chemicals?

AndyGadget says: Aug 29, 2010. 10:29 AM

What is the chemistry of a discharged Energizer Lithium battery - Would I be right in thinking metallic iron and lithium disulphide?
Does this have any interesting properties?

.Unknown. says: Jul 21, 2010. 5:48 AM

I did this, right, but on my last go, after pulling out the core, I started to unravel it, and it suddenly burst in to red flames....wth?

thorpenny says: Jul 9, 2010. 3:37 PM

what is the chance that this metal (powdered) would act as a good fuel in a flash powder composition?

insolest says: Jun 2, 2010. 10:48 AM

Another way to remove the shell of the battery is with a hand held pipe cutter. I used the type for cutting copper pipe. First remove the label. Second, cut around the indent at the top of the battery to simultaneously remove the inner cap, spacer, and release valve from the main portion of the battery. Third, I cut the battery's casing with the pipe cutter near the middle. This process bends some of the metal casing into the core of the battery, but if the metal casing is cut gently, then no real damage occurs. Fourth, the core must be extracted. This requires some force (due to the bent edge where the pipe cutter was used). Then follow NurdRage's instructions. Thank you NurdRage for the idea!

Darter76 says: May 24, 2010. 5:18 PM

Is there any way to un-ionize the lithium metal from a lithium ion battery? If there is i would like to know because i have about 30 sitting around collecting dust and would like to do anything with them.

NurdRage (author) in reply to Darter76May 24, 2010. 6:10 PM

technically yeah.... but it's so complicated, expensive, and requires specialized equipment that it's not worth doing for the home experimenter.

At least that's from the methods i know currently, if i ever find a way to do it i'll post an instructable.

robotman3 says: May 1, 2010. 12:06 PM

im so doing that.

Alec Eiffel says: Jun 19, 2009. 1:04 PM

I tried this instructable and it worked really well. It's a lot harder than it looks . I was wondering why does the metal fizz when you put into water?

NurdRage (author) in reply to Alec EiffelJun 19, 2009. 1:06 PM

It's like sodium, it reacts with water to produce hydrogen

lobo_pal in reply to NurdRageJun 19, 2009. 11:26 PM

If I recall correctly, sometimes it will form H3 instead of H2 and cause an even more violent reaction.

NurdRage (author) in reply to lobo_palJun 19, 2009. 11:29 PM

H3 doesn't exist under normal conditions.

lobo_pal in reply to NurdRageJun 20, 2009. 8:34 AM

In Chem AP we watched a sodium reaction, and he explained the sometimes the Hydrogen rush to meet and three of them hit at once causing H3 which then reacts again to make two H2 with another Hydrogen. Right?

NurdRage (author) in reply to lobo_palJun 20, 2009. 9:29 AM

O_o whoa... the sheer idiocy.... Would explain why he's a teacher and not an actual scientist. Trihydrogen cations are present in extreme gaseous conditions like gas plasma discharges and interstellar clouds. But in an aqueous medium, anything powerful enough to protonate hydrogen gas would already be reactive with other things like the water or whatever else happens to be nearby long before it can produce trihyrogen cations.

lobo_pal in reply to NurdRageJun 20, 2009. 2:00 PM

I may not be repeating it right, but he said that for some reason that escapes me that some reactions are more violent than others.

NurdRage (author) in reply to lobo_palJun 20, 2009. 3:10 PM

there are plenty of reasons for alkali metal reations to be violent. maybe that's what he meant but didn't properly explain why.

lobo_pal in reply to NurdRageJun 20, 2009. 5:14 PM

Well, I'm starting my major in Chem E in the fall, so I'm trying to study up on stuff.

ARVash in reply to lobo_palJan 31, 2010. 12:02 PM

Perhaps our Lobo misheard and he was instead saying Deuterium and Tritium aka ^2H and ^3H, Hydrogen Isotopes.