Introduction Flashcards
Mineralogy
Characterizes properties and chemical composition of minerals and studies the conditions of their formation.
Mineral Definition
1) Naturally occurring 2) Homogeneous solid 3) Inorganically formed 4) Definite chemical composition 5) Highly ordered atomic arrangement
Homogeneous solid
Excludes gases and liquids The mineral has same composition throughout its volume, regardless of location sampled.
Highly Ordered Atomic Arrangement
Internal framework of atoms/ions arranged in regular repeating geometric pattern.
Amorphous
Solids that lack an ordered atomic arrangement
Atom Representation
A
X
Z
A-mass number, sum of protons and nuetrons Z-atomic number, number of protons
Isotope
Atoms of the same element with same number of protons but differing number of neutrons
Alkali Metals
First column of periodic table. One valence electron each. Highly reactive and not found in elemental form in nature.
Earth Metals
Second column of periodic table. 2 valence electrons each. High melting temp, remain solids in fires. Silver colored, soft metals that react with halogens and water to form alkaline hydroxides.
Transition Metals
Middle block of periodic table. Varying Valence electrons Have multiple oxidation states, loss of d orbital electron with no high energy penalty. Often found as colored compounds.
Other metals
Lower step portion of right side of periodic table. Varying Valence Electrons. Melting/boiling points lower than transitional metals. Distinguished from metalloids b/c of high boiling points in same row.
Non-Metals
Upper step portion of right side of periodic table. Varying Valence Electrons. Behave as semiconductors. Staircase marks poor metals(left and down) and nonmetals(right and up). Halogens highly reactive.
Noble Gases
Far right column of periodic table. 8 Valence electrons each. Colorless, odorless, monatomic gases with very low chemical reactivity under standard conditions.
Rare Earth Elements
Lower block of periodic table. Varying valence electrons. Positive metals that react violently with most nonmetals. Actinoids exhibit a wide range of oxidation states and are radioactive.
1) Electron donors 2) Electron acceptors
1) metals (left side of periodic table) 2) non-metals (right side of periodic table)
Ionic Bonds
1 or more e- transferred from metal to nonmetal atom. Attraction between oppositely charged ions. Example: Halite (NaCl)
Metallic Bond
Attractive force between positive nuclei and negative valence electron holds these crystal structures together. Mobile e- gives high electrical and thermal conductivity of metals. Electrostatic attraction of atoms in a metal cause atom to surround itself by as many neighbors as geometrically possible.
Covalent Bond
2 or more atoms share outer valence electrons. Intermediate bond type between ionic and metallic. Force from mutual sharing of e-, involving overlap orbitals. Strongest chemical bond.
Van der Waals Bond
Residual surface charges give force of bond. ‘weak dipole effect’ Effective over large distance Weakest chemical bond, usually defines zone of cleavage.
Hydrogen Bond
Electrostatic bond between Hydrogen ion and negatively charged ion. Stronger than Van der Waals. Relatively strong material results from many of these weak bonds.
Crust
Silicates, Carbonates, Oxides, Hydroxides, Phosphates and Sulfates. Almost entirely Oxygen compounds. Silicon and Aluminum rich
Mantle
Silicon poor Magnesium/Iron rich Dominated by Olivine and Pyroxene.
Core
Liquid outer core primarily Iron and 2% Nickel. Solid inner core Iron and 20% Nickel. Density 9.9 g/cm3
Electron Configuration
