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GLE 2024 (Day 2) > MINERALOGY BASIC CONCEPTS (GEOCHEM OF MINERALS) > Flashcards

MINERALOGY BASIC CONCEPTS (GEOCHEM OF MINERALS) Flashcards

1
Q

Differentiate Monomineralic from Polyminerallic rock?

A

Naturally occuring,
Inorganic,
Homogenous solid
Defined chemical composition,
Orderly Cyrstal Structure, Solid

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2
Q

Basic pattern of atoms

A

Motif

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3
Q

long range pattern of atom characteristic of each mineral species

A

Crystal structure

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4
Q

Materials that possess geometric crystal structure

A

Crystalline

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5
Q

A solid material that lacks long range crystal structue

A

amorphous

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6
Q

Naturally ocuring solid which lack unique combination of crystal sturcture and chemical composition

A

Mineraloid

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7
Q

Examples of mineraloids

A

Volcanic Glass and Coal

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8
Q

What is a rock?

A

Aggregare of minerals crystals, and/or mineraloids

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9
Q

Differentiate Monomineralic from Polyminerallic rock?

A

A monomineralic is composed of cyrstals of a single minerals like quartzite, quartz sandstone and dunite (Purely OLivine) while polyminerallic are composed of many types of mineral crystals

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10
Q

How many m is 1 angstrom?

A

10^-10

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11
Q

1 amu (atomic mass unit or dalton) is how much in kg

A

1.661*10^-27

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12
Q

What’s the equivalent of 1amu?

A

1/12 mass of carbon atom

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13
Q

Mass of P, N and E?

A

P 1.000728 amu ,
N 1.000867 amu,
E 0.0000054 amu

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14
Q

No. of Protons which distinguishes atom of one element from that of another

A

Nucleus (Z,lower left)

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15
Q

What is the highest atomic number for naturally occuring elements?

A

Z=92, Uranium

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16
Q

No of Protons and Neutrons normally written at the upper left of the element

A

atomic mass

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17
Q

atomic mass of Oxygen

A

16 amu

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18
Q

Atoms of the same element which possess different atomic mass number?

A

Isotopes

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19
Q

H isotope with 0 neutron?

A

Protium 1H

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20
Q

H isotope with 2 atomic mass number (1neutron)?

A

Deuterium 2H

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21
Q

H isotope with 3 atomic mass number (2 neutron)?

A

Tritium 3H

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22
Q

Isotopes of oxygen?

A

16,17,18

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23
Q

Average atomic mass of an element?

A

Weighted average for all the isotopes
(e.g: O16, O17, O18)

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24
Q

Differentiate Stable Isotopes and Radioactive isotopes?

A

Stable isotopes have stable nuclei and remain unchanged which means they retains same number of protons and neutrons over time, on the other hand, Radioactive isotopes have unstable nuclear configuration w/c changes overtime via decay processes

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25
Q

3D configuration or shapes of electron clouds

A

Orbitals

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26
Q

This siginifies the principal quantum energy level or shell in which a particular electron occurs usually numbered from 1-7

A

Principal quantum number (n)

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27
Q

This signify the directional quantum energy region or subshell in which electron occurs usually labeled s,p,d,f

A

Azimuthal quantum number

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28
Q

Whats the max electron for S,P,D,F (by 4s)

A

2,6,10,14

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29
Q

Stable Octet

A

S2, P6 electron configuration

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30
Q

Elements with completely filled shells and S-andPshells that have very stable electron configuration

A

Helium
Neon
Argon
Krypton

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31
Q

Tables which attempt to portray the periodic behavior of elements

A

Periodic table of elements

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32
Q

What do the numbers on the left side of the table represents

A

Rows/Periods Numbers 1-7- indicate highest Principle Quantum Level (Energy level of the valence electrons of elements in that row) or the highest ground state quantum level

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33
Q

How are elements classified in each row?

A

Their position depends on the distribution of electrons w/in principal quantum levels

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34
Q

HOw are elements classified into columns/group?

A

By their tendency to lose or gain electrons forming positive or negative charged ions

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35
Q

electrically charge atoms?

A

ions

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36
Q

process by which atoms acquire charge?

