CHEM 6A Lecture Notes - Lecture 5: Principal Quantum Number, Magnetic Quantum Number, Spin Quantum Number

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

Document Summary

Assumptions bohr made cannot be applied to atoms with more than one electron. On the mass scale of atomic particles, we cannot determine exactly the position, direction, and speed simultaneously: the very act of locating an electron causes uncertainty in another property. For electrons, we cannot determine their momentum and position simultaneously ( x)(m v) >= h/4pi: we can calculate the uncertainty in position (x) or velocity (v) Schrodinger"s model: assumes that electrons waves, describe 3d regions of space called orbitals where electrons are likely to be found, instead of where they are, we talk about regions where the electron is highly probable to be found. Bohr model of the hydrogen atom was 1-d: only needed 1 piece of information to define the distribution of the electron in the atom. Energy level = principal quantum number = n. Spherical: p orbital when l = 1 c. i. Dumbbell: d orbital when l = 2 d. i.