Catalyst:

1. Catalyst: 10 minutes Please have study guide #3 out. 11 weeks have passed since the first day of school, how many SCHOOL days is that? You must use dimensional analysis to figure this out. End Homework: Study Guide #6-8 due Mon Bring some Snack/Junk Food Wrappers with ingredients • Table of Contents: • 63 Around the World 8 Squares • 64 Benchmark Annotated Answer Key • 65 - Six Types of Rxns Sheet • 66 – Notes: Conversions/DA • 67 – Dimensional Analysis Practice • 68 – Alka-Seltzer Lab

2. For A-S Lab, you will: 1) Work with ALL your group members to complete the alka-seltzer lab 2) Ask your teacher for your materials when you reach #11. If done early, begin HW 3) Go over the handout as a class

3. Catalyst: 10 minutes Please have Study Guide #3 out Draw the lewis dot structure for C2H4 End Homework: Mole conversion Worksheet • Table of Contents: • 66 – Notes: Conversions/DA • 67 – Dimensional Analysis Practice • 68 – Alka-Seltzer Lab • 69 – Jigsaw Takeaways • 70 – Notes:Mole and Avogadro’s #

4. Jigsaw Activity (60 min) • In your home groups, you will read the passage given • You will create some sort of graphic organizer to summarize this passage • Creativity is a must. You may create an ad, a magazine cover, etc. • You will have 5 minutes to present this to your classmates.

5. Presentation Take-aways • Fold your paper twice, so that there are 4 squares on the front and on the back. • We we will write as an entire class the major takeaways from the brief presentations. • Two Stars and a Wish for your classmates. • At the end you will reflect on the peer feedback in the form of a reflection

6. How High Can You Count? 602,200,000,000,000,000,000,000

7. Atoms, ions, and molecules are so small, that a grain of carbon may have over trillions of atoms/molecules/particles. • to make counting large numbers easier, scientist use the mole.

8. What is the mole?

9. 6.022 x 1023

10. The Mole • The mole is a unit that describes the amount of particles that a substance has. • Just like 1 dozen = 12 eggs, 1 deck = 52 card: 1 mole = 6.02 x 1023particles Avogadro’s Number

11. It’s a conversion factor! 6.022 x 1023 particles mole

12. What does 1 mole look like?

13. How did Amedeo Avogadro come up with this conversion factor or relationship for counting particles? He observed that The # of C atoms in exactly 12 grams of Carbon-12 had 6.022 x 1023 atoms, so let 1 mole of any substance = 6.02 X 1023 particles/ions/atoms/compounds

14. Get it? • 1 mole of C = 6.02 x 1023 C atoms • 1 mole of H2O = 6.02 x 1023 H2O molecules • 1 mole of Skittles = 6.02 x 1023 skittles • 1 mole of electrons = 6.02 x 1023 electrons

15. What does 1 mole look like?

16. Example 1 How many atoms are there 2.66 moles of sulfur? Hint: You will be using avogadro’s number b/c you want # of particles (atoms)

17. Example 2 Find the # of molecules in 2.5 moles of sulfur dioxide (S02)

18. What does all this mean? Don’t just do the math. • 2.5 moles of SO2 is like saying one dozen. • 1 mole of any substance has 6.022 X 1023 molecules • 2.5 moles of SO2 has 1.5 X 1024 molecules. • Chemists can’t deal with 1.5 X 1024 molecules, it’s too large so we convert it into a smaller number.

19. Example 3 How many moles are in 2.54 X 1022 Fe3+ cations?

20. You try these 4) How many ions are there in 0.187 moles of Na+ cations? Answer: 1.13 X 1023 5) How many atoms are there in 1.45 X 10-17 moles of arsenic? Ans: 8.73 X 106 atoms 6) How many compounds in 4.224 moles of acetic acid, C2H4O2? Ans: 2.54 X 1024 acetic acid compounds 7) How many moles of xenon does 5.66 X 1023 atoms have? Ans: 0.94 moles of Xe 8) A sample of SO2 has 3.01 X 1023 molecules, how many moles is this? Ans: 0.500 mol SO2

21. Moles can be converted to mass

22. Molar Mass • Molar mass is the mass, in grams, of 1 mole of substance. • The molar mass is equal to the mass listed on the periodic table • Units of Molar mass are g/mol Molar mass of carbon is 12 g / mol Means 1 mol of C has 12 grams Molar Mass

23. One more example… What is the molar mass of Thorium? What does that mean?

24. One more example… Molar mass of Th = 232 g/ mol 1 mole of Th has 232 grams

25. You can find the mass from moles or # of particles Example 9: You are given 2.44 X 1024 atoms of carbon whose molar mass is 12.01g/mol according to your PT. • How many moles is that? • How many grams of carbon is that?

26. Try: Example 10: Find the mass of each substance in g: • 2.11 x 1024 atoms of copper • 3.99 x 1025 molecules of methane, whose MM = 16 g/mol

27. Example 11: You typically find the molar mass of an element using the atomic mass but what if you have a compound like glycerol, C3H8O3

28. You Try - Example 12: Use the answer from Ex 11 to find the amount of molecules in 47.5 g of glycerol.

29. Example 13: Find the molar mass of ZnCl2

30. You try - Example 14: Find the molar mass of (NH4)2SO4

31. Example 15 • If there are 2 moles of ZnSO4, how many atoms are there total? • 2 moles of ZnSO4 has what mass?

32. Exit Slip (10 min) • Find the MM of toluene, C6H5CH3. • Find the # of moles in 7.51 g of toluene • How many covalently bonded compounds are found in 5 grams of toluene?

33. Review BINGO • Take out a sheet of paper and make a 4 x 4 grid by folding the paper in half 4 times. • Write the following terms/numbers on the sheet:

34. Questions 1. The mass, in grams, of 1 mole of substance 2. This is the molar mass for an element on the Periodic Table 3. This is the units for molar mass 4. Calculate the molar mass for H2SO4 5. Calculate the molar mass for Ca(OH)2 6. Calculate the molar mass for AlPO4 7. Calculate the molar mass for HCl 8. Calculate the molar mass for MgO2

35. Lab Conduct • Follow the procedure that has been given to you • Respect the equipment. It costs a lot of money to replace this stuff • Use the chemicals in a responsible and safe way • Clean up the space when you are done • Read the steps, they will tell you what to do.