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Mineralogy and Crystal Chem > Test 1 > Flashcards

Test 1 Flashcards

1
Q

Georgius Agricola

A

(1494-1555) German Mineralogist, “Father of Mineralogy”

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2
Q

Nicholas Steno

A

(1638-1684) Danish Scientist, One of the OG’s of Stratigraphy and Geology. (Principle of original horizontality, Princ. of lateral continuity, Princ. of Coss-cutting relationships)

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3
Q

Hardness (Physical Property)

A

How resistant an object is to Scratching. Uses Practical Scale/Moh’s Scale. Increases exponentially.

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4
Q

Moh’s Scale (Info)

A

Austrian Mineralogist Friedrich Mohs. 1 to 10 Hardness scale.

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5
Q

Moh’s Scale (Actual Scale)

A 
1-Talc
2-Gypsum
3-Calcite
4-Fluorite
5-Apatite
6-Orthoclase Feldspar
7-Quartz
8-Topaz
9-Corundum
10-Diamond
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6
Q

Density (Units)

A

(g/cm^3)

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7
Q

Avogadro’s #

A

6.022e23

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8
Q

Specific Gravity

A

Relative Density. Dimensionless. Ratio of; Substance weight : Weight of an equal volume of water @ 4C

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9
Q

Tenacity

A

Resistance to breaking or scratching. Relates to internal bonding.

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10
Q

Tenacity - Brittle

A

A mineral that breaks and powders easily. Ex// Halite.

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11
Q

Tenacity - Malleable

A

A mineral that can be hammered out into a sheet. Ex// Copper

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12
Q

Tenacity - Sectile

A

A mineral that can be cut into thin shavings with a knife. Ex// Chalcocite.

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13
Q

Tenacity - Ductile

A

A mineral that can be drawn into a wire. Ex// Gold

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14
Q

Tenacity - Flexible

A

A mineral that bends but does not return to its original shape when pressure is released. Ex// Sheets of Chlorite, Talc.

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15
Q

Tenacity - Elastic

A

A mineral that bends and returns to its original position upon the release of pressure. Ex// Micas

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16
Q

Tenacity - Tough

A

Its Tough (?)

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17
Q

Luster

A

General appearance of a mineral surface in reflected light. 2 types, Metallic and Nonmetallic

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18
Q

Luster - Metallic

A

Luster of a polished metal surface. They reflect light like metals and are opaque to transmitted light.

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19
Q

Luster - Non-metallic

A

Most common. Shown by many minerals that transmit light. Varies widely in appearance.

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20
Q

Luster - Non-met. - Adamantine

A

Luster of a Diamond, Highly reflective. “Brilliant”. Ex// Diamonds and Garnets

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21
Q

Luster - Non-met. - Vitreous

A

Appears as a piece of polished glass. Ex// Quartz and Emerald.

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22
Q

Luster - Non-met. - Resinous

A

Appears as a piece of resin. Ex// Sphalerite.

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23
Q

Luster - Non-met. - Pearly

A

Appears as Mother-of-Pearl with iridescent sheen. Parallel to well-developed cleavage plains. Ex// Talc and Apophyllite.

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24
Q

Luster - Non-met. - Greasy

A

Appears to be covered in a thin layer of oil. Caused by light scattering on a microscopically rough surface. Ex// some milky Quartz and Nepheline)

