The structure of the atom, particularly the arrangement of electrons, directly influences chemical reactivity, with atoms having incomplete outer shells tending to react to achieve stability.
The distribution of electrons in an atom's electron shells and subshells.
Proposed the atom as a solid, indivisible sphere.
The rule stating that electrons will occupy degenerate orbitals singly before pairing up.
The number of protons in the nucleus, defining the element.
Positively charged particles found in the nucleus that determine the atomic number and identity of the element.
Also known as the Plum Pudding Model, it suggested that atoms are composed of a positively charged 'soup' with negatively charged electrons embedded.
The principle stating that electrons fill the lowest energy orbitals first.
Negatively charged particles that orbit the nucleus in electron shells and are involved in chemical bonding and reactions.
The type of bonds formed (ionic, covalent) is determined by electron configuration.
Proposed that electrons travel in fixed orbits around the nucleus with quantized energy levels.
The total number of protons and neutrons in the nucleus.
Neutral particles located in the nucleus that contribute to the atomic mass but do not affect the charge.
Introduced the concept of a dense nucleus surrounded by orbiting electrons.
Atoms of the same element with the same number of protons but different numbers of neutrons.
The principle stating that no two electrons can have the same set of quantum numbers.
