CHY 123 Lecture Notes - Lecture 10: Bohr Model, Photon, Pauli Exclusion Principle

• School: Ryerson University
• Department: Chemistry
• Course: CHY 123
• Professor: Derick Rousseau

Document Summary

Absorption and emission energy (cont, bohr completed his model by concluding that the electron could jump from one orbit to another by either emitting or absorbing photons with specific frequencies. However, it is important to know that there are a total of 7 orbitals (corresponding to ml = - The total number of electrons in a neutral atom is equal to the atomic number, z: 2. Electrons fill orbitals starting with the lowest n and moving upwards, with no more than two electrons per orbital (aufbau principle): link: 3. No two electrons can fill one orbital with the same spin (pauli"s exclusion principle): 4. 5. 8 orbital shapes and energies s orbitals. The p orbitals have an electron density concentrated on the sides of the nucleus in two lobes with a node at the nucleus. The d orbitals (in subshell l = 2) have a variety of shapes.