<p>Honors Chemistry Name ______</p><p>Chapter 2 – Atoms, Molecules and a Ions</p><p>Introduction</p><p>Atoms:</p><p>Molecules:</p><p>Ions:</p><p>2.1 Atoms and the Atomic Theory</p><p>Greeks: Empedocles and Democritus</p><p>John Dalton:</p><p>Atomic Theory</p><p>1.)</p><p>2.)</p><p>3.)</p><p>4.)</p><p>1 Fundamental Laws of Matter</p><p>Law of Conservation of Mass:</p><p>Law of Constant Composition:</p><p>Law of Multiple Proportions:</p><p>2.2 Components of the atom</p><p>2 J.J Thomson:</p><p>Cathode Ray Tube:</p><p>Electrons</p><p>J.J. Thomson’s Model </p><p>3 Ernest Rutherford:</p><p>Gold Foil Experiment:</p><p>Nuclear Particles:</p><p>Atomic Mass –</p><p>Properties of subatomic particles</p><p>Particle Location Relative charge Relative Mass Proton Neutron Electron</p><p>4 Terminology:</p><p>Atomic Number, Z A Mass number, A Z X</p><p>Isotopes</p><p>Examples:</p><p>5 Radioactivity Radioactive isotopes are unstable</p><p>1)</p><p>2)</p><p>Particles emitted</p><p>1)</p><p>2)</p><p>3)</p><p>Nuclear Stability</p><p>Depends on …</p><p>2.3 Introduction to the Periodic Table Dmitri Mendeleev:</p><p>Modern Periodic Table</p><p>6 Period –</p><p>Group –</p><p>Blocks – </p><p>Families - </p><p>Blocks in the Periodic Table</p><p>7 2.4 Molecules and Ions molecule:</p><p>1.</p><p>2.</p><p>8 Molecular formulas:</p><p>Structural formulas:</p><p>Ion :</p><p>Cation:</p><p>Anion:</p><p>Examples: </p><p>2.5 Ionic Compounds</p><p>Forces –</p><p>Solutions –</p><p>Conductivity –</p><p>9 Formulas for Ionic Compounds</p><p>Transition Metals:</p><p>Polyatomic ions:  Memorize 24 given on hand out </p><p>Noble Gases:</p><p>10 2.6 Naming of compounds</p><p>Cations:</p><p>Anions:</p><p>To name an ionic compound: name the cation first, then, name the anion (with the word 'ion' omitted). It is not necessary to indicate the number of cations and anions in the compound because it is understood that the total positive charges carried by the cations must equal the total negative charges carried by the anions. A few examples are listed below: KI potassium ion + iodide ion = potassium iodide</p><p>CoCl2 cobalt(II) ion + two chloride ions = cobalt(II) chloride</p><p>CoCl3cobalt(III) ion + three chloride ions = cobalt(III) chloride mercury(I) ion + two chloride ions = mercury(I) chloride or Hg Cl 2 2 mercurous chloride</p><p>AgNO3 silver ion + nitrate ion = silver nitrate</p><p>11 Oxoanions:</p><p>-ate</p><p>-ite</p><p>-per</p><p>-hypo</p><p>Practice Examples : </p><p>Sodium bromide ______Calcium phosphate ______Magnesium oxide ______Sodium hypochorite ______Potassium nitrite ______Iron (III) sulfate ______</p><p>Binary Molecular Compounds</p><p>Systematic Naming</p><p>12 1-</p><p>2-</p><p>Examples: diphosphorus pentaoxide sulfur dioxide dinitrogen tetraoxide hydrogen dioxide carbon monoxide phosphorus trichloride</p><p>Acids:</p><p>Naming: Common</p><p>Oxoacids</p><p>Acids of chlorine</p><p>Examples: </p><p>Hydrogen chloride (hydrochloric acid) Nitric acid Sulfuric acid Hypobromous acid Nitrous acid Phosphoric acid</p><p>13</p>