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Quiz Two (9:30-9:35 AM) UNIVERSITY OF SOUTH ALABAMA GY 111: Physical Geology Lecture 4: Basic Mineral Chemistry Instructor: Dr. Douglas W. Haywick Last Time 1. Introduction to rocks 2. The Rock Cycle Rocks Rocks are naturally occurring solids containing one or more minerals. e.g., Granite Rocks We recognize 3 major rock groups: 1) Igneous (“born of fire”); originally molten 2) Sedimentary; originally particulate material or produced from precipitation out of water 3) Metamorphic; pre-existing rocks modified by pressure or temperature Igneous Rocks Can be either extrusive (volcanic) or intrusive (plutonic): Extrusive (volcanic) rocks can be erupted as lava… Sedimentary Rocks We recognize 4 major classes of sedimentary rocks: 1) Siliciclastic: composed of broken bits of silicate minerals 2) Biochemical: mostly composed of the remains of calcium carbonate-secreting beasties 3) Chemical; formed through chemical precipitation alteration 4) Organic; formed from plant material Peat bog Metamorphic Rocks We recognize 3 divisions of metamorphic rocks: 1) Foliated; display a prominent layering 2) Non-foliated; do not display layering 3) Cataclastic; composed of broken up bits of rock mylonite The Rock Cycle The Rock Cycle The Rock Cycle Igneous Loop Metamorphic Loop Sedimentary Loop Today’s Agenda 1. Elementary Chemistry (atomic structure) 2. Isotopes 3. The Periodic Table 4. Bonding Web notes 4: Why Chemistry in GY 111… Why Chemistry in GY 111… Math Physics Geology Chemisty Biology Why Chemistry in GY 111… Math Physics Geology Geochemistry Chemisty Biology Fluorite: CaF2 Copper: Cu Calcite: CaCO3 Source: csm.jmu.edu Fluorite: CaF2 Copper: Cu Calcite: CaCO3 Source: csm.jmu.edu Basic Chemistry •Geologists need to understand chemistry because minerals (and the rocks that contain them) are chemical compounds Basic Chemistry •The origins of chemistry go way back to prehistoric times Basic Chemistry •The origins of chemistry go way back to prehistoric times •Alchemists identified 4 “elements” (basic building blocks of everything) 1) Fire 2) Water 3) Earth 4) Air Basic Chemistry •The origins of chemistry go way back to prehistoric times •Alchemists identified 4 “elements” (basic building blocks of everything) 1) Fire A worthwhile quest, 2) Water but completely wrong 3) Earth 4) Air Basic Chemistry Halite NaCl Basic Chemistry Halite NaCl Basic Chemistry Halite NaCl Basic Chemistry Halite NaCl Basic Chemistry Halite NaCl Basic Chemistry Halite NaCl Basic Chemistry Halite NaCl 0.0000000001 m Atoms & Atomic Particles Na Cl • The sodium-chlorine pairing is called a molecule Atoms & Atomic Particles Na Cl • The sodium-chlorine pairing is called a molecule • Molecules are composed of uncharged atoms and/or charged atoms (ions) Atoms & Atomic Particles Na Cl • The sodium-chlorine pairing is called a molecule • Molecules are composed of uncharged atoms and/or charged atoms (ions) • An atom is the smallest component of an element that can retain the properties of that element Atoms & Atomic Particles • Atoms are composed of 3 fundamental particles: 1) Protons 2) Neutrons 3)Electrons Atoms & Atomic Particles • Atoms are composed of 3 fundamental particles: 1) Protons 2) Neutrons 3)Electrons • Protons & Neutrons always reside in the center of the atom termed the nucleus Nucleus (Protons + Neutrons) Atoms & Atomic Particles • Atoms are composed of 3 fundamental particles: 1) Protons 2) Neutrons 3)Electrons • Protons & Neutrons always reside in the center of the atom termed the nucleus • Electrons are always located in the electron cloud in complex orbitals where they “orbit” the nucleus Electron Cloud (Electrons) Nucleus (Protons + Neutrons) Atoms & Atomic Particles • Proton: has a mass of 1 and a positive charge (+) • Neutron: has a mass of 1 and a neutral charge (o) • Electron: has a mass of 0 and a negative charge (-) Atoms & Atomic Particles • Proton: has a mass of 1 and a positive charge • Neutron: has a mass of 1 