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Lecture 2 (9/11/2006) – Crystal Chemistry Part 1: Atoms, Elements, and Ions

Lecture 2 (9/11/2006) – Crystal Chemistry Part 1: Atoms, Elements, and Ions. Mineralogy Website. www.d.umn.edu/~mille066/Teaching/Mineralogy06.htm. What is Crystal Chemistry?. study of the atomic structure, physical properties, and chemical composition of crystalline material

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Lecture 2 (9/11/2006) – Crystal Chemistry Part 1: Atoms, Elements, and Ions

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  1. Lecture 2 (9/11/2006) – Crystal ChemistryPart 1: Atoms, Elements, and Ions

  2. Mineralogy Website www.d.umn.edu/~mille066/Teaching/Mineralogy06.htm

  3. What is Crystal Chemistry? • study of the atomic structure, physical properties, and chemical composition of crystalline material • basically inorganic chemistry of solids • the structure and chemical properties of the atom and elements are at the core of crystal chemistry • there are only a handful of elements that make up most of the rock-forming minerals of the earth

  4. Chemical Layers of the Earth SiO2 – 45% MgO – 37% FeO – 8% Al2O3 – 4% CaO – 3% others – 3% Fe – 86% S – 10% Ni – 4%

  5. Composition of the Earth’s Crust

  6. Average composition of the Earth’s Crust(by weight, elements, and volume)

  7. The Atom The Bohr Model The Schrodinger Model Nucleus - contains most of the weight (mass) of the atom - composed of positively charge particles (protons) and neutrally charged particles (neutrons) Electron Shell - insignificant mass - occupies space around the nucleus defining atomic radius - controls chemical bonding behavior of atoms

  8. Elements and Isotopes • Elements are defined by the number of protons in the nucleus (atomic number). • In a stable element (non-ionized), the number of electrons is equal to the number of protons • Isotopes of a particular element are defined by the total number of neutrons in addition to the number of protons in the nucleus (isotopic number). • Various elements can have multiple (2-38) stable isotopes, some of which are unstable (radioactive) • Isotopes of a particular element have the same chemical properties, but different masses.

  9. Isotopes of Titanium (Z=22) IsotopeHalf-lifeSpinParityDecay Mode(s) or Abundance 38Ti 0+ 39Ti 26 ms (3/2+) EC=100, ECP+EC2P ~ 14 40Ti 50 ms 0+ EC+B+=100 41Ti 80 ms 3/2+ EC+B+=100, ECP ~ 100 42Ti 199 ms 0+ EC+B+=100 43Ti 509 ms 7/2- EC+B+=100 44Ti 63 y 0+ EC=100 45Ti 184.8 m 7/2- EC+B+=100 46Ti stable 0+ Abundance=8.0 1 47Ti stable 5/2- Abundance=7.3 1 48Ti stable 0+ Abundance=73.8 1 49Ti stable 7/2- Abundance=5.5 1 50Ti stable 0+ Abundance=5.4 1 51Ti 5.76 m 3/2- B-=100 52Ti 1.7 m 0+ B-=100 53Ti 32.7 s (3/2)- B-=100 54Ti 0+ 55Ti 320 ms (3/2-) B-=100 56Ti 160 ms 0+ B-=100, B-N=0.06 sys 57Ti 180 ms (5/2-) B-=100, B-N=0.04 sys 58Ti 0+ 59Ti (5/2-) B-=? 60Ti 0+ B-=? 61Ti (1/2-) B-=?, B-N=? Source: R.B. Firestone UC-Berkeley

  10. Properties of Electrons • Occur in discrete (quantized) energy levels or orbitals around the nucleus • Behave as particles with wave-like properties • Position of an electron in space around the nucleus is a probability function defined by 4 quantum numbers n– principle quantum number (= 1, 2, 3, 4...) defines the energy level of the primary electron shell l – azimuthal quantum number (= n -1) defines the type and number of electron subshells (s, p, d, f, ...) m – magnetic quantum number (= +l to -l ) defines orientation and number of orbitals in each subshell s – spin quantum number (= +1/2 or -1/2) defines direction of spin of the electron in each orbital

  11. Electron Shells, Subshells, and Orbitals

  12. Filling up the Orbitals Controlled by the energy of the orbitals

  13. Structure of the Periodic Table # of Electrons in Outermost Shell Noble Gases Anions --------------------Transition Metals------------------ Primary Shell being filled

  14. Ions, Ionization Potential, and Valence States Cations – elements prone to give up one or more electrons from their outer shells; typically a metal element Anions – elements prone to accept one or more electrons to their outer shells; always a non-metal element Ionization Potential – measure of the energy necessary to strip an element of its outermost electron Electronegativity – measure strength with which a nucleus attracts electrons to its outer shell Valence State (or oxidation state) – the common ionic configuration(s) of a particular element determined by how many electrons are typically stripped or added to an ion

  15. 1st Ionization Potential Anions Cations Elements with a single outer s orbital electron Electronegativity

  16. Valence States of Ions common to Rock-forming Minerals Cations – generally relates to column in the periodic table; most transition metals have a +2 valence state for transition metals, relates to having two electrons in outer Anions – relates electrons needed to completely fill outer shell Anionic Groups – tightly bound ionic complexes with net negative charge +1 +2 +3 +4 +5 +6 +7 -2 -1 -----------------Transition Metals---------------

  17. Next Lecture • Crystal Chemistry II Bonding Atomic and Ionic Radii • Read p. 56-69

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