Stoic demo vod

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Chemistry:Mole Basics

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Stoic demo vod

  1. 1. Moles and Stoichiometry<br /> Ms. Randall<br />
  2. 2. I. Moles<br />WRITE<br />DOWN<br />1 mole is 6.02 x 1023of anything!!<br />6.02 x 1023 is called Avogadro's number.<br />A mole can be 6.02 x 1023atoms or molecules<br />A Mole is a Unit<br />Sing-a-long!!!<br />
  3. 3. II. Interpreting Chemical Formulas<br />
  4. 4. A. Empirical Formula<br /><ul><li>Simplest ratio of atoms in a compound (Ex. C2H5)
  5. 5. The subscript tells you how many moles of each ion in the compound.
  6. 6. Ex. Al2O3 = 2 mol Al+3 3 mol O-2</li></ul>WRITE<br />DOWN<br />
  7. 7. WRITE<br />DOWN<br />WRITE<br />DOWN<br />B. Molecular Formula<br />Actual ratios of atoms in a molecule or compound (Ex. C4H10) <br />Molecular formulas are whole-number multiples of an empirical formula<br />Ex: C4H10 molecular formula<br /> C2H5 empirical formula <br />
  8. 8. C. Structural Formula<br />Shows the arrangement of the atoms in the actual compound <br />WRITE<br />DOWN<br />
  9. 9. III. Stoichiometry<br />The study of quantitative relationships that can be derived from chemical formulas and equations<br />WRITE<br />DOWN<br />
  10. 10. 1 mole of atoms has a mass equal to the atom’s atomic mass in grams. <br />Atomic mass located on periodic table.<br />Round to the nearest TENTH ( 0.1)<br />Example:<br />C= 12.0 amu = 12.0 g/mol<br />O= 16.0 amu = 16.0 g/mol<br />A. Gram Atomic Mass<br />WRITE<br />DOWN<br />
  11. 11. B. Gram Formula Mass (GFM) <br />WRITE<br />DOWN<br />the sum of all the atomic masses in the formula of the substance <br />add up the mass of each atom in the formula.<br />Multiply by the number of each atom if there is more than one of each atom.<br />
  12. 12. Example: silver nitrate<br />AgNO3<br />Element# of atomsMassProduct<br /> Ag = 1 × 108amu = 108 g<br /> N = 1 × 14amu = 14 g<br /> O = 3 × 16 amu = 48 g<br /> 170g/mol<br />
  13. 13. 11<br />Regents Practice<br />The gram formula mass of NH4Cl is <br />22.4 g/mole<br />28.0 g/mole<br />53.5 g/mole<br />95.5 g/mole<br />N 1 x 14.0 =<br />H 4 x 1.0 =<br />Cl 1 x 35.5 = _______<br /> g/mole<br />þ<br />
  14. 14. 1. Calculating Moles from Mass<br />Formula on table T in reference table<br />given mass (g)<br /> Gram formula mass<br />Mole =<br />WRITE<br />DOWN<br />
  15. 15. WRITE<br />DOWN<br />2. Calculating Grams from Moles<br />given mass (g)<br /> Gram formula mass<br />Rearrange the formula in <br /> table T to solve for grams <br />Mole =<br />Mole x GFM<br />Grams =<br />
  16. 16. Summary<br />Grams Moles<br />÷ gfm<br />x gfm<br />
  17. 17. Example:How many moles are in 390g of calcium chloride?<br />Step1: Find the formula mass of the substance and express it in grams per mole<br />Step 2: Apply the formula<br />CaCl2<br /> Ca = 40 × 1 = 40<br />Cl = 35 × 2 = 70<br /> 110 g/mol<br /> grams_<br /> 390g__<br />mol =<br />mol =<br />GFM<br /> 110 g/mol<br />= 3.5 mol<br />
  18. 18. What is the mass of 2 moles of sodium thiosulfate?<br />Regents Practice<br /> Na2S2O3<br /> Na = 23 × 2 = 46<br /> S = 32 × 2 = 64<br /> O = 16 × 3 = 48<br /> 158 g/mol= GFM<br />step 1<br />grams = moles × GFM<br /> = 2 mol × 158 g/mol<br /> = 316 g<br />step 2<br />

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