and a neutral charge • Electron: has a mass of 0 and a negative charge This is not entirely correct (at least as far as mass is concerned) Atoms & Atomic Particles • Proton: has a mass of 1 and a positive charge • Neutron: has a mass of 1 and a neutral charge • Electron: has a mass of 0 and a negative charge • The number of protons and neutrons in the nucleus is variable and defines the different chemical elements (refer to the periodic table) Atoms & Atomic Particles • Proton: has a mass of 1 and a positive charge • Neutron: has a mass of 1 and a neutral charge • Electron: has a mass of 0 and a negative charge • The number of protons and neutrons in the nucleus is variable and defines the different chemical elements (refer to the periodic table) • For an uncharged atom: # of protons = # of electrons Atoms & Atomic Particles Hydrogen: 1 proton, 1 electron Atoms & Atomic Particles Helium: 2 protons, 2 neutrons, 2 electrons Atoms & Atomic Particles Carbon: 6 protons 6 neutrons 6 electrons Atomic Number & Weight • Atomic Number: the sum of the protons in the atom; The number uniquely identifies the element. Hydrogen = 1 Helium = 2 Carbon = 6 Atomic Number & Weight • Atomic Number: the sum of the protons in the atom; The number uniquely identifies the element. • Atomic Weight: the sum of the protons and neutrons in the nucleus of the atom Hydrogen = 1 Helium = 4 Carbon = 12 Atomic Number & Weight • By convention, we put both numbers on a letter that symbolizes that particular element: 1H1 2He4 6C12 Atomic Number & Weight • By convention, we put both numbers on a letter that symbolizes that particular element: 1H1 2He4 Atomic Number Atomic Weight 6C12 Isotopes • The number of protons and electrons for an element does not vary, but the number of neutrons can. Isotopes • The number of protons and electrons for an element does not vary, but the number of neutrons can. e.g., hydrogen + - 1H1 Proton Neutron - Electron Isotopes • The number of protons and electrons for an element does not vary, but the number of neutrons can. e.g., hydrogen + - - 1H1 1H2 Proton Neutron - Electron Isotopes • The number of protons and electrons for an element does not vary, but the number of neutrons can. e.g., hydrogen + - - - 1H1 1H2 1H3 Proton Neutron - Electron Isotopes • The number of protons and electrons for an element does not vary, but the number of neutrons can. e.g., hydrogen + - - - 1H1 1H2 1H3 Stable Unstable Ions Ions • When an atom in its elemental state receives or gives up one or more electrons it is then termed an “ion” Ions • When an atom in its elemental state receives or gives up one or more electrons it is then termed an “Ion” • Positively charged ions are cations Ions • When an atom in its elemental state receives or gives up one or more electrons it is then termed an “Ion” • Positively charged ions are cations • Negatively charged ions are anions Ions • When an atom in its elemental state receives or gives up one or more electrons it is then termed an “Ion” • Positively charged ions are cations • Negatively charged ions are anions • The ability to give up or take on electrons in an atom is dependent on the atomic number (i.e. the number of electrons in the electron shells) Simple atomic structure: Simple atomic structure: The Bohr atomic model Source:http://www.amptek.com/xrf_3.gif Simple atomic structure: Source:http://www.amptek.com/xrf_3.gif Level (n) "Name" # of electrons (2n2) 1 K 2 2 L 8 3 M 18 4 N 32 5 O 50 The Periodic Table The Periodic Table 1 electron in outer shell The Periodic Table 2 electrons in outer shell 1 electron in outer shell The Periodic Table 3 Es in outer shell 2 electrons in outer shell 1 electron in outer shell The Periodic Table 4 Es in outer shell 3 Es in outer shell 2 electrons in outer shell 1 electron in outer shell The Periodic Table 5 Es in outer shell 4 Es in outer shell 3 Es in outer shell 2 electrons in outer shell 1 electron in outer shell The Periodic Table 6 Es in outer shell 5 Es in outer shell 4 Es in outer