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Chapter 10 - The Mole & Avogadro’s Number

Chapter 10 - The Mole & Avogadro’s Number. Measuring Matter Sections 10.1  10.3. Measuring Matter/Counting Units. One pair = 2 (boots, shoes) One dozen = 12 (eggs, donuts, roses) One gross = 144 (pencils) One ream = 500 (sheets of paper).

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Chapter 10 - The Mole & Avogadro’s Number

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  1. Chapter 10 - The Mole & Avogadro’s Number Measuring Matter Sections 10.1  10.3

  2. Measuring Matter/Counting Units One pair = 2 (boots, shoes) One dozen = 12 (eggs, donuts, roses) One gross = 144 (pencils) One ream = 500 (sheets of paper)

  3. Measuring a Mole – units used to count particles • Atoms are so tiny chemists count them using a unit of measurement called a “mole” • 1 mole = 6.02 x 1023 (Avogadro’s Number) atoms/particles/ions/formula units/molecules • This is a very large number because it measures extremely tiny items • 602,000,000,000,000,000,000,000

  4. How Big is a Mole? • One mole of pennies would allow every person on Earth to spend a million dollars an hour, day and night, and still have half of it unspent when they died • One mole of popcorn would cover every dry surface of the Earth to a depth of six miles One mole of stacked pennies would reach to the moon and back 16 times • One mole of marshmallows would cover the United States to a depth of 650 miles

  5. History of Avogadro’s Number • Avogadro: 1811 – equal volumes of gases at the same temperature and pressure contain equal numbers of molecules • Cannizzaro: 1861 – developed atomic weights for known elements • Loschmidt: 1865 – determined the number of atoms present in a given volume of air • Ostwald: 1902 – developed the concept of the mole • 1971 – the true value, 6.02x1023, was actually determined and is called Avogadro’snumber since the entire string of events started with his findings in 1811

  6. The Law of Conservation of Mass • According to the Law of Conservation of Mass, Mass of reactants = mass of products Mass of starting substances = mass of ending substances • So the production of one water molecule requires 2 hydrogen atoms and 1 oxygen atom. Therefore: two atoms of hydrogen + one atom of oxygen  1 water molecule And 12.04x1023 hydrogen atoms + 6.02x1023 oxygen atoms  6.02x1023 water molecules

  7. The Law of Definite Proportions and Ratios of Atoms • Law of Definite Proportions – atoms combine in small whole number ratios to form compounds • Example: Water- two atoms of Hydrogen will always combine with one atom of Oxygen to form one molecule of water

  8. Relationships between moles, atoms and the gram mole The atomic mass ratio of hydrogen to oxygen is 1 amu : 16 amu The gram mole ratio between hydrogen and oxygen is 1 g : 16 g So, chemists can determine how many atoms are present in a sample. One gram of hydrogen would contain exactly 6.02x1023 atoms, or Avogadro’s Number of atoms. Two grams of hydrogen atoms would contain 12.04x1023 hydrogen atoms. Also, 16 gram moles of oxygen would contain 6.02x1023 atoms. Therefore: 1 gram of hydrogen = 6.02x1023 atoms = 1 mole 2 grams of hydrogen = 12.04x1023 atoms = 2 moles 16 grams of oxygen = 6.02x1023 atoms = 1 mole 32 grams of oxygen = 12.04x1023 atoms = 2 moles

  9. In Conclusion: • 2 atoms of hydrogen + 1 atom of oxygen = 1 water molecule • 2 amu of hydrogen + 16 amu’s of oxygen = 18 amu’s of water molecules • 2 g of hydrogen + 16 grams of oxygen = 18 grams of water molecules • 12.04x1023 atoms H + 6.02x1023 atoms O = 6.02x1023 atoms H2O molecules • 2 moles of H atoms + 1 mole of O atoms = 1 mole of water molecules

  10. x 6.02 x 1023 Moles Particles Atoms, molecules, ions, formula units ÷ 6.02 x 1023 Moles Particles Conversion

  11. Convert 3.5 moles to atoms • Convert 18.06 x 1023 atoms to moles Example Problems:

  12. Convert from moles to particles 3) 2.7 moles of lithium 4) 1.8 moles of sodium chloride 5) 5.3 moles of bromine 6) 4.7 moles of potassium oxide

  13. Convert from particles to moles 7) 4.32 x 1024 atoms of calcium 8) 2.7 x 1020 atoms of copper 9) 2.5 x 1024 molecules of sodium chloride 10) 5.32 x 1023 molecules of calcium chloride

  14. You try these… 11) 25 moles to particles 12) 4.08 x 104 particles to moles 13) 0.002 moles to particles 14) 2.3 x 1016 particles

  15. HomeworkComplete on another sheet of paper showing your work! Particles to moles5) 4.32 X 1024 6) 2.70 X 1020 7) 2.50 X 1024 8) 5.32 X 1023 Moles to particles • 1) 2.7 moles • 2) 1.8 moles • 3) 5.3 moles • 4) 4.7 moles

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