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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