DOCSLIB.ORG

Chapter 8 Periodicity 2010

Total Page：16

File Type：pdf, Size：1020Kb

Download full-text PDF Read full-text
Chapter 8 Periodicity 2010 EM radiation Announcements is a wave and a --Exam 3 Oct 3..............Includes chapters 7/8/9/10 units called particle The excluded items include: 1. Classical distinction between energy and matter (p. 217) are Quant having 2. Numerical problems involving the Rydberg equation (equations a 7.3 and 7.4) absorbe emitted amplitude energy frequency wavelength 3. Spectral analysis in the laboratory (pp. 226-227) d 4. Numerical problems involving the Heisenberg uncertainty involve energy changes in related by related by principle (p. 231) 5. Trends among the transition elements (p. 261) atomsatoms c = !v 6. Trends in electron affinity (pp. 265-266) electron E = hv 7. Pseudo-noble gas configuration (p. 269) s molecules 8. Lattice energy (pp. 283-285) described by 9. IR spectroscopy (p. 292) e- filling e- configuration comprising 10.Numerical problems involving electronegativity (p. 296) Wave functions gives 11.Electronegativity and oxidation number (p. 297) 12.Section 11.3: MO theory and electron delocalization having quantum determined by 13.All sections in chapter 12 except 12.3 uunmbers Aufbau Rules Quantum described by Core Numbers Electrons Wave Function e- filling spdf electronic configuration comprising Orbital size (Orbital) Valence Principal define & energy determined by Electrons n = 1,2,3,.. s described by Aufbau basis for defines Rules Periodic Quantum which involve Table Angular Numbers momentum, l Orbital which summarizes defines Oribital Pauli Hund’s shape which are Energy Exclusion Rule Periodic Properties Magnetic Orbital defines ml orientation Electron Spin, ms defines spin I. The Periodic Law and the Periodic Table • 1864 Newland “Law of Octaves • 1869 Dimitri Mendeleev and Lother Meyer When the elements are arranged in order of increasing atomic mass, certain sets of chemical and physical properties recur periodically. Electronic Configuration and Periodicity • 1913 Henry Mosely relates X-ray frequency to Chapter 8 atomic number When the Elements Were Discovered Quantum numbers (n,l,ml,ms) specify “allowed states” or “orbitals” which are regions of space where electrons are likely to be found around the nucleus. 1. Principal Quantum Number (n): Defines the size and energy level of the orbital. n = {1,2,3,4,.....}. Also called a shell (K = 1, L = 2, M = 3, N = 4, .....). 2. Angular Momemtum Quantum Number (l): Defines the “shape” of the orbital which is a volume in space where the electron is likely to be found. Also called a subshell. l = {0,1,2,3...up to n-1} where (0=s, 1=p, 2=d, 3=f) 3. Magnetic Quantum Number (ml): Defines the spatial orientation of an orbital of the same energy. ml = {-l, 0, +l} 4. Magnetic Spin Quantum Number (ms): Defines the orientation of “electron spin”. ms = {+1/2 or -1/2}. Electronic configuration of the elements: The lowest energy (ground state) four quantum numbers describe an electron electronic configuration of all in a ground state atom. elements are constructed by filling lowest energy orbitals sequentially in what is called the “Aufbau Process”. 4s Name Symbol Permitted Values Property 3p 1. Lower energy (n-quantum number) principal n positive integers (1,2,3, orbital energy (size) orbitals fill first. 