# In a battery, what happens to LiCoO2 when the lithium leaves? It becomes CoO2?

What chemical compound exists at the cathode of a lithium-ion battery when the lithium is not there?

The cathode is usually described as $$\ce{LiCoO2}$$, so does it become $$\ce{CoO2}$$?

$$\ce{CoO2}$$ puts cobalt in an oxidation state of +4, which is possible but rare and unstable. I think $$\ce{CoO2}$$ doesn't even have a Wikipedia page.

• CoO2 exists: cobalt.atomistry.com/cobalt_dioxide.html Jun 2 '20 at 16:00
• Not an expert on this, but I think this is one of the reasons you don't ever want to overcharge a LiCoO2 battery... Jun 2 '20 at 16:12
• It is quite complicated. See sciencedirect.com/science/article/pii/S0364591613000035 for some of the thermodynamics and crystal structures. Jun 2 '20 at 20:31
• @JonCuster That statement is a bit over the top, as is the paper you link as a first read. The general principles of the Li ion battery have been textbook knowledge for quite a few years now.
– Karl
Jun 2 '20 at 20:36
• @Karl - but you did a good job at it! Jun 2 '20 at 23:47

## 1 Answer

The general textbook formula for the Li ion battery is

$$\ce{Li_{1-a}Ni_{1-x-y}Mn_{x}Co_{y}O2}$$

, and the simplest/earliest type has $$y=1$$, i.e. cobalt-only. These "mixed (lithium transition metal) oxides" have a layered structure (see e.g. wikipedia), where you can relatively easily electrochemically remove (and later reinsert) a part $$a$$ of the Li atoms, without destroying the whole structure. You cannot increase $$a$$ to much more than 0.1 - 0.3 or so, depending on the exact formulation/grain size/quality/temperature/etc., before the structure does break down.

Even the "uncharged" $$a=0$$ Li-cobalt(III) oxide gives off oxygen (!) if heated above 180°C. (It is produced by tempering at ~800°C in a pure oxygen atmosphere.) With $$a>0$$, this happens earlier already, and basically always leads to a runaway destruction of your whole battery setup. With higher contents of Ni and Mn, this danger becomes less pronounced. I´m not sure the Co-only variant was ever commercialised. (?)

Simply speaking, a cobalt-rich battery blows up when overcharged, and in ones with more nickel and manganese the layered structure still breaks down, and you get somewhat stable Ni/Mn(III/IV) species (and still quite a lot of overheating/general destruction). In any case this happens long, long before you reach the ideal $$\ce{CoO2}$$ (or generally $$\ce{MO2}$$) stochiometry.

If you look closely (e.g. via XRD) at the crystal structure during charging, you seemingly find that there are a number of intermediate deformed structures, and even more mixed/disordered states in between. And that of course becomes even more complicated (or washed out) with a (more or less) random arrangement of different transition metals in the structure, which will depend also on the specific synthesis route.