is so large in the seventh period that seaborgium is expected to lose its 6d electrons before its 7s electrons (Sg, [Rn]5f146d47s2; Sg+, [Rn]5f146d37s2; Sg2+, [Rn]5f146d37s1; Sg4+, [Rn]5f146d2; Sg6+, [Rn]5f14). Because of the great destabilisation of the 7s orbital, SgIV should be even more unstable than WIV and should be very readily oxidised to SgVI. The predicted ionic radius of the hexacoordinate Sg6+ ion is 65 pm, while the predicted atomic radius of seaborgium is 128 pm. Nevertheless, the stability of the highest oxidation state is still expected to decrease as LrIII > RfIV > DbV > SgVI. Some predicted standard reduction potentials for seaborgium ions in aqueous acidic solution are as follows: {| |- | 2 SgO3 + 2 H+ + 2 e− || Sg2O5 + H2O || E0 = −0.046 V |- | Sg2O5 + 2 H+ + 2 e− || 2 SgO2 + H2O || E0 = +0.11 V |- | SgO2 + 4 H+ + e− || Sg3+ + 2 H2O || E0 = −1.34 V |- | Sg3+ + e− || Sg2+ || E0 = −0.11 V |- | Sg3+ + 3 e− || Sg || E0 = +0.27 V |} Seaborgium should form a very volatile hexafluoride (SgF6) as well as a moderately volatile hexachloride (SgCl6), pentachloride (SgCl5), and oxychlorides SgO2Cl2 and SgOCl4. SgO2Cl2 is expected to be the most stable of the seaborgium oxychlorides and to be the least volatile of the group 6 oxychlorides, with the sequence MoO2Cl2 > WO2Cl2 > SgO2Cl2. The volatile seaborgium(VI) compounds SgCl6 and SgOCl4 are expected to be unstable to decomposition to seaborgium(V) compounds at high temperatures, analogous to MoCl6 and MoOCl4; this should not happen for SgO2Cl2 due to the much higher energy gap between the highest occupied and lowest unoccupied molecular orbitals, despite the similar Sg–Cl bond strengths (similarly to molybdenum and tungsten). Molybdenum and tungsten are very similar to each other and show important differences to the smaller chromium, and seaborgium is expected to follow the chemistry of tungsten and molybdenum quite closely, forming an even greater variety of oxoanions, the simplest among them being seaborgate, , which would form from the rapid hydrolysis of , although this would take place less readily than with molybdenum and tungsten as expected from seaborgium's greater size. Seaborgium should hydrolyse less readily than tungsten in hydrofluoric acid at low concentrations, but more readily at high concentrations, also