1. Prepare for Test Bellwork Turn in Chapter 9 EQ
Cellphones off and in backpack
All back packs at the front of the classroom
You need:
A piece of paper and a pencil

2. Chapter 10
The Mole

3. MAKE A NEW SECTION Chapter 10
Copy down the Main Idea and Essential Questions
Main Idea: Chemists use the mole to count atoms, molecules, ions, and formula units
Essential Questions:
Unit
What is a mole and why do we use moles in chemistry?
Lesson
How are moles calculated?
How is percent composition calculated?
What is the difference between an empirical and molecular formula?
What does a chemical formula tell you?

4. Chapter 10 Word Study Guide
Word, Definition, Your Definition, Picture Optional
Avogadro’s Number
Mole
Representative particle
Molar mass
Empirical formula
Molecular formula
Percent composition

5. Launch Lab Complete Launch Lab (Work with a group of 2-3 plp) Page 319
Analysis #’s 1-3

6. Homework
Complete Word Study guide
Read Chapter 10
Outline

7. Bellwork
What is a mole? Be ready to present your answer to the class.

8. Bellwork Mrs. Stewart is 5 feet tall.
If you have 10 of me, how far will it be if I am lined up from head to toe?
If my son, Gunner, is 2 feet tall, how many of him would it take to cover the same distance?

9. Apples Problem Here is how converting works
Important: 1 dozen apples = 12 apples
1 dozen apples = 2.0 kg
1 dozen apples = .20 bushels
What is the mass of 90 average-sized apples if 1 dozen of the apples has a mass of 2.0 kg?

10. Why use the mole?
Chemists need a convenient method for accurately counting the number of atoms, molecules, or formula units in a sample of a substance.
Because atoms are so small its impossible to count them directly.
Therefore, the MOLE was developed.

11. The Mole SI base unit used to measure the amount of a substance.
Mole = Mol
Representative particle = any particle
Atom
Molecule
Formula unit
Electron
Ion
1 mol = 6.02 x 1023 representative particles
Avogadro’s number

12. Converting between Moles and Particles
IMPORTANT
1 mol = 6.02 x 1023 representative particles
Watch!!!
How many particle of sucrose are in 3.5 mol of sucrose?

13. Your Turn Practice Problem 1 teach 2’s 2’s teach 1’s
Page 323 #’s 1 and 3
2’s teach 1’s
Page 323 #’s 2 and 4
Hint: 4 has one extra step!!!! TRICKY!

14. Particles to Moles Remember:
1 mol = 6.02 x 1023 representative particles
How many moles of sucrose do you have if you contain 2.11 x 1024 molecules of sucrose?

15. Classwork Complete the following problems 2’s teach 1’s 1’s teach 2’s
Page 324 # 5
1’s teach 2’s
Page 324 # 6

16. Practice How many molecules are in 23 moles of oxygen?
How many moles are in 3.4 x 1023 molecules of H2SO4?
How many molecules are there in moles of C6H14?
How many moles are there in 2.35 x 1024 atoms of Fe?

17. Journal – By yourself
Page 324
#’s 13 and 14

18. Classwork How many atoms are in 3.68 moles of CO2?
How many molecules are in 4.3 moles of N2O2?
If you have 3.98 x 1021atoms of Mg, how many moles do you have?
If you have 7.2 moles of Na+, how many ions do you have?
How many formula units are in .35 moles of NaCl?
Determine the number of moles in 8.92 x 1023 ions of Fe+2.
Determine the number of atoms in 2.6 moles of Pb.
How many molecules are in 6.21 moles of SO2?
If you have 5.6 x 1021 formula units of PbSO4, how many moles do you have?
Determine the number of moles in 5.78 x 1026 atoms of Hg.

19. Molar Mass
The atomic mass of an element expressed in grams, is the mass of one mole of the element.
This is called Molar Mass
Carbons molar mass is 12g
Molar masses are rounded off to one place after the decimal point.
You know that 12.0 g is the molar mass of carbon, so 12.0g is 1 mol of carbon (6.02 X 1023 atoms of carbon).
UNITS are g/mol

20. Molar Mass of Compound
To find the mass of a mole of a compound, you must know the formula of the compound.
EX: Formula of sulfur trioxide is SO3
1 atom of sulfur and 3 atoms of oxygen
Calculate the mass of a molecule by adding atomic masses of atoms making up the molecule.
S = 32.1 amu O = 3 X 16.0 = 48.0 amu
SO, SO3 = = 80.1 amu
What does this mean?
80.1 g is the mass of 6.02 X 1023 molecules of SO3
80.1 g SO3 = 1 mol SO3

21. Classwork Find the molar mass of the following compounds
PbSO4
N3O4
Al2O3
You measure 34.6 grams of H2O. How many moles are present in this sample of H2O? How many molecules?

