Question #4e19a

1 Answer
Truong-Son N.
Jun 12, 2015

That looks like #Ti#.

The "rule" has exceptions most prevalent past the third row on the Periodic Table (although #P#, #S#, and #Cl# are especially known to behave like this as well; there exist #PCl_5#, #SF_6#, and #ClF_6^-#, for example).

There is a trend that the s and p orbitals approach the d orbitals in energy as you move down the periodic table. By the time you get to the third energy level (#n = 3#), the electrons have access to the #3d# orbitals too. This access allows more than 8 electrons in the valence shell.

http://www.mikeblaber.org/

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