The Quantum Model of the Atom and Periodicity

These flashcards cover essential vocabulary related to the quantum model of the atom, periodicity, and electronic structure.

Photon

A particle of light that carries energy.

Electron Configuration

The distribution of electrons in an atom's orbitals.

Orbital

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

Valence Electrons

The electrons in the outermost energy level of an atom, involved in chemical bonding.

Ionization Energy

The energy required to remove an electron from an atom.

Effective Nuclear Charge (Z_eff)

The net positive charge experienced by outer shell electrons, considering shielding by inner electrons.

Slater's Rules

A set of rules used to calculate the shielding effect of inner electrons on outer electrons.

Wave-Particle Duality

The concept that light and matter exhibit properties of both waves and particles.

Bohr Model

A model of the atom proposing that electrons travel in fixed orbits around the nucleus.

Ground State

The lowest energy state of an atom, where electrons are in the closest orbitals to the nucleus.

Excited State

A state of an atom where electrons have absorbed energy and moved to higher energy levels.

Photoelectric Effect

The phenomenon whereby electrons are emitted from a material when it absorbs light.

Electromagnetic Spectrum

The range of all types of electromagnetic radiation.

Wave Function

A mathematical description of the quantum state of a system; in quantum mechanics, it gives information about the probability amplitude of position.

Quantum Numbers

Numbers that describe the size, shape, and orientation of orbitals, as well as the spin of electrons.

Aufbau Principle

The principle that electrons occupy the lowest energy orbitals first.

Hund's Rule

A rule stating that electrons will fill degenerate orbitals singly before pairing up.

Pauli Exclusion Principle

A principle that states no two electrons can have the same set of four quantum numbers.

Anomalous Electron Configurations

Electron configurations that differ from expected because of stability considerations, often seen in transition metals.

Cation

A positively charged ion formed by the loss of one or more electrons.

Anion

A negatively charged ion formed by the gain of one or more electrons.

Electron Affinity

The amount of energy released or absorbed when an electron is added to a neutral atom.