Get Lithium Metal From an Energizer Battery

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Introduction: Get Lithium Metal From an Energizer Battery

About: NurdRage is a dedicate group of science nerds trying to further amateur science with direct how-to instructions in video format. We saw what was already online and we thought "we could do better"... …

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.

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    100 Discussions

    0
    carlos1984
    carlos1984

    Reply 3 years ago

    well that answers my question but the two batteries I tried , the lithium had no reaction at all with water, this obviously due to the batteries being completely dead.

    0
    carlos1984
    carlos1984

    3 years ago

    hi guys , I have tried this using an old samsung lithium battery and an 18650 lithium battery, the problem i had was that although I did extract the metal when I tested a small peice in water to see if it was reactive nothing happened. Is this because the cells were completely dead? Should I only attempt to get viable lithium from fresh batteries?

    0
    history323
    history323

    10 years ago on Introduction

    Thanks for the instrucable i have an element collection and could not find cheap lithium (my budget is fairly low) for the life of me!
    Also thanks for all your effort in helping aspiring chemists like me to learn all about chemistry!!!
     Also have you ever read/heard of the Golden book of Chemistry? It has lots of cool experiments to try in it heres a link to the pdf since its banned from the library :(  http://chemistry.about.com/b/2008/08/05/banned-book-the-golden-book-of-chemistry-experiments.htm
    Thanks again!

    0
    RogerD5
    RogerD5

    Reply 4 years ago

    OK, good. Try adding a cube of Astatine and Francium XDXD

    0
    RogerD5
    RogerD5

    Reply 4 years ago

    OK, good. Try adding a cube of Astatine and Francium XDXD

    0
    Breygon
    Breygon

    Reply 4 years ago

    Thanks for the book link. It's great! ?

    0
    Alec Eiffel
    Alec Eiffel

    11 years ago on Introduction

    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?

    0
    NurdRage
    NurdRage

    Reply 11 years ago on Introduction

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

    0
    lobo_pal
    lobo_pal

    Reply 11 years ago on Introduction

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

    0
    NurdRage
    NurdRage

    Reply 11 years ago on Introduction

    H3 doesn't exist under normal conditions.

    0
    lobo_pal
    lobo_pal

    Reply 11 years ago on Introduction

    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?

    0
    NurdRage
    NurdRage

    Reply 11 years ago on Introduction

    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.

    0
    lobo_pal
    lobo_pal

    Reply 11 years ago on Introduction

    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.

    0
    NurdRage
    NurdRage

    Reply 11 years ago on Introduction

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

    0
    lobo_pal
    lobo_pal

    Reply 11 years ago on Introduction

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