Ionization of the transition metals in the central portion of the table (groups 3 through 12) is less predictable than ionization of elements near the table’s sides. ![]() Elements in Group 13, Group 14, and Group 15 typically ionized to form cations with charge of +3, +4, and +5, respectively, although other valences are possible. Oxygen and other elements in Group 16 typically form divalent anions (-2). So, they typically become monovalent anions (charge of -1) because they acquire an extra electron to fill the shell. Elements in group 17 ( halogens) are lacking a single electron to fill their outer shells completely. Elements in Groups 16 and 17 have room for a small number of additional electrons in their outer shells and consequently accept extra electrons to become anions. On the other side of the chart, helium and other elements in Group 18 of the Periodic Table have completely filled outer shells and, consequently, do not ionize. Those in group 2 ( alkaline earth elements) usually have an ionic charge of +2. Elements in group 1 ( alkali elements) generally have an ionic charge of +1. Elements in groups on the left side of the table have “extra” electrons in outer shells, and readily give up those electrons to become cations. The red numbers below the columns are typical ionic charges. But, when they do, for most elements, their likely ionic form is predictable as shown. This table is not to suggest that all the elements always form ions. ![]() Common cations are shaded blue and common anions are shaded red. The chart seen here shows the most common ions for different columns in the Periodic Table.
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