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Introduction to Minerals
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Questions…
• Why learn about minerals?– They are the source of great wealth and beauty.– Minerals provide clues about the geologic past.
• How could knowing about minerals assist you in buying a home?– Some minerals are very unstable when exposed
to water and air.
• How do minerals form?
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DEFINITION OF A MINERAL
•naturally occurring
•inorganic
•solid
•orderly internal structure (crystal)
•with a definite chemical composition. (can vary within a specified range)
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MINERAL CLASSIFICATION
•Minerals are classified based on their:
– Physical properties –Chemical composition– Crystal Structure
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ATOMIC STRUCTURE OF MATTER
•Elements–Form of matter than cannot be reduced to a simpler form by heat, cold, or chemical reactions.
•Atoms – basic form of an element.–Protons – positive charge particle in the nucleus–Neutrons – neutrally charged particle in the nucleus–Electrons – negatively charged particle outside the nucleus.
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pure substances that cannot be decomposed by ordinary means to other substances.
Sodium Bromine
Aluminum
CHEMICAL ELEMENTS
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Chemical Symbols
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Atoms
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Electron energy levels
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The red compound is composed of• nickel (Ni) (silver)• carbon (C) (black)• hydrogen (H) (white) • oxygen (O) (red)• nitrogen (N) (blue)
The red compound is composed of• nickel (Ni) (silver)• carbon (C) (black)• hydrogen (H) (white) • oxygen (O) (red)• nitrogen (N) (blue)
CHEMICAL COMPOUNDS are composed of atoms and so can be decomposed to those atoms.
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Compounds
– composed of 2 or more elements in a fixed ratio
– properties differ from those of individual elements
– EX: table salt (NaCl)
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A MOLECULE is the smallest unit of a compound that retains the chemical characteristics of the compound.
Composition of molecules is given by
a MOLECULAR FORMULA
HH22OOCC88HH1010NN44OO22 - caffeine - caffeine
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Octet Rule = atoms tend to gain, lose or share electrons so as to have 8 electrons (All atom aspire to be “NOBLE”)
C would like to N would like toO would like to
Gain 4 electronsGain 3 electronsGain 2 electrons
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1). Ionic bond – electron from Na is transferred to Cl, this causes a charge imbalance in each atom. The Na becomes (Na+) and the Cl becomes (Cl-), charged particles or ions.
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2. Covalent bonds- Two atoms share one or more pairs of outer-shell electrons.
Oxygen AtomOxygen Atom Oxygen AtomOxygen Atom
Oxygen Molecule (O2)
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Double and even triple bonds are commonly observed for C, N, P, O, and S
••O OC
•• ••
••
••O OC
•• ••
••
HH22COCO
SOSO33
CC22FF44
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- water is a polar molecule because oxygen is more electronegative than hydrogen, and therefore electrons are pulled closer to oxygen.
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Ice (water crystals) takes up more space than liquid water because of
hydrogen bonding
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Metallic Bonding- electrons flow freely around metal atoms
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The balance of energy
• Atoms have a desire to have their outermost energy level full of electrons, otherwise a “lone” electron may be lost to other elements or may be paired with a “lone” electron from another atom.
• Think of a teeter-totter with only one person, or one with an unbalanced number of participants.
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Periodic Tablehttp://www.webelements.com/webelements/scholar/index.html
Atomic number –Number of protons and electrons
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Periodic TableTendency to lose outer electrons in order to become more “stable.”
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Periodic TableTendency to gain outer electrons in order to become more “stable.”
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Periodic TableTransition elements – also known as the heavy metalsTend to share electrons to become stable
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Periodic TableInert gases, which are already stable and don’t need additional electrons
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MINERAL COMPOSITION
•Minerals are made of different ions bonded together (gain, lose, or share electrons)
•Ions are charged atoms.
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Figure 2.4, Page 28
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Chemical Bonding of Sodium (Na) and Chlorine (Cl)
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Diagrammatic arrangement of sodium and chlorine ions in table
salt
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Sharing of electrons between two chlorine ions to for a molecule of
chlorine gas (Cl2)
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Stacking ions to form different crystal structures
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From atomic theory to a real crystal
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In Minerals (Crystals)
Physical Arrangement is more important than
Chemical Composition
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BONDING IN MINERALS
•Ionic bondingopposite charges attract (gain or lose electrons)
•Covalent bonding–ions share electrons
•Metallic bonding–free moving electrons
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Atomic Structure of Minerals
•Arrangement of atoms or ions in an orderly, repeating three-dimensional array.
(Gases)
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Atomic Structure of Minerals
•External shape is a reflection of the internal crystal structure.
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W. W. Norton
halite diamond staurolite quartz
garnet stibnite calcite kyanite
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Atomic Structure of Minerals
• Polymorphism - diamond and graphite
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Two Minerals from a Single ElementDiamond and Graphite
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Atomic structure can lead to symmetry in some minerals
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Halite
Atomic structure can lead to symmetry in
some minerals
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What is the difference between a mineral and a rock?
