Atomic Theory, Electron Configurations, and Chemical Nomenclature

Vocabulary flashcards reviewing core definitions of atomic models, orbital types, electron configurations, ion formation, and IUPAC/traditional nomenclature rules.

Orbital

A region in space where there is a $90\%$ probability of finding an electron.

Dalton's Model ($1803$)

An atomic model proposed by John Dalton that pictures atoms as tiny, indestructible particles with no internal structure.

Thomson's Plum-Pudding Model ($1897$)

An atomic model proposed by J.J. Thomson following the discovery of the electron, picturing electrons embedded inside a sphere of positive electric charge.

Rutherford's Model ($1911$)

An atomic model proposed by Ernest Rutherford stating that an atom consists of a dense, positively charged nucleus surrounded by randomly moving electrons.

Bohr's Model ($1913$)

An atomic model proposed by Niels Bohr in which electrons move in spherical orbits at fixed distances from the nucleus.

Electron Cloud Model ($1926$)

An atomic model developed by Erwin Schrödinger using mathematical equations to describe electron behavior in regions called orbitals rather than fixed orbits.

Octet Rule

The chemical rule stating that atoms react to achieve a stable noble gas electron configuration containing eight valence electrons (two $s$ and six $p$ electrons).

Cation

A positively charged ion formed when a metal atom loses valence electrons to achieve a noble gas configuration.

Anion

A negatively charged ion formed when a non-metal atom gains valence electrons to achieve a noble gas configuration.

Salt

An ionic compound formed by the transfer of electrons, composed of cations and anions held together by electrostatic attraction.

Formula Unit

The simplest whole-number ratio of ions present in an ionic compound.

Polyatomic Ion

A group of atoms that stay bound together as a unit and carry a single overall net charge.

Stock System of Nomenclature

A system for naming variable-charge cations that uses a Roman numeral in parentheses immediately following the cation name to indicate its charge.

Traditional System of Nomenclature

An older system for naming variable-charge cations using the Latin root with the suffix -ic for higher charges and -ous for lower charges.

Binary Acid

An acid composed of hydrogen and a non-metal dissolved in water, named with the prefix hydro- and the suffix -ic acid.

Oxyacid

An acid containing hydrogen, oxygen, and another element, named by changing polyatomic ion endings from -ate to -ic acid or -ite to -ous acid.

Covalent Compound

A compound formed between two or more non-metals that is named using Greek numerical prefixes to specify atomic counts and ending the second element in -ide.

Core Electrons

The electrons occupying inner energy levels that are not located in the highest principal energy level.

Valence Electrons

The electrons located in the highest principal energy level of an atom that participate in chemical reactions and bonding.

$s$ Orbital

A spherically shaped atomic orbital that can hold a maximum of $2$ electrons.

$p$ Orbitals

A set of $3$ dumbbell-shaped orbitals oriented along orthogonal axes that can hold a maximum total of $6$ electrons.

$d$ Orbitals

A set of $5$ atomic orbitals that can hold a maximum total of $10$ electrons ($2$ electrons per orbital).

$f$ Orbitals

A set of $7$ complex atomic orbitals that can hold a maximum total of $14$ electrons ($2$ electrons per orbital).