DOCSLIB.ORG

Nuclear Chemistry Packet

Total Page：16

File Type：pdf, Size：1020Kb

Download full-text PDF Read full-text

Load more

Science Learning Packet CHEM A: Nuclear Chemistry Packet science learning activities for SPS students during the COVID-19 school closure. Seattle Public Schools is committed to making its online information accessible and usable to all people, regardless of ability or technology. Meeting web accessibility guidelines and standards is an ongoing process that we are consistently working to improve. While Seattle Public Schools endeavors to only post documents optimized for accessibility, due to the nature and complexity of some documents, an accessible version of the document may not be available. In these limited circumstances, the District will provide equally effective alternate access. Due to the COVID-19 closure, teachers were asked to provide packets of home activities. This is not intended to take the place of regular classroom instruction but will help supplement student learning and provide opportunities for student learning while they are absent from school. Assignments are not required or graded. Because of the unprecedented nature of this health crisis and the District’s swift closure, some home activities may not be accessible. If you have difficulty accessing the material or have any questions, please contact your student’s teacher. CHEM A (Nuclear Science) Seattle Public Schools Science Learning Packet March 2020 INTRODUCTION: Take Home Unit – Nuclear Science Nuclear science is a hotly debated area of research. Many people feel uncomfortable with nuclear energy because of how it has been used or famous meltdowns such as Chernobyl. The scientific community views nuclear research as the next step toward a sustainable future. Both sides of the debate have valid reasoning, but to participate fully, you must fully understand the science and arguments on both sides. Throughout this unit, you will complete an activity or group of activities to understand different forms of nuclear change. You will then read a pro and con article about the effects of this type of nuclear change. Why should you do this? The nuclear unit dives into two key standards that all high school students are expected to know by their Junior year. These two standards are not taught in any other science course in high school. How can you do the labs? The nuclear unit has a few labs that are used to model different changes. 4.5a requires 15 marshmallows and 15 gummy bears. These can be replaced with any candies or items (candy is more fun because you can eat them!). You could also just use your imagination and draw the different atoms. 4.8a requires 50-100 pennies (or any item with two sides) and the same amount of paper clips (or another item to replace the pennies over time). Following the instructions should make it easy to complete. There is a video at the end of the assignment if you do not have materials. 4.4a and 4.7a both require java. Many home computers have java and you are able to download it onto your school computer, butit is difficult. There are linked videos as alternatives if you cannot get them to work. What resources do I have to be successful? All the materials you need are on this OneNote. In order to participate in the final discussion, you will need to go onto schoology. Your teachers are still available to you and will communicate in means that work for them and you. Use the timeline below to keep track and learn as much as you can within the time you have away from the school building. Week 1: Finish 4.1, 4.2, and 4.3a-c, SIR PART 1 - be sure you understand the band of stability, fill in the learning tracking tool Week 2: Finish 4.4, 4.5, and 4.6, SIR PART 2- be sure you can draw simple models of fission and fusion, fill in learning tracking tool Week 3: Finish 4.7a-c – be sure you can draw simple models of alpha and beta decay, fill in learning tracking tool Week 4: Finish 4.8a-b, SIR PART 3, and 4.9 - be sure you can explain half-life and what happens to unstable atoms, finish learning tracking tool Week 5: Finalize understanding of Nuclear Sciences, fill in discussion assignment on schoology (4.9), contact teacher for any assessments Chem A Unit Page 1 4.1 Nuclear Phenomenon Tuesday, March 17, 2020 11:20 AM Driving Question: Does the pursuit of Nuclear Science benefit or harm society? Intro: For the Nuclear Unit, we will be developing a pro/con argument for the study of nuclear science. By the end of the unit, you shall be able to argue FOR and AGAINST the pursuit of nuclear science. Directions: Answer the two questions below BEFORE continuing in the activity. Then watch videos showing the costs of nuclear science. You will then answer questions about the costs. After that, you will do independent research about the benefits. BEFORE watching the videos or hearing the story, answer these two questions: 1. What are some costs of nuclear science? 