Glossary of Chemistry AS Level - 10.1.3 - Electrons and Energy Levels
Other Decks By This User
- Main level 1, sublevels:
- Main level 2, sublevels:
- Main level 3, sublevels:
- Main level 4, sublevels:
- 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?
- 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.
- fills up before 3d, loses electrons before 3d.
- Ion electron configuration:
- different - lost or gained electrons
- 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.
You must Login or Register to add cards