3s !) 2. Hund’s Rule-orbitals fill one electron at angular l 2p momentum integers from 0 to n-1 orbital shape a time before electrons are paired. 3. Pauli Exclusion Principle: No two orbital orientation in 2s magnetic ml integers from -l to 0 to electrons can have same 4-quantum +l space numbers) - spin ms +1/2 or -1/2 direction of e spin Electrons fill the lowest energy orbitals first, 2 at a time! 1s The order of filling of the orbitals can be Chemists use spdf notation and orbital box remembered using a mnemonic device. diagrams to denote or show the “ground state Memorize this to help you! electronic configuration” of elements. For an Hydrogen atom spdf orbital box Spin quantum orbital energy only depends Element Notation diagram number. An on the n quantum number. arrow denotes 1 an electron For many electrons atoms H 1s with “spin the energy of an orbital or up” (+1/2) or electron depends on both “spin- n and l (3s < 3p < 3d) He 1s2 down” (-1/2). n principal quantum # l quantum number # of electrons in orbital The Pauli Exclusion principle states: “No two The order of filling of the orbitals can be remembered electrons can have the same 4-quantum numbers”. using a mnemonic device. Memorize how to write it The spin numbers can not be the same (spin up out as it determines electronic structure. and spin down allowed only). (n, l, ml and ms) Example: Atomic Orbital Box Full-electronic Condensed-electronic Number/Element Diagram configuration configuration Li 1s22s1 [He]2s1 Electronic configuration using Aufbau Process s-block Atomic Orbital Box Full-electronic Condensed-electronic main group p-block Number/Element Diagram configuration configuration main group d-block H 1s1 1s1 transition metals He 1s2 1s2 f-block written with noble inner transition metals gas configuration Li 1s22s1 [He]2s1 Be 1s22s2 [He]2s2 Atomic Orbital Box Full-electronic Condensed-electronic Number/Element Diagram configuration configuration B 1s22s22p1 [He]2s22p1 2 2 2 2 2 C 1s 2s 2p [He]2s 2p 1s22s22p3 [He]2s22p3 1s22s22p4 [He]2s22p4 1s22s22p5 [He]2s22p5 1s22s22p6 [He]2s22p6 Unpaired electrons in orbitals gives rise to Odd-filling behavior here! paramagnetism and is attracted to a magnetic field. 4th and 9th position. Diamagnetic species contain all paired electrons and is “repelled” by the magnetic field. • Diamagnetic atoms or ions: Diamagnetic – All e- are paired. all electrons paired – Weakly repelled in a magnetic field. 2p • Paramagnetic atoms or ions: Paramagnetic – Unpaired e- exist in an orbital unpaired electrons – Attracted to an external magnetic field. 2p Unpaired electrons in orbitals gives rise to When a cation is formed from an atom of a paramagnetism and is attracted to a magnetic field. transition metal, electrons are removed first from Diamagnetic species contain all paired electrons and the ns orbital, then from the (n-1)d orbital. is “repelled” by the magnetic field. Magnetic field off Magnetic field on Magnetic field on Fe: [Ar]4s23d6 Fe2+: [Ar]4s03d6 or [Ar]3d6 Fe: [Ar]4s23d6 Fe3+: [Ar]4s03d5 or [Ar]3d5 Mn: [Ar]4s23d5 Mn2+: [Ar]4s03d5 or [Ar]3d5 Paramagentic Diamagentic Paramagnetic Diamagnetic Metals loose electrons (oxidized) to become Isoelectronic species are two different elements