2. What are some benefits of nuclear science? WARNING: You are going to watch a video about the devastation from the Atomic Bombs dropped on Hiroshima and Nagasaki. These are real events where numerous people died. CBBC Newsround: Hiroshima - A survivor's story in animation Now watch these videos to continue thinking about the costs of Nuclear Science: The Atomic Bombing of Hiroshima | The Daily 360 | The New York Times Chem A Unit Page 2 Hanford nuclear site is America's most toxic place COSTS: Reflect on what you've seen so far. 3. What are some costs to nuclear research and technology? 4. Discuss the costs with a family member or friend. What did they say? BENEFITS: Go to this website and look around: https://www.nei.org/advantages Pick TWO advantages to read about and take notes. 5. Take notes from the site: Topic 1 Picked: Notes (must take at least 3 notes on the benefits): Chem A Unit Page 3 Topic 2 Picked: Notes (must take at least 3 notes on the benefits): 6. Discuss your advantage with a family member or a friend. Summarize what they said: 7. Add to your Learning Tracking Tool what you discovered in this first activity. Be sure to had a BENEFIT and a COST. Chem A Unit Page 4 4.2 Isotopes Tuesday, March 17, 2020 11:23 AM Pre Activity questions: 1. What is an isotope? Atom Protons Electrons Neutrons A 3 3 4 B 3 2 3 2. Examine the table above - are the atoms A and B of the same element? Explain how you know. Lab Objective: Why is there a decimal for the mass of elements on the periodic table? Below is a data set for a same of hydrogen atoms. A 1 gram sample of hydrogen was evaluated for all the different types of isotopes within the sample: Isotopes Found Hydrogen-1 Hydrogen-2 Hydrogen-3 Atomic Mass 1 AMU 2 AMU 3 AMU Total mass within 1g sample 0.99g 0.099g 0.001g Percent of total mass 99% 0.99% 0.01% 3. The atomic mass recorded on the periodic table for Hydrogen is 1.01 AMU. Notice that each isotope of Hydrogen is ALWAYS a whole number. Where do you think the decimal came from looking at the data above? The mass on the periodic table is called a WEIGHTED AVERAGE. This means that the mass is not of a single atom, but it is the average of all possible isotopes found of that atom. To calculate weighted average, you take the mass of each isotope, multiply it by the percent of the sample it makes up, and then add them together. Divide this number by 100 and you get the AVERAGE ATOMIC MASS. (99 X 1) + (.99 X 2) + (.01 X 3) = 101 ÷ 100 = 1.01 AMU 4. Using the above paragraph, explain why the mass on the periodic table is a decimal. 5. For hydrogen, which isotope is closest to the mass recorded on the periodic table? Why do you think this is based on the data for hydrogen? Below is the data set for a sample of Carbon Isotopes Found Carbon-12 Carbon-13 Carbon-14 Other Isotopes Atomic Mass 12 AMU 13 AMU 14 AMU Various Total Mass within 1g sample 0.99g 0.009 0.0009 0.0001g Percent of total mass 99% 0.9% 0.09% 0.01% 6. Based on the data above, which of these would most likely be the recorded mass of Carbon on the periodic table? a. 12 b. 12.01 c. 13 Chem A Unit Page 5 c. 13 d. 13.01 e. 14 f. 14.01 7. Explain your answer to 6: 8. If you had 1000 carbon atoms and pulled out just one atom, what would its mass most likely be? 9. Explain your answer to 8: 10. Based on the average atomic mass on the periodic table, examine the 3 isotopes of Sulfur. a. Fill in the table below comparing the 3 isotopes. Protons Electrons Neutrons Mass b. If were able to separate out a single sulfur atom from a 1g sample, how many neutrons would you expect it to have? Explain your answer using the mass on the periodic table. The chart below shows the isotopes that exist for the first six elements. Use the chart and a periodic table to answer questions 11 and 12. Chem A Unit Page 6 11. How many isotopes does hydrogen have? How are they different from each other? 12. Fill in the bolded boxes with the isotope symbol for the isotopes of lithium, beryllium, and boron.
Recommended publications
  • Chlorine Stable Isotopes in Sedimentary Systems: Does Size Matter?

