The shielding of electrons gives rise to an effective nuclear charge, Z_eff, which explains why boron is larger than oxygen. Estimate the approximate Z_eff felt by a valence electron of boron and oxygen, respectively?

How does electron shielding in multielectron atoms give rise to energy differences among 3s, 3p, and 3d orbitals?

Order the electrons in the following orbitals according to their shielding ability: 4s, 4d, 4f.

One method for calculating Zeff is to use the equation

where E is the energy necessary to remove an electron from an atom and n is the principal quantum number of the elec-tron. Use this equation to calculate Zeff values for the highest-energy electrons in potassium (E = 418.8 kJ/mol) and krypton (E = 1350.7 kJ/mol).

Classify each statement about effective nuclear charge, 𝑍eff , as true or false.

Rank the elements by effective nuclear charge, 𝑍eff, for a valence electron.

In which orbital below would an electron (on average) be closest to the nucleus?