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ATOMS, MOLECULES, AND IONS
Chapter Two: ATOMS, MOLECULES, AND IONS
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Fundamental Chemical Laws
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Figure 2.1 The Priestley Medal is the Highest Honor Given by the American Chemical Society
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Three Important Laws Law of conservation of mass
Mass is neither created nor destroyed Law of definite proportion A given compound always contains exactly the same proportion of elements by mass Copyright © Houghton Mifflin Company. All rights reserved.
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Three Important Laws (continued)
Law of multiple proportions When two elements form a series of compounds, the ratios of the masses of the second element that combine with 1 gram of the first element can always be reduced to small whole numbers. Copyright © Houghton Mifflin Company. All rights reserved.
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Dalton’s Atomic Theory
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Dalton’s Atomic Theory (1808)
Each element is made up of tiny particles called atoms. Copyright © Houghton Mifflin Company. All rights reserved.
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Dalton’s Atomic Theory (1808) (continued)
The atoms of a given element are identical; the atoms of different elements are different in some fundamental way or ways. Copyright © Houghton Mifflin Company. All rights reserved.
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Dalton’s Atomic Theory (continued)
Chemical compounds are formed when atoms combine with each other. A given compound always has the same relative numbers and types of atoms. Copyright © Houghton Mifflin Company. All rights reserved.
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Dalton’s Atomic Theory (continued)
Chemical reactions involve reorganization of the atoms - changes in the way they are bound together. The atoms themselves are not changed in a chemical reaction. Copyright © Houghton Mifflin Company. All rights reserved.
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Plant is Newly Discovered Source of Gold
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Avogadro’s Hypothesis (1811)
At the same temperature and pressure, equal volumes of different gases contain the same number of particles. 5 liters of oxygen 5 liters of nitrogen Same number of particles! Copyright © Houghton Mifflin Company. All rights reserved.
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Representing Gay-Lussac’s Results
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Representing Gay-Lussac’s Results
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Early Experiments to Characterize the Atom
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Early Experiments to Characterize the Atom
J. J. Thomson - postulated the existence of electrons using cathode ray tubes. Ernest Rutherford - explained the nuclear atom, containing a dense nucleus with electrons traveling around the nucleus at a large distance. Copyright © Houghton Mifflin Company. All rights reserved.
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Figure 2.7 A Cathode-Ray Tube
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Figure 2.8 Deflection of Cathode Rays by an Applied Electric Field
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Cathode Ray Tube Copyright © Houghton Mifflin Company. All rights reserved.
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Figure 2.9 The Plum Pudding Model of the Atom
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Figure 2.12 Rutherford's Experiment On a-Particle Bombardment of Metal Foil
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Rutherford’s Gold Foil Experiment
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Figure 2.13 a & b (a) Expected Results of the Metal Foil Experiment if Thomson's Model Were Correct (b) Actual Results
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Figure A Schematic Representation of the Apparatus Millikan Used to Determine the Charge on the Electron
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Milliken Oil Drop Experiment
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The Modern View of Atomic Structure: An Introduction
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A Silicon Chip
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The Modern View of Atomic Structure
The atom contains: electrons protons: found in the nucleus; positive charge equal in magnitude to the electron’s negative charge. neutrons: found in the nucleus; no charge; virtually same mass as a proton. Copyright © Houghton Mifflin Company. All rights reserved.
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Table 2.1 The Mass and Charge of the Electron, Proton, and Neutron
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Nuclear Atom Viewed in Cross Section
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Atomic Nucleus
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Two Isotopes of Sodium Copyright © Houghton Mifflin Company. All rights reserved.
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Molecules and Ions
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Molecular vs. Ionic Compounds
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Covalent Bonding Copyright © Houghton Mifflin Company. All rights reserved.
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Figure 2.17 Space-Filling Model of Methane
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Figure 2.18 Ball-and-Stick Model of Methane
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Formation of Ionic Compounds
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Figure 2.20 Ball-and-Stick Models of the Ammonium Ion and the Nitrate Ion
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An Introduction to the Periodic Table
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The Periodic Table Copyright © Houghton Mifflin Company. All rights reserved.
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Table 2.2 The Symbols for the Elements That Are Based on the Original Names
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Crystals of Copper(II) Sulfate
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Table 2.3 Common Monatomic Cations and Anions
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Figure 2.22 Common Cations and Anions
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Table 2.4 Common Type II Cations
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Various Chromium Compounds Dissolved in Water
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Table 2.5 Common Polyatomic Ions
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Naming Simple Compounds
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Overall Strategy for Naming Chemical Compounds
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Flowchart for Naming Binary Compounds
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Table 2.6 Prefixes Used to Indicate Number in Chemical Names
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Flowchart for Naming Acids
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Table 2.7 Names of Acids* that Do Not Contain Oxygen
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Table 2.8 Names of Some Oxygen-Containing Acids
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React 1 Explain any problems with each of the names given in the table in your Interactive Course Guide. Complete the table. Copyright © Houghton Mifflin Company. All rights reserved.
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React 2 Determine the number of particles in solution and either the name or formulas for the compounds given in your Interactive Course Guide. Copyright © Houghton Mifflin Company. All rights reserved.
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