Chem 1465 1st Edition Lecture 14Outline of Last Lecture 1. Quantum mechanics and the Heisenberg uncertainty principle2. Quantum numbers3. Electron configurationA. RulesB. Terms to knowC. Using periodic table4. Periodic trends 5. Atomic and ionic radii6. Ionization energy7. Electron affinity Outline of Current Lecture 1. Carbon2. Condensed phases- crystallineA. Packing of spheres 3. Condensed phases- amorphous4. Unit cell5. Coordination number 6. Metallic bonding7. PolymersA. DefinitionsB. Wallace CarothersC. Two monomersD. Polymer stereochemistryE. Degree of polymerizationCurrent Lecture1. Carbon: originally believed to only have two elemental forms- diamond and graphite. In 1985 at Rice University Bucky Were discovered C60 which has been used for carbon nanotubes and carbon fibers2. Condensed phase- crystalline: regular repeating geometric arrangementsA. Packing of spheres-cubic close-packed: ABCABC stacking pattern where B and C will be over the open spaces of AThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.-hexagonal close-packed: ABABAB stacking pattern where A and B are over the open spaces3. Condensed phases- amorphous: solids that form random structures 4. Unit cell: smallest repeating unit structureA. Three types of unit cells-Simple cubic: 1 atoms per cell-Body center cubic (BCC): 2 atoms per cell-Face centered cubic (FCC): 4 atoms per cellB. Calculating the number of atoms per cell: all the atoms completely contained in the cell + ½ the number of face centered atoms + 1/8 of corner atomsC. Volume of a unit cell = 22.63r3D. Packing efficiency: the percentage of space that is occupied by atoms. Calculated by = volume of atoms in unit cell / volume of unit cell x 100 = %5. Coordination number: number of atoms immediately adjacent to any other atomsA. Simple cubic has 6 CNB. Body centered cubic has 8 CNC. Face centered cubic has 12 CN6. Metallic bondingA. Terms to know: malleable (metals can form shapes and foils) and ductile (can be pulled into wires)B. Qualitative model: sea of electrons where valence electrons of the meta are delocalized and free to move about the solidC. Quantitative model: band theory where there are bonding orbitals and anti-bonding orbitals. These two bonding areas can have sometimes have gaps in between them. When there is no gap= metal bonds. A small gap = semi-conductors. A big gap = insulators7. Polymers A. Definitions-Monomers: a single part or unit-Dimer: 2 monomers covalently attached-Trimer: 3 monomers covalently attached-Oligomer: a few monomers covalently attached-Polymer: many monomers covalently attachedB. Wallace Carothers: gives us modern day definition of polymers. Polymers are large molecules compromised of repeating units called monomers. Carothers recognized two types of polymers:-Addition polymers: the molecular formula of a structural unit is identical to that of the monomer -Condensation polymer: the molecular formula of the structural units differ from that of the monomerC. If two monomers are present there are 4 possible situations:-Random copolymer where there is no pattern-Alternating copolymer: ABABAB-Block copolymer: AAAAABBBBB-Graft copolymer similar to block except new strands can build off anotherD. Polymer stereochemistry:-isotactic: all the groups of the backbone are the same direction-syndiotactic: the groups alternate-atactic: random E. degree of polymerization = molar mass of polymer / molar mass of