The discussion centers on the conductivity of transition metals, particularly gold and silver. Key factors include the presence of a large density of free electrons and the proximity of conduction and valence bands, explained through band theory. The d-orbitals of transition metals extend far from the nucleus, allowing for significant overlap and hybridization, which enhances conductivity. Silver is identified as the best conductor, although it oxidizes quickly, reducing its effectiveness compared to gold and other metals.
PREREQUISITESChemistry students, materials scientists, and electrical engineers interested in the properties and applications of transition metals in conductivity.
KingNothing said:What about the molecules and bonds of transition metals make them (such as gold) such good conductors? I'm in AP chemistry, so we may have gone over it, but I don't know right now.
I see. Is there no way it can be coated in carbon or tungsten to help this problem?chroot said:Silver is, indeed, the best elemental metal in electrical conduction. The problem is that silver rapidly oxidizes when exposed to air, and silver oxides are not good conductors at all.
Like Zz said, I believe that it is to do with the lattice and, therefore, the fact (given above) about the metal that makes it conduct well.ZapperZ said:The major reason why the transition elements are such good conductors is because the valence shell for these elements is the d-orbitals. This orbital extends very far out from the nucleus of the atom (look at the average position of an electron in the 3d orbital when compared to the 4s). When atoms of these elements are "locked" into place in a solid, the d-orbitals have a larger tendency to overlap and hybridize with their neighbors (nearest neighbors and even next nearest neighbors), forming the familiar conduction bands.