cations. Non-metals gain electrons to become with the same electronic configuration--but not the anions. The electronic configuration of each same nuclear configuration. reflects this change in the number of electrons. oxidation Na: [1s22s22p63s1] =====> Na+: [1s22s22p6] = [Ne] Na [Ne]3s1 Na+ [Ne] Metals lose electrons so oxidation 2 2 6 2 p1 3+ 2 2 6 Ca [Ar]4s2 Ca2+ [Ar] that cation has a noble-gas Al: [1s 2s 2p 3s 3 ] =====> Al : [1s 2s 2p ] = [Ne] 2 1 3+ outer electron configuration. reduced Al [Ne]3s 3p Al [Ne] N: [1s22s22p3] =====> N3-: [1s22s22p6] = [Ne] reduced O: [1s22s22p4] =====> O2-: [1s22s22p6] = [Ne] H 1s1 H- 1s2 or [He] reduced Non-metals gain F: [1s22s22p5] =====> F-: [1s22s22p6] = [Ne] F 1s22s22p5 F- 1s22s22p6 or [Ne] electrons so that anion has a noble-gas outer O 1s22s22p4 O2- 1s22s22p6 or [Ne] Na+, Al3+, F-, O2-, and N3- are all said to be “isoelectronic electron configuration. with Ne” as they have the same electronic N 1s22s22p3 3- 2 2 6 N 1s 2s 2p or [Ne] configuration....all subshells are filled. Metals and non-metals form ions with electronic Metals and non-metal ions tend to form electronic configurations closest to their nearest noble gas states closest to their nearest noble gas configuration. configuration. 1A 2A 3A 4A 5A 6A 7A 8A What is the spdf and condensed electron Using the periodic table on the inside cover of the configuration of Mg and Mg2+ ? Mg 12 electrons text and give the full and condensed electrons configurations, partial orbital diagrams showing 2 2 6 2 2 Mg 1s 2s 2p 3s [Ne]3s valence electrons, and number of inner electrons for 2+ 2 2 6 0 0 the following elements: Mg 1s 2s 2p 3s [Ne]3s = [Ne] (a) potassium (K: (b) molybdenum (c) lead (Pb: Z What are the possible quantum numbers for the last Z = 19) (Mo: Z = 42) = 82) (outermost) electron in Cl? Cl 17 electrons 1s < 2s < 2p < 3s < 3p < 4s 1s22s22p63s23p5 2 + 2 + 6 + 2 + 5 = 17 electrons Last electron added to 3p orbital n = 3 l = 1 ml = -1, 0, or +1 ms = ! or -! C) Is ground state F paramagenetic or diamagnetic? (a) for K (Z = 19) There are 18 inner electrons. Use condensed electron configurations to write the reaction 2 2 6 2 6 1 full configuration 1s 2s 2p 3s 3p 4s for the formation of each transition metal ion, and predict 1 condensed [Ar] 4s whether the ion is paramagnetic. orbital diagram 4s1 3d 4p (a) Mn2+(Z = 25) (b) Cr3+(Z = 24) (c) Hg2+(Z = 80) (b) for Mo (Z = 42) 36 inner electrons and 6 valence electrons full configuration 1s22s22p63s23p64s23d104p65s14d5 condensed [Kr] 5s14d5 partial orbital diagram Write the electron configuration and remove electrons starting with ns to match the charge on the ion. If the remaining 5s1 4d5 5p configuration has unpaired electrons, it is paramagnetic. (c) for Pb (Z = 82) 78 inner electrons and 4 valence electrons. 1s22s22p63s23p64s23d104p65s24d10 full configuration 5p66s24f145d106p2 condensed [Xe] 6s24f145d106p2 partial orbital diagram 6s2 6p2 Use condensed electron configurations to write the reaction Identify n and l quantum numbers for each of the for the formation of each transition metal ion, and predict following. whether the ion is paramagnetic. (a) Mn2+(Z = 25) (b) Cr3+(Z = 24) (c) Hg2+(Z = 80) Write the electron configuration and remove electrons starting with ns to match the charge on the ion.
