In the group 3 to group 12 transition metals, the outermost s electron shell con

Question

In the group 3 to group 12 transition metals, the outermost s electron shell contains one or two electrons. However, in these metals, it is the d subshells that fill up going across the row. In period 4 of the table, the 3d subshell fills, and in periods 5 and 6, the 4d and 5d subshells fill, respectively. It is important to keep in mind that this filling is not always regular. For example, in period 4, element 23, vanadium, has an electron configuration of [Ar]3d34s2, but element 24, chromium, has an electron configuration of [Ar]3d54s.


Why is the electron Configuration backwards. I always see it with S first then d p f basically. Why is this one d then s????
Why isnt it [Ar]4s3d5 instead of [Ar]3d54s??????

Answer the specific Question I have please.

Explanation / Answer

The energy gap between the 3d and 4s levels has widened. In this case, it isn't energetically profitable to promote any electrons to the 4s level until the very end. In the ions, all the electrons have gone into the 3d orbitals. You couldn't predict this just by looking at it.

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