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Camosun College GEOS 250 Lectures: 9:30-10:20 M T Th F300 Lab: 9:30-12:20 W F300

Introduction to Mineralogy Dr. Tark Hamilton Chapter 3: Lecture 7 The Chemical Basis of Minerals (sizes, shapes & directions). Camosun College GEOS 250 Lectures: 9:30-10:20 M T Th F300 Lab: 9:30-12:20 W F300. Controls of Size in Atoms & Ions. In lone atoms (few and far between):

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Camosun College GEOS 250 Lectures: 9:30-10:20 M T Th F300 Lab: 9:30-12:20 W F300

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  1. Introduction to MineralogyDr. Tark HamiltonChapter 3: Lecture 7The Chemical Basis of Minerals(sizes, shapes & directions) Camosun College GEOS 250 Lectures: 9:30-10:20 M T Th F300 Lab: 9:30-12:20 W F300

  2. Controls of Size in Atoms & Ions • In lone atoms (few and far between): • Electrons are attracted by Z = Atomic # • 92U1s < 1H1s • Electrons in same shell repel each other • 9F > 3Li • Heavier atoms/ions are bigger down groups • 56Ba > 12Mg • +/- charges of nearest neighbours count • Al+3 is smaller in (AlO4)-5 than with (AlO6)-9

  3. Ice - Covalent BondedMineral & Rock: H2O H-O-H bond angle 104.5° (Tetrahedral = 109.5° 1.8 Angstrom Weak Hydrogen bonds between waters 1 Angstrom Strong molecular bonds within waters Open Channels (low density) Each Oxygen is Tetrahedrally coordinated by 4 Hydrogens Low O High O There are many Higher Pressure Polymorphs!

  4. Sub-Atomic Physicsfor Dummies & Mineralogists

  5. The Bohr Hydrogen Atom Better than Rutherford’s Plum Pudding Model Explains H emission lines Classical orbits decay

  6. Elements & Isotopes Carbon Atomic # 6 At.wt. 12.011 Nitrogen Atomic # 7 At.wt. 14.0067 Oxygen Atomic # 8 At. wt. 15.9994 Stable Isotopes

  7. Geologically Common & Important Elements in Minerals Major Elements: Al, Ar, Ca, C, H, K, Fe, Mg, Mn, N, Na, O, P, S, Si, Ti (16) Minor Elements: As, B, Ba, Be, Bi, Br, Ce, Cd, Cs, Cl, Cr, Co, Cu, F, He, La, Pb, Hg, Mo, Nb, Ni, Ra, Rn, Sc, Se, Sr, Sn, W, V, Y, Zn, Zr (32) Trace Elements: Ag, Au, Dy, Eu, Ga, Gd, Hf, Ho, I, Ir, Li, Lu, Nd, Os, Pd, Pt, Rb, Rh, Sm, Ta, Tb, Te, Tl, Th, Tm (25)

  8. Electrons Locations as Schroedinger’s Wave Functions S Orbital S Orbital Radius

  9. Subshell Orbital Geometries P2 x y z Orbitals S1,2,3 Orbitals D3 Orbitals

  10. Orbital Quantum Numbers& Order of Filling Sub-shells Spectral Line Names: s – Sharp p – Principal d – Diffuse f - Fundamental

  11. Quantum Numbers for Dummies & Mineralogists n Principal Quantum # = size of atom & row in periodic table K, L, M: important shells for X-ray generation & identification s, p, d, f – Electron energy levels orbital shapes & directions Every electron in every element has a unique set of quantum numbers & an energy level all its own. Electron jumps = Δ energy, photons

  12. Quantum Numbers = Electron E’s

  13. Magnetic Spin Quantum #Stern-Gerlach Experiment Spin +/- ½ Deflected Ag beam by strong Magnetic field Gave 2 spots Half filled 5s1 Magnetic Field & Induction

  14. Pauli Exclusion Principle:No 2 electrons may have identical valuesfor all quantum numbers Schroedinger’s Quantum Numbers • n – principal shell (distance from nucleus) • l – azimuthal, shape of orbital • ml – magnetic, direction/orientation of orbital Spin Quantum Number (empirical) • ms – spin magnetic • Pairs of electrons in subshells: s, p, d, f differ in the sign of their spin magnetic #

  15. Elements and Ions Low Ionization potential forms Ions easily Electronegativity attracts electrons to atom in covalent bonds Lone electrons ionize easily Noble gases need X-rays to ionize Geeze-Louise! This looks like the list of major & minor elements!

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