CHEM 101 Lecture Notes - Lecture 3: Electron Configuration, Emission Spectrum, Transition Metal

• School: Drexel University
• Department: Chemistry
• Course: CHEM 101
• Professor: Monica Ilies

Document Summary

Developed model that explains how the structure changes during energy transitions. Quantized=the atom can only have certain amounts of energy. Distances between rings are proportional and stationary. Electrons emit radiation when they fall down orbitals (higher to lower) Quantum numbers determine shape, size and orientation in space of lower higher=absorption of energy the orbitals (to describe both particle and wave-like behavior) ^^^these are all the quantum numbers that completely describe l=orbital type. (cid:1865) =position of orbital in an xyz plot. (cid:1865) (cid:3046)=orientation of the spin of the electron integer 1 the movement of the electron. Principal quantum number (n): the energy level. The larger n is, the higher energy in the orbital. The larger the value of n , the energy between orbitals lowers. If energy=0, the electron escapes from the atom. (cid:1866) (cid:3041)= (cid:4666)1(cid:3041)2(cid:4667) energy between the two energy states. Each line in the emission spectrum corresponds to the difference in.