    Chlorine Stable Isotopes in Sedimentary Systems: Does Size Matter?

    Chlorine stable isotopes in sedimentary systems: does size matter? Max Coleman Jet Propulsion Laboratory, Caltech, Pasadena, California, USA ABSTRACT: Stable isotope abundances vary because of size (atomic mass) differences. The chlorine stable isotope system was one of the first described theoretically, but had a slow, disappointment-strewn develop- ment, relative to other elements. Method improvement gave only small, but significant, differences (-1 %.) in compositions of geological materials. Eventually, brines and groundwater chlorides gave larger differences (-5%0). Physical processes like diffusion and adsorption, probably are the main controls of groundwater com- positions. In contrast, the processes producing brine compositions are still enigmatic and need further work for full understanding. Recent work on anthropogenic groundwater contaminants (chlorinated aliphatic hy- drocarbons and perchlorate) shows variations resulting from manufacturing processes; implying possibilities of tracing sources. However, they are subject to microbial degradation, producing much larger fractionations (115%0),but therefore offering better possibility of monitoring natural attenuation. So atomic size is important to give isotopic fractionation and the size of fractionation matters, allowing observation of otherwise unde- tectable processes. lecular and atomic weights by weighing the gases and relating them to the weight of hydrogen. All 1 INTRODUCTION atomic weights were integer multiples the weight of This paper aims to give a short and selective
  • Ichtj Annual Report 2002

    Ichtj Annual Report 2002

    NUCLEAR TECHNOLOGIES AND METHODS 121 PROCESS ENGINEERING CERAMIC MEMBRANES APPLIED FOR RADIOACTIVE WASTES PROCESSING Grażyna Zakrzewska-Trznadel, Marian Harasimowicz, Bogdan Tymiński, Andrzej G. Chmielewski Ceramic membranes (MEMBRALOX® and CeRAM use of different complexing agents are shown in INSIDE®) were used for filtration of liquid radio- Fig.1. Best removal of cobalt, europium and am- active wastes. The experimental runs with samples ericium was observed when chelating polymers of original radioactive wastes were carried out. The NaPAA or PEI were applied. Complexing with poly- waste was characterized by a relatively low salinity acrylic acid of molecular weight 1200 and 8000 did (<1 g/dm3), however, the specific radioactivity not result in sufficient increase of decontamina- was in the medium-level liquid waste range (~150 tion factor. For the membrane of 15 nm pore size, kBq/dm3). The main activity came from radioac- which was used in experiments, the proper molecu- tive cobalt and caesium, but also a significant lar weight of NaPAA was 15 000 or 30 000. In most amount of lanthanides and actinides was present. of experiments the removal of Eu-154 and Am-241 To enhance the separation, membrane filtration was complete (specific activity below the detection was combined with complexation (sole ultrafiltra- limit). Binding the caesium ions with all tested poly- tion gave decontamination factors in the range of mers gave rather poor results. The best complexing 1.1-1.7). Soluble polymers like polyacrylic acid agent for caesium was cobalt hexacyanoferrate, (PAA) derivatives of different average molecular which gave decontamination factors higher than weight, polyethylenimine (PEI) and cyanoferrates 100.
  • 12 Natural Isotopes of Elements Other Than H, C, O

    12 Natural Isotopes of Elements Other Than H, C, O

    12 NATURAL ISOTOPES OF ELEMENTS OTHER THAN H, C, O In this chapter we are dealing with the less common applications of natural isotopes. Our discussions will be restricted to their origin and isotopic abundances and the main characteristics. Only brief indications are given about possible applications. More details are presented in the other volumes of this series. A few isotopes are mentioned only briefly, as they are of little relevance to water studies. Based on their half-life, the isotopes concerned can be subdivided: 1) stable isotopes of some elements (He, Li, B, N, S, Cl), of which the abundance variations point to certain geochemical and hydrogeological processes, and which can be applied as tracers in the hydrological systems, 2) radioactive isotopes with half-lives exceeding the age of the universe (232Th, 235U, 238U), 3) radioactive isotopes with shorter half-lives, mainly daughter nuclides of the previous catagory of isotopes, 4) radioactive isotopes with shorter half-lives that are of cosmogenic origin, i.e. that are being produced in the atmosphere by interactions of cosmic radiation particles with atmospheric molecules (7Be, 10Be, 26Al, 32Si, 36Cl, 36Ar, 39Ar, 81Kr, 85Kr, 129I) (Lal and Peters, 1967). The isotopes can also be distinguished by their chemical characteristics: 1) the isotopes of noble gases (He, Ar, Kr) play an important role, because of their solubility in water and because of their chemically inert and thus conservative character. Table 12.1 gives the solubility values in water (data from Benson and Krause, 1976); the table also contains the atmospheric concentrations (Andrews, 1992: error in his Eq.4, where Ti/(T1) should read (Ti/T)1); 2) another category consists of the isotopes of elements that are only slightly soluble and have very low concentrations in water under moderate conditions (Be, Al).
  • Sulfur and Lead Isotope Characteristics of the Greens Creek Polymetallic Massive Sulfide Deposit, Admiralty Island, Southeastern Alaska

