Introduction

Question 1

Mineralogy

Answer 1

Characterizes properties and chemical composition of minerals and studies the conditions of their formation.

Question 2

Mineral Definition

Answer 2

1) Naturally occurring 2) Homogeneous solid 3) Inorganically formed 4) Definite chemical composition 5) Highly ordered atomic arrangement

Question 3

Homogeneous solid

Answer 3

Excludes gases and liquids The mineral has same composition throughout its volume, regardless of location sampled.

Question 4

Highly Ordered Atomic Arrangement

Answer 4

Internal framework of atoms/ions arranged in regular repeating geometric pattern.

Question 5

Amorphous

Answer 5

Solids that lack an ordered atomic arrangement

Question 6

Atom Representation

Answer 6

A

X

Z

A-mass number, sum of protons and nuetrons Z-atomic number, number of protons

Question 7

Isotope

Answer 7

Atoms of the same element with same number of protons but differing number of neutrons

Question 8

Alkali Metals

Answer 8

First column of periodic table. One valence electron each. Highly reactive and not found in elemental form in nature.

Question 9

Earth Metals

Answer 9

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.

Question 10

Transition Metals

Answer 10

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.

Question 11

Other metals

Answer 11

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.

Question 12

Non-Metals

Answer 12

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.

Question 13

Noble Gases

Answer 13

Far right column of periodic table. 8 Valence electrons each. Colorless, odorless, monatomic gases with very low chemical reactivity under standard conditions.

Question 14

Rare Earth Elements

Answer 14

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.

Question 15

1) Electron donors 2) Electron acceptors

Answer 15

1) metals (left side of periodic table) 2) non-metals (right side of periodic table)

Question 16

Ionic Bonds

Answer 16

1 or more e- transferred from metal to nonmetal atom. Attraction between oppositely charged ions. Example: Halite (NaCl)

Question 17

Metallic Bond

Answer 17

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.

Question 18

Covalent Bond

Answer 18

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.

Question 19

Van der Waals Bond

Answer 19

Residual surface charges give force of bond. ‘weak dipole effect’ Effective over large distance Weakest chemical bond, usually defines zone of cleavage.

Question 20

Hydrogen Bond

Answer 20

Electrostatic bond between Hydrogen ion and negatively charged ion. Stronger than Van der Waals. Relatively strong material results from many of these weak bonds.

Question 21

Crust

Answer 21

Silicates, Carbonates, Oxides, Hydroxides, Phosphates and Sulfates. Almost entirely Oxygen compounds. Silicon and Aluminum rich

Question 22

Mantle

Answer 22

Silicon poor Magnesium/Iron rich Dominated by Olivine and Pyroxene.

Question 23

Core

Answer 23

Liquid outer core primarily Iron and 2% Nickel. Solid inner core Iron and 20% Nickel. Density 9.9 g/cm3

Question 24

Electron Configuration

Answer 24