...Harry S. Truman was born on May 8th, 1884 in Missouri and spent most of his childhood on his family’s farm. His name was chosen after his mother’s brother. He had a brother and a sister. Their names were john Vivian (1886-1965), and Mary Jane (1889-1978). His father’s name is john Anderson Truman (1851-1914), and his mother’s name is Martha Ellen young Truman (1846-1916). John was a livestock dealer. Harry and his family moved to a farm near harrisonville when he was 10 months old. They went on to live in Belton and in 1887 they moved to his grandparent’s 600 acre farm in Grandview. When he was 6 years old his family moved into a small town called independence, so he could attend a Presbyterian Church Sunday school. Harry did not go...
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...In a speech given by Harry S. Truman, announcing the usage of the A-Bomb in Hiroshima, he informs the people of the United States what has happened and why it happened. The speech was given sixteen hours after the bomb was dropped. Harry Truman then explains why the American airplane dropped the bomb in the first place, “The Japanese began the war from the air at Pearl Harbor. They have been repaid…”(Truman, Paragraph 2). Truman then goes on the explain the bomb and why it was so effective. He explains how powerful this bomb actually was and how it was a new weapon of war. “That bomb had more power than 20,000 tons of T.N.T. It had more than two thousand times the blast power of the british ‘Grand Slam’ which is the largest bomb ever yet used in the history of warfare”(Truman, Paragraph 1) Largest is what Truman explains the bomb as. That means that the military...
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...Name Lab Section Date The Mole Concept and Atomic Weights Text Reference: Tro, Chemistry: Structure and Properties Section 2.8 - Atoms and the Mole: How Many Particles? Section 1.9 – Atomic Mass: The Average of an Element’s Atoms The purpose of this activity is to better understand the concepts of relative atomic mass, counting by weighing and the mole. Per cent composition and average atomic mass are included. Part I. Relative Atomic Masses and the Mole – Early Method When John Dalton proposed his atomic theory, he stated that the atoms of each element had a characteristic mass. He carried out experiments to determine the relative atomic mass of each element. To do this, he had to establish a standard because a single atom was too small to weigh. The standard he chose was that the mass of hydrogen would be set equal to 1.000. In a simple experiment, Dalton would measure the grams of an element such as sulfur that reacted with 1.00 gram of hydrogen. For sulfur, the reacting mass was found to be 32.0 grams, and so 32.0 was the relative mass of sulfur with respect to the standard hydrogen. (Note: The current standard for atomic mass is the most abundant isotope of carbon, C-12, with an assigned mass of exactly 12.000 amu.) The following activity will demonstrate how the relative mass method works. 1. Weigh five of the red color balls to three decimal places. Be sure to tare out the mass of the plastic cup. Record the mass in the table below. 2. Weigh five...
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... The Office of the Deputy Chief of Staff for Intelligence J2 is publishing this “Human Rights-Based Intelligence Operations Guidebook (Rules of Behavior for Military Intelligence Personnel)” with this objective in mind, to broaden the public’s understanding of our mission and challenges, and to help us become better and stronger partners committed to serve and defend our country. Designed to further harmonize all intelligence operations with the principles of human rights and International Humanitarian Law (IHL), this Guidebook is one of the contributions of the AFPIC to the Internal Peace and Security Plan (IPSP) “Bayanihan” of the AFP and to the Security Sector Reform Agenda of the Commanderin-Chief, President Benigno S Aquino III. The essential characteristics of this Guidebook can be best expressed by the acronym: AFPCAReS AFPCAReS Adherence to International Humanitarian Law and the Rule of Law The AFPIC strictly adheres to the Constitution and the principles of the International Humanitarian Law. Focused in the Conduct of Intelligence Operations Intelligence operations shall be conducted only against known military targets and armed insurgents....
