'Atomic mass' presentation slideshows

CHEM 106. The Periodic Table and Atoms & Nucleii. The Periodic Table. View: ‪The genius of Mendeleev's periodic table Lou Serico‬ . https://www.youtube.com/watch?v=fPnwBITSmgU. Periodic Table (May 2016) Los Alamos National Lab. http://periodic.lanl.gov/index.shtml. Elements in Song

Thomas O. Malone 1 , Jon F. Miller 2,5 , Karen Andriacchi 2 , John Heilmann 3 , Ann Nockerts 2,5 and Liz Schoonveld 4 1 School District of Brown Deer, Wisconsin 2 University of Wisconsin – Madison 3 East Carolina University 4 Madison Metropolitan School District 5 SALT Software, LLC

Atomic Structure. Mass Number. Actual masses of atoms are frustrating to work with.Therefore we use relative comparisons of the masses of atoms. We use the atomic mass unit (amu) which is one-twelfth the mass of a carbon atom that contains six protons and six neutrons.

Chapter 3 - Stoichiometry Average Atomic Mass. Many elements have a # of naturally occurring isotopes. Their atom percents in nature are known as their isotopic abundances. Isotopic abundances and isotopic masses can be measured using mass spectroscopy. When calculating average atomic mass:.

The Periodic Table. G R O U P S. P E R I O D S. The Periodic Table. HALOGENS. The Periodic Table. The Noble Gases. Representing Atoms. The Atomic Number is also the number of PROTONS (or electrons). The Atomic Symbol. Na. 11. The Atomic Mass in amu’s. 22.99.

Elements and The Periodic Table. The “Super 7” Diatomic Elements “ I H ave N o Br ight O r Cl ever F riends” HOFBrICl. History of the Periodic Table. 330 B.C - 4 elements 1800 - 31 elements 1865 - 63 elements Chemists required a systematic method to organize the elements.

ATOMIC STRUCTURE. Atomic Structure. All matter is composed of atoms . Understanding the structure of atoms is critical to understanding the properties of matter. HISTORY OF THE ATOM. John Dalton. 1808.

Chemistry Comes Alive. Anatomy & Physiology. Basic Chemistry. Matter The “stuff” of the universe. Anything that occupies space and has mass. States of matter Solid Liquid Gas. Basic Chemistry. Energy

Ch. 3 & 7 – The Mole. Molar Conversions (p.80-85, 221-226). VERY. A large amount!!!!. A. What is the Mole?. A counting number (like a dozen) Avogadro’s number (N A ) 1 mol = 6.02  10 23 items. A. What is the Mole?. HOW LARGE IS IT???.

P. Sci. Unit 9 Chapter 4 Atoms. Atomic Structure – timeline. Ancient Greece - Democritus proposed the atom – a tiny solid particle that could not be subdivided. 1904 – J.J. Thomson – discovered that atoms contained small, negatively charged particles called electrons.

Atoms. Chapter 4. Section 1: “The Development of the Atomic Theory”. The atom is the smallest unit of all matter. Section 1: “The Development of the Atomic Theory”. Who: Democritis When: 4 th century B.C. What: Suggested that the universe was made of indivisible units.

Organizing the Elements 6.1. Organizing the Elements. 6.1.

How do you know how many atoms and how many elements are in a symbol equation?. CO 2. Tells you how many ELEMENTS there are (an easy way to do this is to count the capital letters). The number tells you how many ATOMS of each of that element there is. Have a go….

Chapter 5: The Periodic Table. 5.1 Organizing the elements 5.2 The Modern Periodic Table 5.3 Representative groups. Section 5.1. Organization of the Elements. Search for Order. 1750 only 17 elements known 1789 Antoine Lavoisier grouped known elements (4 groups) Metals Non-metals Gases

Elements and the Periodic Table. Classification is arranging items into groups or categories according to some criteria. The act of classifying creates a pattern that helps you recognize and understand the behavior of fish, chemicals, or any matter in your surroundings. Classifying Matter.

CHEM 1011. Calorimetry: The Determination of the Specific Heat of a Metal. Calorimetry. Calorimetry – the science of measuring heat transfer. Calorimetry. Principle of Conservation of Energy-

Scandium. By: Jeremy Enneking. Discovered. 1878 Lars Nilson. Atom. Atomic number 21 21 protons 21 electrons 24 neutrons Atomic mass 45. Physical Properties . Silver-white Solid Soft Metallic Density: 2.2989 g/cm³ Melting point: 2802°F Boiling point: 5129.6°F

Review. Isotopes. J.J. Thomson saw that there were two different neon atoms in the cathode ray tube These atoms were different in mass, but the same chemically Atoms of the same element that have a different mass are known as Isotopes. Isotopes. Contain the same number of protons

Ch 2 Atoms/Molecules. Basic structure. John Daltons-Atomic theory JJ Thomson/Crookes-Cathode Ray Tube Experiments & Plum pudding model Rutherford-Gold Foil Experiment Millikin’s Oil Drop Experiment. Protons mass = 1 amu charge +1 Neutrons mass = 1 amu charge 0

1.1.2 Atomic Structure • Describe protons, neutrons and electrons. • Describe the distribution of mass and charge in an atom. • Describe the contribution of protons and neutrons to the nucleus in terms of atomic number and mass number. • Explain the term isotopes.