Load more

Recommended publications
  • Chapter 8 2013
    described by Core Chapter 8 Electrons Wave Function e- filling spdf electronic configuration comprising (Orbital) Valence determined by Electrons described by Aufbau basis for Rules Periodic Quantum which involve Table Numbers which summarizes Orbital Pauli Hund’s which are Energy Exclusion Rule Periodic Properties Electron Configuration and Chemical Periodicity Quantum 4-quantum numbers specify the energy and location of Numbers electrons around a nucleus (all we can know). This numbers are the framework for the “electronic structure Orbital size of an atom”. Principal define & energy n = 1,2,3,.. s defines Name Symbol Permitted Values Property principal n positive integers (1,2,3...) orbital energy (size) Angular Orbital angular l orbital shape (0, 1, 2, and 3 momentum, l defines momentum integers from 0 to n-1 correspond to s, p, d, and f shape orbitals, respectively.) Magnetic Orbital magnetic integers from -l to 0 to +l orbital orientation in space defines ml ml orientation direction of e- spin spin m +1/2 or -1/2 Electron s Spin, ms defines spin Quantum Allowed Schrodinger’s equation gives an exact solution for H- Possible Orbitals Number Values atom, but does not for many electron-atoms. Electron- n Positive integers 1 2 3 electron repulsion in multi-electron split energy levels. 1,2,3,4.... Hydrogen Atom Multi-electron atoms 0 0 1 0 1 2 l 0 up to max Orbitals are of n-1 “degenerate” or Energy the same energy in Hydrogen! ml -l,...0...+l 0 0 -1 0 1 0 -1 0 1 -2-1 0 12 Orbital Name 1s 2s 2p 3s 3p 3d Electrons will Shapes or Boundry fill lowest Surface Plots energy orbitals first! Inner core electrons “shield” or “screen” outer 4-quantum numbers specify all the information we can know the energy electrons from the positive charge of the nucleus.
    [Show full text]
  • Ultrasoft Pseudopotentials for Lanthanide Solvation Complexes: Core Or Valence Character of the 4F Electrons Rodolphe Pollet, C
    Ultrasoft pseudopotentials for lanthanide solvation complexes: Core or valence character of the 4f electrons Rodolphe Pollet, C. Clavaguéra, J.-P. Dognon To cite this version: Rodolphe Pollet, C. Clavaguéra, J.-P. Dognon. Ultrasoft pseudopotentials for lanthanide solvation complexes: Core or valence character of the 4f electrons. Journal of Chemical Physics, American Institute of Physics, 2006, 124, pp.164103 - 1-6. 10.1063/1.2191498. hal-00083928 HAL Id: hal-00083928 https://hal.archives-ouvertes.fr/hal-00083928 Submitted on 21 Jul 2006 HAL is a multi-disciplinary open access L’archive ouverte pluridisciplinaire HAL, est archive for the deposit and dissemination of sci- destinée au dépôt et à la diffusion de documents entific research documents, whether they are pub- scientifiques de niveau recherche, publiés ou non, lished or not. The documents may come from émanant des établissements d’enseignement et de teaching and research institutions in France or recherche français ou étrangers, des laboratoires abroad, or from public or private research centers. publics ou privés. Ultrasoft pseudopotentials for lanthanide solvation complexes: Core or valence character of the 4f electrons Rodolphe Pollet,∗ Carine Clavagu´era, Jean-Pierre Dognon Theoretical Chemistry Laboratory DSM/DRECAM/SPAM-LFP (CEA-CNRS URA2453) CEA/SACLAY, Bat. 522, 91191 GIF SUR YVETTE, FRANCE March 6, 2006 Abstract The 4f electrons of lanthanides, because of their strong localiza- tion in the region around the nucleus, are traditionally included in a pseudopotential core. This approximation is scrutinized by optimizing 3+ the structures and calculating the interaction energies of Gd (H2O) 3+ and Gd (NH3) microsolvation complexes within plane wave PBE cal- culations using ultrasoft pseudopotentials where the 4f electrons are included either in the core or in the valence space.
