z = proton number = atomic number n = neutron number a = mass number (z+n) atomic mass of nuclide =...
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Z = proton number = atomic numberN = neutron number A = mass number (Z+N)
Atomic mass of nuclide = (rest mass – binding energy) relative to 1/12 mass of 12C atom, measured in atomic mass units – amu’s (must be looked up)
Atomic weight of element = sum of the masses of the isotopes of that element times their atomic abundance (found in most textbooks)
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•Pauli exclusion principle•Hunds rule
Electrons & orbitals
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•Aufbau principle
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•Charges•Ionization potential
More stable:Filled shellsFilled subshellsFilled and half filled orbital types
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Ionization potential = energy required to remove an electron
Electron affinity = energy given off when adding an electron to a neutral atom
S and px, py and pz orbitals
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Electronegativity = (sum of IP & EA) x constant
Electronegativity difference of 1.7 = 50% ionic character
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Electronegativity differences: Examples: >2.1 - high ionic character (electrons exchanged) halite, Mg-O, Ca-O, K-O, Na-O bonds in silicates,
carbonates and other oxidiized complex anions1.6-2.1 - metal and non-metal - weak ionic character Fe-O, also Ti, V, Cr-O bonds in silicates1.6-2.1 - nonmetals - polar covalent bond Rare (except for Si-O)0.5-1.6 - polar covalent bond Fe-S, also Ni, Cu, Pb, Hg bonds in sulfides
also C-O, S-O, Si-O, P-O, N-O in complex ions<0.5 - nonmetals - non -polar covalent bond Graphite, sulfur, realgar, orpiment,
<0.5 - high electronegativity metals Gold, silver, platinum group, metallic bonding
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Goldschmidt’s classification
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Covalent bond character – hybrid orbitals form
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Ionic bonding produces close-packed structures. There is a balance between attraction of oppositely charged ions and repulsion by outer electrons on both.
Radius ratio = radius of cation/anion in a bond. Thisdetermines the coordinationnumber
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Ionic Radii
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Crystal field splitting – orbitals change energy in a surrounding crystal lattice
Leads to high spin (larger radius) and low spin electron configurations
Produces color in minerals
(example Fe+3 with 5 d electrons)
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Common silicates and oxides:
CN = 4 (Si, Al)CN = 6 (Mg, Fe)CN = 8 (Ca, Na)
In mantle:olivine, orthopyroxene,clinopyroxene, spinel, garnet
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In the earth, abundant elements form minerals with specific coordination polyhedra or sites. Minor elements either substitute or form rare minerals.
The ability to substitute is controlled by:1) radius; 2) charge (valence); 3) electronegativity (bonding behavior)
Contours are enrichment in crust/mantle
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Mineral/melt partition or distribution coefficients
Ionic radius
KD = concentration in mineral concentration in liquid
Eu has two valences:Eu+2 and Eu+3
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You can calculate partition coefficients for any element in any mineral from the radius of the mineral site and elastic properties of the mineral.
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Continental crust is complement to depleted mantle
Bulk partition coefficient = sum of each mineral Kd X the abundance of the mineral during melting or crystallization
Bulk Kd > 1 – element is compatible, Bulk Kd < 1 - incompatible
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Increasing compatibility for mantle melting
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Kinds of incompatible trace elements:Rb, K, Ba, Sr = large ion lithophile elements (LILE)Th, U, Zr, Hf, Nb = high field strength elements (HFSE) (Field strength = charge/ionic radius)
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Water and Aqueous solutions
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Ionic potential
= field strength
= charge/radius
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Residence time = Total mass of element in reservoir (oceans)/influxGrams/(grams/year)
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Basalts from subduction zones – island arc basalt
Fluid mobile elements (FME) = Rb, Ba, K, Pb, SrFluid immobile elements = Nb,Ta, Zr (Hf), Ti
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