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Electron arrangement
Chapter 3
| Question | Answer |
|---|---|
| energy level | fixed energy value that an electron in an atom can have |
| energy sublevel | a subdivision of an energy level containing one or more atomic orbitals |
| s orbital shape | spherical |
| p orbital shape | dumbbell |
| atomic orbital | a region in space where there is a high probability of finding a electron |
| dual wave particle nature of a electron | Louis De Brogile suggested that all moving particles have a wave motion |
| Heisenbergs uncertainty principle | states that it is impossible to measure velocity and the position of a electron at the same time |
| evidence that energy levels exist | flame tests. |
| example of real life energy levels | fireworks! |
| how flame tests provide evidence for energy levels | electrons absorb and release energy in fixed amounts. If energy levels were continuous, atoms would emit a continuous spectrum (rainbow). we see discrete lines—evidence that only specific energy transitions are allowed. |
| uses of atomic absorption spectrum (AAS) | detecting the analysis of heavy metals (lead) in water or blood. also used to test for gunshot residue. |
| line spectrum | A series of narrow coloured lines |
| atomic emission spectrum | Atoms emit light, giving a series of coloured lines on a black background |
| atomic absorption spectrum | Atoms absorb light, giving a series of black lines on a coloured background. |
| ground state | electrons occupy lowest energy level |
| excited state | electrons occupy higher energy levels than the ground state |
| paschen | series of lines in the Infra red region |
| balmer | series of lines in the visible region |
| lyman | series of lines in the Ultra violet spectrum |
| limitations of bohrs theory | didn't account the wave nature of a electron and conflicts with Heseinbergs principle |
| aufbau's principle | electrons fill the lowest energy level first |
| hunds rule | electrons fill orbitals singly before filling them in pairs |
| pauli's exclusion principle | no more than two electrons can occupy an orbital - if they do, they must have a opposite spin |
Created by:
Kamilex
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