Quantum Mechanics and Atomic Theory

Flashcards about Quantum Mechanics and Atomic Theory.

Line Spectrum

Light emitted by an element when subjected to high voltage passed through a spectrometer.

Rutherford's planetary model

Model suggesting the electron spirals into the nucleus and emits all colors sequentially.

Bohr's Postulate 1

Electrons can only move in certain fixed orbits corresponding to specific energy levels.

Bohr's Postulate 2

An electron can only move from one orbit to another when it gains or loses energy.

Hydrogen Spectrum

The wavelengths of emitted light are related to the distances between energy levels.

Quanta

Small amounts of energy or light.

Principal quantum number (n)

Related to the size of the electron cloud.

Secondary quantum number (l)

Related to the shape of the electron cloud.

Magnetic quantum number (ml)

Related to the orientation of the shape in 3D space.

Spin number (ms)

Used to designate the different electron spins.

Pauli's Exclusion Principle

No two electrons can have the same quantum numbers.

Quantum Number (n)

The value of n corresponds to the size of the cloud/distance to cloud's edge or shell.

Secondary quantum number (l)

The value of l corresponds to the basic shape of the electron cloud or shell.

Planck, Einstein Theory

Light/energy can be described as a particle.

De Broglie Theory

Matter can be described using waves.

Heisenberg's Uncertainty Principle

The position and velocity of an electron cannot be simultaneously measured

Schrödinger's wave function (Ψ)

Describes the regions in which it is highly probable to find an electron.

Magnetic quantum number (ml)

The value of ml corresponds to the orientation of the cloud in 3D space or its subshell.

Hund's Rule

Every subshell's cloud is singly occupied with one electron before any one orbital has two, and all electrons in singly occupied orbitals have the same spin.

Spin quantum number (ms)

The value of ms corresponds to the spin of an electron in a cloud, and is either +½ (positive spin) or -½ (negative spin).

Electron Configuration

The way an atom's electrons are distributed among its orbitals.

Pauli Exclusion Principle

Each orbital can hold, at most, 2 electrons.

Aufbau Principle

The levels are built up with the lowest levels receiving the electrons first.