Course.Outline - General Chemistry 1404 Columbia University...

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General Chemistry 1404 Dr. Beer Columbia University Tentative Course Outline - DRAFT Notes: This is a brief list of topics to be covered in the course and on exams. Refer to the file “Assignments” for specific reading assignments in the text. Part 1. Molecular Description of the States of Matter Excluded Topics Chapter 5: Section 5.12 (atmospheric chemistry), gaseous diffusion on p. 166 Chapter 16: Sections on "Bonding in Metals" and "Metal Alloys" in Section 16.4 as well as 16.5, 16.8, 16.9 and 16.12 Chapter 17: "Water as a solvent" pp. 851-3, "Reverse Osmosis" p. 870, Section 17.8 Chapter 5 – The Gaseous State Characteristics of gases, Pressure Empirical Gas Laws: Boyle’s Law, PV = constant (at const. n, T), Charles Law, V/T = constant (at const. n, P), Avogadro’s Law, V/n = constant, the absolute temperature scale, Combined Gas Laws, PV/T = constant, Ideal Gas Law, PV = nRT; PM m = dRT and other chemical calculations with the gas laws Partial pressures - Dalton’s Law (P A = X A P T ); applications: collecting a gas over water Kinetic Molecular Theory (KMT) – postulates and relation to gas laws, derivation of PV = nRT Kinetic energy and temperature: types of molecular speeds, e. g. rms speed, u rms = (3RT/M m ) 1/2 Molecular effusion; rate is proportional to 1/(M m ) 1/2 Effusion rates, collision theory (collision rates with a wall or other particles and mean free path) Real gases; the van der Waals equation; interpretation of the deviations from P and V in the ideal gas law (constants a, b) and their relation to energetics of gas motion (the Lennard-Jones potential, i. e. volume effects and intermolecular interactions). Memorization/Operational Skills List Definition of pressure Plots of empirical gas laws and use of them to calculate P, V, T, n, M m , d and in stoichiometric chemical equation calculations Calculating partial pressures including collecting a gas over water Know KMT postulates and how they can be used to derive gas laws Plots of molecular speed vs. temperature; calculation of molecular speeds and effusion rates Use of equations from collision theory and rates Understanding the effects of gases due to deviations from non-ideal gas behavior; calculations of P and V with the van der Waals equation Chapter 16 – Solids, Liquids and Phase Transitions Differences between gases and condensed phases (lecture) Intermolecular forces – ion, dipole, induced dipole effects. London forces (molar mass dependence) and van der Waals radii, hydrogen bonding The basis and energies of intermolecular forces (Lennard-Jones potential revisited) Kinetic molecular theory and condensed phases (escape energies) Interpretation of properties of condensed phases (melting, boiling etc…)
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Types of solids, X-ray crystallography (structure determination), the unit cell and metrical parameters from a cubic crystal system (including calculations using unit cell information for three types, primitive, body- and face-centered). Hexagonal and cubic close packing in solids.
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This note was uploaded on 03/04/2010 for the course CHEM 1404 taught by Professor Luarakaufman/rubengonzalez during the Spring '09 term at Columbia.

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Course.Outline - General Chemistry 1404 Columbia University...

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