![]() (number)(letter) (raised number)(number)(letter) (raised number). Notice that this electron configuration is just a repeating string that goes like this:.Let's look at an example configuration for the element sodium (Na):.These may at first look complicated, but they're just a way to represent the electron orbitals in an atom with letters and numbers and they're easy once you know what you're looking at. Another way to find an element's valence electrons is with something called an electron configuration. Learn how to read an electron configuration. This means that an atom can have multiple numbers of valence electrons depending on how it is manipulated. For reasons that are a little too complex to explain here, when electrons are added to the outermost d shell of a transition metal (more on this below), the first electrons that go into the shell tend to act like normal valence electrons, but after that, they don't, and electrons from other orbital layers sometimes act as valence electrons instead.Generally, the valence electrons are the electrons in the outermost shell - in other words, the last electrons added. As electrons are added to an atom, they are sorted into different "orbitals" - basically different areas around the nucleus that the electrons congregate in.See below for a quick run-through or skip this step to get right to the answers. Understanding why transition metals don't really "work" like the rest of the periodic table requires a little explanation of the way electrons behave in atoms. Understand that transition metals don't have "traditional" valence electrons.
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