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On Test 3, there was a question involving drawing the most stable Lewis structure for a molecule that contained a transition metal. I was really confused as to how to figure out how many valence electrons are in each different transition metal. Any help is appreciated!!
I believe the most stable structure would have been the one which made the charge of the entire molecule 0. So, for example, the transition metal was bonded to Nitrogen, then it would need a charge of +3. Hope this helps!
to find the valence electron of a transition metal I would try using the electron configuration, it would require you to use the (n-1) concept. For the energy levels you subtract one when you are working with transition metals. Then the amount of electrons in the last energy level would be your valence.
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