Anionic Hydrogen Clusters As a Source of Diffuse Interstellar Bands (Dibs)1
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CNSC Research Report 2016-17
The Science of Safety: CNSC Research Report 2016–17 © Canadian Nuclear Safety Commission (CNSC) 2018 Cat. No. CC171-24E-PDF ISSN 2369-4351 Extracts from this document may be reproduced for individual use without permission provided the source is fully acknowledged. However, reproduction in whole or in part for purposes of resale or redistribution requires prior written permission from the Canadian Nuclear Safety Commission. Également publié en français sous le titre : La science de la sûreté : Rapport de recherche de la CCSN 2016-2017 Document availability This document can be viewed on the CNSC website. To request a copy of the document in English or French, please contact: Canadian Nuclear Safety Commission 280 Slater Street P.O. Box 1046, Station B Ottawa, Ontario K1P 5S9 CANADA Tel.: 613-995-5894 or 1-800-668-5284 (in Canada only) Facsimile: 613-995-5086 Email: [email protected] Website: nuclearsafety.gc.ca Facebook: facebook.com/CanadianNuclearSafetyCommission YouTube: youtube.com/cnscccsn Twitter: @CNSC_CCSN Publishing History June 2018 Edition 1.0 Table of contents Message from the President .......................................................................................................................... 1 Introduction ................................................................................................................................................... 2 Ensuring the safety of nuclear power plants ................................................................................................. 6 Protecting -
Source of Atomic Hydrogen for Ion Trap Experiments: Review and Basic Properties
WDS'15 Proceedings of Contributed Papers — Physics, 155–161, 2015. ISBN 978-80-7378-311-2 © MATFYZPRESS Source of Atomic Hydrogen for Ion Trap Experiments: Review and Basic Properties A. Kovalenko, Š Roučka, S. Rednyk, T. D. Tran, D. Mulin, R. Plašil, J. Glosík Charles University in Prague, Faculty of Mathematics and Physics, Prague, Czech Republic. Abstract. The H-atom source was used to produce atomic hydrogen for study of ion-molecule reactions relevant to astrochemistry at low temperatures. H atoms were cooled and formed into an effusive beam, passing through a 22-pole ion trap. Here we present the basic operating principles of the H-atom source and give a review of this apparatus with some calculations of vacuum conditions and parameters of the produced H-atom beam. Introduction Hydrogen is the most abundant element in the Universe [Field et al., 1966]. It is the main component of stars, giant planets and interstellar clouds. Reactions with atomic or molecular hydrogen are important for understanding the processes which occur in the interstellar medium and during the formation of the new stars. There are three isotopes of hydrogen: protium, deuterium and tritium. The reactions of ions with H atoms have to be studied for better understanding of formation and destruction of more complex ions and molecules observed in interstellar medium. There are regions in space called H I and H II regions where hydrogen is mostly neutral in H I regions, rather than ionized or molecular in the H II regions. The atomic hydrogen plays fundamental role in many astrophysical contexts especially in formation H2 molecules [Habart et al., 2005; Sternberg et al., 2014]. -
Crystal Chemistry of Perovskite-Type Hydride Namgh3: Implications for Hydrogen Storage
Chem. Mater. 2008, 20, 2335–2342 2335 Crystal Chemistry of Perovskite-Type Hydride NaMgH3: Implications for Hydrogen Storage Hui Wu,*,†,‡ Wei Zhou,†,‡ Terrence J. Udovic,† John J. Rush,†,‡ and Taner Yildirim†,§ NIST Center for Neutron Research, National Institute of Standards and Technology, 100 Bureau DriVe, MS 6102, Gaithersburg, Maryland 20899-6102, Department of Materials Science and Engineering, UniVersity of Maryland, College Park, Maryland 20742-2115, and Department of Materials Science and Engineering, UniVersity of PennsylVania, 3231 Walnut Street, Philadelphia, PennsylVania 19104-6272 ReceiVed NoVember 26, 2007. ReVised Manuscript ReceiVed