Once copernicium is ionized, its chemistry may present several differences from those of zinc, cadmium, and mercury. Due to the stabilization of 7s electronic orbitals and destabilization of 6d ones caused by relativistic effects, Cn is likely to have a [Rn]5f 6d 7s electronic configuration, using the 6d orbitals before the 7s one, unlike its homologues. The fact that the 6d electrons participate more readily in chemical bonding means that once copernicium is ionized, it may behave more like a transition metal than its lighter homologues, especially in the possible +4 oxidation state. In aqueous solutions, copernicium may form the +2 and perhaps +4 oxidation states. The diatomic ion Hg 2, featuring mercury in the +1 oxidation state, is well-known, but the Cn 2 ion is predicted to be unstable or even non-existent. Copernicium(II) fluoride, CnF 2, should be more unstable than the analogous mercury compound, mercury(II) fluoride (HgF 2), and may even decompose spontaneously into its constituent elements. As the most electronegative reactive element, fluorine may be the only element able to oxidise copernicium even further to the +4 and even +6 oxidation states in CnF 4 and CnF 6 ; the latter may require matrix-isolation conditions to be detected, as in the disputed detection of HgF 4. CnF 4 should be more stable than CnF 2. In polar solvents, copernicium is predicted to preferentially form the CnF 5 and CnF 3 anions rather than the analogous neutral fluorides (CnF 4 and CnF 2, respectively), although the analogous bromide or iodide ions may be more stable towards hydrolysis in aqueous solution. The anions CnCl 4 and CnBr 4 should also be able to exist in aqueous solution. The formation of thermodynamically stable copernicium(II) and (IV) fluorides would be analogous to the chemistry of xenon. Analogous to mercury(II) cyanide (Hg(CN) 2), copernicium is expected to form a stable cyanide, Cn(CN) 2.