Effective Nuclear Charge Calculator

Effective nuclear charge (Zeff or Z*) is the net positive charge experienced by an electron in an atom. It's the actual nuclear charge minus the shielding effect of other electrons, calculated as Z* = Z - S.

To calculate Zeff, first determine the atomic number (Z), then calculate the shielding constant (S) using Slater's rules based on electron configuration and orbital type. Finally, subtract: Zeff = Z - S.

Electron shielding is the reduction in effective nuclear charge felt by an electron due to the presence of other electrons between it and the nucleus. Inner electrons shield outer electrons from the full nuclear charge.

Zeff increases across a period because the nuclear charge increases while electrons are added to the same shell. The shielding effect remains relatively constant, so the net nuclear charge felt by valence electrons increases.

Yes, higher Zeff pulls electrons closer to the nucleus, resulting in smaller atomic radius. This explains why atomic radius decreases across a period and increases down a group.

Slater's rules are a set of guidelines for calculating the shielding constant (S) in atoms. They assign different shielding values based on the electron's position and the type of orbital it occupies.

Electron shielding is influenced by the number of electrons between the nucleus and the electron of interest, the type of orbitals involved, and the electron configuration. S orbitals shield more effectively than p orbitals, which shield more than d orbitals.

For carbon's 2p electrons, the effective nuclear charge is approximately 3.25. This is calculated as Z* = 6 (atomic number) - 2.75 (shielding constant from Slater's rules).