22. BELLWORK
1. How many moles of magnesium is 3.01 x 1022 atoms of magnesium?  
2. How many molecules are there in 4.00 moles of glucose, C6H12O6? 
3. How many moles are 1.20 x 1025 atoms of phosphorous?
4. How many atoms are in moles of zinc?
5. How many molecules are in moles of N2O5?

23. Practice Problems
The decomposition of Hydrogen peroxide (H2O2) provides sufficient energy to launch a rocket. What is the molar mass of hydrogen peroxide?
Find the molar mass of PCl3.
What is the mass of 1.00 mol of sodium hydrogen carbonate?

24. Mole to grams conversions
What is the mass of 4.56 mol of H2O?
There is 3.65 x 10-5 mol of NaCl, find the mass of the substance.
How many moles are in 5.64 x 102 grams of Ca(OH)2?

25. Practice
Page 328 and 329
#’s 15-18

26. Practice Problems Page 336 and 337 1’s teach 2’s 2’s teach 1’s

27. practice If I have 4.7 moles of CO2, how many grams do I have?
How many moles does SnO have with a mass of 765.9?
Determine the number of moles in grams of MgS.
How many grams are in 8.23 moles of K2O?
You measure 34.6 grams of H2O. How many moles are present in this sample of H2O? How many molecules?

28. Journal
Identify the conversion factors that we have discussed up until now.
Identify the 4 types of representative particles and give an example of each.
Find the molar mass of the following compounds
Cr2O3
MgS

29. Practice How many grams are in 3.2 moles of PbCl2?
How many moles are in 3.45 x 1025 atoms of Na?

30. Mole Conversions (GRADE)
What is the mass of 2.0 moles of LiOH?
How many moles of glucose does 1.2 x 1024 molecules represent?
How many moles does 22.0 grams of CO2 represent?
How many moles does 56.0 grams of N2 represent?
How many atoms does 2.2 x 101 moles of He represent?

31. Two Step Process Page 331 #’s 19, 20, 21 TWO STEP PROCESS
Atoms to mass
Mass to atoms or molecules
TWO STEP PROCESS
Representative particles to mass
Change representative particles to moles
Change moles to grams
Mass to representative particles
Change mass to moles
Change moles to representative particles (atoms or molecules)

32. Bellwork: Mole conversions
How many formula units are in 3.65 x 102 g of NaCl?
How many molecules does 45.0 grams of C6H12O6 represent?
How many moles of water does 6.02 x 1023 molecules represent?
Convert 3.01 x 1023 molecules of C2H6 to moles.
What is the mass of 7.23 x 1025 formula units of CuSO4 ?

33. Practice How many grams are in 5.23 x 1023 molecules of SO3?
How many grams are in 5.6 moles of KCl?
If you have 4.3 moles of AgNO3, how many formula units do you have?

34. Avogadro’s Hypothesis
States that equal volumes of gases at same temp and pressure contain equal # of particles.
Particles are different sizes
However, because the particles of gases are spread so far apart, the number of smaller particles are usually equal to the number of larger particles in a given area.

35. Here is our LAST conversion Factor
At standard temperature and pressure
1 mol = 22.4 L (volume) or
6.02 X 10^23 representative particles = 22.4 L
Example
You collect L H2 at STP, calculate the number of moles of H2.

36. Practice Determine the volume in liters, of 0.60 mol SO2 gas at STP.
Determine the volume in liters, of 3.20 X 10-3 mol CO2.
Determine the volume in liters, of 3.70 mol N2.

37. More Practice How many total atoms are in 1.0 moles of H2O ?
How many moles of water does 6.02 x 1023 molecules represent?
How many moles does 80.0 grams of H2O represent?
What is the mass of 5.0 moles of Ba(CN)2 ?
At STP, what volume does 1.25 mol H2 occupy?
At STP, how many moles are in 43.3 L C2H6?

38. Last Set!!! How many moles are 73.8 L Na ions?
Convert 5.00 moles of carbon trioxide to grams.
Convert 4.86 x 104g of Mg3N2 to moles.
A sample of NH3 gas occupies 75.0 liters at STP. How many molecules is this?

39. Grade SHOW ALL YOUR WORK!!!!!
NO WORK = NO CREDIT
How many liters are in 5.4 moles of NaCl?
If you have g of NH3, how many moles do you have?
How many molecules are in 3.2 moles of CO2?
How many moles are in 2.68 x 1022 atoms of Mg?
There is L of KBr, how many moles are there?
If you have 5.2 moles of C2H6, how many grams do you have?

40. Grade Continued How many molecules are in 1.2 moles of C6H12O6?
How many formula Units are in 2.3 x 1022 moles of Ca(OH)2 ?
How many grams are in 5.26 x 1023 molecules of NO2?
How many liters are in 56.3 g of BaO?

