1. Drill: What is a chemical reaction? What is conserved for every chemical reaction?

2. Objective: The student will be able to: –Use the periodic table in order to calculate the molar mass (gram formula mass) of a compound.

3. SAT/HSA Enrichment: … is the exact opposite of decomposition. a.Analysis b.Combustion c.Direct combination d.Double Replacement e.Single Replacement

4. Engagement How many jellybeans are in the Jar?? –How will you determine the number of Jellybeans in the Jar? Work together in a group of 3 or 4 and come up with 1 key idea to report to the class.

5. Key Questions For The UNIT! 1.What is the basic unit for measuring numbers of particles? 2.What is the relationship between particles and mass in a substance? 3.How are chemical quantities determined? 4.How do available materials limit the amount of products?

6. The MOLE! A unit of measurement!

7. The Mole: A Measurement of Matter You could measure the amount of sand in a sand sculpture by counting each grain of sand, but it would be much easier to weigh the sand. You’ll discover how chemists measure the amount of a substance using a unit called a mole, which relates the number of particles to the mass.

8. Measuring Matter You often measure the amount of something by one of three different methods—by count, by mass, and by volume.

9. Sample Problem

13. What Is a Mole? A mole of any substance contains Avogadro’s number of representative particles, or 6.02  10 23 representative particles. –The term representative particle refers to the species present in a substance: usually atoms, molecules, or formula units.

14. Converting Number of Particles to Moles One mole (mol) of a substance is 6.02  10 23 representative particles of that substance and is the SI unit for measuring the amount of a substance. –The number of representative particles in a mole, 6.02  10 23, is called Avogadro’s number.

15. Converting Number of Particles to Moles

16. Sample Problem 2

18. Converting Moles to Number of Particles

19. Sample Problem 3

23. The Mass of a Mole of an Element The atomic mass of an element expressed in grams is the mass of a mole of the element. The mass of a mole of an element is its molar mass. One molar mass of carbon, sulfur, mercury, and iron are shown.

24. The Mass of a Mole of an Element

25. The Mass of a Mole of a Compound To calculate the molar mass of a compound – Find the number of grams of each element in one mole of the compound. –Then add the masses of the elements in the compound.

26. The Mass of a Mole of a Compound Substitute the unit grams for atomic mass units. Thus 1 mol of SO 3 has a mass of 80.1 g.

27. The Mass of a Mole of a Compound Molar Masses of Glucose, Water, and Para- dichlorobenzene

28. Sample Problem 4

31. Determining Molar Mass Gram Atomic Mass: –The molar mass of an element Gram Molecular Mass: –The molar mass of a molecule Gram Formula Mass: –The molar mass of an Ionic compound

32. Quick Quiz 1.The atomic mass of fluorine is 19.0 amu, so the molar mass is a.19.0 amu. b.19.0 g. c.6.02 x 10 23 amu. d.6.02 x 10 23 g.

33. Quick Quiz 2. Calculate the molar mass of ammonium nitrate. a.45.02 g b.80.05 g c.60.06 g d.48.05 g

34. Class work Formula and Molar Mass Worksheet Molar Mass worksheet: Do it yourself!

35. Summary Did we complete our objective? Explain. Define Molar Mass. Compare and Contrast Gram Molar Mass, Gram Formula Mass, and Gram Atomic Mass.

36. Summary Identify the steps used to determine the Molar or Formula Mass of a compound. Determine the unit used for Gram Molar Mass.

37. Homework: Molar mass and Formula mass worksheet. Exit Ticket –Pick 1 Place in the bin when finished!