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### 17 Cards in this Set

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 Main level 1, sublevels: s Main level 2, sublevels: s,p Main level 3, sublevels: s,p,d Main level 4, sublevels: s,p,d,f How many electrons can fit into each level: 2n^2 (2,8,18,32) but 4s gets two electrons when 3p has 8, before 3d starts to fill. How many electrons can fit into each sub-level? 2,6,10. How are electron configuration diagrams drawn? 1s at bottom, moves up levels. 3d above 4s. Electrons ^down^down arrows. Go into sublevels unpaired before pairing takes place. Electron configuration e.g.: 1s^2 2s^2 2p^6 3s^2 3p^1.. Save time by [Ar] or [Ne] - only after. Copper is exception to energy level rule: [Ar] 4s^1 3d^10 Chromium is exception to energy level rule: [Ar] 4s^1 3d^5 Blocks of elements electron within highest energy is in an s/d/f/p sub-level. Periodic table shaded. 4s fills up before 3d, loses electrons before 3d. Ion electron configuration: different - lost or gained electrons Orbitals can't know exact location of electron - found from electron density measurement that there are regions where it is highly probably to find an electron of certain energe. High probably to find an electron = orbital. sub-levels and orbitals Each of the s p and d sub-levels corresponds to a different shaped orbital. Each orbital can hold 2 electrons which spin in different difections. Shape of s orbitals s - spheres getting larger per shell Shape of p orbitals p>x orbital on x axis - diagonal when z at top p>y horizontal when z at top. p>z straight up. Hourglass.