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...Proton Nucleus 1 amu Positive Neutron Nucleus 1 amu Neutral Electrons Electron Cloud 0 amu Negative Valence electrons: electrons in the outermost shell of an atom. Atomic Weight: the ratio of the average mass of atoms of an element (average weight of all the isotopes) (# of protons + # of electrons) Atomic Mass: the mass of a specific isotope Atomic number: the number of protons found in the nucleus of an atom Periods: In the periodic table, each horizontal row is called a period. The elements in each period have the same number of shells. Groups: Each vertical column is called a group. Each of the elements in the same group has the same number of valence electrons in their outer shells. Covalent Bond: atoms share the electrons. Ionic Bond: one atom wants to give away an extra electron(s) that it doesn’t need, and one atom wants more electrons to have a complete shell. The atom that gives away an electron becomes positive (*at first it was neutral, but since it gave an electron, which is negative, away, it became positive.), and the one that gains an electron becomes negative. They are held together like magnets (static-magnetic force). Important info: Number of Protons = Atomic Number Number of Electrons = Number of Protons = Atomic Number Number of Neutrons = Mass Number - Atomic...
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...Atomic structure was originally devised by ancient Greek philosophers; However over recent years this theory has been modified and changed by many different scientists, such as Dalton, Thompson, Rutherford, Bohr and Chadwick. In 1808 John Dalton in his book “new systems of chemical philosophy.” Proposed that elements are composed of many discrete and invisible particles which are called atoms, atoms of the same element have identical properties and atoms of different elements have different properties. Compounds are composed of atoms of more than one element and also that a chemical reaction involves the separation, combining or rearranging of atoms. He was also responsible for part of the periodic table, as it was he who introduced the idea of chemical symbols, being the first to discover carbon dioxide. In the late 1800s and early 1900s J. J. Thomson conducted some experiments that did not agree with Dalton’s earlier atomic theory. He performed experiments using a Cathode ray tube. He conducted electricity through gases, causing a glow to be seen at the furthest end of the cathode tube. This proved that cathode rays must be made of something which has a negative charge. Thomson then concluded that atoms have tiny particles inside them called electrons which have a negative charge. He knew that on the whole atoms were neutral, so he came up with a theory that there must be a positive charge within the atom which would balance out the charge of the negative electrons. He suggested...
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...SQ 1-1 Define the term ‘element’, and state the number of naturally occurring elements. Identify by name and the chemical symbol the 4 most abundant elements found in the human body. Identify by name and chemical symbol at least 4 trace elements. An element is the simplest form of matter and cannot be broken down into simpler substances in a chemical reaction. Elements have unique properties. There are 91 natural occurring elements, 24 of these elements play a normal physiological role in humans. The 4 most abundant elements found in the body are oxygen (O), carbon(C), Hydrogen (H) and Nitrogen (N). there are 8 major or less elements in the body include calcium(Ca), phosphorus(P), sulfur(S), potassium(K), sodium(Na), chlorine(Cl), Magnesium(Mg) and iron(Fe). Trace elements account 0.7% of body weight and play a vital roles in physiology, they include, cobalt (Co), copper (Cu), fluorine (F), and iodine (I) Define the term ‘atom’. Discuss the structure of an atom including A) the name of the 3 major types of subatomic particles, B) the electrical properties of each of these subatomic properties, and C) the arrangement of these subatomic particles in the atom including a brief description of electron shells or energy levels. An atom is the smallest unit of an element which consists of a proton (P), neutron (n) and an electron (e). Protons are positively charges, electrons are negatively charged and neutrons have no charges i.e. are neutral. Both the proton and neutron are...
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...Postulates of Dalton’s Atomic Theory The main points of Dalton’s atomic theory, an explanation of the structure of matter in terms of different combinations of very small particles, are given by the following postulates: 1. All matter is composed of indivisible atoms. An atom is an extremely small particle of matter that retains its identity during chemical reactions. 2. An element is a type of matter composed of only one kind of atom, each atom of a given kind having the same properties. Mass is one such property. Thus, the atoms of a given element have a characteristic mass. 3. A compound is a type of matter composed of atoms of two or more elements chemically combined in fixed proportions. The relative numbers of any two kinds of atoms in a compound occur in simple ratios. Water, for example, a compound of the elements hydrogen and oxygen, consists of hydrogen and oxygen atoms in the ratio of 2 to 1. 4. A chemical reaction consists of the rearrangement of the atoms present in the reacting substances to give new chemical combinations present in the substances formed by the reaction. Atoms are not created, destroyed, or broken into smaller particles by any chemical reaction. Main Points of the Bohr Model Postulate 1: An electron in an atom moves in a circular orbit under the influence of coulomb attraction between the electron and the nucleus obeying the rules of classical mechanics. Postulate 2: An atom can exist in certain allowed or stationary states, with each...