January 11, 2008 The crystal structure, lattice dynamics, and local metal-hydrogen bonding of the perovskite hydride NaMgH3 were investigated using combined neutron powder diffraction, neutron vibrational spectroscopy, and first-principles calculations. NaMgH3 crystallizes in the orthorhombic GdFeO3-type perovskite structure (Pnma) with a-b+a- octahedral tilting in the temperature range of 4 to 370 K. In contrast with previous structure studies, the refined Mg-H lengths and H-Mg-H angles indicate that the MgH6 octahedra maintain a near ideal configuration, which is corroborated by bond valence methods and our DFT calculations, and is consistent with perovskite oxides with similar tolerance factor values. The temperature dependences of the lattice distortion, octahedral tilting angle, and atomic displacement of H are also consistent with the recently observed high H mobility at elevated temperature. The stability and dynamics of NaMgH3 are discussed and rationalized in terms of the details of our observed perovskite structure. Further experiments reveal that its perovskite crystal structure and associated rapid hydrogen motion can be used to improve the slow hydrogenation kinetics of some strongly bound light-metal-hydride systems such as MgH2 and possibly to design new alloy hydrides with desirable hydrogen-storage properties. -
Highly Conductive Antiperovskites with Soft Anion Lattices 12 January 2021, by I
Highly conductive antiperovskites with soft anion lattices 12 January 2021, by I. Mindy Takamiya, Mari Toyama 'cation." They also have numerous intriguing properties, including superconductivity and, in contrast to most materials, contraction upon heating. Lithium- and sodium-rich antiperovskites, such as Li3OCl and Na3OCl, have been attracting much attention due to their high ionic conductivity and alkali metal concentration, making them promising candidates to replace liquid electrolytes used in lithium ion batteries. "But achieving a comparable lithium ion conductivity in solid materials has been challenging," explains iCeMS solid-state chemist Hiroshi Kageyama, who led the study. Soft anions, like sulfur ions (S2-), provide an ideal conduction path for sodium (Na+) and lithium (Li+) ions, Kageyama and his team synthesized a new family with the hydride ions (H-) helping to stabilize the of lithium- and sodium-rich antiperovskites that compound's structure. Credit: Mindy Takamiya/Kyoto begins to overcome this issue. Instead of 'hard' University iCeMS oxygen and halogen anions, their antiperovskites contain a hydrogen anion, called a hydride, and 'soft' chalcogen anions like sulfur. A new structural arrangement of atoms shows The scientists conducted a wide range of promise for developing safer batteries made with theoretical and experimental investigations on solid materials. Scientists at Kyoto University's these antiperovskites, and found that the soft anion Institute for Integrated Cell-Material Sciences lattice provides an ideal conduction path for lithium (iCeMS) designed a new type of 'antiperovskite' and sodium ions, which can be further enhanced by that could help efforts to replace the flammable chemical substitutions. organic electrolytes currently used in lithium ion batteries. -
Answer Key Chapter 16: Standard Review Worksheet – + 1
Answer Key Chapter 16: Standard Review Worksheet – + 1. H3PO4(aq) + H2O(l) H2PO4 (aq) + H3O (aq) + + NH4 (aq) + H2O(l) NH3(aq) + H3O (aq) 2. When we say that acetic acid is a weak acid, we can take either of two points of view. Usually we say that acetic acid is a weak acid because it doesn’t ionize very much when dissolved in water. We say that not very many acetic acid molecules dissociate. However, we can describe this situation from another point of view. We could say that the reason acetic acid doesn’t dissociate much when we dissolve it in water is because the acetate ion (the conjugate base of acetic acid) is extremely effective at holding onto protons and specifically is better at holding onto protons than water is in attracting them. + – HC2H3O2 + H2O H3O + C2H3O2 Now what would happen if we had a source of free acetate ions (for example, sodium acetate) and placed them into water? Since acetate ion is better at attracting protons than is water, the acetate ions would pull protons out of water molecules, leaving hydroxide ions. That is, – – C2H3O2 + H2O HC2H3O2 + OH Since an increase in hydroxide ion concentration would take place in the solution, the solution would be basic. Because acetic acid is a weak acid, the acetate ion is a base in aqueous solution. – – 3. Since HCl, HNO3, and HClO4 are all strong acids, we know that their anions (Cl , NO3 , – and ClO4 ) must be very weak bases and that solutions of the sodium salts of these anions would not be basic. -
