<Tr> <Th> Compound </Th> <Td> UbuX </Td> <Td> UbbX </Td> <Td> UbtX </Td> <Td> UbqX </Td> <Td> UbpX UbpO 2 + </Td> <Td> UbhF UbhF UbhO </Td> <Td> </Td> <Td> UqbX UqbX </Td> <Td> UqtF </Td> <Td> UqqX UqqO 2 + UqqF UqqO </Td> <Td> UqpF </Td> <Td> </Td> <Td> UqoO </Td> <Td> </Td> <Td> </Td> <Td> </Td> <Td> </Td> <Td> </Td> </Tr> <Tr> <Th> Analogs </Th> <Td> La X Ac X </Td> <Td> Ce X Th X </Td> <Td> </Td> <Td> </Td> <Td> Np O2 + </Td> <Td> </Td> <Td> </Td> <Td> ThF </Td> <Td> </Td> <Td> UF UO 2 + Pu F PuO </Td> <Td> </Td> <Td> </Td> <Td> UO </Td> <Td> </Td> <Td> </Td> <Td> </Td> <Td> </Td> <Td> </Td> </Tr> <Tr> <Th> Oxidation states </Th> <Td> </Td> <Td> </Td> <Td> 5 </Td> <Td> 6 </Td> <Td> 6 </Td> <Td> 1, 2, 4, 6, 8 </Td> <Td> 6 </Td> <Td> 4, 6 </Td> <Td> 6, 8 </Td> <Td> 3, 4, 5, 6, 8 </Td> <Td> 6 </Td> <Td> 8 </Td> <Td> 12 </Td> <Td> </Td> <Td> 0, 2 </Td> <Td> 3, 5 </Td> <Td> </Td> <Td> </Td> </Tr> <P> In the later superactinides, the oxidation states should become lower . By element 132, the predominant most stable oxidation state will be only + 6; this is further reduced to + 3 and + 4 by element 144, and at the end of the superactinide series it will be only + 2 (and possibly even 0) because the 6f shell, which is being filled at that point, is deep inside the electron cloud and the 8s and 8p electrons are bound too strongly to be chemically active . The 5g shell should be filled at element 144 and the 6f shell at around element 154, and at this region of the superactinides the 8p electrons are bound so strongly that they are no longer active chemically, so that only a few electrons can participate in chemical reactions . Calculations by Fricke et al. predict that at element 154, the 6f shell is full and there are no d - or other electron wave functions outside the chemically inactive 8s and 8p shells . This would cause element 154 to be very unreactive, so that it may exhibit properties similar to those of the noble gases . </P>

What element is g on the periodic table