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Silver is one of the few exceptions to the common rule. While filling the s-orbital then filling the d-orbital typically achieves the lowest energy state for an atom, Silver, among other elements like Chromium and Copper, has a lower energy state with only 1 electron in the s-orbital and a full d-orbital. This is because Silver is a transition metal. However, because we only need to know the electron configurations of the elements in the 1st row of the d-block, you'll just to remember Chromium's and Copper's configuration.
The rule is to write 5s e- after 4d e-. As for silver, d^10 has lower energy. A lower total energy may be achieved if an electron enters a 4d orbital instead of expected 5s orbital, if that arrangement completes a full subshell. You can find other exceptions to the building-up principle in Appendix 2C of the textbook [6th edition for me].
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