Periodic Trends and Electron Configurations

These flashcards cover vocabulary and concepts from electron configurations and periodic trends, essential for understanding atomic behavior and properties.

Atomic Radius

The distance from the nucleus of an atom to the outermost shell of electrons.

Valence Electrons

Electrons in the outermost shell of an atom that are involved in forming bonds.

Hund’s Rule

When orbitals of equal energy are available, the lowest energy electron configuration has the maximum number of unpaired electrons with parallel spins.

Effective Nuclear Charge

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

Aufbau Principle

The principle that electrons occupy the lowest energy orbitals first.

Pauli Exclusion Principle

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

Sublevel

A subdivision of an energy level in an atom, represented by the letters s, p, d, and f.

Metallic Radius

Half the distance between the nuclei of two metal atoms in a metallic lattice.

Covalent Radius

Half the distance between the nuclei of two nonmetal atoms bonded together.

Electron Configuration

The distribution of electrons among the orbitals of an atom.

Condensed Electron Configuration

An electron configuration that uses the element symbol of the nearest noble gas in square brackets to simplify notation.

Electron Affinity

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

Ionization Energy

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

Transition Metals

Elements that are found in the d-block of the periodic table and have partially filled d-subshells.

Core Electrons

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

Excited State

A state of an atom where one or more electrons have absorbed energy and moved to a higher energy level.

Quantum Mechanical Model

A model that describes the behavior of electrons in atoms as wave functions rather than fixed orbits.

Periodic Trends

Patterns in the periodic table that show how certain properties vary with atomic number.

Electron Configuration Rules

Guidelines governing how electrons fill atomic orbitals: Aufbau, Pauli Exclusion, and Hund’s Rule.

Orbital Diagram

A visual representation of the arrangement of electrons in an atom’s orbitals.

S Block Elements

Elements in groups 1 and 2 of the periodic table, characterized by their s orbital filling.

P Block Elements

Elements in groups 13-18 of the periodic table, characterized by their p orbital filling.

D Block Elements

Transition metals characterized by their d orbital filling.

F Block Elements

Lanthanoids and actinoids characterized by their f orbital filling.

Chemical Behavior

The way atoms interact during a reaction, often influenced by their electron configuration.

Inner Transition Metals

The lanthanides and actinides series, which are typically placed below the main body of the periodic table.