CHE 131 Lecture Notes - Lecture 24: Isoelectronicity, Pauli Exclusion Principle, Rede Ferroviária Nacional

• School: Stony Brook University
• Department: Chemistry
• Course: CHE 131
• Professor: Benjamin Hsaio, Jiangyong Jia, Roy Lacey

Document Summary

Aufbau principle- electrons enter and fill lower energy orbitals before higher energy orbitals. Hund"s rule- electrons will enter the orbitals one at a time to maximize degeneracy. Ground-state electron configurations are the basis for the recurring pattern of chemical behavior. 3d orbitals are more compact than 4s, and as a result any electrons entering 3d orbitals will experience greater mutual repulsion. Start with the configuration for the neutral atom; then add or remove electrons from the. Atoms or ions that are isoelectronic with each other have identical numbers and valence shells to make the desired ion. configurations of electrons. Electron configuration of an element describes the distribution of electrons in the orbitals of its atoms. Among main group elements the outer electron configurations within a group are. The period number of an element corresponds to the n value of the highest energy level containing electrons. Core electrons- electrons in the previous noble gas and any filled d or f sublevels.