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Mineralogy and Crystal Chem > Test 1 > Flashcards

Test 1 Flashcards

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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
Q

Luster - Non-met. -Silky

A

Appears as a skein of silk or a piece of satin. Fibrous aggregates. Ex// Fibrous Gypsum.

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26
Q

Luster - Non-met. - Earthy

A

Appears dull. Aggregates of very fine-grained materials. Ex// Goethite and Limonite.

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27
Q

Diaphaneity

A

The power of transmitting light

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28
Q

Diaphaneity - Transparent

A

Ability to see an object through the mineral, clear.

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29
Q

Diaphaneity - Translucent

A

Light transmits through mineral but objects not clear

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30
Q

Diaphaneity - Opaque

A

No light can get through, even on the thin edges

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31
Q

Color - Idiochromatic

A

Of the same color

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32
Q

Color - Allochromatic

A

Pertaining to change of color

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33
Q

Iridescence

A

exhibition of alternating or intermingling colors like those of the rainbow, as in mother-of-pearl.

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34
Q

Iridescence - Opalescence

A

milky iridescence displayed by an opal

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35
Q

Iridescence - Schiller luster

A

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

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36
Q

Iridescence - Play of Colors

A

Brilliant flashes of color, against a white or black background. Series of colors as the angle of the incident light changes

37
Q

Cleavage

A

the tendency of a mineral to break along smooth planes parallel to zones of weak bonding.

38
Q

Cleavage - American System

A

Perfect, Good, Fair, Poor

39
Q

Cleavage - # of Directions

A

1, 2, 3, 4, 6

40
Q

Fracture

A

The breakage of minerals when they do not yield along cleavage of parting surfaces.

41
Q

Fracture - Even

A

Even breakage

42
Q

Fracture - Uneven

A

Rough and irregular surface

43
Q

Fracture - Conchoidal

A

Smooth curved edges resembling the interior surface of a shell

44
Q

Fracture - Fibrous/Splintery

A

It is fibrous or splintery

45
Q

Fracture - Hackly

A

jagged and sharp edges

46
Q

Parting

A

Like cleavage, but the surface has discontinuities and is not smooth, even fracture, different side lengths

47
Q

Pyroelectric

A

Mineral develops electric charge when heated, used in heat detectors

48
Q

Piezoelectricity

A

Electric charged developed under pressure, used to control radio frequencies. Discovered by the Curies, Pierre and Jacques

49
Q

Non-centrosymmetric

A

When a material is not inversely symmetrical throughout its volume REQUIREMENT FOR PIEAZOELCTRICTY

50
Q

Tensor

A

A linear mapping of a vector onto another vector

51
Q

First-order (vector) through fourth order

A

1st order = Polarization vector, 3 components
2nd order = Stress tensor, 9 Components
3rd order = Piezoelectric modulus, 27 Components
4th order = 81 Components

52
Q

Scaler

A

a Quantity specified by its magnitude only

53
Q

Piezometer

A

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
Q

electrostriction

A

a property of all electrical non-conductors, or dielectrics, that causes them to change their shape under the application of an electric field

55
Q

Quartz oscillator

A

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
Q

Radioactivity

A

the property possessed by some elements or isotopes of spontaneously emitting energetic particles by the disintegration of their atomic nuclei.

57
Q

Acid Reaction

A

Fizzes to HCl indicates the presence of carbon/carbonate

58
Q

Atom
Proton
Neutron
Electron

A

Proton, neutron, electron
In nucleus +1
In Nucleus 0
In the surrounding cloud -1

59
Q

Cation

A

an ion with fewer electrons than protons, giving it a positive charge.

60
Q

Anion

A

is an ion with more electrons than protons, giving it a net negative charge

61
Q

Isotope

A

two or more types of atoms that have the same atomic number and position in the periodic table but different numbers of neutrons

62
Q

Harold Urey

A

discovered deuterium, heavy isotope of hydrogen

63
Q

Isotope - Stable

A

do not decay into other elements. (14C)`

64
Q

Isotope - Unstable

A

Radioactive, decay into other elements

65
Q

Marie Sklodowska–Curie

A

the first theory of radioactivity

66
Q

Size of the atom and nucleus

A

Most of the volume consumed by electron cloud

67
Q

Johann Balmer

A

Swiss mathematician, discovered Blamer lines AKA spectral lines, emission spectra of different elements contain discrete lines.

68
Q

Bohr model of the atom

A

Niels Bohr, like planetary model, but with energy states instead of gravity

69
Q

Quantum model of the atom

A

Uses standing waves and the Schrodinger equation. Wave-particle duality

70
Q

Louis de Broglie

A

Predicted particles had wave-like properties

71
Q

Schrödinger’s equation

A

gives the evolution over time of a wave function, cannot be solved only approximated

72
Q

Principle quantum number, n

A

no limit (1,2,3) Related to angular momentum

73
Q

Azimuthal quantum number, ℓ

A

(0,1,2,3)(n-1) Indicates symmetry of orbital. Determines e subshell

74
Q

Magnetic quantum number, m

A

(0,±1,±2,±3,±L) Orientation of orbital in space

75
Q

Spin quantum number, s

A

±1/2 Direction of e- rotation

76
Q

Wolfgang Pauli

A

Austrian physicist who proposed the Pauli Exclusion Principle

77
Q

The Pauli Exclusion Principle

A

No two fermions can occupy the same quantum state at the same time

78
Q

Henry G.J. Moseley

A

English physicist Came up with the concept of atomic number

79
Q

Alkali metals

A

Row I H down

80
Q

Alkaline Earths

A

Row II

81
Q

Halogens

A

Row 17 (Row before halogens)

82
Q

Rare earth elements, REE

A

Row 3 and top row at bottom

83
Q

Actinides

A

bottom row at bottom

84
Q

Ionization energy

A

the minimum amount of energy required to remove the most loosely bound electron of an atom or molecule.

85
Q

Chemical bonding - Ionic

A

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
Q

Chemical Bonding - Covalent

A

When two elements share electrons. Diretional, Very high melting and boiling points. Does not yield ions to solution.

87
Q

Chemical Bonding - Metallic

A

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
Q

Chemical Bonding - H-Bonds

A

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
Q

Van der Waals Bonding

A

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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