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The Mole Unit

Learn about the mole unit, Avogadro's number, representative particles, converting moles to particles and vice versa, calculating molar mass, and finding percent composition.

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The Mole Unit

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  1. The Mole Unit No, not that mole!

  2. Essential Question: What is a Mole?

  3. What are some common things to count? Pair = 2 Dozen = 12 Baker’s dozen= 13

  4. So, how do we count particles? We use a Mole!

  5. What is a Mole? A unit of measurement used to count the number of particles in a chemical substance. One Mole = Avogadro’s number

  6. What is Avogadro’s number? 6.02 x 1023representative particles

  7. What are the 3 representative particles? -Atoms (elements from P.T.) -Molecules (Covalent, 2 or more non-metals) -Formula Units (Ionic, metal + non metal)

  8. Let’s practice

  9. Mole Map 1 Mole = 6.02 x 1023representative particles 1 Mole 6.02x1023 -atoms -molecules -Formula units

  10. How do you calculate the number of particles in a Mole?

  11. Example #1 How many atoms are in 2 moles of helium?

  12. Example #2 How many molecules are in 7.5 moles of water?

  13. How do you calculate the number of moles when given the number of particles?

  14. Example #3 A sample of lead contains 1.5 x 1024 atoms. How many moles of lead atoms are there?

  15. Example #4 A sample of iron chloride contains 2.15 x 1021 formula units. How many moles of iron chloride are there?

  16. Essential Question: How do you find the mass of a mole?

  17. What does the mass on the periodic table represent? One mole of particles in grams

  18. What is the name for this value called? Molar mass

  19. 1 Mole= 6.02 x 1023representative particles 1 Mole = Molar Mass from Periodic Table 1 Mole 6.02x1023 -Atoms -Molecules -Formula Units Mass from P.T. (in grams)

  20. How do you convert the number of moles to mass of an element?

  21. Example #5 What is the mass of 0.25 moles of chromium?

  22. Example #6 A container has 6.44 moles of carbon, what is the mass of this carbon?

  23. How do you convert the mass of an element to moles?

  24. Example #7 If a sample of aluminum has a mass 81 g, how many moles are present?

  25. Example #8 How many moles are there in 256g of Mercury?

  26. How do you find the mass of a compound? • Count the number atoms for each element • Multiply each atom’s mass by the number of atoms for that element. • Add

  27. What are the units for molar mass? g/mol

  28. Example #9 What is the molar mass of lithium nitrate, LiNO3?

  29. Example #10 What is the molar mass of calcium acetate, Ca(C2H3O2)2?

  30. How do you convert from the mass of a compound to moles?

  31. Example #11 How many moles are present in 12.78g of CO2?

  32. How do you convert from moles to mass of a compound?

  33. Example #12 Convert 0.57 moles of H2O to grams.

  34. Multiple step conversions Remember the mole is the base unit!!!!

  35. 1 Mole= 6.02 x 1023representative particles 1 Mole = Molar Mass from Periodic Table 1 Mole 6.02x1023 Representative particles Mass from P.T. (in grams)

  36. Example #13 How many molecules of ammonia, NH3 are in a 68g sample?

  37. Example #14 Convert 9.82 x 1027 formula units of KCl to grams.

  38. Percent Composition

  39. What is Percent Composition? This is the percentage by mass of each element in a compound

  40. How do you find the percent composition for an element in a compound? • Calculate the Molar Mass of the compound

  41. Example #15 CaCl2

  42. Example #16 H2SO4

  43. On your own! NaHCO3

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