CHEM 131 Chapter Notes - Chapter 8: Paramagnetism, Electronegativity, Lewis Structure

• School: University of Maryland
• Department: Chemistry and Biochemistry
• Course: CHEM 131
• Professor: Ferraoli

Document Summary

How e fit into orbitals around atoms. Based of coulumb"s law opposites attract and like charges repel. Pauli exclusion principle: no 2 e in the same atom may have the same quantum numbers. Aufbau principle: fill lowest e orbitals before higher e orbitals. Hund"s rule: half fill all orbitals before totally filling any. *4s comes before 3d because 4s has e penetration, but 3d does not. Unpaired e in electron configurations give paramagnetic qualities: attracted to magnetic fields. All e paired = diamagnetic: not attracted to magnetic fields. Half filled and fully filled orbitals are more stable. Exceptions: be, b, al do not form octets. Ie, ea, radius, en + metallic behavior all predicted by periodic table trends.