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Min Test 1
Question | Answer |
---|---|
Diamond - Native Element | C |
Graphite - Native Element | C |
Pyrite - Sulfide | FeS2 |
Chalcopyrite - Sulfide | CuFeS2 |
Galena - Sulfide | PbS |
Sphalerite - Sulfide | ZnS |
Hematite - Oxide | Fe2O3 |
Magnetite - Oxide | Fe3O4 |
Corundum - Oxide | Al2O3 |
Ilmenite - Oxide | FeTiO3 |
Rutile - Oxide | TiO2 |
Halite - Halide | NaCl |
Fluorite - Halide | CaF2 |
Calcite - Carbonate | CaCO3 |
Aragonite - Carbonate | CaCO3 |
Siderite - Carbonate | FeCO3 |
Dolomite - Carbonate | CaMg(CO3)2 |
What is a mineral? | a naturally occurring crystalline solid with a definite, but not necessarily fixed, chemical composition |
What is a crystalline solid? | repeating crystal structure, dictated by cations and anions |
Why do we have so few minerals (compared to animal species)? | they’re fundamental building blocks. there are a finite number of ways in which cations and anions can combine in order to form minerals |
How do we know about the chemical composition of the earth? | Composition of the Sun, Composition of chondrites, Clues from seismology |
What is the relative composition of crust? | • Oxygen 46% • Silicon 28% • Aluminum 8% • Iron 5% • Calcium 4% |
What are the most common minerals in the Earth’s crust? | • Plagioclase feldspar • Quartz • K-feldspar • Pyroxene • Mica • Amphibole • Clay • Olivine |
What are the major crustal elements? | -O -Si -Al -Fe -Ca -Na -K -Mg |
What are the siderophile (iron-loving) elements? | • Fe Co Ni • Ru Rh Pd • Re Os Ir Pt Au • Mo Ge Sn C P • (Pb) (As) (W) |
What are the chalcophone (sulfur-loving) elements? | • Cu Ag (Au) • Zn Cd Hg • Ga In Tl • (Ge) (Sn) Pb • As Ab Bi • S Se Te • (Fe) (Mo) (Re) |
What are the lithophile (crust-loving?) elements? | • Li Na K Rb Cs • Be Mg Ca Sr Ba • B Al Sc Y REE • (C) Si Ti Zr Hf Th • (P) V Nb Ta • O Cr W U • (Fe) Mn • F Cl Br I • (H) (Tl) (Ga) (Ge) (N) |
Common cations (lose electrons, positive charge) include... | H, Li, C, N, Na, Mg, P |
Common anions (gain electrons, negative charge) include... | O, F, S, Cl, |
Properties of Ionic bonding include... | • electron transfer • one gets a positive charge, one gets a negative charge, they’re attracted to one another • medium to hard • high symmetry • fully to partially transparent • highly water soluble |
Properties of Covalent bonding include... | • electron sharing • very hard • high melting temperature • low symmetry • brittle, often break by conchoidal fracture |
Properties of Metallic bonding include... | • electrons aren’t linked, free to move • this is why they’re good conductors • not water soluble • variable hardness and breaking • highly symmetrical and opaque |
Properties of Hydrogen bonding include... | • fairly weak bond • has to do with polarity |
Properties of Van der Waals bonding include... | • at any given moment, there may be a positive charge on one side and a negative charge on the other side • one of the weakest bonds, between sheets |
Common Cation charges | • Si 4+ • Ti 4+ • Al 3+ • Fe 2+,3+ o Ferrous 2+ o Ferric 3+ • Mg 2+ • Mn 2+ • Ca 2+ • Na 1+ • K 1+ • P 5+ |
Common Anion charges | • O 2- • S 2- • (OH) 1- o (ClH)- o (FH)- |
Coordination | the number of nearest neighbors (ions in contact) to any ion |
What is the formula for radius ratio? | radius of cation/radius of anion |
What factors affect atomic radius? | Increase in charge (decreases radius), Increase in coordination (increases radius), Increase in temperature (increases radius), Increase in atomic number (decreases radius, unless you are also adding shells) |
How do we think we know elemental abundances? | • taking samples • analyzing glacial lakes (mechanical weathering) • analyzing loess (windblown sediment) • research literature |
How did Goldschmidt come up with his classification scheme? | siderophile, chalcophile, lithophile, atmophile. Based on greeks? |
How are minerals classified? | chemical composition & anion group |
What are the types of packing? | hexagonal closest packing, cubic closest packing |
How do you calculate bond strength? | charge/coordination # |
Cubic closest packing examples | tetrahedral or octahedral |
How do you figure out coordination number? | NaCl: each Na surrounded by 6 Cl (CN=6) |
Hexagonal closest packing | ABABABABABABAB stacking Arrangement of equal size spheres |
Cubic closest packing | ABCABCABCABCABCABC stacking |
Types of insterstitial holes? | o Trigonal hole o Tetrahedral hole o Octahedral hole |
Pauling's rule 1 | • a coordination polyhedron of anions is formed about each cation, the cation-anion distance being determined by the radius sum and the coordination number of the cation by the radius ratio |
Pauling's rule 2 | • The electrostatic valency principle, or bond strength – in a stable crystal structure, the total strength of the valency bonds that reach an anion from all the neighboring cations is equal to the charge of the anion |
Pauling's rule 3 | • The existence of edges, and particularly of faces, common to two anion polyhedra in a coordinated structure reduces its stability |
Pauling's rule 4.1 | • In a crystal containing different cations, those of high valency and small coordination tend not to share polyhedral elements with each other, and when they do, |
Pauling's rule 4.2 | the shared edges contract (to put more negative charge between the cations), and the cations are displaced from their polyhedral centers, away from the shared edge or face |
The principle of parsimony | the number of essentially different kinds of constituents in a crystal tends to be small, because, characteristically there are only a few types of contrasting cation and anion sites |
Isodesmic | all the bond strengths are the same (halite) |
anisodesmic | all the bond strengths are not uniform (carbonates, sulfates) |
mesodesmic | the bond strength between the cation and the anion equals exactly half of the charge of the…? |
Siderophile | metallic (core) |
Chalcophile | sulfide (core and sulfide ore deposits) |
Lithophile | silicates and oxides (crust and mantle) |