shell 3 Es in outer shell 2 electrons in outer shell 1 electron in outer shell The Periodic Table 7 Es in outer shell 6 Es in outer shell 5 Es in outer shell 4 Es in outer shell 3 Es in outer shell 2 electrons in outer shell 1 electron in outer shell The Periodic Table 8 electronss in outer shell 7 Es in outer shell 6 Es in outer shell 5 Es in outer shell 4 Es in outer shell 3 Es in outer shell 2 electrons in outer shell 1 electron in outer shell The Periodic Table Chemical Bonding Chemical Bonding Occurs through the action of the electrons in the outer shells of atoms. Chemical Bonding Occurs through the action of the electrons in the outer shells of atoms. Partially filled shells are less stable (higher energy) than filled shells (lower energy) Chemical Bonding Occurs through the action of the electrons in the outer shells of atoms Partially filled shells are less stable (higher energy) than filled shells (lower energy) Level (n) "Name" # of electrons (2n2) 1 K 2 2 L 8 3 M 18 4 N 32 5 O 50 Chemical Bonding Occurs through the action of the electrons in the outer shells of atoms. Partially filled shells are less stable (higher energy) than filled shells (lower energy) Chemical reactions forming molecules strive to fill shells in atoms Level (n) "Name" # of electrons (2n2) 1 K 2 2 L 8 3 M 18 4 N 32 5 O 50 Already have filled shells Gain 1 electron Gain 2 electrons Gain 3 electrons Loose/gain 4 Es Loose 3 electrons Loose 2 electrons Loose 1 electron Chemical Bonding Chemical Bonding Chemical Bonding Three Major types: Chemical Bonding Three Major types: 1) Ionic bonding; exchange of electrons between atoms to form ions Na Cl Chemical Bonding Three Major types: 1) Ionic bonding; exchange of electrons between atoms to form ions Na Cl Chemical Bonding Three Major types: 1) Ionic bonding; exchange of electrons between atoms to form ions Na+ Cl- Ionic Radius Source:http://intro.chem.okstate.edu Determines the length of chemical bonds Chemical Bonding Three Major types: 1) Ionic bonding; exchange of electrons between atoms to form ions 2) Covalent bonding: sharing of electrons between atoms Chemical Bonding Three Major types: 1) Ionic bonding; exchange of electrons between atoms to form ions 2) Covalent bonding: sharing of electrons between atoms - - - - - - - - Cl - - Cl Chemical Bonding Three Major types: 1) Ionic bonding; exchange of electrons between atoms to form ions 2) Covalent bonding: sharing of electrons between atoms - - - - - - - - - Cl2 - Chemical Bonding Three Major types: 1) Ionic bonding; exchange of electrons between atoms to form ions 2) Covalent bonding: sharing of electrons between atoms - - - - - - - - - Cl2 - Chemical Bonding Three Major types: 1) Ionic bonding; exchange of electrons between atoms to form ions 2) Covalent bonding: sharing of electrons between atoms 3) Metallic bonding: freely exchangeable electrons between nuclei Chemical Bonding Three Major types: 1) Ionic bonding; exchange of electrons between atoms to form ions 2) Covalent bonding: sharing of electrons between atoms 3) Metallic bonding: freely exchangeable electrons between nuclei Chemical Bonding One Minor type: 1) Hydrogen Bonding (Van der Waals): weak attraction between ions of opposite charge Chemical Bonding One Minor type: 1) Hydrogen Bonding (Van der Waals): weak attraction between ions of opposite charge Bonding (Properties) Bond Mineral properties Ionic -strong bond -high melting points -vitreous lusters -higher solubility Covalent - strong bonds - hard minerals - very high melting points - vitreous – adamantine lusters Metallic - weak bonds - low to high melting points - metallic lusters -electrically conductive Today’s Homework 1. Download and read web notes 4 2. Study your minerals in GY 111L Next Time Crystal chemistry and mineral classes (web notes 5) GY 111: Physical Geology Lecture 4: Basic Mineral Chemistry Instructor: Dr. Doug Haywick [email protected] This is a free open access lecture, but not for commercial purposes. For personal use only.
