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Yum. The M & M Lab: What if we had 6.02 x 10 23 M&M’s and we spread them out over the whole state of Washington, how deep would it be?. The Mole. 1 dozen =. 12. 1 gross =. 144. 1 ream =. 500. 1 mole =. 6.02 x 10 23. That is a REALLY BIG number…. Learning Check.

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  1. Yum The M & M Lab: What if we had 6.02 x 1023 M&M’s and we spread them out over the whole state of Washington, how deep would it be?

  2. The Mole 1 dozen = 12 1 gross = 144 1 ream = 500 1 mole = 6.02 x 1023 That is a REALLY BIG number…

  3. Learning Check Suppose we invented a new collection unit called a Wik. One Wik contains 8 objects. 1. How many paper clips in 1 Wik? a) 1 b) 4 c) 8 2. How many oranges in 2.0 Wik? a) 4 b) 8 c) 16 3. 40 gummy bears is how many Wiks? a) 5 b) 10 c) 20

  4. Just How Big is a Mole? • Enough soft drink cans to cover the surface of the earth to a depth of over 200 miles. • If you had Avogadro's number of unpopped popcorn kernels, and spread them across the United States of America, the country would be covered in popcorn to a depth of over 9 miles. • If we were able to count atoms at the rate of 10 million per second, it would take about 2 billion years to count the atoms in one mole.

  5. A mole = Avogadro’s Number 6.02 x 1023 Otherwise known as“Avogadro’s Number” in honor of the Italian chemist Amadeo Avogadro (1776-1855). Amadeo Avogadro

  6. The Mole • 1 dozen cookies = 12 cookies • 1 mole of cookies = 6.02 X 1023 cookies • 1 dozen cars = 12 cars • 1 mole of cars = 6.02 X 1023 cars • 1 dozen Al atoms = 12 Al atoms • 1 mole of Al atoms = 6.02 X 1023 Al atoms Note that the NUMBER is always the same, but the MASS is very different! Mole is abbreviated mol

  7. A Mole of ParticlesContains 6.02 x 1023 particles = 6.02 x 1023 C atoms = 6.02 x 1023H2O molecules = 6.02 x 1023NaCl “molecules” 1 mole C atoms 1 mole H2O molecules 1 mole NaCl molecules

  8. Avogadro’s Number as Conversion Factor 6.02 x 1023 particles 1 mole particles or 1 mole particles 6.02 x 1023 particles Note that a particle could be anything!

  9. The Mole • So how do we use the mole in Chemistry? • There are 6.94 grams of lithium in one mole of Li atoms. • If we have one mole of Carbon how many grams do we have? • Notice, these are called atomic weights • on your periodic charts

  10. Using the Mole • We use the mole to convert a measured mass of an element to find the # of atoms that are present. • Ex: Mass 12g of carbon-12 and you know you’ll have 1 mole of carbon which is 6.02 x 1023 atoms of carbon.(cool, eh?)

  11. Calculations with Moles:Converting moles to grams How many grams of lithium are in 3.50 moles of lithium? 3.50 mol Li 6.94 g Li = g Li 24.3 1 mol Li There are 24.3 grams of lithium in 3.50 moles of lithium.

  12. Calculations with Moles:Converting grams to moles How many moles of lithium are in 18.2 grams of lithium? 18.2 g Li 1 mol Li = mol Li 2.62 6.94 g Li There are 2.62 moles of lithium in 18.2 grams of lithium.

  13. Calculations with Moles:Using Avogadro’s Number How many atoms of lithium are in 3.50 moles of lithium? 3.50 mol Li 6.02 x 1023 atoms Li = atoms Li 2.11 x 1024 1 mol Li There are 2.11 x 1024atoms of lithium in 3.50 moles of lithium.

  14. Calculations with Moles:Using Avogadro’s Number How many atoms of lithium are in 18.2 g of lithium? 18.2 g Li 1 mol Li 6.02 x 1023 atoms Li 6.94 g Li 1 mol Li = atoms Li 1.58 x 1024

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