• Rocks are made up of more than one mineral– Example: Granite contains the minerals quartz,
plagioclase, and mica.
• Minerals contain a specific chemical composition– Example: Quartz - SiO2
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Growth and Destruction of Minerals
• Growth occurs through crystallization, which is the addition of atoms to a crystal face, in a liquid environment.– Requires: (1) sufficient quantity of the ions, (2)
proper temperature and pressure (space).
• Growth generally occurs in a confined space. Thus, external shape may not reflect internal structure.
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ROCK-FORMING MINERALS
•Silicates
•Carbonates
•Sulfates
•Halides
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Silicates
•Silica Tetrahedron–1 silicon ion bonded to 4 oxygen ions
•Silicon is positively charged (+4)
•Oxygen is negatively charged (-2)
•Net charge on tetrahedron : -4
•(SiO44-)
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More details on the Silicates
• Make up 95% of the Earth’s Volume• Basic structural shape is the tetrahedron,
which defines the mineral groups:– Isolated tetrahedron (olivine)
– Single chain (pyroxene - augite)
– Double chain (amphibole)
– Two-dimensional sheet (micas, clays)
– Three-dimensional framework (quartz, feldspars)
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Clay minerals
• Form at or near Earth’s surface in the presence of air and water from the breakdown of other silicates
• Sheet silicates like the micas.
• Very small crystals.
• Low density– Example: kaolinite
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Isolated tetrahedron
Isolated
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Isolated tetrahedron (olivine)-Does not break a certain way
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Isolated tetrahedron
Single Chain
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Single chain (pyroxene - augite)-Breaks on 2 planes at right angles
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Isolated tetrahedron
Double Chain
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Double chain (amphibole - hornblend)
-Breaks on 2 planes at 60° and 120°
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Isolated tetrahedron
Two dimensional sheet
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Two-dimensional sheet (micas - muscovite)
-Breaks in 1 plane
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Isolated tetrahedron
Three dimensional framework
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Three-dimensional framework (quartz, feldspars - orthoclase)
-Breaks on 2 planes at 90°
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MINERAL IDENTIFICATION
Color Luster
Streak Cleavage
Fracture Taste
Habit Smell
Specific Gravity Magnetic
Hardness Effervescence–Mohs Hardness Scale
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Bowen’s Reaction Seriesthe realationship between temperature and
the formation of crystals in magma1400 oC
800 oC
Mafic
Intermediate
Felsic
Plagioclase
Calcium-rich
Sodium-rich
Olivine
Pyroxene
Amphibole
Biotite
Orthoclase
Muscovite
Quartz
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Crust composition – most common elements
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Mafic
• Minerals rich in iron and magnesium
• Representative of high density, high temperature magmas.
• Examples:– Olivine, pyroxenes, amphiboles
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Felsic minerals
• Minerals rich in silicon and aluminum.
• Representative of low density, low temperature magmas.
• Examples:– Feldspars, quartz, micas
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Mineral Destruction
• Minerals can melt under high temperatures, removing of outer atoms - melting
• Under high pressures, some minerals melt, while others may partially melt, resulting in same chemical composition, but different crystal structure.
• Weathering - physical and chemical breakdown of minerals– Some atoms can be pried loose from the structure by
water – dissolving (example: NaCl)
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Carbonates
• Basic structure contains the strong, covalent bonded carbonate ion CO3
2-
– Bonds easily (ionic) with metals, such as calcium to form calcium carbonate or calcite (CaCO3) CaCO3 is often precipitated directly from carbonate rich seawater.
– Shell organisms capture carbonate and combine it with calcium to form CaCO3.
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Carbonates #2• Most common mineral is calcite and found readily in
limestone and dolomite rock.• Calcite is relatively soft, 3-4 on Mohs hardness scale, and
can dissolve in acids (even mild carbonic acid).– Results in cave formation– Weathering of statues and buildings due to acid rain.
• Calcite is one mineral that easily deforms and reforms at the Earth’s surface. Often find calcite crystals in the cracks of rocks
• Calcite can be easily mistaken for quartz, but a scratch test can remedy the dilemma.
• Dolomite (CaMg(CO3)2 bonds a little more tightly with two carbonate ions, resulting in more resistance to acid destruction.
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Sulfates
• Gypsum (CaSO4 ·2H2O)
• Anhydrite (CaSO4) – note the two missing water molecules, hence the “An” in the mineral name. Plaster contains anhydrite.
• Barite (BaSO4) is soft and “greasy” feeling. Since it doesn’t burn under intense friction, barite serves as an excellent lubricant for drilling.
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Halides
• Common Salt (NaCl)– Halite
• Found in thick layers where ancient seas have since evaporated.
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Elements as Minerals
• Sulfur• Gold• Silver• Platinum• Diamond• Many of these metals are often associated
with sulfide minerals and low temperature silicates (e.g. quartz veins).
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References
• The Mineral Gallery (commercial site)– http://mineral.galleries.com/