1. Unit 8 Day 1

2. Warm Up 1) What would be the easiest way to determine how many peanuts are in this container? EQ: What is a mole? HOT Q1: How do we convert between particles and moles? HOT Q2: What is molar mass? HOT Q3: How do we convert between moles and grams?

3. Let’s say that 100 peanuts have a mass of 55 grams. The peanuts inside the container weigh 110 grams. How can we determine how many peanuts we have without counting them one by one?

4. What do peanuts have to do with chemistry? How many hydrogen atoms are in this container of water? Can you count them? …In this unit we will use mass to determine how many atoms are in substances.

5. Agenda Warm Up / Objectives Demo: The Mole Molar Mass and 1 step conversions Practice Exit Ticket BECOME LEGENDARY HOMEWORK: WORKSHEET 8.1

6. Objectives Students will calculate molar mass for a given substance Students will convert between number of particles and moles, vise versa Students will convert between grams and moles, vise versa

7. Warm Up If I asked you to go to the store and get M&Ms for all three of my classes (85 students), what would you buy? If I asked you to go to the store and buy tissues for my classroom for the rest of this semester, what would you buy? If I asked you to go to the store and buy eggs, how many would you buy?

8. Just like you want an easy way to buy M&Ms and tissues (in a package!) – scientists wanted an easy way to “package” atoms, molecules, electrons, etc. Instead of one bag of M&Ms or one box of tissues, scientists came up with THE MOLE to count atoms, molecules, etc. Because atoms, electrons, molecules, etc are so tiny this number needed to be really big to make counting easy!

9. Demo: The MoleDate 5/5/11 Eye Level Salt Sugar Water

10. In chemistry we use a unit called the THE MOLE to measure the number of particles in a sample. 1 MOLE of water = 18 grams 1 MOLE of salt = 58 grams 1 MOLE of sugar = 180 grams How many particles do you think are in a mole?????? (remember, it is the same number of particles for all of them)

11. Just like 1 dozen = 12 1 mole = 6.022 x 10 23 …. Or 602,200,000,000,000,000,000,000.0 This number is named Avogadro’s number for Italian scientist Amedeo Avogadro.

12. Conclusion Why do we use this quantity called “The MOLE” in chemistry?

13. Consensus 1 mole = 6.02 x10 23 atoms/molecules 1 mole = molar mass of a compound (measured in grams) 1 mole = 22.4 L of gas @ standard temperature and pressure (STP)

14. THE MOLE = 6.02 x 10 23 particles 60200000000000000000000 particles One mole of ANYTHING = 6.02 x 10 23 particles

15. Chemistry Unit 8 - The Mole Size of the mole!

16. HOW LARGE IS THE MOLE?!?! 1.Assuming that each human being has 60 trillion body cells (6 x 10 13 ) and that the earth's population is 6 billion (6 x 10 9 ), calculate the total number of living human body cells on this planet. Is this number smaller or larger than a mole? 2. If the circumference of the earth is 24,859 miles and the average person takes 2,000 steps to walk one mile. How many steps would it take to walk around the earth one time? Is this greater than or less than the mole?

17. Make a Unit 8 Packet!

18. 1 dozen egg = 12 eggs. How many eggs are in 3 dozen eggs? 1 atm of pressure = 760 torr. How many torr are in 2 atm of pressure? 1 mole of anything = 6.02 x 10 23 particles/atoms/molecules. How many particles are in 2 moles of oxygen? Notes: The Mole - 1 step Date 5/5/11 Converting…Conversion Factor Moles  atoms or molecules or particles 1 mole of anything = 6.02 x 10 23 atoms/molecules/particles Moles  volume 1 mole of gas = 22.4 liters @ standard temperature and pressure (STP) Moles  atoms or molecules 1 mole of anything = molar mass (g)

19. How many particles are in 4.8 moles of hydrogen? How many particles are in 134 moles of sugar? If you have 8.9 x10 35 particles of water, how many moles do you have?

20. Where do we find the mass number on our PToE? What is the mass of Na? What is the mass of Na 2 O?

21. Molar mass= the mass of 1 mole of a given element or compound (use mass numbers on the periodic table) Examples – 1 mole of magnesium = ___________grams – 1 mole of calcium = ____________grams – 1 mole of sodium chloride (NaCl) = ___________grams – 1 mole of sulfur trioxide(SO 3 ) = _____________grams – 1 mole of magnesium phosphate(Mg 3 (PO 4 ) 2 )= ____________grams

22. Putting Molar Mass to use…mole conversions Find the mass of 2 moles of NaCl. Find the mass of 6.7 moles of SO 3 If you have 184 grams of H 2 O, how many moles do you have? If you have 675 grams of copper, how many moles of copper do you have?

23. Jumbo Exit Ticket – 10 mins to complete then trade with partner! 1)What is the molar mass of CaSO 4 ? 2)What is the molar mass of MgCl 2 3)If you have 79 grams of NaCl, how many moles do you have? 4) If you have 4.3 moles of water, how many molecules do you have? 5) How many moles do you have if you have 1.16 x 10 24 atoms of magnesium chloride? 6) If you have 152 grams of water, how many moles of water do you have? 7) If you have 5.5 moles of SO 3, how many grams do you have? HOMEWORK: WORKSHEET #1

24. Molar Volume If you have 2.7 moles of water at STP, how many liters do you have? If you have 78.2 liters of carbon dioxide at STP, how many moles do you have?

25. Calculate the volume of each of the following quantities. 0.200 moles of H 2 S

26. Calculate the volume of each of the following quantities. 0.100 moles of KI

27. Calculate the volume of each of the following quantities. 2.55 mole Cu 2 CrO 4

28. Calculate the volume of each of the following quantities. 1.95 mole HNO 3

29. Calculate the number of moles for each of the following volumes. 1,500L of KClO

30. Calculate the number of moles for each of the following volumes. 200 L HC 2 H 3 O 2

31. Calculate the number of moles for each of the following volumes. 75 L of NaOH

32. Calculate the number of moles for each of the following volumes. 20.0 L NaCl