Protonation and Chloroplast Membrane Structure
PROTONATION AND CHLOROPLAST MEMBRANE STRUCTURE SATORU MURAKAMI and LESTER PACKER From the Department of Physiology-Anatomy, University of California, Berkeley, California 94720 Downloaded from http://rupress.org/jcb/article-pdf/47/2/332/1069424/332.pdf by guest on 29 September 2021 ABSTRACT Light changes the structure of chloroplasts . This effect was investigated by high resolution electron microscopy, photometric methods, and chemical modification . (a) A reversible contraction of chloroplast membrane occurs upon illumination, dark titration with H+, or increasing osmolarity . These gross structural changes arise from a flattening of the thylakoids, with a corresponding decrease in the spacing between membranes . Microdensitometry showed that illumination or dark addition of H+ resulted in a 13-23% decrease in mem- brane thickness. Osmotically contracted chloroplasts do not show this effect . (b) Rapid glutaraldehyde fixation during actual experiments revealed that transmission changes are closely correlated with the spacing changes and therefore reflect an osmotic mechanism, whereas the light scattering changes have kinetics most similar to changes in membrane thickness or conformation . (c) Kinetic analysis of light scattering and transmission changes with the changes in fluorescence of anilinonaphthalene sulfonic acid bound to membranes revealed that fluorescence preceded light scattering or transmission changes. (d) It is concluded that the temporal sequence of events following illumination probably are proto- nation, changes in the environment within the membrane, change in membrane thickness, change in internal osmolarity accompanying ion movements with consequent collapse and flattening of thylakoid, change in the gross morphology of the inner chloroplast membrane system, and change in the gross morphology of whole chloroplasts . INTRODUCTION Ample evidence has been brought forward in changes in chloroplast membranes is still undeter- recent years to demonstrate, both in vitro (1-9) mined . -
Hydrogen Atomic and Molecular Hydrogen
Hydrogen Hydrogen, the simplest atom, combines with itself to make the simplest molecule, H2. Most other elements in the periodic table combine with hydrogen to make compounds. The chemical bonds between hydrogen and other elements result from sharing electrons. The electrons are shared equally in non-polar covalent bonds and unequally in polar covalent bonds. The chemical energy stored in covalent bonds can be transformed into heat or electrical energy. Outline • Atomic and Molecular Hydrogen • Hydrogen Compounds • Energy from Hydrogen • Homework Atomic and Molecular Hydrogen Electronic Structure of Atomic Hydrogen We can represent a hydrogen atom with the symbol H and a dot that stands for the single electron in the neutral atom. In its lowest energy form, the electron occupies the 1s orbital, spherically symmetrical around the hydrogen nucleus. As you saw in the section on electronic configuration, all atoms have many possible energy levels for their electrons. The lowest energy state (ground state) of an atom has its electrons filling orbitals beginning from lowest energy, with 2 electrons per orbital. When energy is added to the ground state atom, an electron can be promoted to one of the higher energy orbitals. The energy added must be exactly the same as the energy between the orbital occupied by the electron and one of the higher energy, unoccupied orbitals. Below you can see an orbital energy diagram showing the ground state hydrogen atom on the left. When hydrogen absorbs a quantity of energy exactly equal to ΔE1, the electron goes from the orbital in the first shell (n = 1) to an orbital in the second shell (n = 2). -
