Electrolysis of Anhydrous Sodium Hypochlorite

Considering liquid anhydrous sodium hypochlorite:

$$\ce{NaClO (l)}$$

Assuming the ions are free, What would be produced if this were electrolysed?

As I've found lots of information for it's hydrated pair (a.k.a. bleach). And while I know the half equation for sodium:

$$\ce{Na+ + e- -> Na}$$

I cannot find any half equation for the hypochlorite ion: $\ce{ClO-}$, apart from in acid, or even what would be the product (maybe $\ce{Cl2O}$ or $\ce{Cl2O2}$?)

Usually, an oxidation of hypochlorite will yield chlorate, $\ce{ClO3-}$. If we attempt to form a redox half-reaction out of that, we can only use $\ce{ClO-}$ as a charge balancing agent:
\begin{align}\ce{ClO- \phantom{\ce{+ 4 ClO-}} &-> ClO3- + 4e-}\tag{Ox1}\\ \ce{ClO- + 4 ClO- &-> ClO3- + 4 e-}\tag{Ox2}\end{align}
If we do this, we have four extraneous chlorine atoms and two extraneous oxygen atoms. Thus, it makes most sense to do the mass balance by adding $\ce{Cl2O}$:
$$\ce{ClO- + 4 ClO- -> ClO3- + 4 e- + 2 Cl2O}\tag{Ox3}$$