| 1010 - Spin |
| 1010 - Use the property of electron spin to explain line splitting. |
| 1020 - Understand two electrons can occupy a single orbital and have either a paired or unpaired relationship. |
| 1030 - Understand the energy of an orbital is equal to and opposite of the energy an electron in that orbital possesses. |
| 1040 - Understand how electron shielding reduces orbital energy in a multi-electron system. |
| 1050 - Understand how electron penetration increases orbital energy in a multi-electron system. |
| 1060 - Explain why sub-level splitting occurs between s, p, and d orbitals with the same principle quantum number. |
| 1070 - Explain why orbital overlap occurs between sub-levels of different principle quantum numbers. |
| 1020 - Ground State |
| 1010 - Draw boxes for orbital diagrams of a multi-electron system. |
| 1020 - Identify degenerate orbitals in a multi-electron system, considering sub-level splitting. |
| 1030 - Label the non-degenerate sets of boxes in an orbital diagram, considering orbital overlap. |
| 1040 - State the auf-bau principle and apply it to finding a ground state of a neutral atom or anion. |
| 1050 - State Hunds rule and apply it to finding a ground state of a neutral atom or anion. |
| 1060 - State the Pauli exclusion principle and apply it to finding a ground state of a neutral atom or anion. |
| 1070 - Identify an orbital diagram as describing a ground state or excited electron configuration. |
| 1030 - Shells |
| 1010 - Identify the valence electrons and core electrons in electron configurations. |
| 1020 - Identify the s, p, d, and f blocks on the periodic table. |
| 1030 - Use the periodic table to predict the ground state configuration of each element. |
| 1040 - Understand that many of the chemical properties of elements are due to their valence electrons. |
| 1050 - Understand that elements in the same group have the same number of valence electrons. |
| 1060 - Explain why elements in the same group or family have similar chemical behavior. |