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The transition metals don't have a traditional method to identify valence electrons like the other groups, but I don't think we have gone over in class how to determine how many valence electrons each transition metal has.
The number of valence electrons in the d-block is usually the group number plus 2 (for the 2 electrons in the preceding s orbital) in the ground state. For example, scandium's configuration is [Ar]3d^14s^2, so it has 3 valence electrons. This may only work for the first 2 rows though because further down there are elements in the f-block.
The valence electrons for the elements in the d block are always the amount of electron in the outermost shell. For example, for Mn: [Ar] 4s^2 3d^5. There are 2 valence electrons because the 4th energy level is the outer most orbital.
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