Effective nuclear charge

Effective nuclear charge is the net positive charge an electron experiences from an atom’s nucleus after the screening effects of other electrons are taken into account.

Slater's rules: A set of empirical rules for estimating electron shielding and effective nuclear charge in atoms. They provide a practical approximation for calculating the charge after shielding.
Periodic trends: Recurring patterns in elemental properties across periods and down groups of the periodic table. Increasing effective charge across a period helps explain several recurring property trends.
Atomic number: The number of protons in an atom's nucleus, which determines the element. It sets the unscreened nuclear charge from which effective charge is estimated.
Nuclear charge: The total positive electric charge of an atomic nucleus, determined by its number of protons. Unlike effective charge, nuclear charge does not subtract electron screening.
Electron shielding: The reduction in nuclear attraction experienced by an electron because other electrons repel it and screen the nucleus. Shielding is the central correction that distinguishes effective charge from full nuclear charge.
Atomic radius: A measure of the size of an atom, commonly inferred from distances between bonded or neighboring atoms. Greater effective nuclear attraction generally contracts an atom's electron cloud.
Electron configuration: The arrangement of electrons among an atom's shells, subshells, and orbitals. The configuration identifies which electrons can shield a chosen electron.
Formal charge: An accounting charge assigned to an atom in a molecule by dividing bonding electrons equally between bonded atoms. Formal charge is bookkeeping for molecules, not an electron's experienced nuclear attraction.
Atomic orbital: A quantum-mechanical description of an electron's spatial state in an atom. Effective charge shapes orbital energies and radial distributions.
Ionization energy: The energy required to remove an electron from an atom or ion in the gas phase. An electron held more strongly by the nucleus generally requires more energy to remove.

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