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...CHM 1101 Introductory Chemistry Dawn Fox Medeba Uzzi August, 2007 Compiled and edited by Medeba Uzzi Authors’ Note This document is an initiative by the authors in an attempt to deal with what they think may be one of the reasons contributing to the relatively high failure rate in the introductory Chemistry course (CHM 1101) at the University of Guyana. It was brought to our attention that many first year students taking CHM 1101 are unable to efficiently cope with the frenetic pace of the Semester system and even less able to deal comprehensively with the large content in CHM 1101. It is hoped that by providing this paper, students will not need to make lots of notes in lectures and so they can focus on grasping the concepts taught. The document is meant to be a guide to the topics covered in CHM 1101 and is by no means exhaustive. Students are still required to attend classes regularly and punctually and to engage meaningfully in lectures and tutorials. Further, supplemental reading of these topics in any good General Chemistry text is expected. Dawn Fox Medeba Uzzi 2 SECTION 1 – Modules A – D: section deals with the foundation for chemistry. It introduces students to matter & its classification, Atom & its structure, Periodic table and chemical rxns. Introduction to Science and Measurement What is Chemistry? – Chemistry is the study of matter and its transformations Natural sciences refer to the systematic study of the natural world (our...
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...Chapter 6: Quantum Mechanics (note: these notes include a review of Chemistry I Honors, the AP notes are in dark red) The Bohr Atom Thompson: plum pudding Rutherford: nucleus in a sea of electrons. Bohr: planetary model. Wave velocity = (wavelength)(frequency). Review of wave mechanics. The electromagnetic spectra: The type of wave is determined by its wavelength and frequency. Speed of light = 2.998 x 108 m/s A light wave has a frequency of 1.74 x 1017 hertz. What is its wavelength? What type of light is it? Planck’s Hypothesis Light is given off in bundles of energy called quanta. E = h( Energy = planck’s constant * wave frequency h = 6.626 x 10-34 J/hz Energy Problems A photon of light is found to have 3.63 x 10-22 Joules of energy. What is the wavelength of this light wave? A photon of light is found to have a wavelength of 5.00 x 102 nm. What is the energy of a photon of this light wave? Planck’s Hypothesis Atomic Spectra: produced when an electron moves from a higher to lower energy level, giving off light in the process. (E = Ehi - Elo = h( = hc/( Ex. For the yellow line in the sodium spectra (( = 589.0 nm), find its frequency, quantum energy, and the energy released by one mol of sodium electrons.What is the energy difference between two energy levels of Na? Planck’s Hypothesis ( ( 5.090 x 1014s-1 (E = 3.373 x 10-19 J For one mol of electrons: (E = 203.1 kJ Hence a two energy level difference = 203.1 kJ/mol Bohr Model Bohr postulated...
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...Pre-lab discussions The arrangement of the periodic table is according to the periodic law. The periodic law states that arrangements of the elements are in order of increasing atomic number with both their chemical and physical properties showing a periodic pattern. Students through carrying of laboratory experiments discover these properties of elements in the periodic table. Major properties to be examined are first ionization energy, atomic radius, physical and chemical properties. Purpose To understand periodic trends as it relates to atomic radius, first ionization energy, physical and chemical properties of elements. Equipments and Materials 8 test-tubes Aluminum (Al) Magnesium (Mg) Silicon (Si) Bunsen burner...
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...Employee Absenteeism Kmart Corporation Alvin Williams Professor Whatley LG415 Quality Control Park University INTRODUCTION The purpose of this research paper is to identify employee absenteeism and explain the process of how Kmart was able to successfully merge with Sears effectively without completely diminishing employee morale and loyalty. Let us first begin by going into detail to primarily explain what employee absenteeism is. In the workforce it is described as a failure to appear for work in a routine period of time. It also means the number of occurrences of missed work without valid reasoning. Picture the scenario that you are shopping in Kmart and you have finally completed your shopping to proceed to check out. The time just so happens to be three o’clock, which are the shift change hours for cashiers. There are three customers ahead of you and only two lanes open. You notice that there is a delay in check out times. You finally get to the counter to pay and over hear the cashier complaining that she will have to stay another two hours because her replacement has called out sick once again, without proper notice. At this point the cashier becomes a little irritated in her responses and appears to be in no way interested in pleasing the customer. What happened to the employee that was smiling just three customers before you? I can easily explain. The motivation the...