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25
Luster - Non-met. -Silky
Appears as a skein of silk or a piece of satin. Fibrous aggregates. Ex// Fibrous Gypsum.
26
Luster - Non-met. - Earthy
Appears dull. Aggregates of very fine-grained materials. Ex// Goethite and Limonite.
27
Diaphaneity
The power of transmitting light
28
Diaphaneity - Transparent
Ability to see an object through the mineral, clear.
29
Diaphaneity - Translucent
Light transmits through mineral but objects not clear
30
Diaphaneity - Opaque
No light can get through, even on the thin edges
31
Color - Idiochromatic
Of the same color
32
Color - Allochromatic
Pertaining to change of color
33
Iridescence
exhibition of alternating or intermingling colors like those of the rainbow, as in mother-of-pearl.
34
Iridescence - Opalescence
milky iridescence displayed by an opal
35
Iridescence - Schiller luster
A peculiar, nearly metallic luster, sometimes accompanied by iridescence, is observed on some minerals, as hyper-sthene, and due to internal reflection from microscopic inclusions: in some cases, this is an effect produced by alteration
36
Iridescence - Play of Colors
Brilliant flashes of color, against a white or black background. Series of colors as the angle of the incident light changes
37
Cleavage
the tendency of a mineral to break along smooth planes parallel to zones of weak bonding.
38
Cleavage - American System
Perfect, Good, Fair, Poor
39
Cleavage - # of Directions
1, 2, 3, 4, 6
40
Fracture
The breakage of minerals when they do not yield along cleavage of parting surfaces.
41
Fracture - Even
Even breakage
42
Fracture - Uneven
Rough and irregular surface
43
Fracture - Conchoidal
Smooth curved edges resembling the interior surface of a shell
44
Fracture - Fibrous/Splintery
It is fibrous or splintery
45
Fracture - Hackly
jagged and sharp edges
46
Parting
Like cleavage, but the surface has discontinuities and is not smooth, even fracture, different side lengths
47
Pyroelectric
Mineral develops electric charge when heated, used in heat detectors
48
Piezoelectricity
Electric charged developed under pressure, used to control radio frequencies. Discovered by the Curies, Pierre and Jacques
49
Non-centrosymmetric
When a material is not inversely symmetrical throughout its volume REQUIREMENT FOR PIEAZOELCTRICTY
50
Tensor
A linear mapping of a vector onto another vector
51
First-order (vector) through fourth order
1st order = Polarization vector, 3 components 2nd order = Stress tensor, 9 Components 3rd order = Piezoelectric modulus, 27 Components 4th order = 81 Components
52
Scaler
a Quantity specified by its magnitude only
53
Piezometer
a device used to measure liquid pressure in a system by measuring the height to which a column of the liquid rises against gravity, a measure of static pressure
54
electrostriction
a property of all electrical non-conductors, or dielectrics, that causes them to change their shape under the application of an electric field
55
Quartz oscillator
electronic oscillator circuit that uses the mechanical resonance of a vibrating crystal of piezoelectric material to create an electrical signal with a constant frequency. A watch
56
Radioactivity
the property possessed by some elements or isotopes of spontaneously emitting energetic particles by the disintegration of their atomic nuclei.
57
Acid Reaction
Fizzes to HCl indicates the presence of carbon/carbonate
58
Atom Proton Neutron Electron
Proton, neutron, electron In nucleus +1 In Nucleus 0 In the surrounding cloud -1
59
Cation
an ion with fewer electrons than protons, giving it a positive charge.
60
Anion
is an ion with more electrons than protons, giving it a net negative charge
61
Isotope
two or more types of atoms that have the same atomic number and position in the periodic table but different numbers of neutrons
62
Harold Urey
discovered deuterium, heavy isotope of hydrogen
63
Isotope - Stable
do not decay into other elements. (14C)`
64
Isotope - Unstable
Radioactive, decay into other elements
65
Marie Sklodowska–Curie
the first theory of radioactivity
66
Size of the atom and nucleus
Most of the volume consumed by electron cloud
67
Johann Balmer
Swiss mathematician, discovered Blamer lines AKA spectral lines, emission spectra of different elements contain discrete lines.
68
Bohr model of the atom
Niels Bohr, like planetary model, but with energy states instead of gravity
69
Quantum model of the atom
Uses standing waves and the Schrodinger equation. Wave-particle duality
70
Louis de Broglie
Predicted particles had wave-like properties
71
Schrödinger’s equation
gives the evolution over time of a wave function, cannot be solved only approximated
72
Principle quantum number, n
no limit (1,2,3) Related to angular momentum
73
Azimuthal quantum number, ℓ
(0,1,2,3)(n-1) Indicates symmetry of orbital. Determines e subshell
74
Magnetic quantum number, m
(0,±1,±2,±3,±L) Orientation of orbital in space
75
Spin quantum number, s
±1/2 Direction of e- rotation
76
Wolfgang Pauli
Austrian physicist who proposed the Pauli Exclusion Principle
77
The Pauli Exclusion Principle
No two fermions can occupy the same quantum state at the same time
78
Henry G.J. Moseley
English physicist Came up with the concept of atomic number
79
Alkali metals
Row I H down
80
Alkaline Earths
Row II
81
Halogens
Row 17 (Row before halogens)
82
Rare earth elements, REE
Row 3 and top row at bottom
83
Actinides
bottom row at bottom
84
Ionization energy
the minimum amount of energy required to remove the most loosely bound electron of an atom or molecule.
85
Chemical bonding - Ionic
between opposite charged particles, + ions form metals, - ions from non-metals. Moderate hardness, high melting, and boiling points. Poor conductors, unless near melting point.
86
Chemical Bonding - Covalent
When two elements share electrons. Diretional, Very high melting and boiling points. Does not yield ions to solution.
87
Chemical Bonding - Metallic
Sea of e- holds it together. Only native metals, Gold, Silver, Copper, and Platinum group are metallically bonded. Good conductors. Low hardness and melting point. Opaque
88
Chemical Bonding - H-Bonds
Requires electronegative elements which have lone pairs. H20 and ammonia. 1/10 the strength of covalent bonds. Constantly broken and reformed in H2O. Holds DNA together.
89
Van der Waals Bonding
Dispersion forces, and dipole forces. e- mobile and find themselves on one end of the molecule. "sloshing" around. Much weaker than covalent Bigger molecules have bigger boiling points. Ex// HCl

Mineralogy and Crystal Chem (3 decks)

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