    Sulfur and Lead Isotope Characteristics of the Greens Creek Polymetallic Massive Sulfide Deposit, Admiralty Island, Southeastern Alaska

    Sulfur and Lead Isotope Characteristics of the Greens Creek Polymetallic Massive Sulfide Deposit, Admiralty Island, Southeastern Alaska By Cliff D. Taylor, Wayne R. Premo, and Craig A. Johnson Chapter 10 of Geology, Geochemistry, and Genesis of the Greens Creek Massive Sulfide Deposit, Admiralty Island, Southeastern Alaska Edited by Cliff D. Taylor and Craig A. Johnson Professional Paper 1763 U.S. Department of the Interior U.S. Geological Survey Contents Abstract .......................................................................................................................................................241 Introduction.................................................................................................................................................241 Regional and District Setting ...................................................................................................................242 Terrane Relationships ......................................................................................................................242 District Geology ..........................................................................................................................................242 Deposit Geology .........................................................................................................................................243 Mine Sequence Nomenclature and Stratigraphy .......................................................................243 Ore Types and Ore Mineralogy ................................................................................................................244
  • Pathways for Neoarchean Pyrite Formation Constrained by Mass

    Pathways for Neoarchean Pyrite Formation Constrained by Mass

    Pathways for Neoarchean pyrite formation constrained SPECIAL FEATURE by mass-independent sulfur isotopes James Farquhara,b,1, John Cliffb, Aubrey L. Zerklec, Alexey Kamyshnyd, Simon W. Poultone, Mark Clairef, David Adamsb, and Brian Harmsa aDepartment of Geology and Earth System Science Interdisciplinary Center, University of Maryland, College Park, MD 20742; bCentre for Microscopy and Microanalysis, University of Western Australia, Perth, WA 6009, Australia; cSchool of Civil Engineering and Geosciences, Newcastle University, Newcastle upon Tyne NE1 7RU, United Kingdom; dDepartment of Geological and Environmental Sciences, Faculty of Natural Sciences, Ben-Gurion University of the Negev, Beer Sheva 84105, Israel; eSchool of Earth and Environment, University of Leeds, Leeds LS2 9JT, United Kingdom; and fSchool of Environmental Sciences, University of East Anglia, Norwich NR4 7TJ, United Kingdom Edited by Mark H. Thiemens, University of California at San Diego, La Jolla, CA, and approved December 28, 2012 (received for review November 1, 2012) It is generally thought that the sulfate reduction metabolism is range of variability for Δ33S is significantly greater in samples older ancient and would have been established well before the Neo- than ∼2.4 Ga than in younger samples (e.g., compilation in refs. archean. It is puzzling, therefore, that the sulfur isotope record of 4 and 5). This observation has been linked to the production, the Neoarchean is characterized by a signal of atmospheric mass- transfer, and preservation of mass-independent sulfur isotope independent chemistry rather than a strong overprint by sulfate signals (presumably of atmospheric origin) early in Earth history. reducers. Here, we present a study of the four sulfur isotopes The production of this signal in the atmosphere and its subsequent obtained using secondary ion MS that seeks to reconcile a number transfer to the Earth surface is sensitive to atmospheric O2 levels of features seen in the Neoarchean sulfur isotope record.
  • A Simple and Reliable Method Reducing Sulfate to Sulfide For