41. Understanding Check Answer the following questions:
What is a mole and why do we use moles in chemistry?
How are moles calculated?
3 conversion factors?
Identify all the types of representative particles

42. Percent composition Percent mass = mass of element x 100
mass of compound
Determine the percent composition of Sodium hydrogen carbonate (NaHCO3), also called baking soda.

43. Page 344 #’s 54-57 Practice Problems
Complete these problems with your shoulder partner

44. Classwork Find the percent composition of the following compounds
1’s Teach 2’s
NaOH
(NH4)2S
2’s teach 1’s
N2S2
PbSO4

45. Homework How many Mg atoms are in 3.24 moles of Mg?
How many liters of Mg are in 1.6 moles of Mg?
2.68 x 1024 atoms of Cu equal how many moles?
How many grams are there in 1.5 x1025 molecules
of CO2?
5. How many moles are x 1023 NaCl formula Units?
6. How many moles are in 812 grams of Ca?
How many moles are 73.8 L Na ions?

46. Bellwork
Calculate the percent composition of the compounds that are formed from these reactions:
9.03 g of Magnesium combine completely with 3.48 g of Nitrogen.
29.0 g of Argon combine completely with 4.30 g of Sulfur.
222.6 g of Sodium combine completely with 77.4 g of Oxygen.

47. Complete Practice
Calculate the mass of the element in the given mass of compound:
Mass of Hydrogen in 350 g C2H6
Mass of Oxygen in 20.2 g of NaHSO4
Mass of Hydrogen in 124 g of Ca(C2H3O2)2
Mass of Nitrogen in 378 g HCN
Mass of Oxygen in 100 g H2O

48. Empirical Formula
The formula with the smallest whole number moles-ratio of the elements.
May or may not be the same at the molecular formula.
WHY?????
Step 1 – Take percent sign and change to grams
Step 2 - Solve for moles
Step 3 – if not in whole numbers divide each number by the lowest decimal.
Step 4 – if still not a whole number, multiply by the lowest factor that would make it a whole number

49. Example
Determine the empirical formula for methyl acetate which is made up of 48.64% C, 8.16%H, and 43.20%O

50. Complete Practice Problems
1’s teach 2’s
Problems 58 and 59
2’s teach 1’s
Problems 60-61
PAGE 346

51. Go over Pg 346 #’s 58-61

52. More Practice
What is the empirical formula for a compound which contains g of iron, g of sulfur and g of oxygen?
Find the empirical formula for a compound which contains 32.8% chromium and 67.2% chlorine.

53. Practice
Barry Um has a sample of a compound which weighs 200 grams and contains only carbon, hydrogen, oxygen and nitrogen. By analysis, he finds that it contains grams of carbon, g of hydrogen, g of oxygen and g of nitrogen. Find its empirical formula.

54. Practice Problems
grams of an organic compound is known to contain grams of carbon, grams of hydrogen, grams of oxygen. What is the empirical formula of the compound?

55. Molecular Formula
Specifies the actual number of atoms of each element in one molecule or formula unit of the substance.
Step 1 – divide the experimentally determined molar mass by the mass of the empirical formula.
Step 2 – take the previous answer and multiply it times the subscripts of the empirical formula.

56. Example
The chemical analysis of succinic acid is 40.68% C, 5.08%H, and % O and has a molar mass of 118.1g/mol. Determine the empirical and molecular formulas.

57. Complete Practice With your shoulder partner complete the following:
Page 350 #’s 62-66
Also copy down the graphic organizer on page 347, figure 10.15

58. Study Guide How many moles are in 4.3 x 1022 atoms of Mg?
How many liters are in 4.6 moles on NaCl?
How many grams are in 8.9 moles of MgCl2?
How many liters are in grams of KCl?
Calculate the percent composition
NaHSO4
222.6 g of Sodium combine completely with 77.4 g of Oxygen

59. Study Guide Continued
What’s the empirical formula of a molecule containing 65.5% carbon, 5.5% hydrogen, and 29.0% oxygen?
A compound with an empirical formula of C2OH4 and a molar mass of 88 grams per mole, calculate the molecular formula
A component of protein called serine has an approximate molar mass of 100 g/mole. If the percent composition is as follows, what is the empirical and molecular formula of serine?
C = % H= % O = % N= %

60. Chapter 10 Study Guide How many moles are in 34.6 L of BaO?
How many grams are in 4.6 moles of PbSO4?
How many molecules are in 6.5 x 103 moles of CO2?
If you have 2.68 moles of S2O3, how many atoms of S do you have?
How many liters are in 4.39 x 1022 atoms of Mg?
The compound methyl butanoate smells like apples. It’s percent composition is 58.8% C, 9.8% H, and 31.4% O and its molar mass is 204 g/mol. What is its empirical formula? What is its molecular formula?
Find the molecular formula of ethylene glycol, which is used as antifreeze. The molar mass is 62 g/mol and the empirical formula is CH3O.
Determine the molecular formula if you have 34.98g Al and 64.02g S and a molar mass of