PPT-Atomic model

Atom map Solvent mask F calcomit F maskomit F modelomit k total F calcomit k mask F maskomit Atom map omit Solvent mask omit F obs Atom map Solvent mask F diff. At the start of WWII in 1939 the atomic bomb had not yet been invented. However, scientists discovered about that time that a powerful explosion might be possible by splitting an atom. This type of bomb could destroy large cities in a single blast and would change warfare forever!. Bell Ringer . Review..Frame. your argument. Bell Ringer: What was the name of the program to build the Atomic Bomb? Who was the lead scientist?. Agenda: Notes/discussion. Objective: Through Discussion and notes students will begin to understands the steps leading to the dropping of the atomic bomb.. #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:. Chemistry. Learning Goals . To be able to . explain and draw atomic structure. Elements. Elements are the . building blocks. of all . matter. on Earth. Elements are made up of . atoms. Differences in . . By Sophia Bocast. What are the Physics behind an Atomic Bomb?. . The immense destructive power of atomic weapons derives from a sudden release of energy produced by splitting the nuclei of the fissile elements making up the bombs' core. The U.S. developed two types of atomic bombs during the Second World War. The first, . On your bell work . sheet, answer the following.. When . are zeros significant? . . When . do you use the fewest number of Significant Figures?. Objectives. The Structure of the Atom. Properties of Subatomic Particles. Chemistry. Videos . Atomic Theory: Dalton, Democritus, Thomson, Rutherford, and Quantum. History of the . atom. . History of the atom Video #2. The Development of the Atomic Theory. J.J. Thomson . Contribution. 1.c. – Students know how to use the periodic table to identify alkali metals, alkaline earth metals and transition metals, trends in ionization energy, electronegativity, and the relative sizes of ions and atoms.. From Astronomy To Biomedicine. Light and Matter .  Spectroscopy. . Generalized interactions  Radiation. . Atomic physics. . Astrophysics. . Plasma physics. . Molecular physics. . Biophysics. Advanced Chemistry. Ms. . Grobsky. Food For Thought. Rutherford’s model became known as the “planetary model”. The “sun” was the positively-charged dense nucleus and the negatively-charged electrons were the “planets”. Bohr’s model explained an unusual event. When electric current flows through a gaseous element, the gas . produces a glowing light, like a neon sign.. If this light is passed through a prism, a pattern of lines appears, with each line having a different color. The pattern depends on the element- neon has one pattern and helium another. What causes these lines and why are they always the same for a given element?. The Nature of Light . The quantum-mechanical model (a.k.a. the electron cloud model) – An atomic model that explains the strange behavior of electrons.. Electrons determine the chemical and physical properties of elements.. Chapter 5. Sub Topics. Introduction to Atomic Spectroscopy. Atomic . Absorption Spectroscopy AAS. Atomic . Emission . Spectroscopy. AES. Interferences and Comparisons. Atomic Absorption and Emission Spectroscopy. Science is based off of observations.. A Scientific Law is a summary of what is seen in observations. . A Scientific Theory is an explanation of why these observations are occurring.. Both laws and theories are tested by using them to predict what would happen in certain situations..