A

ionization

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37
Q

The amount of energy required to remove an electron from its electron cloud

A

Ionization Energy (kjoules/mole)

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38
Q

Elemetns which relatively low first ionization energy and tend to lose one or more electrons

A

Electropositive Elements

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39
Q

Elements which high first ionization energy

A

Electronegative Elements

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40
Q

positivey charged ions in which P>e, they lose electrons and their charhe s equal to the number of excess proton P-e

A

Cation

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41
Q

Negatively chaged ion that has a charge equal to the umber of excess electron, gains electron

A

Anion

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42
Q

Compare and contrast ionization energies of Metallic and nonmetallic elements

A

Metallic elements have low ionization energy electronpositive elements and thus tend to give up one or more weakly held electrons while NonMetallic elements have high first ionization energy electronegative elements and thus tend to absorn loosely bound electrons

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43
Q

Metallic

A

Low first Ionization Energy (Madaling Bumitaw) (<900 kJ/mol)electropositive

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44
Q

Non Metallic

A

High first Ionization Energy (Linta ayaw Bumitaw) (>900 kL/mol), Have high electron affinity and tend to be electronegative

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45
Q

These are monovalent cations due to low first ionization energy tend to lose 1 electron to be stable

A

1 (IA)

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46
Q

These are divalent cations tend to lose 2 electron

A

2 (IIA)

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47
Q

These elements lose variable number of electrons depending upon the environments

A

Transition elements 3-12 (IIIB-IIB)
(8-10, VIIIB)

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48
Q

Elements which lose three electrons

A

13 (IIIA)

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49
Q

Elements which lose four electron or small number of electrons

A

14 (IVA)

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50
Q

Elements which lose five electrons or capture 3 electrons

A

15 (VA)

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51
Q

Gain two electrons or six in some environments

A

16 (VIA)

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52
Q

Gain 1 electrons

A

17 (VIIA)

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53
Q

Stable electron configuration

A

18 (VIIIA)

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54
Q

Elements in the middle of the periodic table are chracterized by

A

Electropositive
tend to lose various numbers of electrons to become ccations

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55
Q

This is the half distance between the nuclei of bonded identical neighboring atoms

A

Atomic Radii

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56
Q

Whats the trend of atomic radii in columns and rows?

A

1-7 increading from top to bottom, decreases from left to right

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57
Q

These are electrons in the outermost shell which are the least bound to the nucleaous and are usually involved in wide variety of chemical reactions especially in ionization processes

A

Valence Electrons

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58
Q

When atoms are charged their radius becomes?

A

Ionic radii

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59
Q

Relationship of charge of cations an its radii?

A

higher the charge smaller the radius

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60
Q

ralationship of charge of anion and its effective radii?

A

higher the charge the larger the radius

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61
Q

Sodium

A

1.86 A

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62
Q

Calcium

A

1.97 A

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63
Q

Aluminum

A

1.46 A

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64
Q

Silicon

A

1.18 A

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65
Q

Iron

A

1.23 A

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66
Q

Nitrogen

A

0.75 A

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67
Q

Oxygen

A

0.73 A

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68
Q

Flourine

A

0.72 A

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69
Q

forces which held together atoms in minerals and rocks and strongly influence the properties and behavior of minerals, rocks, and other Earth materials

A

Chemical bonds

70
Q

Bonds which links together metallic and non metallic elements?

A

Ionic or electrostatic

71
Q

non metallic to non metallic bonds

A

Covalent bonds

72
Q

Metallic to metallic bonds

A

Metallic bonds

73
Q

This is an empirical measure of the tendency of an element to attract electrons when atoms bonds

A

Electronegativity (En)

74
Q

The measure of energy released when an electron is added to an unbound atom

A

Electron Affinity

75
Q

Energy required to remove an electron from an ion

A

Ionization energy

76
Q

This happens when very metallic atoms bond with very non-metallic atoms by Metallic atoms give up or donate their valence electrons to non metallic atoms

A

Electrostatic bond or ionic bonds

77
Q

What columns in the periodic table are very metallic atoms and tend to be cations

A

Columns 1 and 2

78
Q

What columns in the periodic table are very non metallic and tend to be anion

A

Columns 16 an 17

79
Q

Ionic pairs in the periodic table

A

IA and VII A, IIA and VIA

80
Q

What are the properties of crystal with ionic bond?

A

Variable hardness, Brittle, quite solube in polar substances, intermediate melting temp, transparent to transluscent minerals with light colors and virteous to sub-vitreous luster

81
Q

When non-metallic atoms bond with non metallic atoms and share electrons?

A

Covalent Bonds

82
Q

diatomic gases with covalent bonding

A

O, Cl, F, I, N

83
Q

Mineral with covalent bonding

A

Diamond

84
Q

What column is carbon and its implication?