(12) United States Patent (10) Patent No.: US 8,333,944 B2 Constantz Et Al
USOO833394.4B2 (12) United States Patent (10) Patent No.: US 8,333,944 B2 Constantz et al. (45) Date of Patent: *Dec. 18, 2012 (54) METHODS OF SEQUESTERING CO2 61/073,319, filed on Jun. 17, 2008, provisional application No. 61/082,766, filed on Jul. 22, 2008, (75) Inventors: Brent R. Constantz, Portola Valley, CA provisional application No. 61/088,340, filed on Aug. (US); Andrew Youngs, Antelope, CA 12, 2008, provisional application No. 61/088,347, (US); Philip Brian Tuet, Milpitas, CA filed on Aug. 13, 2008, provisional application No. (US); Sidney Omelon, Willowdale (CA): 61/101,626, filed on Sep. 30, 2008, provisional Kasra Farsad, San Jose, CA (US); application No. 61/121,872, filed on Dec. 11, 2008. Ryan J. Gilliam, San Jose, CA (US); Valentin Decker, San Jose, CA (US); (51) Int. C. Donald W. Kirk, Caledon (CA); J. BOID 53/62 (2006.01) Douglas Way, Boulder, CO (US); Allen BOID 53/78 (2006.01) J. Bard, Austin, TX (US); Robert (52) U.S. C. ......... 423/225; 423/220; 423/230; 423/234 Danziger, Carmel, CA (US); Miguel (58) Field of Classification Search .................. 423/210, Fernandez, San Jose, CA (US); Cecily 423/220, 225, 230, 234 Ryan, San Jose, CA (US) See application file for complete search history. (73) Assignee: Calera Corporation, Los Gatos, CA (56) References Cited (US) U.S. PATENT DOCUMENTS (*) Notice: Subject to any disclaimer, the term of this 1,169,766 A 2f1916 Brassert patent is extended or adjusted under 35 (Continued) U.S.C. 154(b) by 40 days. FOREIGN PATENT DOCUMENTS This patent is Subject to a terminal dis claimer. -
Chem 150, Spring 2015 Unit 4
Chem 150, Spring 2015 Unit 4 - Acids & Bases Introduction • Patients with emphysema cannot expel CO2 from their lungs rapidly enough. ✦ This can lead to an increase of carbonic acid (H2CO3) levels in the blood and to a lowering of the pH of the blood by a process called respiratory acidosis. CO2 + H2O → H2CO3 Chem 150, Unit 4: Acids & Bases 2 Introduction • Carbonic acid (H2CO3), along with its conjugate - base, the bicarbonate ion (HCO3 ), play an important role as a buffer that maintains blood pH at around 7.4. − + H2CO3 ! HCO3 + H Chem 150, Unit 4: Acids & Bases 3 Introduction • Carbonic acid (H2CO3), along with its conjugate - base, the bicarbonate ion (HCO3 ), play an important role as a buffer that maintains blood pH at around 7.4. − + H2CO3 ! HCO3 + H acid base Chem 150, Unit 4: Acids & Bases 3 7.1 The Self-Ionization of Water • When two water molecules are hydrogen bonded to one another, the acceptor (base) occasionally pulls a hydrogen ion away from the donor (acid). The products are a hydronium ion + (H3O ) and a hydroxide ion. Chem 150, Unit 4: Acids & Bases 4 7.1 The Self-Ionization of Water • When two water molecules are hydrogen bonded to one another, the acceptor (base) occasionally pulls a hydrogen ion away from the donor (acid). The products are a hydronium ion + (H3O ) and a hydroxide ion. base acid Chem 150, Unit 4: Acids & Bases 4 7.1 The Self-Ionization of Water • When two water molecules are hydrogen bonded to one another, the acceptor (base) occasionally pulls a hydrogen ion away from the donor (acid). -
Hydrogen Ion Input to the Hubbard Brook Experimental Fomst, New Hampshire, During the Last Decade^
HYDROGEN ION INPUT TO THE HUBBARD BROOK EXPERIMENTAL FOMST, NEW HAMPSHIRE, DURING THE LAST DECADE^ GENE E. LIKENS, Section of Ecology & Systematics, Cornell University, Ithaca, New York 14853; F. HERBERT BORMANN, School of Forestry and Environmental Studies, Yale Univer- sity, 370 Prospect Street, New Haven, Connecticut 06511; JOHN S. EATON, Section of Ecology & Systematics, Cornell University, Ithaca, New York 14853; ROBERT S. PIERCE, Northeastern Forest Experiment Station, Forestry Sciences Lab.; P. 0. Box 640, Durham, New Hampshire 03824; and NOYE M. JOHNSON, Department of Earth Sciences, Dartmouth College, Hanover, New Hampshire 03755. ABSTRACT Being downwind of eastern and midwestern industrial centers, the Hubbard Brook Experimental Forest offers a