Chapter 6 Chemistry Notes

# The perfect scaling factor recall a carbon 12 atom

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Unformatted text preview: ctly 12 amu. 12 g of carbon is a nice macroscopic size to measure. The bad: there was a simple relationship between the chemical formula and the mass when we used amu, but this lost when we switched to grams. How do we solve this problem? The ugly: Ans: Instead of Yotta use the mole 1 amu/1.66x10-24g =1, (or 6.02x1023amu/ 1 g) This is an inspired choice. The mole will make amu to gram conversion of chemical amounts EASY! How many atoms are in 12 g of carbon-12? 1 C − 12 atom 1 amu 12g = 6.02214x10 23 C − 12 atoms − 24 g 12 amu 1.6605388x10 Notice: 1 amu= 1.6605x10-24 g is the same thing as 6.02214x1023 amu = 1 g. KEY IDEA: instead of using 1024 particles (Yotta-particles), let’s use 6.02214x1023 particles instead. This will make the conversion from sub-microscopic (amu masses) to macroscopic (gram masses) easy. A mole is defined as 6.02214x1023 (Avogadro’s Number.) (It is simple a equivalence 1 mole = 6.02x1023 things) The Convenience of Scaling The mole is just a convenient collection of objects. A dozen (12) is used for eggs, a score (20) is used in Lincoln’s Gettysburg address, and a ream (500) is used for paper. A mole (6.02214x1023) is a convenient amount in chemistry. The mole together with the chemical formula enables two important things: 1. One nuclear particle (p or n) has a mass of ~1 amu Similarly, 1 mol of nuclear particles have a mass of 1 gram! Easy conversion from individual molecules to macroscopic amounts. Chemical Formula 2. How does it work? Mass molecules (g) Easy conversion from macroscopic mass amounts to counting numbers. # molecules (in mol) Therefore, grams simply count (moles, i.e. collections of particles). For the same reasons: The formula mass of a substance is numerically equal to the mass (in grams) of 1 mol of that substance. This mass is known as the molar mass and is simple found from the chemical formula and the atomic masses. Mass molecules (in g) Therefore, amu’s simply count (particles). molar mass (g/mol) = formula mass (amu) Met...
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## This note was uploaded on 02/04/2014 for the course CHEM 004:007 taught by Professor Russellarsen during the Fall '13 term at University of Iowa.

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