    [Show full text]
  • Chapter 7 Periodic Properties of the Elements Learning Outcomes
    Chapter 7 Periodic Properties of the Elements Learning Outcomes: Explain the meaning of effective nuclear charge, Zeff, and how Zeff depends on nuclear charge and electron configuration. Predict the trends in atomic radii, ionic radii, ionization energy, and electron affinity by using the periodic table. Explain how the radius of an atom changes upon losing electrons to form a cation or gaining electrons to form an anion. Write the electron configurations of ions. Explain how the ionization energy changes as we remove successive electrons, and the jump in ionization energy that occurs when the ionization corresponds to removing a core electron. Explain how irregularities in the periodic trends for electron affinity can be related to electron configuration. Explain the differences in chemical and physical properties of metals and nonmetals, including the basicity of metal oxides and the acidity of nonmetal oxides. Correlate atomic properties, such as ionization energy, with electron configuration, and explain how these relate to the chemical reactivity and physical properties of the alkali and alkaline earth metals (groups 1A and 2A). Write balanced equations for the reactions of the group 1A and 2A metals with water, oxygen, hydrogen, and the halogens. List and explain the unique characteristics of hydrogen. Correlate the atomic properties (such as ionization energy, electron configuration, and electron affinity) of group 6A, 7A, and 8A elements with their chemical reactivity and physical properties. Development of Periodic Table •Dmitri Mendeleev and Lothar Meyer (~1869) independently came to the same conclusion about how elements should be grouped in the periodic table. •Henry Moseley (1913) developed the concept of atomic numbers (the number of protons in the nucleus of an atom) 1 Predictions and the Periodic Table Mendeleev, for instance, predicted the discovery of germanium (which he called eka-silicon) as an element with an atomic weight between that of zinc and arsenic, but with chemical properties similar to those of silicon.
    [Show full text]
  • Relativistic Energy-Consistent Ab Initio Pseudopotentials — New Developments for Actinides
    Winterschool on Michael Dolg Actinide Chemistry Institut fur¨ Theoretische Chemie Helsinki Universit¨at zu K¨oln December 10-14, 2007 Relativistic Energy-consistent Ab Initio Pseudopotentials — New Developments for Actinides. ‘Stuttgart-(Dresden→Bonn→Cologne)‘ PPs: http://www.theochem.uni-stuttgart.de Valence orbital densities and core densities of Th 30+ 12+ 4+ Th Th Th 1.0 + 0.9 Σ 2 1 0.8 σ 5f 0.7 0.6 ThO 7sp e R 1 h =7 2 h =8 3 h =9 0.5 0.4 6d density (a.u.) 7s 0.3 0.2 0.1 4 h − 1=7 5 h − 1=8 0.0 0 1 2 3 4 5 6 7 8 radius (a.u.) Contents • Short introduction to energy-consistent relativistic pseudopotentials • What we currently can provide for lanthanides and actinides: Wood-Boring adjusted scalar-relativistic (one-component) large-core (Ln 4f-in-core, An 5f-in-core) and small-core (Ln 4f-in-valence, An 5f-in-valence) pseudopotentials, valence spin-orbit operators in the small core case and corresponding valence basis sets of different quality (VDZ to VQZ) and contraction schemes (segmented, generalized) based on ANOs. – some general considerations concerning the choice of the core: small-core vs. large-core PPs; f-in-core PPs (superconfiguration model (R.W.Field); feudal model (B.Bursten) ?) – calibration for atoms/molecules – examples for applications • What we would like to have for lanthanides and actinides: Multi-configuration Dirac-Hartree-Fock/Dirac-Coulomb-Breit adjusted relativistic (two- and one-component) small-core pseudopotentials and corresponding correlation- consistent valence basis sets.
    [Show full text]
  • QMEPC Discovery of Light's Medium Explains Why Gravity Is Larger and Weaker Odin Von Aesir* PO Box 50252, Austin, TX 78763, 925-202-6631, USA
    Research & Reviews: Journal of Pure and Applied Physics QMEPC Discovery of Light's Medium Explains Why Gravity Is Larger and Weaker Odin Von Aesir* PO Box 50252, Austin, TX 78763, 925-202-6631, USA Review Article Received date: 17/11/2015 ABSTRACT Accepted date: 25/02/2016 The MEPC – The Magnetic Electron Plasma Cloud – is plasma solely Published date: 30/03/2016 composed of electrons that is the source and recipient of electrons that exist outside of the atom. The ramifications of this are nothing short of *For Correspondence phenomenal, because it not only explains where electrons come from and how they are available for distribution around the atomic nucleus, but it also Odin Von Aesir, Po Box 50252, Austin, TX explains: 78763, 925-202-6631, USA • What occupies the space in between the atoms? E-mail: [email protected] • The existence of a hierarchy of forces surrounding the atomic core, • Why gravity is larger and weaker than the other known forces, Keywords: Ramifications; Hierarchy; Proximity; • What the medium of light is, Stratosphere • Why light is both a particle and a wave, and • What dark matter and dark energy are? INTRODUCTION Furthermore, the MEPC makes logical sense of the quirkiness of quantum mechanics and the progression of time and space, because it explains the composition and connection of everything. It even gives an insight into the makeup of the atomic nucleus itself [1]. It is common knowledge that the space that surrounds us and that separates us from each other and other things here on earth is composed of air molecules that are made up of even smaller atoms.
