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????

Explanation / Answer

hmm...where to star....

ya,

now if we see scandium, there is only one transition eletron. so, it goes directly into the d state. now, there is a exception with chromium. it has a chance to fill all the places in the transition state to be stable. so, the configuration changes.

scandium has- 3d1 4s2

titanium has- 3d2 4s2

vanadium has- 3d3 4s2

but when it comes to chromium, i must have been 3d4 4s2 but it will be 3d5 4s1.

the above must have been the configuration. but the problem is last shell of D is not filled and S has 2 electrons.

so, the electron added is done in the D state. the configuration varies as,

to make it stable, the above thing is done. :)

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