prime location to monitor long-term trends in atmospheric chemistry. Con- tinuous measurements of precipitation chemistry during the last 10 years provide a measure of recent changes in precipi- tation inputs of hydrogen ion. The weighted average pH of precipitation during 1964-65 to 1973-74 was 4.14, with a minimum annual value of 4.03 in 1970-71 and a maximum annual value of 4.21 in 1973-74. The sum of all cations except hydrogen ion decreased from 51 peq/R in 1964-65 to 23 peq/R in 1973-74 providing a significant drop in neutralizing capacity during this period. Based upon regression analysis, the input in equivalents of hydrogen ion and nitrate increased by 1.4-fold and 2.3-fold respectively, from 1964-65 to 1973-74. Input of all other ions either decreased or showed no trend. Based upon a stoichiometric formation process in which a sea-salt, anionic component is subtracted from the total anions in precipitation, SOZ contribution to acidity dropped from 83% to 66%, whereas NO: increased from 15% to 30% during 1964-65 to 1973-74. -
GRADES 6-12 DISTANCE LEARNING School Name Aledo High School
GRADES 6-12 DISTANCE LEARNING School Name Aledo High School Grade Level Chemistry - Mrs. Henyon Week of 4/20/20, 4/27/20, 5/4/20 *All assigned work due by Sunday at midnight on 5/10/2020 (SUBJECT AREA) Estimated Time to Complete: 6 hours Resources Needed: Computer (if applicable), Scientific calculator, Journal, pen/pencil, Color pencils Lesson Delivery (What do we want you to learn?): 1. Define acids and bases and distinguish between Arrhenius and Bronsted-Lowrey definitions. 2. Predict products in acid-base reactions that form water. 3. Define pH. 4. Calculate the pH of a solution using the hydrogen ion concentration. Engage and Practice (What do we want you to do?): Digital Students: 1. Watch Video #1 Acids and Bases titled “How to Name Acids”. Due 4/26/20 2. Complete the Classifying Map and Critical Writing in journal. Upload picture of assignments to Google Classroom Due 4/26/20 *these are found in your NOTES. 3. Watch Video #2 Acids and Bases titled “Acid and Base Definitions”. Due 4/26/20 4. Complete HW #1 in your journal. Upload a picture of answers to Google Classroom. Due 5/3/20 5. Watch Video #3 titled “Self-Ionization of Water and Calculating pH”. Due 5/3/20 6. Complete the pH Worksheet, questions #1-8. Upload a picture of your answers to Google Classroom. Due 5/10/20 7. Complete the Acids and Bases Lab using the pHet simulator. Upload a picture of your work or a saved document to Google Classroom. Due 5/10/20 8. -
Discharge of Hydrogen Ions at Metal Cathodes in Alkaline Solutions JW
Discharge of Hydrogen Ions at Metal Cathodes in Alkaline Solutions S. A. AWAD Department of Chemistry, University College for Girls, Ain Shams University, Heliopolis, Cairo, Egypt Received 15 December 1992 A survey is given for the measured pH effects in alkaline solutions on hydrogen overpotential. The results are not in accord with the theoretical value for H+ ion discharge, or with that for the discharge of water molecules. This problem arises from neglecting the role of the stoichiometric number of the reaction in the rate equation. It is suggested that H+ ions are discharged, and the adsorbed hydrogen atoms undergo rapid catalytic combination. In this case the stoichiometric number is 2, and the reaction order with respect to H+ ion is 1/2. This mechanism requires that the overpotential is independent of the alkali concentration. The mechanism accounts satisfactorily for the slight changes in overpotential with the alkali concentration. Evolution of hydrogen at metal cathodes from acid a value of 26 mV, whereas for silver [5] they ob solutions takes place through the discharge of H+ served that the pH effect lies between 25 and 30 ions. In alkaline solutions, however, hydrogen might mV. It is obvious from this survey that the experi originate from the discharge of H+ ions, or from the mental pH effects are too small to indicate exclusively discharge of water molecules. Distinction between the discharge of water molecules. these two entities could be made with the help of It is worth mentioning that in case of mercury the the effect of pH on the overpotential 77.