Download Electron Orbital Helpsheet

Name__________________________________Date_______________________Period____________
Chemistry
S sublevel – holds 2 electrons
P sublevel – holds 6 electrons
Each orbital holds 2 electrons – px, py, pz
D sublevel – holds 10 electrons
Each orbital holds 2 electrons – dxy, dxz, dyz, dx2–y2, dz2
F sublevel – holds 14 electrons
Each orbital holds 2 electrons
Diagonal Diagram
Aufbau_Diagram
Rules for Filling Orbitals
Aufbau Principle – Electrons enter orbitals of lowest energy first.
Pauli Exclusion Principle – An atomic orbital may describe at most two electrons.
When occupying the same orbital, the two electrons must have opposite spins.
Hund’s Rule – When electrons occupy orbitals of equal energy, one electron enters each orbital
until all the orbitals contain one electron with parallel spins.