Chemistry 1 Friday, August 25, 2006

Chemistry 1 Friday, August 25, 2006 - Friday Chemistry SEE...

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Friday, August 25, 2006 Chemistry SEE BIG, THINK SMALL -Moles? -How do you quantify a material? TEXT SECTION 1.3, 1.5(part) Appendix A1-A5 Statements of observation ATOMOS (Gk) – “uncuttable” John Dalton-1803 = Tried to explain mass laws (see section 1.2) Daltons Atomic Theory Explanation of observations 1. Atoms and Moles a. Daltons Atomic Theory – Part 1 i. Smallest unity of elements = atoms have unique props and mass 2. Atomic Mass H atom:1 atomic mass unit C atom: 12 amu etc. H 1 12 C 10 120 1g 12g If we have equal numbers of atoms, then a 1 : 12 mass ratio If a 1 : 12 mass ratio then equal number of atoms 3) Standard unit for counting atoms # atoms in 1g H # atoms in 12g etc. Called the mole (lat, pile) Avogadro’s number (N A ) 6.02 x 10 23 THREE PHILOSOSPHICAL POINTS: 1. Mass has double meaning atom scale; mole scale 2. the mole is an unfathomably large quantity 3. Atoms and molecules are unimaginably small
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Friday, August 25, 2006 -We encounter atoms on the Mole (Macroscopic) Scale
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This note was uploaded on 03/20/2008 for the course CH 101 taught by Professor Bigham during the Fall '08 term at N.C. State.

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Chemistry 1 Friday, August 25, 2006 - Friday Chemistry SEE...

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