Atomic_structure_s09 - CHEM 1311A E Kent Barefield Course web page http/web.chemistry.gatech.edu/~barefield/1311/chem1311a.html Two requests cell

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CHEM 1311A Course web page http://web.chemistry.gatech.edu/~barefield/1311/chem1311a.html E. Kent Barefield Two requests: cell phones to silent/off no lap tops in operation during class Bring your transmitter to class on Friday
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Outline for first exam period Atomic structure and periodic properties Structures and bonding models for covalent compounds of p-block elements Lewis Structures, Valence Shell Electron Repulsion (VSEPR) concepts and oxidation state Hybridization Composition and bond energies in binary p-block compounds Structure and bonding in organic compounds First Exam – Wednesday, January 28
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Atomic structure and periodic properties Early experiments concerning atomic structure and properties of electromagnetic radiation Bohr model of the hydrogen atom Demise of Bohr model Wave equation and wave model for atom Wave functions and properties Orbital representations Multielectron atoms Periodic properties and their origin
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Properties of Atoms Consist of small positively charged nucleus surrounded by negatively charged electrons, some at large distances from the nucleus Nucleus consists of positively charged protons and neutral neutrons Charges of proton and electron are equal The atomic number (and nuclear charge) of an atom is equal to the number of protons in its nucleus. The mass number of an atom is equal to the number of protons plus the number of neutrons Isotopes are atoms with the same atomic number but different mass numbers, i.e., 1 H, 2 H, 3 H or 12 C, 13 C, 14 C
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Atomic Spectra Irradiation from electronically excited atoms is not continuous Visible region line spectra could be fitted to simple (empirical) formula 1/ λ = 1.097 x 10 7 m -1 (1/2 2 -1/n 2 ) E = hc/ λ = 2.178 x 10 -18 J (1/2 2 -1/n 2 ) Later work showed several series of lines E = 2.178 x 10 -18 J (1/n 2 2 -1/n 1 2 ) (n 2 <n 1 )
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> 10 5 > 3 x 10 19 < 10 -9 < 0.1 γ -Rays 10 3 -10 5 3 x 10 17 -3±x±10 19 10 -7 -9 10 - 0.1 X-Rays 3 - 10 3 7.5 x 10 14 17 4 x 10 -5 -7 4000 - 10 Ultraviolet 2 - 3 4.3 x 10 14 -7.5±x±10 14 7 x 10 -5 -4±x±10 -5 7000 - 4000 Visible 0.01 - 2 3 x 10 12 - 4.3 x 10 14 0.01 - 7 x 10 -5 10 6 - 7000 Infrared 10 -5 -0.01 3 x 10 9 12 10 - 0.01 10 9 6 Microwave < 10 -5 < 3 x 10 9 > 10 > 10 9 Radio Energy (eV) Frequency (Hz) Wavelength (centimeters) Wavelength (Angstroms) Region Spectrum of Electromagnetic Radiation
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Wavelength, nm Yellow green Indigo Yellow Violet Orange Blue Blue green Red Purple Green 400 500 600 700 800 Color of transmitted light Complementary color 400 nm 4000 Å 4x10 -5 cm
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This note was uploaded on 05/23/2011 for the course CHEMISTRY 1311 taught by Professor Cox during the Spring '10 term at Georgia Institute of Technology.

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Atomic_structure_s09 - CHEM 1311A E Kent Barefield Course web page http/web.chemistry.gatech.edu/~barefield/1311/chem1311a.html Two requests cell

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