A

Column 14 IVA, C tends to absorb or donate 4 electrons

85
Q

Properties of covalently bonded minerals?

A

Hard and brittle, insoluble in water, crystallize from metls, moderate to high melting temp, tranparent to translucent with vitreous, subvitreous and adamantine lusters

86
Q

Bonding of metallic to metallic atoms which is usally protrayed as positivelt chargen atoms in a matrix of delocalized valance electrons and are only temporarily associated with individual atoms

A

Metallic

87
Q

Properties of Minerals with metallic bond

A

failrly soft and moderately hard, plastic, malleable and ductile, excellent electrical and thermal condctors, frequently high SG, excellent absrobers and refletors of light commonly opaque with metallic luster

88
Q

The difference between the electronegativities of two elements sharing the bond

A

Electronegativity difference

89
Q

When does transitional bond become dominantly ionic or dominantly covalent?

A

<1.68 En.D. dominantly covalent,
>1.68 En.D. dominantly ionic

90
Q

Mineral which have a transitional bond of ionic-metallic which gives it brittle and soluble property and soft, opaque and metallic luster dominantly metallic?

A

Galena (PbS)

91
Q

Mineral which have a transitional bond between metallic and covalent?

A

Pyrite

92
Q

What type of hybrid is Silica minerals?

A

Covalent-Ionic (En: 1.54) dominantly covalent

93
Q

Minerals which have a transional ionic-covalent but are dominantly ionic?

A

Halite

94
Q

Bond which is caused by weak electric dipole forces which are caused by assymetrical distribution of electrons in the electron cloud

A

Van der waals

95
Q

Characteristic of Van de Waals bonding

A

Very weak and soft like
Talc and graphite

96
Q

A bond which exists between hyrdogen or hydroxyl ion and an electronegative ion and is relatively weak which occur in hydrated or hydroxyl minerals

A

Hydrogen bonds

97
Q

These are rules describing anion-cation relationships in ionically bonded substancs

A

Pauling’s Rule

98
Q

Who established these rules?

A

Linus Paulings 1929

99
Q

What is Rule #1?

A

1.1 The distance between anion and cation in a polyhedron is the sum of their radii (Radium Sum)
1.2 the number of coordinated anions is determined by cation:anion ratio

100
Q

What is Rule#2?

A

Elecrostatic valency rule
When the sum of the strength of the bonds that join cation and anion in the polyhedron is equals to the charge on the cation and anion, then the ionic structure is stable

101
Q

What is Rule #3?

A

Sharing of edges and particularly faces of adjacent anions decreases the stability of an ionic structure since similar charges tend to repel. Ajdacent polyhedra tend to share corners rather than edges

102
Q

What is Rule#4?

A

Cations with high valence electrons and small cooridnation number tend not to share polyhedral elements since their charges tend to repel

103
Q

What is Rule#5?

A

Rule of Parsimony - the number of different cations and anions in a crystal structure tends to be small

104
Q

Coordination Polyhedra

A

the basic unit of Crystal Structure which are Clusters of atoms or ions bonded together to other coordinating atoms

and that Creates a link between crystal structure and crystal chemistry

105
Q

Cordination Number

A

The number of nearest neighbor ions or atoms on which the depended on the Radius Ratio

106
Q

What is Radius Ratio RR?

A

Rc/Ra

107
Q

Caveats of predicting CN using RR

A

1) Increasnig effective Ionic Radius means increasing CN
2) the more a bond becomes covalent or polaried, RR becomes ineffective to predict CN
3) RR is not applicable to Metallic Bonds

108
Q

Peaks of RR

A

0.155 0.225 0.414 0.732 1.00

109
Q

If the RR <0.155 what is CN and the Coordination Polyhedra?

A

2, Line

110
Q

If RR is 0.155-0.225, what is CN and coordination polyhedra?

A

3, Triangle

111
Q

If RR is 0.255-0.414, what is CN and coordination polyhedra?

A

4, Tetrahedron

112
Q

If RR is 0.414-0.732 what is CN and CP?

A

6, Octahedron

113
Q

If RR is 0.732 - 1.00 what is CN an CP?

A

8, Cube

114
Q

if RR is >1.00, what is CN and CP?

