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17 Cards in this Set
- Front
- Back
Main level 1, sublevels:
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s
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Main level 2, sublevels:
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s,p
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Main level 3, sublevels:
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s,p,d
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Main level 4, sublevels:
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s,p,d,f
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How many electrons can fit into each level:
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2n^2 (2,8,18,32) but 4s gets two electrons when 3p has 8, before 3d starts to fill.
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How many electrons can fit into each sub-level?
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2,6,10.
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How are electron configuration diagrams drawn?
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1s at bottom, moves up levels. 3d above 4s. Electrons ^down^down arrows. Go into sublevels unpaired before pairing takes place.
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Electron configuration e.g.:
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1s^2 2s^2 2p^6 3s^2 3p^1.. Save time by [Ar] or [Ne] - only after.
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Copper is exception to energy level rule:
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[Ar] 4s^1 3d^10
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Chromium is exception to energy level rule:
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[Ar] 4s^1 3d^5
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Blocks of elements
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electron within highest energy is in an s/d/f/p sub-level. Periodic table shaded.
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4s
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fills up before 3d, loses electrons before 3d.
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Ion electron configuration:
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different - lost or gained electrons
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Orbitals
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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.
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sub-levels and orbitals
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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.
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Shape of s orbitals
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s - spheres getting larger per shell
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Shape of p orbitals
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p>x orbital on x axis - diagonal when z at top
p>y horizontal when z at top. p>z straight up. Hourglass. |