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Bohr Model

Explains electron energy levels for hydrogen-like atoms.

Quantum Model

Describes electrons as wave-particle duality.

Wave Characteristics

Includes wavelength, frequency, and speed of light.

Particle Characteristics

Described by energy equation E = hv.

de Broglie's Hypothesis

Particles exhibit wave properties like light.

Heisenberg's Uncertainty Principle

More position certainty leads to momentum uncertainty.

Schrödinger's Equations

Predict probable electron locations around nucleus.

Atomic Orbitals

Regions where electrons are likely found.

Principal Quantum Number

Indicates energy level and orbital size.

Angular Momentum Quantum Number

Describes sublevel shape of electron cloud.

Magnetic Quantum Number

Specifies orientation of electron cloud in space.

Spin Quantum Number

Indicates electron spin direction, +1/2 or -1/2.

Pauli Exclusion Principle

No two electrons can share identical quantum numbers.

Hund's Rule

Electrons fill degenerate orbitals singly first.

Aufbau Order

Electrons fill lowest energy orbitals first.

Electron Configuration

Arrangement of electrons in an atom's orbitals.

Orbital Notation

Diagram showing electron distribution in orbitals.

s Orbital

Spherical shape, holds up to 2 electrons.

p Orbitals

Dumbbell shape, holds up to 6 electrons.

d Orbitals

Complex shapes, holds up to 10 electrons.

f Orbitals

Even more complex, holds up to 14 electrons.

Degenerate Orbitals

Orbitals with the same energy level.

Energy Level

Distance from nucleus, determines electron energy.

Electron Density Clouds

Visual representation of probable electron locations.

Maximum Electrons

2n² formula determines electron capacity per level.