A

12, cubeoctahedron complex

115
Q

Concept of Electrostatic Valency

A

EV evokes that the charge of a cation and anion is balanced by the electrostatic charge compensating of the bonds between them. Formula is EV= Z (Charge)/CN

116
Q

EV formulaz

A

EV=Z / CN

117
Q

The most common minerals in the Earth’s crust and upper mantle

A

Silicates

118
Q

Native Elemen

A

none

119
Q

Halides

A

F-1, Cl-1, Br-1

120
Q

Sulfides

A

S-2, S-4

121
Q

Arsenides

A

As-2, As-3

122
Q

Sulfarsenides

A

As-2, As-3 and S-2 or S-4

123
Q

Selenides

A

Se-2

124
Q

Tellurides

A

Te-2

125
Q

Oxides

A

O-2

126
Q

Hydroxides

A

(OH)-1

127
Q

Carbonates

A

(CO3)-2

128
Q

Nitrates

A

(NO3)-1

129
Q

Borates

A

(BO3)-3 and (BO4)-5

130
Q

Sulfates

A

(SO4)-2

131
Q

Phosphates

A

(PO4)-3

132
Q

Chromates

A

(CrO4)-5

133
Q

Arsenates

A

(AsO4)-3

134
Q

Vandates

A

(VO4)-3

135
Q

Molybdates

A

(MoO4)-2

136
Q

Tungstates

A

(WO4)-2

137
Q

Silicates

A

(SiO4)-4

138
Q

Silica

A

No of shared Oxygen Ions

139
Q

Nesosilicates

A

0

140
Q

Sorosilicates

A

1

141
Q

Cyclosilicates

A

2

142
Q

Inosilicates Single Chain

A

2

143
Q

Inosilicates Double Chain

A

2-3 alternately

144
Q

Phyllosilicates

A

3

145
Q

Tectosilicates

A

4

146
Q

Substitution is favored when radius difference is within this range at Normal Surface Temp

A

10-15%

147
Q

When cation radii exceed this mark, cation substitution becomes negligible

A

30%

148
Q

when can Larger difference in radius be possible in cationic substitution

A

at higher temps

149
Q

when does two or more substitution happen?

A

When there are multple coordination sites

150
Q

Favorable Conditios for subtitutions

A

1) Same Ionic Radii or small differnce
2) Same Charge or can be different charge if there are multiple site
3) Ions are widely available in the environment at which the mineral is growing

151
Q

This exist when two or more ions of similar radius and charge substitute for one another in a coordination site in any proportion

A

Simple Complete Substitution

152
Q

Mg ionic radius

A

0.66 Angstroms

153
Q

Fe ionic Radius

A

0.74 Angstroms

154
Q

When two end members can substitute for one another in any proportion this solid solution exists

A

Complete Solid Solution Series

155
Q

a line which can represent two component solid soln series

A

Tie Line

156
Q

Three end members of pure carbonates

A

siderite, Magnesite and Rhodocrosite

157
Q

Involves Simultaneous substitution of ions of different charges in two different structureal sites that preserves electric neutrality of the crystal lattice

A

Coupled Ionic Subtitution

158
Q

Best example for Coupled Ionic Substitution

A

Plagioclase

159
Q

Whats different in Na and Ca

A

Charge Na+1 Ca+2

160
Q

What neutralized the charge imbalance caused by the substitution of Na+1 and Ca+2?

A

Substitution of Al+3 and Si+4

161
Q

What ions are in tandem during ionic couples subsitution

A

(Na+1 and Si+4)
(Ca+2 and Al+3)

162
Q

General Chemical Formular for Plag

A

(Na,Ca)(Si,Al) AlSi2O8

163
Q

Pure Sodium Plag

A

Albite (NaAlSi3O8)

164
Q

Pure Calcium Plag

A

Anorthite (CaAl2Si2O8)

165
Q

In a tie line where does albite and anorthite positioned

A

Left end and right end respectively

166
Q

A substitution involving ions of substantially different size that limits the amount of substitution between end members

A

Limited Solid Solution

167
Q

examples of Limites Solid Soln

A

Magnesite and Calcite

168
Q

Gaps in solid solutions which represents potential compositions that do not exist in nature due to limited substituition

A

Miscibility Gaps

169
Q

Miscibility Gap between Clacite Magnesite Tie Line

A

Ct75Ms25 to Ct60Ms40
60-75% Ca
25-45% Mg

170
Q

Low Mg Calcite

A

Less than 4% Mg >96% Ca

171
Q

High Mg Clacite

A

4-25% Mg (Ct75-96 and Ms4-25)
75-96% Ca

172
Q

Carbonates with composition Ms40-55 and Cs45-60

A

Dolomite (40-55% Mg, 45-60% Ca)

GLE 2024 (Day 2) (41 decks)

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