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Atoms, Molecules, and Ions Chapter 2 Atomic Theory and the Structure of the Atom Democritus Greek era All matter consists of very small, indivisible particles, which he named atomos Lavoisier Law of conservation of mass Proust Law of definite proportions Dalton Law of multiple proportions and the first model of the atom Concept Review The atoms of elements A (blue) and B (orange) form two compounds shown here. Do these compounds obey the law of multiple proportions? Radiation Cathode Ray Tube Cathode Evacuated tube Anode − + Battery α β ϒ J.J. Thomson Charge to mass ratio and the Plum-Pudding Model R.A. Millikan Millikan Oil Drop Rutherford Gold Foil Experiment Bohr Planetary Model Schrödinger Quantum Mechanical Model Chadwick The Neutron Atomic Symbols Isotopes Hydrogen-1 Hydrogen-2 Hydrogen-3 The Periodic Table Molecules Diatomic HCl CO Molecules Polyatomic O3 CO2 NH3 H2O Compound Molecular Compound CO2 NH3 H2O Binary Molecular Compound HCl CO Compound Ionic Compound Chemical Formulas MOLECULAR FORMULA EMPIRICAL FORMULA Butane C4H10 C 2 H5 Nomenclature Organic compounds Nomenclature Inorganic compounds: Ionic Compounds NaCl sodium chloride Mn2O3 manganese(III) oxide Nomenclature Inorganic compounds: Binary Molecular Compounds Greek Prefixes NO2 nitrogen dioxide N2O4 dinitrogen tetraoxide Nomenclature Summary Nomenclature Inorganic compounds: Acids Anion: chloride Acid: hydrochloric acid Anion: chlorate Acid: chloric acid Anion: chlorite Acid: chlorous acid Nomenclature Inorganic compounds: Bases *Named like ionic compounds; cation followed by anion with “–ide” NaOH Sodium Hydroxide Mg(OH)2 Magnesium Hydroxide Nomenclature Inorganic compounds: Hydrates CuSO4 5H2O Ionic compound Greek prefix Hydrate Copper(II) sulfate pentahydrate
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