Atomic Structure Review

Flashcards include key terms and definitions related to atomic structure and quantum mechanics.

Quantum Number

A set of four numbers (n, ℓ, mℓ, ms) that describe the unique state of an electron in an atom.

Electromagnetic Radiation

A type of radiation that includes visible light, characterized by fluctuating electric and magnetic fields.

Wavelength (λ)

The distance between two successive peaks of a wave, typically measured in meters.

Frequency (ν)

The number of waves that pass a given point per second, measured in hertz (Hz).

Planck's Constant (h)

A universal constant (6.63×10–34 J s) that relates the energy of a photon to its frequency.

Orbital

A region in an atom where there is a high probability of finding an electron.

Hund's Rule of Maximum Multiplicity

Electrons will fill degenerate orbitals singly first before pairing up.

Pauli Exclusion Principle

No two electrons can have the same set of four quantum numbers.

Diagrams of Electron Configuration

Representations of the distribution of electrons across various atomic orbitals.

Diamagnetism

A property of materials that are not attracted to magnetic fields, often due to paired electrons.

Paramagnetism

A property of materials that are attracted to magnetic fields, usually due to unpaired electrons.

Ionization Energy

The energy required to remove an electron from an atom in its gaseous state.

Electron Affinity

The energy change that occurs when an electron is added to a neutral atom in the gas phase.

Core Electrons

Electrons in the inner shells of an atom that are not involved in bonding.

Valence Electrons

Electrons in the outermost shell of an atom that can participate in forming bonds.

Principal Quantum Number (n)

Describes the main energy level of an electron and its distance from the nucleus; can be any positive integer (1, 2, 3…). The larger the 'n', the higher the energy and the larger the orbital.

Azimuthal (Angular Momentum) Quantum Number (ℓ)

Defines the shape of an electron's orbital and the subshell (s, p, d, f) it occupies; its value ranges from 0 to n-1.

Magnetic Quantum Number (mℓ)

Describes the orientation of an orbital in space; its values range from -\ell to +\ell, including 0.

Spin Quantum Number (ms)

Indicates the intrinsic angular momentum of an electron, which creates a magnetic moment. Its values are +\frac{1}{2} or -\frac{1}{2}.

Aufbau Principle

Electrons fill atomic orbitals of the lowest available energy levels before occupying higher energy levels.

Heisenberg Uncertainty Principle

States that it is impossible to precisely determine both the position and momentum of an electron (or any particle) simultaneously.