Chemistry

Silver is a transition metal, so its electron configuration involves filling the $d$ orbitals—but here's the key: silver actually has a filled $d$ subshell, which is unusually stable. Rather than following the expected pattern, silver "steals" an electron from the $s$ orbital to complete its $d$ block, giving it a half-filled or full $d$ configuration. Use the noble-gas notation by starting with the nearest noble gas below silver, then carefully account for which orbitals fill and in what order.

Silver is a transition metal, so its electron configuration involves filling the $d$ orbitals—but here's the key: silver actually has a filled $d$ subshell, which is unusually stable. Rather than following the expected pattern, silver "steals" an electron from the $s$ orbital to complete its $d$ block, giving it a half-filled or full $d$ configuration. Use the noble-gas notation by starting with the nearest noble gas below silver, then carefully account for which orbitals fill and in what order.