Would cerium(III) in solution be oxidized to cerium(IV) in ESI mass spectroscopy?

During ESI (assuming positive ion mode for now), we apply a strong voltage ($$1.0{-}\pu{5.0 kV}$$) to induce ionization.

Therefore, it is common to see oxidation of metal ions (e.g. $$\ce{Cu^{+I} -> Cu^{+II}}$$).

I wonder if a $$\ce{Ce^{+III}}$$ solution would be observed as $$\ce{Ce^{+III}}$$ or as $$\ce{Ce^{+IV}}$$ due to in-source oxidation.

I feel like there should be a systematic study on this kind of effect but could not find any references for it. Any hints would be appreciated.

• I remember I submitted a few $\ce{Ce^3+}$ complexes with oxoanions in DMSO and DMF for ESI-MS (4.5 kV) a while ago, as from what I remember there were no shards attributed to $\ce{Ce^4+}$ species. But I suspect it may depend on solvent and compound itself. – andselisk Oct 2 '17 at 9:08
• Systematic study maybe not. But you could get lucky in checking a few papers that report such solutions and the species therein by MS. – Jan Oct 2 '17 at 9:47
• @Jan I tried that (google scholar), but couldn't really find anything. – logical x 2 Oct 2 '17 at 11:28
• It would be hard to have a systematic study as it strongly depends on the nature of the ligands / solvent / counteranions. Although not systematic, some studies have looked at several cations (doi.org/10.1016/S1387-3806(98)14044-7) and even shown that some reduction might occur due to the flow of electrons (doi.org/10.1016/S1044-0305(98)00100-7). – PLD Oct 13 '17 at 19:11
• @PLD Nice references, thanks : ) Yeah, I figured that the coordinative surrounds can be very different. On the other hand, if the bare ions (e.g. weakly coordinating anion salts, let's say Ce(OTf)3) don't get oxidized, it will certainly not happen for stronger coordinating ligands. So a study of ESI oxidation in "bare metal ions" is certainly very useful for a broad range of applications. – logical x 2 Oct 13 '17 at 20:25

I found one study that examined cerium(III) polyoxometalate salts and concluded that at least under the conditions of their study, $$\ce{Ce(III)}$$ did not oxidize under electrospray conditions. The study is Bray et al. 2011 in the International Journal of Mass Spectrometry.
The presence of the redox active $$\ce{Ce}$$ metal ion introduces additional complicating effects as it would be difficult to differentiate such ions as $$\ce{HCe(IV)P2Mo22O75^3−}$$ from $$\ce{H2Ce(III)P2Mo22O75^3−}$$. However, successive degradation of $$\ce{H_{g}Li_{2−g}Ce(III)P2Mo22O75^3−}$$ to eventually form $$\ce{HCe(III)PMo7O26−}$$ yields an ion that can be directly compared to $$\ce{LiCe(III)PMo7O26−}$$. In particular, the two ions $$\ce{HCe(III)PMo7O26−}$$ and $$\ce{LiCe(III)PMo7O26−}$$, are separated by ∼6 m/z (Fig. 6), supporting the proposition of substitution of H+ by Li+ and, therefore, the identity of $$\ce{LiCe(III)PMo7O26−}$$. These results also aid in assigning the proton count on $$\ce{H2Ce(III)P2Mo22O75^3−}$$, $$\ce{HCe(III)P2Mo18O62^2−}$$, and $$\ce{HCe(III)PMo13O44−}$$, thereby indicating the trivalent oxidation state of cerium throughout. Although Ce(III) would not necessarily expected to be oxidized to Ce(IV) under the conditions of these experiments, confirming that cerium remains in the Ce(III) oxidation state from solution throughout the electrospray and CID processes is a useful methodology for oxidation state determination of redox active metal-complexes with f-block elements such as Ce(IV) and Pu(III/IV).