    [Show full text]
  • What Is XPS? X‐Ray Photoelectron Spectroscopy (XPS) Is a Surface Analytical Technique, Which Is Based Upon the Photoelectric Effect
    What is XPS? X‐ray photoelectron spectroscopy (XPS) is a surface analytical technique, which is based upon the photoelectric effect. Each atom in the surface has core electron with the characteristic binding energy that is conceptually, not strictly, equal to the ionization energy of that electron. When an X‐ray beam directs to the sample surface, the energy of the X‐ray photon is adsorbed completely by the core electron of an atom. If the photon energy, h , is large enough, the core electron will then escape from the atom and emit out of the surface. The emitted electron with the kinetic energy of Ek is referred to as the photoelectron. The binding energy of the core electron is given by the Einstein relationship: Where h is the X‐ray photon energy (for monochromatic Al Ka, h = 1486.6eV);Ek is the kinetic energy of photoelectron, which can be measured by the energy analyzer; and Φ is the work function induced by the analyzer, about 4%7e5eV. Since the work function, Φ, can be compensated artificially, it is eliminated, giving the binding energy as follows: For insulating samples, once the photoelectrons are emitted out of the sample surface, a positive charge zone will establish quickly in the sample surface. As a result, the sample surface acquires a positive potential (varying typically from several volts to tens of volts) and the kinetic energies of core electrons are reduced by the same amount,C. It can be seen that the surface charging results in the shift of the XPS peaks to higher binding energy.
    [Show full text]
  • Understanding the Role of Water on Electron-Initiated Processes and Radical Chemistry
    Understanding the Role of Water on Electron- Initiated Processes and Radical Chemistry September 26-28, 2002 • Pacific Northwest National Laboratory • Richland, Washington Plane B Plane A Report Sponsored by the Division of Chemical Sciences Office of Basic Energy Sciences June 10, 2003 Cover illustrations: TOP LEFT: Secondary electrons produced by fast ion tracks in radioactive waste. TOP CENTER: Singly occupied molecular orbital (SOMO) for the solvated electron (blue shape) – in the e (H2O)8 cluster surrounded by a continuum dielectric model. Thick lines indicate hydrogen bonds from solvating waters to the electron. (D. A. Dixon and C. G. Zhan) TOP RIGHT: Snapshot from a molecular dynamics simulation of the HOMO of the charge- transfer-to-solvent triplet state for I–. (S. E. Bradforth and P. Jungwirth) BOTTOM LEFT: Optimized structure of a 72-molecule water cluster starting from an initial hexagonal ice Ih configuration with the TTM2-F potential (S. S. Xantheas and C. J. Burnham) BOTTOM RIGHT: Difference in charge density between free water molecules and a pentamer with an ice like local structure (M. Nyberg, L. Pettersson and A. Nilsson) ii June 10, 2003 Understanding the Role of Water on Electron-Initiated Processes and Radical Chemistry Report of the Workshop held at Pacific Northwest National Laboratory, September 26-28, 2002 Sponsored by the Chemical Sciences Division, Office of Basic Energy Sciences, Department of Energy Organizing Committee Bruce C. Garrett, Pacific Northwest National Laboratory Steven D. Colson, Pacific Northwest National Laboratory David A. Dixon, Pacific Northwest National Laboratory Allan H. Laufer, Office of Basic Energy Sciences, DOE Douglas Ray, Pacific Northwest National Laboratory Writing Team Leaders Donald M.
