MSE 2034 Lecture Notes - Lecture 2: Atomic Orbital, Thermal Expansion, Ionic Bonding
22 Feb 2017
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Document Summary
Two of the wavelike characteristics are: electrons are in orbitals defined by a probability, each orbital at discrete energy level is determined by quantum numbers. How strongly does an atom want an additional electron: electropositivity --> how much they want to give up one. Further left and down --> electronegatively goes down. Further right and up --> electronegativity does up: higher values want more electrons. Ionic bonds: large difference in electronegativity --> most likely ionic bond, typically a metal and nonmetal element, requires electron transfer, coulombic attraction --> much higher than gravitational attraction. Happens when atoms have different charges: energy. For a potential energy vs. interatomic separation graph. Depth of well = e0 = melting point. Covalent bonds: similar electronegativity --> share electrons, carbon can share form sp3 hybrid orbitals. Primary bonding: metallic bond -- delocalized as electron cloud. Bigger difference in electronegativity more ionic of a bond.
