chapter-10-notes-4-1

# chapter-10-notes-4-1 - Chapter10 Yes you will need a...

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Chapter 10 Yes , you will need a calculator for this chapter!

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OBJECTIVES: Describe  methods of  measuring  the amount of  something. Define   Avogadro’s number  as it relates to a  mole of a substance. Distinguish  between the  atomic mass  of an  element and its  molar mass. Describe  how the mass of a mole of a  compound is  calculated .
You can measure  mass or  volume , or you can  count pieces . We measure mass in  grams . We measure volume in  liters . We count pieces in  MOLES .

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It is an amount , defined as the number of carbon  atoms in exactly 12 grams of carbon-12. 1 mole = 6.02 x 10 23   of the representative  particles. 6.02 x 10 23   is called:  Avogadro’s number . Treat it like a very large dozen

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Pair : 1 pair of shoelaces = 2 shoelaces Dozen : 1 dozen oranges = 12 oranges Gross : 1 gross of pencils = 144 pencils Ream : 1 ream of paper = 500 sheets of paper
The smallest pieces of a substance: 1) For a molecular compound: it is the molecule . 2) For an ionic compound: it is the formula unit (made of ions). 3) For an element: it is the atom . Remember the 7 diatomic elements? (made of molecules)

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How many  oxygen atoms  in the following? CaCO 3 Al 2 (SO 4 ) 3  How many  ions  in the following? CaCl 2 NaOH Al 2 (SO 4 ) 3 3 atoms of oxygen (3 x 4)=12 atoms of oxygen 3 total ions (1 Ca ion and 2 Cl ions) 2 total ions (1 Na ion and 1 OH ion) 5 total ions (2 Al + 3 SO ions)
How many molecules of CO 2  are in 4.56 moles of  CO 2 ? How many moles of water is 5.87 x 10 22    molecules? How many atoms  of  carbon are in 1.23 moles of  C 6 H 12 O 6 ? How many moles is 7.78 x 10 24  formula units of  MgCl 2 ? 2.75 x 10 molecules 0.0975 mol (or 9.75 x 10 ) 4.44 x 10 atoms C 12.9 moles

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Remember relative atomic mass? - The amu was one twelfth the mass of a  carbon-12 atom. Since the mole is the number of atoms in 12
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chapter-10-notes-4-1 - Chapter10 Yes you will need a...

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