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When presented with an positive ion of an element for example like Fe2+, I go about writing the electron configuration of the original element itself but afterwards I feel as though I may still be confused on how to write the configuration correctly. My thought was that you would remove electrons from the outermost shell, but I'm not sure thats right. Whats the correct way to approach this?
Fe2+ and other metals within the d-block are much harder to write the electron configuration for due to their nature. Some of them are transition metals and can have different oxidation numbers too. For the most part, focus on the s-block and p-block in order to write electron configuration and create ions from them. And yes, you are right. To create ions, you remove electrons or add electrons to the valence shell.
Therefore the electron configuration for Fe in its ground state would be [Ar] 3d^6 4s^2 and then you remove the two valence electrons from the d orbital to make Fe^2+ which would be [Ar] 3d^5 4s^1 because it is isoelectronic with Chromium.
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