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UI CHEM 1110 - Atoms, Molecules, and Ions
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CHEM 1001 1st Edition Lecture 3 Outline of Last Lecture I. Definitions a. Chemistry II. Classifications a. States of MatterIII. Properties of Mattera. Physical and Chemical b. Intensive and Extensive IV. Measurement Units a. SI Units V. Measurement Uncertainty a. Significant Figures Outline of Current Lecture I. The Atomic Theory of Matter a. Greek Philosophersb. John Dalton (1766-1844)c. Three Classical Lawsd. J. J. Thompson (1856-1940)e. Robert Millikan (1868-1953)These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.f. Ernest Rutherford (1871-1937)II. The Discovery of Atomic Structure a. IsotopesIII. Atomic weights a. Molecular MassIV. The Periodic Table a. The Significance of Groups V. Molecules and Molecular CompoundsVI. Ions and Ionic Compoundsa. Naming Compounds Current LectureI. Atomic Theory a. Two Greek Philosophersi. Empedocles: fund amental substances are air, earth, fire and waterii. Democritus: matter is particulate b. John Dalton (1766-1844)i. Daltons Atomic Theory (1803-1807)1. All Matter consists of tiny indivisible atoms 2. Atoms of an element are identical, but different from those of other elements3. Atoms of one element cannot converted into those of another element4. Compounds result from chemical combinations of different elements; atom ratio are integers ii. Law of Conservation of Mass1. Total mass of materials after reaction = mass before reaction iii. Law of Constant Composition 1. In a given compound the relative numbers and kinds of atoms are constant iv. Law of Multiple Proportions1. If A and B combine to form more than one compound, mass of A and B are a small whole number ratio c. J.J. Thomson (1856-1940)i. English physicist (Nobel Prize in 1906)ii. Cathode rays are independent of the electrode material iii. Cathode rays are streams of negatively charged particles (now called electrons)iv. Measured the charge to mass ratio of the electron (1.76 x 108 C/g)d. Robert Millikan (1868-1953)i. American physicist (Nobel Prize in 1923)ii. Oil-Drop experiment 1. Caused oil drops to become charged and observed their behavior a. Charge of the electron (1.602 x 10-19 C)2. Computed the electron mass (9.1 x 10-28 g)e. Ernest Rutherford (1871-1937)i. New Zealand physicist (Noble Prize in 1908)ii. Discovered the nature of radioactivity iii. Gold- Foil Experiment (1910)1. Studies at which alpha particles were scattered after passing through then gold foil 2. Disproved plum pudding model iv. Proposed the nuclear atoms as a small, very dense, positive nucleus surrounded by negative electrons 1. Atom diameters: ~100-500 pm2. Nuclei diameters: ~10-2 pm II. Modern Atomic Structure a. Isotopes- atoms with identical atomic numbers but different mass numbers III. Atomic Masses a. Atomic mass- mass with a single atom in atomic mass units (amu) b. Molecular mass – mass of a single molecule in amui. Computing1. the sum of the atomic masses of each atom in a molecule c. Formula unit mass- mass of all the atoms in a formula unit in amu i. Computing 1. The sum of the atomic masses of each atom in a formula unit IV. Periodic Table a. Elements in the same group often have similar physical and chemical propertiesb. Keyed to similarities in the arrangement of their electrons i. 1A: Alkali Metalsii. 2A: Alkaline earth metalsiii. 6A: Chalcogens iv. 7A: Halogens v. 8A: Noble gases (plus Hydrogen)V. Molecular & Ionic Compounds a. Molecules and molecular compounds i. 2 or more atoms bound together by chemical bondsii. Diatomic molecules 1. H, O, N, F, Cl, Br, Iiii. Is composed of molecules that contain more than one type of atoms iv. Usually contain only nonmetals and/or metalloids b. Ions – formed when an atom gains or loses electronsi. Cation – positive ion formed when electrons are lostii. Anion – negative ion formed when electrons are gained iii. Ionic Compounds – a compound that contains both a metal and nonmetalVI. Nomenclature a. Binary Inorganic Compounds i. Ionic Compounds 1. Metal (one ion type)a. Metal name + nonmetal name with ide suffix 2. Metal (2 or more ion type)a. Metal name with Roman Numeral + nonmetal with ide suffix 3. Hydrates- compounds whose crystals contain discrete whater molecules a. Name as other ionic compounds except add prefix number + hydrate as a third wordii. Molecular compounds 1. Nonmetal and nonmetala. Number prefix (except one) +name prefix (including one) + name with ide as suffix b. Polyatomic Ions i. Suffix “ate” – one more oxygen than “ite”c. Acidsi. Binary Aqueous Acids 1. Hydro + element name with ic suffix + acid ii. Oxyacids iii. Element name + suffix + acid 1. Suffix a. Ate – icb. Ite –


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