PowerPoint PresentationSlide 2Slide 3Slide 4“Babel” of Chemical Nomenclature 1770Slide 6Slide 7Antoine Lavoisier: 1743-1794Slide 9Slide 10Slide 11Slide 12Slide 13Slide 14Slide 15(Goal 1) Distinguish between elements, compounds and mixtures.Slide 17The four elements of ancient times.Slide 19Slide 20Slide 21Slide 22Slide 23Slide 24Slide 25Slide 26Slide 27Slide 28Slide 29Slide 30Slide 31Slide 321Lecture02_C1403 Fall 2005Please Turn Off Cellular Phones!ThankYou!2Tentative Course Material To Be Covered this termExam 1: Wednesday, September 29 (6 lectures covered).Chapter 1. The Atomic Nature of Matter.Chapter 2. Stoichiometry.Chapter 3. Chemical Periodicity and the Formation of Simple Compounds.Exam 2: Wednesday, November 2 (9 lectures covered)Chapter 16. Quantum Mechanics and the Hydrogen Atom.Chapter 17. Many-electron Atoms and Chemical Bonding.Chapter 18. Molecular Orbitals, Spectroscopy, and Atmospheric Chemistry.Exam 3: Wednesday, November 30 1 (6 lectures covered)Chapter 19. Coordination Complexes.Chapter 24. From Petroleum to Pharmaceuticals.Period before final (3 lectures covered)Chapter 25. Synthetic and Biological Polymers (plus spectroscopy of organic molecules)..Date of the final exam will be announced by the registrar.3Science: An attitude or world view. The systematic logical and self-consistent investigation, creation and organization of knowledge through observations. Rules which are found to be universal and without exceptions lead to laws.Observations in the form or experiments lead to classifications and classifications lead to rules.45“Babel” of Chemical Nomenclature 1770•Chemistry Symbols from the 18th century encyclopedia published by philosopher Denis Diderot and mathemetician Jan Le Rond D’Alembert•These symbols describe Alloys, compounds, chemical operations, quantities, glassware, etc.6Chemistry employs the scientific method to investigate, create and organize knowledge that provides an understanding of the structure and transformation of matter and the interaction of light and matter.Provide a chemist with any observation and he/she interprets it in terms of the structure and dynamics of atoms, molecules, photons (and friends) as the key intellectual units.7Molecular Structure: The key intellectual unit of all of chemistry. From structure to function.CHHHHConfiguration: How all the atoms are distributed in space relative to one another in three dimensions. The 4 hydrogen atoms point to the vertices of a tetrahedron.CHHHHConstitution: How all the atoms are connected by bonds to one another. 4 hydrogens connectedto carbon, not to other hydrogens.Composition: Number and kinds of atomsCH4: one carbon atom, 4 hydrogen atoms8Antoine Lavoisier: 1743-1794He established the Law of Conservation of Mass by burning phosphorus and sulfur in air, and proving that the products weighed more than the original. The weight gained was lost from the air. Repeating the experiments of Priestley, he demonstrated that air is composed of two parts, one of which combines with metals to form calxes. He named this portion oxygen (Greek for acid-former), and the other azote (Greek for no life). He also discovered that the inflammable air of Cavendish which he termed hydrogen (Greek for water-former), combined with oxygen to produce a dew, as Priestley had reported, which appeared to be water. He begins therefore a first systematic list of the elements.9Schematic description of the scientific process10From atoms to the Periodic Table: Key ideas and proponentsLucretius (400 BC) Postulated atoms exist1600-1800 Discovery of elements, compoundsLavosier (1780) Law of conservation of massProust (1790) Law of definite proportions of massDalton (1800) Atomic theory to explain laws of conservation and definite proportionsGay-Lussac (1808) Law of combining volumes of gasesAvogadro (1811) Equal volumes of gases, equal particlesCannizzaro (1860) Scale of relative molecular weightsMendeleev (1861) Periodic table based on relative atomic weights1112Chapter 1: Learning goals concerning the atomic nature of matter(7) Understand the mole concept.(6) Understand Avogadro’s hypothesis and Cannizzaro’s proposal.(5) Understand the Law of combining volumes of gases.(4) Understand the principles of Dalton’s atomic theory.(3) Understand the Laws leading to the Dalton’s atomic theory of matter (Conservation of mass and definite proportions).(2) Understand the atomic and molecular interpretation of elements, compounds and mixtures.(1) Distinguish between elements, compounds and mixtures.13Chapter 1: Some learning goals dealing with molecular structure and the relationship between weights of elements in a compound and the number of atoms in a formula.(9) Perform calculations employing the mole (the chemical amount) concept.(8) Distinguish between empirical formula, molecular formula,structural formula.14Chapter 1: Some learning skills and techniques:(1) Translate coefficients of a balanced chemical equation into moles. Obtain relative number of moles of reactants and products independent of the actual chemical amounts.(4) Volume relationships in chemical reactions. Translate liters into moles.(3) Mass relationships in chemical reactions. Translate moles into grams (weight) or moles into liters (volume of gas).(2) Translate coefficients into molecules. Obtain relative number of molecules of reactants and products independent of the actual chemical amounts.15(1) Distinguish between elements, compounds and mixtures.Pure substance (an idealization): A pure substance does not change its chemical characteristics upon exhaustive attempts of purification.Atomic interpretation: A pure substance possesses a structure that is composed of a definite number and kinds of atoms that are connected in a specific manner. Element: An element is a substance which cannot be decomposed into simpler substances by chemical processes. Exemplars: hydrogen, carbon, oxygen.Atomic interpretation: An element is a substance that contains only one kind of atom. Exemplars: Hydrogen (H) atoms, carbon atoms (C), oxygen atoms (O).Compound: A compound is a substance that can be decomposed into simpler substances by chemical processes. Exemplars: water, carbon dioxide, carbon monoxide.Atomic interpretation: A compound is a substance that contains atoms of two or more chemical elements. Exemplars: H, C, O.16(Goal 1) Distinguish between elements, compounds and mixtures.17The intellectual history of