![]() Therefore, after striking a metallic object, light is immediatelyĪbsorbed and an electron jumps up a quantum level into an excited state. There are a large number of these low-lyingĮxcited states, all with energy differences in the visible light range. Or a " band" of energies, with only a small energy gap between the Note that every nearest neighbor atom has a bond in Cu, but not in NaCl.Įg Li metal, 1s 22s 1: Each atom has 8 nearest neighbor atoms, 6Ģ nd nearest neighbors, spherical symmetry on 2s electronic orbitals.Īll these 2s orbitals interpenetrate to give de-localized or multi-centered Gas, then the atoms are closed shell and assumed to beĬompare the two figures below, one is a map, or slice, of the electron density of the metal Cu, and the other is a map of the electron density of the ionic compound NaCl. Since we assume that all the valence electrons have been given to the electron ![]() To atom, or even place to place, within the crystal with no significant energy Their density is so diffuse to begin with, they are free to move around from atom Of positive Na ions immersed in a gas of negative charged space.Įach of the valence electrons has about the same energy and since The electron gas model envisions an array TheĮach Na atom gives up its 3s 1 electrons. Like the cation in ionic crystals, these atoms give up their valenceĮlectrons, but instead of giving the electrons to some other specificĪtom, they are redistributed to all, and are shared by all. They all have diffuse electron densities. We assume that all the atoms in metallic bonds are alike, in that Geos 306, Lecture 4, The Chemical Bond II Geos 306, Lecture 4
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