PPT-Calculating the Average Atomic Mass

Steps for Calculating Average Atomic Mass When given percentages of each isotope and each isotopes mass 1 Convert the percentages into decimals This percentage is known as its relative . Energy Loss. WEATHERIZATION ENERGY AUDITOR SINGLE FAMILY. WEATHERIZATION ASSISTANCE PROGRAM STANDARDIZED CURRICULUM . – December 2012. By attending this session, participants will be able to:. Define basic energy movement. . #1: Rubidium has two common isotopes, . 85. Rb and . 87. Rb. . If the abundance of . 85. Rb is 72.2% and the abundance of . 87. Rb is 27.8%, what is the average atomic mass of rubidium?. PROCEDURE:. All atoms of an element have the same number of protons and the same atomic number.. Learning Goal . Given the atomic number and the mass number of an atom, state the number of protons, neutrons, and electrons.. https://youtu.be/. hhbqIJZ8wCM. What is an Atom?. The simplest particle of an element that retains its properties.. Who is Democritus?. This Greek philosopher was among the first to suggest the existence of atoms . Lesson objectives relative mass. Understand the term ‘isotopes’. Define the terms ‘relative isotopic mass’ and ‘relative atomic mass’ based on the . 12. C scale. Understand the terms ‘relative molecular mass’ and ‘relative formula mass’ including calculating these from relative atomic masses . I. Foundations of the Atomic Theory. A. 400 B.C. –Democritus. 1. Defined nature’s basic particles as . atoms. a. means indivisible. B. 350 B.C. Aristotle. 1. said matter was made of the 4 “elements”. Pre-AP Chemistry. Charles Page High School. Stephen L. Cotton . Section 4.1 Defining the Atom. OBJECTIVES:. Describe. Democritus’s ideas about atoms.. Section 4.1 Defining the Atom. OBJECTIVES:. Explain. Chapter 3. Types of Models – Why do we use models?. Physical Model vs. Conceptual Model. Physical model. is a representation of a very large or small object shown at a convenient scale. . FDR receives a letter from Albert Einstein. Informed FDR of recent developments in splitting uranium atoms. Could lead to “extremely powerful bombs of a new type” by means of nuclear fission. Nucleus absorbs a neutron, breaks into two equal fragments. Composition of Substances and Solutions Atomic Mass and Formula Mass; Mole & Molar Mass; Percent Composition of Compounds; Determination of Empirical & Molecular Formulas; Molarity Other Units for Solution Concentrations III. How atoms differ. . A. Atomic Number. Equal to the number of protons – never changes; equals the number of electrons if AND ONLY IF the atom is . neutral. ; Moseley discovered . each atom has a unique number of protons in the nucleus. Atomic . Mass Number. Where did that decimal come from?. Calculating Average Atomic Mass . I CAN . calculate the Average Atomic Mass Number of an element from its isotope data. .. The Case for a Decimal . Atoms of the same element . can. have different . mass numbers.. Isotopes. How can atoms of the same element end up with a different mass?. Shoulder Partners. Frederick Soddy. (1877-1956) proposed the idea of isotopes in 1912. Daltons Atomic Theory. 1. All elements are composed of tiny . indivisible. particles called atoms.. 2. Atoms of the same element are identical. The atoms of one element are different from the atoms of another element..