    [Show full text]
  • Periodic Properties of the Elements
    Periodic Properties of the Elements Review Questions 8.1 A periodic property is one that is predictable based on the element's position within the periodic table. 8.2 The relative size of the sodium and potassium ions is important to nerve signal transmission. The pumps and channels within cell membranes are so sensitive that they can distinguish between the sizes of these two ions and selectively allow only one or the other to pass. The movement of ions is the basis for the transmission of nerve signals in the brain and throughout the body. 8.3 The first attempt to organize the elements according to similarities in their properties was made by the German chemist Johann Dobereiner. He grouped elements into triads; three ele- ments with similar properties. A more complex approach was attempted by the English chemist John Newlands. He organized elements into octaves, analogous to musical notes. When arranged this way, the properties of every eighth element were similar. The modern periodic table is credited primarily to the Russian chemist Dmitri Mendeleev. Mendeleev's table is based on the periodic law, which states that when elements are arranged in order of increasing mass, their properties recur periodically. Mendeleev arranged the ele- ments in a table in which mass increased from left to right and elements with similar proper- ties fell in the same columns. 8.5 Meyer proposed an organization of the known elements based on some periodic properties. Moseley listed elements according to the atomic number rather than atomic mass. This resolved the problems in Mendeleev's table where an increase in atomic mass did not corre- late with similar properties.
    [Show full text]
  • Development and Applications of Relativistic Correlation Consistent Basis Sets for Lanthanide Elements and Accurate Ab Initio T
    DEVELOPMENT AND APPLICATIONS OF RELATIVISTIC CORRELATION CONSISTENT BASIS SETS FOR LANTHANIDE ELEMENTS AND ACCURATE AB INITIO THERMOCHEMISTRY AND SPECTROSCOPY By QING LU A dissertation submitted in partial fulfillment of the requirements for the degree of DOCTOR OF PHILOSOPHY WASHINGTON STATE UNIVERSITY Department of Chemistry MAY 2017 © Copyright by QING LU, 2017 All Rights Reserved © Copyright by QING LU, 2017 All Rights Reserved To the Faculty of Washington State University: The members of the Committee appointed to examine the dissertation of QING LU find it satisfactory and recommend that it be accepted Kirk A. Peterson, Ph.D., Chair Aurora E. Clark, Ph.D. Ursula Mazur, Ph.D. James A. Brozik, Ph.D. ii ACKNOWLEDGEMENT Having been at this step, I feel difficult to hold my emotions and think logically. So for whoever read this part, please tolerate with my ramblings. Chronologically, the first person I want to acknowledge is Prof. Ming Xian, as he offered me to the WSU grad school. Unfortunately, things didn’t work out well during my first year as I had no idea how to do research at that time. Nonetheless, I still have a good time there and I want to appreciate the help from Dr. Jia Pan and Dr. Nelmi Devarie, who were in Prof. Xian’s group and gave me lots of help. Oh, I should also thank the graduate director and search committee, whose names I forget, in the University of New Hampshire, as they gave me the first offer to cheer me up when I was applying for a US grad school back in China, and allowed me to turn down their offer after I had accepted their offer.
    [Show full text]
  • Example Exercise 6.1 Periodic Law Find the Two Elements in the Fifth Row of the Periodic Table That Violate the Original Periodic Law Proposed by Mendeleev
    Example Exercise 6.1 Periodic Law Find the two elements in the fifth row of the periodic table that violate the original periodic law proposed by Mendeleev. Solution Mendeleev proposed that elements be arranged according to increasing atomic mass. Beginning with Rb, each of the elements in the fifth row increases in atomic mass until iodine. Although the atomic numbers of Te (52) and I (53) increase, the atomic masses of Te (127.60) and I (126.90) do not. Experimentally, it is I and not Te, with properties similar to those of F, Cl, and Br. Practice Exercise Find a pair of elements in the periodic table with atomic numbers less than 20 that are an exception to the original periodic law. Answer: Ar and K Concept Exercise The modern periodic law states that elements are arranged according to increasing (atomic mass/atomic number). (Circle the correct choice.) Answer: See Appendix G. Introductory Chemistry: Concepts and Critical Thinking, 6th Edition © 2011 Pearson Education, Inc. Charles H. Corwin Example Exercise 6.2 Groups and Periods of Elements Select the symbol of the element that fits each of the following descriptions: (a) the alkali metal in the fourth period (b) the halogen in the third period (c) the rare earth with the lowest atomic mass (d) the metal in Group VIIB/7 and Period 4 Solution Referring to the periodic table in Figure 6.3, we have (a) K (b) Cl (c) Sc (d) Mn Figure 6.3 Names of Groups and Periods The common names of groups and periods are shown for selected families and series.
