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Chemistry 13 - Transition metals
 At first sight, they look like a confusing and irritating break in the pattern. For one thing, they can't be divided neatly into groups; all of them have very similar properties. Also, unlike the elements we've been talking about, they don't always use the same number of valence electrons in chemical reactions. Iron (Fe), for example, sometimes likes to give away two electrons, and sometimes three. Well, those ten elements fill up the ten 3d orbitals. But the 4s orbitals already have electrons in them before you get to the transition metals--a higher sublevel got filled first. The result is that all the transition metals have the same arrangement of outer electrons; only the 3d orbitals, lower down, are different. Exactly. You can also see why they might keep changing their minds about how many valence electrons they have. Iron sometimes gives up just its two 4s electrons, and sometimes throws in a 3d, since those are so close in energy.
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