    A Simple and Reliable Method Reducing Sulfate to Sulfide For

    A simple and reliable method reducing sulfate to sulfide for multiple sulfur isotope analysis Lei Geng, Joel Savarino, Clara Savarino, Nicolas Caillon, Pierre Cartigny, Shohei Hattori, Sakiko Ishino, | Naohiro Yoshida To cite this version: Lei Geng, Joel Savarino, Clara Savarino, Nicolas Caillon, Pierre Cartigny, et al.. A simple and reliable method reducing sulfate to sulfide for multiple sulfur isotope analysis. Rapid Communications inMass Spectrometry, Wiley, 2017, 32 (4), pp.333-341. 10.1002/rcm.8048. insu-02187037 HAL Id: insu-02187037 https://hal-insu.archives-ouvertes.fr/insu-02187037 Submitted on 17 Jul 2019 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. Received: 12 October 2017 Revised: 5 December 2017 Accepted: 9 December 2017 DOI: 10.1002/rcm.8048 RESEARCH ARTICLE A simple and reliable method reducing sulfate to sulfide for multiple sulfur isotope analysis Lei Geng1 | Joel Savarino1 | Clara A. Savarino1,2 | Nicolas Caillon1 | Pierre Cartigny3 | Shohei Hattori4 | Sakiko Ishino4 | Naohiro Yoshida4,5 1 Univ. Grenoble Alpes, CNRS, IRD, Institut des Rationale: Precise analysis of four sulfur isotopes of sulfate in geological and environmental Géosciences de l'Environnement, IGE, 38000 Grenoble, France samples provides the means to extract unique information in wide geological contexts.
  • Accelerator Mass Spectrometry of 36Cl and 129I Analytical Aspects and Applications

    Accelerator Mass Spectrometry of 36Cl and 129I Analytical Aspects and Applications

    Digital Comprehensive Summaries of Uppsala Dissertations from the Faculty of Science and Technology 1 Accelerator Mass Spectrometry of 36Cl and 129I Analytical Aspects and Applications BY VASILY ALFIMOV ACTA UNIVERSITATIS UPSALIENSIS ISSN 1651-6214 UPPSALA ISBN 91-554-6124-7 2005 urn:nbn:se:uu:diva-4725 Dissertation presented at Uppsala University to be publicly examined in Häggsalen, The Ång- ström Laboratory, Uppsala, Friday, January 21, 2005 at 10:15 for the Degree of Doctor of Philosophy. The examination will be conducted in English. Abstract Alfimov, V. 2005. Accelerator Mass Spectrometry of 36Cl and 129I: Analytical Aspects and Applications. Acta Universitatis Upsaliensis. Digital Comprehensive Summaries of Uppsala Dissertations from the Faculty of Science and Technology 1. 81 pp. Uppsala. ISBN 91-554-6124-7 36 129 Two long-lived halogen radionuclides ( Cl, T1/2 = 301 kyr, and I, T1/2 = 15.7 Myr) have been studied by means of Accelerator Mass Spectrometry (AMS) at the Uppsala Tandem Labo- ratory. The 36Cl measurements in natural samples using a medium-sized tandem accelerator (∼1 MeV/amu) have been considered. A gas-filled magnetic spectrometer (GFM) was proposed for the separation of 36Cl from its isobar, 36S. Semi-empirical Monte-Carlo ion optical calculations were conducted to define optimal conditions for separating 36Cl and 36S. A 180° GFM was constructed and installed at the dedicated AMS beam line. 129I has been measured in waters from the Arctic and North Atlantic Oceans. Most of the 129I currently present in the Earth’s surface environment can be traced back to liquid and gaseous releases from the nuclear reprocessing facilities at Sellafield (UK) and La Hague (France).
  • Technical and Regulatory Guidance Environmental Molecular Diagnostics

    Technical and Regulatory Guidance Environmental Molecular Diagnostics

    Technical and Regulatory Guidance Environmental Molecular Diagnostics New Site Characterization and Remediation Enhancement Tools April 2013 Prepared by The Interstate Technology & Regulatory Council Environmental Molecular Diagnostics Team ABOUT ITRC The Interstate Technology and Regulatory Council (ITRC) is a public-private coalition working to reduce bar- riers to the use of innovative environmental technologies and approaches so that compliance costs are reduced and cleanup efficacy is maximized. ITRC produces documents and training that broaden and deepen technical knowledge and expedite quality regulatory decision making while protecting human health and the envir- onment. With private and public sector members from all 50 states and the District of Columbia, ITRC truly provides a national perspective. More information on ITRC is available at www.itrcweb.org. ITRC is a pro- gram of the Environmental Research Institute of the States (ERIS), a 501(c)(3) organization incorporated in the District of Columbia and managed by the Environmental Council of the States (ECOS). ECOS is the national, nonprofit, nonpartisan association representing the state and territorial environmental commissioners. Its mission is to serve as a champion for states; to provide a clearinghouse of information for state envir- onmental commissioners; to promote coordination in environmental management; and to articulate state pos- itions on environmental issues to Congress, federal agencies, and the public. DISCLAIMER This material was prepared as an account of work sponsored by an agency of the United States Government. Neither the United States Government nor any agency thereof, nor any of their employees, makes any war- ranty, express or implied, or assumes any legal liability or responsibility for the accuracy, completeness, or use- fulness of any information, apparatus, product, or process disclosed, or represents that its use would not infringe privately owned rights.
  • The Application of S Isotopes and S/Se Ratios in Determining Ore

