2.  What do the following all have in common?

3. DDozen CCouple FFew BBaker’s Dozen TTen

4.  Mole- counting unit standing for 6.02 x 10 23 particles  Tells us how many particles of a compound are actually involved in a reaction  1 mole = 6.02 x 10 23 particles 602,000,000,000,000,000,000,000 particles Avogadro’s Number

5.  1 mole of water = how many particles?  1 mole of sugar = how many particles  6.02 x 10 23 particles = how many moles?

6.  A dozen eggs would make a HUGE omelet!  A mole of eggs would make an omelet big enough to cover the Earth thirty times!

7.  Atoms and Molecules are TINY!  A drop of water contains 10 trillion water particles!

8.  6.02 x 10 23 makes a chemist’s life a lot easier  It’s impossible to keep track of one atom  so scientist discovered this number that gives us the molar mass of an atom  Molar mass is the mass of 6.02 x 10 23 particles of a given substance  Mass is given in grams

9.  We don’t always have exactly 1 mole, though.  When we have different amounts of moles, we can convert between atoms and moles

10. MolesParticles Multiply by Avogadro’s Number Divide by Avogadro’s Number

11.  A lab experiment calls for 2.00 moles of Calcium. How many particles of Calcium are required?  How can we solve this?  Dimensional Analysis! ▪ ID what we’re given and what the question’s asking for and set up the T-Chart 2 moles Calcium 1 mole Calcium 6.02 x 10 23 particles

12.  You have 12.04x10 23 atoms of sulfur. How many moles of sulfur do you have?

14.  Molar Mass = the mass of 1 mole of a substance  Tells us what mass of a substance is used in a reaction

15. Molar mass: mass of 1 mole of in grams 1 mole C atoms = ___________ particles 1 mole of C atoms has a molar mass of_________ g. Molar mass of O = ___________ Molar mass of Li = ____________ For any element, the Molar Mass = Mass Number 3.2

16. What is the mass of one mole of: C S Cu Fe Hg 3.2

17. 1) Count out the atoms in the compound 2) Look up the Molar Mass for each element 3) Multiply the Molar Mass of each element by the # present in the compound 4) Sum the Molar Masses

18.  No more than 4 at a station  10 min at each station max  If completed before 10 min is up, check answers up at the front  Use your station buddies for help before asking Ms. Herndon!

19.  NO2  SO 2  (NH 4 ) 3 PO 4  C 6 H 12 O 6

20. 1) How many particles are in a mole? 2) Determine the Molar Mass for the following problems. Don’t forget your UNITS! a. Helium (He) b. KCl 4 c. Cu(OH) 2

21.  If I had 20 Dollars, and the cost of one pair of kicks is 4 dollars for 1 pair, how many pairs could I have? 20 Dollars 4 Dollars 1 pair(20/4) pairs5 pairs Now... What’s my conversion factor? What unit am I given? What unit is the question asking for?

22.  If I had 20 grams of helium, and one mole of helium is 4 grams, how many moles of helium could I have? 20 grams He 4 grams He 1 mole He(20/4) moles He5 moles He What’s my conversion factor? What unit am I given? What unit is the question asking for?