L07 Chem 111A Lecture Notes - Lecture 9: Valence Electron, Effective Nuclear Charge
28 Dec 2015
School
Department
Course
Professor
Document Summary
Draw the following h-atom radial probabilities for the following orbitals. Energies of the orbitals only depends on n. Orbital energy ordering: e (1s) < e (2s) = e (2p) < e (3s) = e (3p) = e (3d) Orbital energy ordering: e(1s) < e (2s) < e (2p) < e (3s) etc. Shielding/screening: electrons closer to the nucleus shield electrons that are farther from the nucleus from the nuclear charge (z). Z* is used to describe the effective nuclear charge felt by an electron in a particular orbital. Valence electrons screen each other less effectively from the nuclear charge than core electroons screen valence electrons. Z* would equal z with no screening, and would equal 1 with perfect screening. For an electron in mg, rank in order of increasing z*: z*(3s), z*(3p), z(3d). Justify your answer including a radial distribution plot (sketch) to support your answer.
