Mineralogy Minerals – chemical compounds that form naturally as solids with shapes determined by the arrangement of atoms, e.g., quartz (SiO2). Crystals.

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Presentation transcript:

Mineralogy Minerals – chemical compounds that form naturally as solids with shapes determined by the arrangement of atoms, e.g., quartz (SiO2). Crystals – the morphological manifestation of a mineral, e.g., quartz crystals commonly comprise hexagonal prisms topped by hexagonal pyramids and halite (NaCl) crystals commonly occur as cubes.

World’s largest crystals: A cave in the Naica Lead Zinc mine, Mexico

Miners in Cueva de los Crystals: the mineral gypsum Crystals of a variety of gypsum (CaSO4.2H2O) precipitated from hot water at 60 degrees celsius in a limestone cave in the Naica mine

Minerals Tourmaline on Feldspar Beryl (Be3Al2(SiO3)6 Emerald

Pyrite (FeS2) crystals

Feldspars – two of the most important rock-forming minerals Plagioclase Albite – NaAlSi3O8 Anorthite CaAl2Si2O8 K-feldspar Sanidine Orthoclase Microcline KAlSi3O8

Colours and forms of quartz Citrine Amethyst Milky quartz Rose quartz

Quartz crystals displaying prism and pyramid faces

Crystal Shapes Quartz Diamond Halite (SiO2) (C) (NaCl) Calcite Garnet (CaCO3) Garnet (Fe3Al2Si3O12) Stibnite (Sb2S3)

Quartz Crystal Pyramid Faces display consistent angular relationships Angles measured with a goniometer Prism

Crystals have ordered arrangements of atoms Disorder

X-ray diffraction X-ray beam splits into numerous smaller beams. Interference of waves of different beams produces a diffraction pattern on a screen or film. The pattern indicates the spacing and arrangement of atoms.

Surface of galena (PbS) imaged With an atomic force microscope Atomic structure of galena (PbS) Sulphur Lead

The atomic structure of halite (NaCl) Ionic bonding

Ionic bonding – transfer of electrons Anion - Cation +

Relative sizes of ions Ion co-ordination

The atomic structure of diamond Covalent bonding

The source of Diamonds The ‘Big Hole’ at Kimberly, South Africa Kimberlite containing diamond

Cutting diamonds

Covalent bonding – sharing of electrons

Atomic structure of graphite Covalent bonding within sheet Van der Waal’s bonding between sheets

Ice Crystals Hydrogen bonding

The silicon tetrahedron

Silicate Structures Nesosilicate Inosilicate Inosilicate SiO44 - (Single chain) (Double chain) SiO44 - Si4O116 - SiO32- Sheet silicate Framework silicate Si4O104 - SiO2

Nesosilicate Olivine (Fe,Mg)2SiO4

Inosilicate (Single Chain) Diopside Pyroxene CaMgSi2O6 Hypersthene (Fe,Mg)SiO3

Inosilicate (Double Chain) Amphibole Tremolite Ca2Mg5Si8O22(OH)2 Riebeckite Na2Fe5Si8O22(OH)2 Tigers Eye

Sheet Silicate Biotite KAl(Fe,Mg)3Si3O10(OH)2 Muscovite KAl3Si3O10(OH)2

Asbestos Chrysotile (Mg3Si2O5(OH)4 Uses and risks (Insulation, heat, fire resistance) Serpentine (Mg3Si2O5(OH)4

Framework Silicate Quartz SiO2 Plagioclase Amethyst SiO2 Albite NaAlSi3O8 Plagioclase Anorthite CaAl2Si2O8 Amethyst SiO2 K-feldspar KAlSi3O8

Relationship of Quartz structure to Feldspar Structure Imagine four SiO2 molecules 4 x SiO2 = Si4O8 Substitute Al3+ for Si4+ in one of these molecules SiO2 + AlO2 + SiO2 = AlSi3O8- Add Na+ or K+ to supply missing charge = NaAlSi3O8 or KAlSi3O8 Albite K-Feldspar SiO2 + AlO2 + SiO2 = Al2Si2O82- Add Ca2+ to supply missing charge = CaAl2Si2O8 Anorthite