2._Atomic_Structure_and_Wave_Theory_Filled_In

Atomic Structure

The arrangement and interaction of subatomic particles in an atom, including electrons, protons, and neutrons.

Wave Theory

A theory that describes electrons and orbitals as wavefunctions, allowing for the understanding of electron configurations and bonding.

Periodic Table

A tabular arrangement of chemical elements, organized by groups (columns) and periods (rows) based on their atomic structure and properties.

Electromagnetic Waves

Oscillations of electric and magnetic fields that propagate through space at the speed of light.

Spectroscopy

The study of the interaction between electromagnetic waves and matter, used to analyze the composition of substances.

Bohr Model

An early atomic model proposing that electrons orbit the nucleus at fixed distances and energy levels.

Heisenberg Uncertainty Principle

A fundamental limit in quantum mechanics stating that the position and momentum of an electron cannot both be precisely determined simultaneously.

Orbital

A region in an atom where there is a high probability of finding an electron, characterized by specific energy levels.

Wavefunction (Ψ)

A mathematical function describing the probability of finding an electron in a given region of space.

Pauli Exclusion Principle

No two electrons in an atom can have the same set of four quantum numbers, ensuring unique electron states.

Degenerate Orbitals

Orbitals that have the same energy level but different quantum numbers.

Radial Nodes

Points in a radial wavefunction where the probability of finding an electron is zero, indicating areas of wave amplitude cancellation.

Angular Nodes

Regions in a wavefunction where the angular dependency leads to zero probability of finding an electron.

Aufbau Principle

The principle stating that electrons fill the lowest energy orbitals available before moving to higher levels.

Hund’s Rule

The principle that states electrons will fill degenerate orbitals singly first and with parallel spins to maximize total spin.

Effective Nuclear Charge (Zeff)

The net positive charge experienced by an electron in a multi-electron atom, adjusted for shielding effects from other electrons.

Ionization Energy (IE)

The energy required to remove an electron from a gaseous atom or ion.

Electron Affinity (EA)

The amount of energy released when an electron is added to a neutral atom in the gas phase.

Atomic Size

The size of an atom, typically measured by the distance from the nucleus to the outermost electron shell.

Ionic Size

The size of an ion, which varies depending on whether the ion is a cation (positively charged) or anion (negatively charged).