An iron ion with a charge of +8 is not very likely, therefore, the octet rule is not applicable to transition elements. The groups in the periodic table tell us how many electrons the elements have in their outermost electron shell. It can sometimes lose two electrons to form the Fe 2 + ion, while at other times it loses three electrons to. As an example, iron commonly forms two different ions. In order for an element such as iron (Fe) to achieve the same noble gas configuration of argon (Ar), it would need to lose 6 electrons in the 3 d subshell and 2 electrons in the 4s subshell. Most transition metals differ from the metals of Groups 1, 2, and 13 in that they are capable of forming more than one cation with different ionic charges. Because the charge on the chloride ion is 1 and the charge on the calcium ion is +2, for example, consistent with their positions in the periodic table. This is because the transition metals have electrons in d subshell and do not follow the octet rule. Notice that there is no simple pattern for transition metal ions (or for the larger main group elements) as there is with the main group ions. \) shows the characteristic charges for some of these ions. The chemical behavior of the various elements is influenced more by the charge of their ion than by any other intrinsic property.
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