Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
17 Cards in this Set
- Front
- Back
N represents |
What orbital the electrons are in |
|
L represents |
The shape of the orbital, =0 or n-1 |
|
M (sub) L represents |
The sub orbitals and how they exist at different angles |
|
M(sub)S represents |
Spin up/spin down (can only= +1/2 or -1/2 |
|
Dalton's theory |
Matter cannot be created or destroyed |
|
Chadwick |
Discovered the nucleus |
|
Bohr |
Electrons occupy stationary states. When stationary, atoms do not emit energy. Changes states by emitting or absorbing energy |
|
Emission spectra |
When an electron falls to a lower energy level |
|
Absorption spectrum |
When an electron moves to a higher energy level |
|
Thompson |
Raisin bun model |
|
Rutherford |
Gold foil experiment. Determined nucleus |
|
Planck and Einstein |
Light energy increases in small steps. Each step is a photon. Energy increases w frequency |
|
Broglie |
Electrons can behave like a wave |
|
Schrödinger |
Electrons can have certain energy levels bc e- must fit the orbitals in while # of wavelength |
|
Heisenberg |
Uncertainty principle: don't know where e- are or how fast they're going Gave us shapes of various orbitals using e- probability density |
|
Pauli exclusion principle |
No 2 e- can have the same set of four quantum numbers. No atomic orbital can contain more than 2 e- |
|
Hunds Rule |
When e- are assigned to an orbital, fill spin ups first |