    [Show full text]
  • Electron Configuration of Ions
    • In 2002, there were 115 elements known. • The majority of the elements were discovered between 1735 and 1843. • How do we organize 115 different elements in a meaningful way that will allow us to make predictions about undiscovered elements? • Arrange elements to reflect the trends in chemical and physical properties. • First attempt (Mendeleev and Meyer) arranged the elements in order of increasing atomic weight. • Certain elements were missing from this scheme. Example: In 1871, Mendeleev noted that As properly belonged underneath P and not Si, which left a missing element underneath Si. He predicted a number of properties for this element. In 1886 Ge was discovered. The properties of Ge match Mendeleev’s predictions well. • Modern periodic table: arrange elements in order of increasing atomic number. • Electrons ordinarily occupy orbitals of the lowest energy available. • No two electrons in the same atom may have all four quantum numbers alike. • Pauli exclusion principle: one atomic orbital can accommodate no more than two electrons, and these electrons must have opposing spins. • Of a group of orbitals of identical energy, electrons enter empty orbitals whenever possible (Hund’s rule). • Electrons in half-filled orbitals have parallel spins (same direction). • Core electrons: electrons in [Noble Gas]. The spdf notation •Valence electrons: electrons outside of [Noble Gas]. uses numbers to designate a principal shell and letters (s, p, d, f) to identify a subshell; a superscript indicates the number of electrons in a designated subshell. N: orbital (box) diagram • The periodic table can be used as a guide for electron configurations. • The period number is the value of n.
    [Show full text]
  • 19920024495.Pdf
    Z d I The First Mission of the Tethered Satellite System Table of Contents A Line To The Universe 1 The First Tethered Satellite System Mission 2 Major Tethered Satellite System Elements 6 Tether Dynamics 10 TSS-1 Science Background 14 TSS-1 Science Investigations 23 Mission Scenario 28 TSS-1 Crew 30 A Line To The Future 32 Quick Reference To Experiments And Investigators 35 For Further Reading 36 Glossary Of Abbreviations And Acronyms 37 N/ A ORIGINAL PAGE National Aeronautics and PHQTOGRAPH, Space Administration il A Line To The Universe The first Tethered Satellite System (TSS-1) will soon be launched aboard the Space Shuttle. Circling Earth at an altitude of 296 kilometers (kin), the reusable tether system will be well within the tenuous, electrically charged layer of the atmosphere known as the iono- sphere. There, a satellite attached to the orbiter by a thin conducting cord, or tether, will be reeled from the Shuttle payload bay. This will grant scientists experi- mental capabilities never before possible. On this mission, the satellite will be deployed 20 km above the Shuttle. The conducting tether will generate high voltage and electrical currents as it moves through the ionosphere and allow scientists to examine the electrodynamics of a conducting tether system. These studies will not only increase our understanding of physical processes in the near-Earth space environment but will also help provide an explanation for events witnessed elsewhere in the solar system. In addition, the Deployment of the Tethered Satellite System upward mission will explore the mechanical dynamics of teth- from the Shuttle On TSS-I allows scientists to gather ered systems, providing information that will improve data on performance, while providing an excellent future missions and possibly lead to a variety of future platform for a variety of plasma physics and electro@- =....
    [Show full text]