Lecture 6-electron configurations

Electron configuration

The distribution of electrons of an atom or ion in atomic or molecular orbitals.

Quantum mechanical model

A model of the atom that describes electrons as wave functions and includes quantum numbers and atomic orbitals.

Valence electrons

Electrons in the outermost shell of an atom that determine its chemical properties.

Ground state

The lowest energy state of an atom in which electrons occupy the lowest available energy levels.

Atomic orbitals (Ψ)

Regions of space around the nucleus where electrons are likely to be found, defined by quantum numbers.

Bohr model

A model of the atom that depicts electrons traveling in fixed orbits around the nucleus but is limited in application.

Quantum numbers

Numbers that describe the properties of atomic orbitals and the properties of electrons in these orbitals.

Electron configuration exceptions

Deviations from expected electron configurations, such as those observed in chromium and copper.

Heisenberg 'Uncertainty Principle'

The principle stating that it is impossible to know both the exact position and exact momentum of a particle at the same time.

Degenerate orbitals

Orbitals that have the same energy level.

Wavelength

The distance between consecutive crests of a wave, such as light.

Periodic table

A tabular arrangement of the chemical elements, organized by increasing atomic number and grouped by similar chemical properties.

Iodine's electron configuration

The arrangement of electrons in iodine, which is represented as 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d¹⁰ 5p⁵.

Allowed energy levels

Energy levels in an atom in which electrons are permitted to exist.

Spinning electron

Refers to the intrinsic angular momentum of electrons, quantified by the spin quantum number (ms) with values of +1/2 and -1/2.

Cations

Positively charged ions that are formed when an atom loses one or more electrons.

Anions

Negatively charged ions that are formed when an atom gains one or more electrons.

Line spectrum

A spectrum showing a series of specific wavelengths of light emitted by an atom.

Continuous spectrum

A spectrum that shows all the colors of light, without any gaps.

DeBroglie's hypothesis

The theory that all matter exhibits both wave and particle properties.