    The Application of S Isotopes and S/Se Ratios in Determining Ore

    Ore Geology Reviews 73 (2016) 148–174 Contents lists available at ScienceDirect Ore Geology Reviews journal homepage: www.elsevier.com/locate/oregeorev The application of S isotopes and S/Se ratios in determining ore-forming processes of magmatic Ni–Cu–PGE sulfide deposits: A cautionary case study from the northern Bushveld Complex Jennifer W. Smith a,b, David A. Holwell a,⁎, Iain McDonald c, Adrian J. Boyce d a Department of Geology, University of Leicester, University Road, Leicester, LE1 7RH, UK b AMTEL, 100 Collip Circle, Suite 205, University of Western Ontario Research Park, London, Ontario N6G 4X8, Canada c School of Earth and Ocean Sciences, Cardiff, University, Park Place, Cardiff CF10 3YE, UK d Scottish Universities Environmental Research Centre, Rankine Avenue, Scottish Enterprise Technology Park, East Kilbride, G75 0QF, UK article info abstract Article history: The application of S/Se ratios and S isotopes in the study of magmatic Ni–Cu–PGE sulfide deposits has long been Received 17 March 2015 used to trace the source of S and to constrain the role of crustal contamination in triggering sulfide saturation. Received in revised form 16 October 2015 However, both S/Se ratios and S isotopes are subject to syn- and post-magmatic processes that may alter their Accepted 20 October 2015 initial signatures. We present in situ mineral δ34S signatures and S/Se ratios combined with bulk S/Se ratios to Available online 22 October 2015 investigate and assess their utility in constraining ore-forming processes and the source of S within magmatic sul- fide deposits. Keywords: – – fi – – Magmatic sulfides Magmatic Ni Cu PGE sul de mineralization in the Grasvally Norite Pyroxenite Anorthosite (GNPA) member, S/Se ratios northern Bushveld Complex was used as a case study based on well-defined constraints of sulfide paragenesis S isotopes and local S isotope signatures.
  • The Isotope Effect: Prediction, Discussion, and Discovery

    The Isotope Effect: Prediction, Discussion, and Discovery

    1 The isotope effect: Prediction, discussion, and discovery Helge Kragh Centre for Science Studies, Department of Physics and Astronomy, Aarhus University, 8000 Aarhus, Denmark. ABSTRACT The precise position of a spectral line emitted by an atomic system depends on the mass of the atomic nucleus and is therefore different for isotopes belonging to the same element. The possible presence of an isotope effect followed from Bohr’s atomic theory of 1913, but it took several years before it was confirmed experimentally. Its early history involves the childhood not only of the quantum atom, but also of the concept of isotopy. Bohr’s prediction of the isotope effect was apparently at odds with early attempts to distinguish between isotopes by means of their optical spectra. However, in 1920 the effect was discovered in HCl molecules, which gave rise to a fruitful development in molecular spectroscopy. The first detection of an atomic isotope effect was no less important, as it was by this means that the heavy hydrogen isotope deuterium was discovered in 1932. The early development of isotope spectroscopy illustrates the complex relationship between theory and experiment, and is also instructive with regard to the concepts of prediction and discovery. Keywords: isotopes; spectroscopy; Bohr model; atomic theory; deuterium. 1. Introduction The wavelength of a spectral line arising from an excited atom or molecule depends slightly on the isotopic composition, hence on the mass, of the atomic system. The phenomenon is often called the “isotope effect,” although E-mail: [email protected]. 2 the name is also used in other meanings.
  • W. M. White Geochemistry Chapter 9: Stable Isotopes

