Electron Orbitals And Electronic Configurations Flashcards
Define orbit.
A single pathway where a past and future electron location can be predicted.
Define orbital.
A 3D region around the nucleus where you can find an electron 90% of the time.
Why are models used in chemistry?
To help understand atomic properties and behaviour.
Why can’t past and future electron locations be predicted?
Because there are multiple pathways.
How many electrons can an orbital shape host at any given energy level?
Two.
Why are electronic orbitals a more sophisticated model?
They represent electrons distribution in space.
Orbitals are contained into shells numbered what?
1, 2, 3 and 4.
What four things determine the shape of an electronic orbital?
- The number of electrons it contains. 2. The proximity of other orbitals. 3. The distance from the nucleus. 4. The energy carried by the electron.
How many electrons can a S shell hold?
2.
How many electrons can a P shell hold?
6.
How many electrons can a D shell hold?
10.
How many electrons can a F shell hold?
14.
State four reasons why electrons do not spiral down the nucleus.
- Electrons are equally constrained by each other. 2. Electron size is minuscule in relation to the nucleus and its orbital. 3. Orbital theory predicts that a “caged” electron (orbital small enough to overlap with the nucleus) will require immense energy. 4. Electrons precipitate into the nucleus under some conditions (inverse beta decay).
Define the Aufbug principle.
Orbitals fill in order of increasing energy levels.
Define Hund’s rule.
Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron.
How do you remember the order orbitals and shells fill?
What an opposite spins diagram look like? How do they fill?
What part of the periodic table does the s, p, d and f shells belong to?
