z = proton number = atomic number n = neutron number a = mass number (z+n)

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)

•Pauli exclusion principle•Hunds rule

Electrons & orbitals

•Aufbau principle

•Charges•Ionization potential

More stable:Filled shellsFilled subshellsFilled and half filled orbital types

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

Electronegativity = (sum of IP & EA) x constant

Electronegativity difference of 1.7 = 50% ionic character

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

Goldschmidt’s classification

Covalent bond character – hybrid orbitals form

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

Ionic Radii

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)

Common silicates and oxides:

CN = 4 (Si, Al)CN = 6 (Mg, Fe)CN = 8 (Ca, Na)

In mantle:olivine, orthopyroxene,clinopyroxene, spinel, garnet

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

Mineral/melt partition or distribution coefficients

Ionic radius

KD = concentration in mineral concentration in liquid

Eu has two valences:Eu+2 and Eu+3

You can calculate partition coefficients for any element in any mineral from the radius of the mineral site and elastic properties of the mineral.

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

Increasing compatibility for mantle melting

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)

Water and Aqueous solutions

Ionic potential

= field strength

= charge/radius

Residence time = Total mass of element in reservoir (oceans)/influxGrams/(grams/year)

Basalts from subduction zones – island arc basalt

Fluid mobile elements (FME) = Rb, Ba, K, Pb, SrFluid immobile elements = Nb,Ta, Zr (Hf), Ti