CHEM 6A Lecture Notes - Lecture 2: Electron Affinity, Aufbau Principle, Isoelectronicity

• School: UCSD
• Department: Chemistry and Biochemistry
• Course: CHEM 6A
• Professor: Thomas Bussey

Document Summary

Learning objectives chapter 5: reading, read the entire chapter, with the following exception: Bohrs model gave a great explanation of the hydrogen atomic spectrum. In the bohr model, the electron is treated as a particle in fixed orbits around the nucleus. Quantum mechanical model, the electron is treated mathematically as a wave. The electron has properties of both particles and waves. The bohr model was a one-dimensional model that used one quantum number to describe the distribution of electrons in the atom. The only information that was important was the size of the orbit, which was described by n the principle quantum number. Schrodinger"s model (quantum mechanical model) allowed the electron to occupy three- dimensional space. Quantum number determine the size, shape, orientation, and spin of an electron. There are 4 quantum numbers: you need to know the names and symbols for each of the quantum numbers. You should also know what information they represent.