    W. M. White Geochemistry Chapter 9: Stable Isotopes

    W. M. White Geochemistry Chapter 9: Stable Isotopes CHAPTER 9: STABLE ISOTOPE GEOCHEMISTRY 9.1 INTRODUCTION table isotope geochemistry is concerned with variations of the isotopic compositions of elements arising from physicochemical processes rather than nuclear processes. Fractionation* of the iso- S topes of an element might at first seem to be an oxymoron. After all, in the last chapter we saw that the value of radiogenic isotopes was that the various isotopes of an element had identical chemical properties and therefore that isotope ratios such as 87Sr/86Sr are not changed measurably by chemical processes. In this chapter we will find that this is not quite true, and that the very small differences in the chemical behavior of different isotopes of an element can provide a very large amount of useful in- formation about chemical (both geochemical and biochemical) processes. The origins of stable isotope geochemistry are closely tied to the development of modern physics in the first half of the 20th century. The discovery of the neutron in 1932 by H. Urey and the demonstra- tion of variable isotopic compositions of light elements by A. Nier in the 1930’s and 1940’s were the precursors to this development. The real history of stable isotope geochemistry begins in 1947 with the publication of Harold Urey’s paper, “The Thermodynamic Properties of Isotopic Substances”, and Bigeleisen and Mayer’s paper “Calculation of equilibrium constants for isotopic exchange reactions”. Urey not only showed why, on theoretical grounds, isotope fractionations could be expected, but also suggested that these fractionations could provide useful geological information.
  • The Elements.Pdf

    The Elements.Pdf

    A Periodic Table of the Elements at Los Alamos National Laboratory Los Alamos National Laboratory's Chemistry Division Presents Periodic Table of the Elements A Resource for Elementary, Middle School, and High School Students Click an element for more information: Group** Period 1 18 IA VIIIA 1A 8A 1 2 13 14 15 16 17 2 1 H IIA IIIA IVA VA VIAVIIA He 1.008 2A 3A 4A 5A 6A 7A 4.003 3 4 5 6 7 8 9 10 2 Li Be B C N O F Ne 6.941 9.012 10.81 12.01 14.01 16.00 19.00 20.18 11 12 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 3 Na Mg IIIB IVB VB VIB VIIB ------- VIII IB IIB Al Si P S Cl Ar 22.99 24.31 3B 4B 5B 6B 7B ------- 1B 2B 26.98 28.09 30.97 32.07 35.45 39.95 ------- 8 ------- 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 4 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr 39.10 40.08 44.96 47.88 50.94 52.00 54.94 55.85 58.47 58.69 63.55 65.39 69.72 72.59 74.92 78.96 79.90 83.80 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 5 Rb Sr Y Zr NbMo Tc Ru Rh PdAgCd In Sn Sb Te I Xe 85.47 87.62 88.91 91.22 92.91 95.94 (98) 101.1 102.9 106.4 107.9 112.4 114.8 118.7 121.8 127.6 126.9 131.3 55 56 57 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86 6 Cs Ba La* Hf Ta W Re Os Ir Pt AuHg Tl Pb Bi Po At Rn 132.9 137.3 138.9 178.5 180.9 183.9 186.2 190.2 190.2 195.1 197.0 200.5 204.4 207.2 209.0 (210) (210) (222) 87 88 89 104 105 106 107 108 109 110 111 112 114 116 118 7 Fr Ra Ac~RfDb Sg Bh Hs Mt --- --- --- --- --- --- (223) (226) (227) (257) (260) (263) (262) (265) (266) () () () () () () http://pearl1.lanl.gov/periodic/ (1 of 3) [5/17/2001 4:06:20 PM] A Periodic Table of the Elements at Los Alamos National Laboratory 58 59 60 61 62 63 64 65 66 67 68 69 70 71 Lanthanide Series* Ce Pr NdPmSm Eu Gd TbDyHo Er TmYbLu 140.1 140.9 144.2 (147) 150.4 152.0 157.3 158.9 162.5 164.9 167.3 168.9 173.0 175.0 90 91 92 93 94 95 96 97 98 99 100 101 102 103 Actinide Series~ Th Pa U Np Pu AmCmBk Cf Es FmMdNo Lr 232.0 (231) (238) (237) (242) (243) (247) (247) (249) (254) (253) (256) (254) (257) ** Groups are noted by 3 notation conventions.