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...Cl-35 Ar-40 K-39 Ca-40 2. Neutrons have no charge and a mass of 1 amu. 3. Electrons are small and are negatively charged (-) with a mass of almost 0 amu.. 4. Protons & neutrons are in an atom’s nucleus (nucleons). Which has the greatest number of nucleons? Sn-119 Sb-122 Te-128 I-127 5. Electrons are found in “clouds” (orbitals) around an atom’s nucleus. Where is most of the mass of an atom found? Where is most of the size (volume) of an atom found? 6. The mass number is equal to an atom’s number of protons and neutrons added together. What is the mass number of an atom with 18 protons and 22 neutrons? 7. The atomic number is equal to the number of protons in the nucleus of an atom. Which has the greatest atomic number? S Cl Ar K 8. The number of neutrons = mass number – atomic number. Which correctly represents an atom of neon containing 11 neutrons? 11Ne 21Ne 20 Ne 22Ne 9. In a neutral atom the number of protons = the number of electrons. 10. Isotopes are atoms with equal numbers of protons, but differ in their neutron numbers. Two isotopes of the same element will have the same number of neutrons and electrons, neutrons and nucleons, protons and nucleons, protons and electrons 13. Ernest Rutherford’s gold foil experiment showed that an atom is mostly empty space with a small, dense, positively charged nucleus. 14. J.J. Thompson discovered the electron and developed...
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...The University Student Registration System: a Case Study in Building a High-Availability Distributed Application Using General Purpose Components M. C. Little, S. M. Wheater, D. B. Ingham, C. R. Snow, H. Whitfield and S. K. Shrivastava Department of Computing Science, Newcastle University, Newcastle upon Tyne, NE1 7RU, England. Abstract Prior to 1994, student registration at Newcastle University involved students being registered in a single place, where they would present a form which had previously been filled in by the student and their department. After registration this information was then transferred to a computerised format. The University decided that the entire registration process was to be computerised for the Autumn of 1994, with the admission and registration being carried out at the departments of the students. Such a system has a very high availability requirement: admissions tutors and secretaries must be able to access and create student records (particularly at the start of a new academic year when new students arrive). The Arjuna distributed system has been under development in the Department of Computing Science for many years. Arjuna’s design aims are to provide tools to assist in the construction of fault-tolerant, highly available distributed applications using atomic actions (atomic transactions) and replication. Arjuna offers the right set of facilities for this application, and its deployment would enable the University to exploit the existing...
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...AS/A Level GCE GCE Chemistry A OCR Advanced Subsidiary GCE in Chemistry A H034 OCR Advanced GCE in Chemistry A H434 Vertical black lines indicate a significant change to the previous printed version. © OCR 2008 version 2 – February 2008 QAN 500/2425/5 QAN 500/2347/0 Contents 1 About these Qualifications 1.1 1.2 1.3 1.4 1.5 The Three-Unit AS The Six-Unit Advanced GCE Qualification Titles and Levels Aims Prior Learning/Attainment 4 4 4 5 5 5 2 Summary of Content 2.1 2.2 AS Units A2 Units 6 6 7 3 Unit Content 3.1 3.2 3.3 3.4 3.5 3.6 AS Unit F321: Atoms, Bonds and Groups AS Unit F322: Chains, Energy and Resources AS Unit F323: Practical Skills in Chemistry 1 A2 Unit F324: Rings, Polymers and Analysis A2 Unit F325: Equilibria, Energetics and Elements A2 Unit F326: Practical Skills in Chemistry 2 8 8 20 38 40 51 62 4 Schemes of Assessment 4.1 4.2 4.3 4.4 4.5 4.6 4.7 4.8 AS GCE Scheme of Assessment Advanced GCE Scheme of Assessment Unit Order Unit Options (at AS/A2) Synoptic Assessment (A Level GCE) Assessment Availability Assessment Objectives Quality of Written Communication 64 64 65 66 66 66 67 67 68 5 Technical Information 5.1 5.2 5.3 5.4 5.5 5.6 5.7 5.8 5.9 Making Unit Entries Making Qualification Entries Grading Result Enquiries and Appeals Shelf-life of Units Unit and Qualification Re-sits Guided Learning Hours Code of Practice/Subject Criteria/Common Criteria Requirements Arrangements for Candidates with Particular...
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