CHEM 001 Lecture 8: Chem 001 - LEC8

• School: College of The Sequoias
• Department: Chemistry (CHEM)
• Course: CHEM 001
• Professor: guerra

Document Summary

Schrodinger"s wave function uses a wave function to describe the electron in an atom. Uses the concept that an electron, with wavelike properties and indeterminacy in momentum and position, can be described by a wave function. Represents the height of a wave at position x, y, z. 1s is similar to 2s, but they have different energies. 2 represents the probability of finding an e- (heisenberg) Squaring a wave gives you the probability. Wave functions (like electromagnetic wave) can take + or - values. Schrodinger equation: operate a change on (x, y, z) = energy (x, y, z) H = e this works a little like the double derivative of sin since h is a double derivative. Atomic orbitals (oh boy) in general a higher energy corresponds to a larger orbital there are four main types (or shapes) Ml is the orientation l is the shape the four types are s, p, d, f.