CHEM 107 Lecture 7: Chapter 7 - Quantum

• School: Binghamton University
• Department: Chemistry
• Course: CHEM 107
• Professor: Benjamin Turnpenny

Document Summary

Electron states: ground state (lowest level, excited state (above ground state) Predicts energy required to remove electron from aton (ionization) Scientists began using quantum theory to explain matter at atomic level: limitations. Applies only to one-electron systems, doesn"t account for multielectron interactions. Louis de broglie: all particles have wave like character, wavelength inversely proportional to its momentum, so small that wave character of electrons is signi cant. Uncertainty principle: wave and particle theories yield different answers on location of e- around nucleus, can"t predict both location and velocity, heisenberg uncertainly principle. Erwin schr dinger: equation to describe behavior for electron saves, basis of quantum mechanics. Ms = +1/2 or -1/2 (spinning motion) Rules: pauli exclusion principle: no two electrons can have the same set of four quantum numbers. It"s too much energy to spin them aligned. All s orbitals are spheres, equal distribution and dense around nucleus.