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The d-orbital is more stable when it has either 5 electrons or 10 electrons (either half filled or filled entirely). Therefore, whenever the d-orbital seems like it should have 4 electrons or 9 electrons, an electron is taken from the s-orbital to make that number either 5 electrons or 10 electrons in order to make it more stable. Hope that helps!
Elements in the same group as Cu would also “act” like Cu. Copper is one of our exceptions in electron configurations: its d-orbital will have a full shell (3d10 4s1). Any element under Cu will act the same so silver’s d orbital will also have a full shell.
Know that the 5s orbital is of a higher energy level than the 4d level. If the lower levels aren't filled completely first, then the higher energy levels will not be able to carry electrons in a stable state, as they will want to fall to a tighter level.
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