will provide personnel with a foundation for understanding the scientific principles that are associated with various DOE nuclear facility operations and maintenance. Training Material‚ Atomic Physics‚ The Chart of the Nuclides‚ Radioactivity‚ Radioactive Decay‚ Neutron Interaction‚ Fission‚ Reactor Theory‚ Neutron Characteristics‚ Neutron Life Cycle‚ Reactor Kinetics Key Words: Rev. 0 NP DOE-HDBK-1019/1-93 NUCLEAR PHYSICS AND REACTOR THEORY F OREWOR D The Departm ent of Energy (DOE)
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Pure Appl. Chem.‚ Vol. 75‚ No. 6‚ pp. 683–800‚ 2003. © 2003 IUPAC INTERNATIONAL UNION OF PURE AND APPLIED CHEMISTRY INORGANIC CHEMISTRY DIVISION COMMISSION ON ATOMIC WEIGHTS AND ISOTOPIC ABUNDANCES* ATOMIC WEIGHTS OF THE ELEMENTS: REVIEW 2000 (IUPAC Technical Report) Prepared for publication by J. R. DE LAETER1‚ J. K. BÖHLKE2‚‡‚ P. DE BIÈVRE3‚ H. HIDAKA4‚ H. S. PEISER2‚ K. J. R. ROSMAN1‚ AND P. D. P. TAYLOR3 of Applied Physics‚ Curtin University of Technology‚ Perth‚ Australia; 2United States
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will be required. 1. Element "E" (not a real symbol for an element)‚ has three naturally occurring isotopes: 60% 228E‚ 25.0% 222E‚ and 15.0% 232E. Use this information to determine the atomic mass of element "E". Atomic Mass = (0.60 x 228g/mol) + (0.25 x 222g/mol) + (0.15 x 232g/mol) = 227.1g/mol (Actinium) 2. Calculate the approximate percent abundance of gallium’s isotopes (69Ga‚ 71Ga) in a sample of gallium metal. Ga atomic mass is 69.72g/mol. Let x be the % of 69Ga as
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obtain the masses and relative concentrations of atoms and molecules and to detect isotopes in a sample based on their masses. In order to do this the method requires an instrument called the ‘mass spectrometer’‚ of which‚ is able extract accurate information of the relative masses of isotopes and their relative abundance. This makes the mass spectrometer very useful for applications such as carbon dating and radioactive dating processes because the combination of a mass spectrometer and a gas chromatograph
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“identity “ of an element as well as its location on the Periodic Table. No two different elements will have the atomic number. 4. The of an element is the average mass of an element ’s naturally occurring atoms‚ or isotopes‚ taking into account the of each isotope. 5. The of an element is the total number of protons and neutrons in the of the atom. 6. The mass number is used to calculate the number of in one atom of an element. In order to calculate the number
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metals red Transition elements green Chalcogens brown Lanthanides orange Actinides light blue 12. Outline the symbol’s box in dark green if it is RADIOACTIVE in its most common form. Notes The nucleus The nucleus is at the center of the atom and contains the protons and neutrons. Protons and neutrons are collectively known as nucleons. Virtually all the mass of the atom is concentrated
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Asimov On Chemistry by Isaac Asimov The Book Asimov on Chemistry by Isaac Asimov is a collection of seventeen essays that he wrote for The Magazine of Fantasy and Science Fiction. This book is one of ten that were published by Doubleday & Company‚ Inc. Not all of the books centered on chemistry and like science. Most just covered anything Isaac Asimov wondered about. These Essays date back quite aways with a range from January 1959 to April 1966. INORGANIC CHEMISTRY The Weighting Game This
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include pennies that are 1982 or newer. 4. Count the number of pennies in each pile. Record the values. 5. Take the mass of each pile of pennies. (One measurement for each pile.) Data: Measurements of the “Pennium” and its two Isotopes Date Number of Pennies Mass (in grams) Average Mass (in grams) Relative Abundance (percent) Atomic Mass (grams) Total Pennies 20 -------------- ---------- -------- 2.800 Older than 1982 10 30.90 3.090 50 --------------- 1982 or newer 10 25
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CHM130 Lab 5 The Atomic Mass of Beanium Name: Paige Miller A. Data Table: Insert your Data Table here with your sample calculations. You must show at least one sample calculation per procedure step. (16 points) Part I Data Table Sample Mass (mg) Number/Qty Average Mass (mg) Relative Abundance Relative Weight (mg) Kidneybeanium 1660.00 mg 3 553.33 mg 0.2143 118.58 mg Pintobeanium 2830.00 mg 6 471.67 mg 0.4286 202.16 mg Blackeyedpeaium 1110.00 mg 5 222.00 mg
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Assignment Chapter 2 Concept Explorations 2.25. Average Atomic Mass Part 1: Consider the four identical spheres below‚ each with a mass of 4.00 g. a. Calculate the average mass of a sphere in this sample. (4.00 + 4.00 + 4.00 + 4.00)/4= 16.00/4= 4.00g Part 2: Now consider a sample that consists of four spheres‚ each with a different mass: blue mass is 4.00 g‚ red mass is 3.75 g‚ green mass is 3.00 g‚ and yellow mass is 1.25 g. * a. Calculate the average mass of a sphere in this sample
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