= Solution
On discharge, lithium is oxidized at the negative electrode:
$$
\boxed{\mathrm{Li(s)\longrightarrow Li^++e^-}}.
$$
At the positive electrode, carbon monofluoride is reduced:
$$
\boxed{\mathrm{CF(s)+Li^++e^-\longrightarrow C(s)+LiF(s)}}.
$$
The net conversion reaction is therefore
$$
\boxed{\mathrm{Li(s)+CF(s)\longrightarrow C(s)+LiF(s)}}.
$$
For general $\mathrm{CF}_x$, replace Li, lithium ions, electrons and LiF by $x$ equivalents per carbon atom. The carbon–fluorine bonds are consumed in forming different solid phases, rather than lithium simply intercalating reversibly into an unchanged host.
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