1. Chapter 10
The Mole

3. National Standards for Chapter 10
UCP.1 Systems, order, and organization
A.1 Abilities necessary to do scientific inquiry
A.2 Understandings about scientific inquiry
B.1 Structure of atoms
B.2 Structure ad properties of matter
B.3 Chemical reactions
B.6 Interactions of energy and matter
E.1 Abilities of technological design
E.2 Understandings about science and technology
F.5 Natural and human-induced hazards
F.6 Science and technology in local, national, and global challenges
G.1 Science as a human endeavor
G.2 Nature of scientific knowledge
G.3 Historical perspectives

4. Vocabulary/Study Guide
Define each term using the Glossary
Either write on the handout, or use your own paper
This is due on Test Day (tentatively, Monday, March 31)

5. Section 1: Measuring Matter
National Standards:
UCP.1 Systems, order, and organization
A.1 Abilities necessary to do scientific inquiry
B.2 Structure ad properties of matter
E.2 Understandings about science and technology
G.2 Nature of scientific knowledge
G.3 Historical perspectives

6. Objectives – Section 1
Explain how a mole is used to indirectly count the number of particles of matter.
Relate the mole to a common everyday counting unit.
Convert between moles and number of representative particles.
REVIEW VOCABULARY:
molecule: two or more atoms that covalently bond together to form a unit

7. New Vocabulary
mole Avogadro’s number Chemists use the mole to count atoms, molecules, ions, and formula units.

8. Lab: How much is a mole? (pg. 318)

9. Counting Particles
Chemists need a convenient method for accurately counting the number of atoms, molecules, or formula units of a substance.
The mole is the SI base unit used to measure the amount of a substance.
1 mole is the amount of atoms in 12 g of pure carbon-12, or 6.02  1023 representative particles, which is any kind of particle – an atom, a molecule, a formula unit, an electron, an ion, etc.
The number is called Avogadro’s number.

10. Converting Between Moles and Particles
Conversion factors must be used.
Moles to particles
Number of molecules in 3.50 mol of sucrose

11. Converting Between Moles and Particles
Particles to moles
Use the inverse of Avogadro’s number as the conversion factor.

12. Converting Between Moles and Particles
Practice Problems #1-4, page 323
Practice Problems #5-6, page 324

13. Mole Day Facts
Fact 1- It is believed that one mole of paper if stacked can reach the moon more than 80 billion times.
Fact 2- The second fact about one mole of grain of sand would be much more than that what is there at Miami Beach.
Fact 3- The next fact about one mole is that one mole of blood cells would be more than the number of blood cells in every human-being on earth.
Fact 4- It is also believed that one liter of water contains 55.5 moles of water.
Fact 5- An astonishing fact about one mole is that one mole is approximately 1,616,434 light years or it can also be easily 8 times around our galaxy.
Fact 6- Another interesting fact about one mole is that one mole of seconds is approximately 19 quadrillion years. It is 954,150 times the age of the universe or 4,240,666 times earth’s age.
Fact 7- An important fact about one mole is that one mole of cents would be good enough to repay the debt of United States of America 86 million times.

14. Homework, Section 1 SECTION 1 REVIEW, Page 324 Questions #7-14
Answer with complete sentences
Due tomorrow

15. Section 2: Mass and the Mole
National Standards:
UCP.1 Systems, order, and organization
B.1 Structure of atoms
B.2 Structure ad properties of matter
E.2 Understandings about science and technology

16. Objectives – Section 2 Review Vocabulary:
Relate the mass of an atom to the mass of a mole of atoms.
Convert between number of moles and the mass of an element.
Convert between number of moles and number of atoms of an element.
Review Vocabulary:
conversion factor: a ratio of equivalent values used to express the same quantity in different units

17. New Vocabulary
molar mass A mole always contains the same number of particles; however, moles of different substances have different masses.

18. The Mass of a Mole
1 mol of copper (6.02 x 1023 atoms of copper) and 1 mol of carbon (6.02 x 1023 atoms of carbon) have different masses.
One copper atom has a different mass than 1 carbon atom.

19. The Mass of a Mole
Molar mass is the mass in grams of one mole of any pure substance.
The molar mass of any element is numerically equivalent to its atomic mass and has the units g/mol.

20. Lab: Formulate a Model (pg. 326)

21. Using Molar Mass Moles to mass
3.00 moles of copper has a mass of 191 g.

22. Using Molar Mass
Convert mass to moles with the inverse molar mass conversion factor.
Convert moles to atoms with Avogadro’s number as the conversion factor.

23. Using Molar Mass
Practice Problems #15-18, page 328

24. Math Skills Transparency 13

25. Using Molar Mass
This figure shows the steps to complete conversions between mass and atoms.

26. Using Molar Mass
Practice Problems #19-21, page 331

27. Homework, Section 2 SECTION 2 REVIEW, Page 332 Questions #22-28
Answer with complete sentences
Due tomorrow

28. Section 3: Moles of Compounds
National Standards:
UCP.1 Systems, order, and organization
B.2 Structure and properties of matter
E.2 Understandings about science and technology

29. Objectives – Section 3 Review Vocabulary:
Recognize the mole relationships shown by a chemical formula.
Calculate the molar mass of a compound.
Convert between the number of moles and mass of a compound.
Apply conversion factors to determine the number of atoms or ions in a known mass of a compound.
Review Vocabulary:
representative particle: an atom, molecule, formula unit, or ion

30. New Vocabulary
The molar mass of a compound can be calculated from its chemical formula and can be used to convert from mass to moles of that compound.

31. Chemical Formula and the Mole
Chemical formulas indicate the numbers and types of atoms contained in one unit of the compound.
One mole of CCl2F2 contains one mole of C atoms, two moles of Cl atoms, and two moles of F atoms.

32. Chemical Formulas and the Mole
Practice Problems #29-33, page 335

33. The Molar Mass of Compounds
The molar mass of a compound equals the molar mass of each element, multiplied by the moles of that element in the chemical formula, added together.
The molar mass of a compound demonstrates the law of conservation of mass.

34. Molar Mass of Compounds
Practice Problems #34-36, page 335

35. Math Skills Transparency 14: Calculating the Molar Mass of a Compound

36. Converting Moles of a Compound to Mass
For elements, the conversion factor is the molar mass of the compound.
The procedure is the same for compounds, except that you must first calculate the molar mass of the compound.

37. Converting Moles of a Compound to Mass
Practice Problems #37-39, page 336

38. Converting the Mass of a Compound to Moles
The conversion factor is the inverse of the molar mass of the compound.

39. Converting the Mass of a Compound to Moles
Practice Problems #40-41, page 337

40. Converting the Mass of a Compound to Number of Particles
Convert mass to moles of compound with the inverse of molar mass.
Convert moles to particles with Avogadro’s number.

41. Converting the Mass of a Compound to Number of Particles
Practice Problems #42-46, page 339

42. Converting the Mass of a Compound to Number of Particles
This figure summarizes the conversions between mass, moles, and particles.

43. Transparency 34: Mass-to-Mole and Mole-to-Particles Conversions for Compounds

44. Lab: Estimating the Size of a Mole

45. Homework, Section 3 SECTION 3 REVIEW, Page 340 Questions #47-53
Answer with complete sentences
Due tomorrow

46. Section 4: Empirical and Molecular Formulas
National Standards:
UCP.1 Systems, order, and organization
A.1 Abilities necessary to do scientific inquiry
A.2 Understandings about scientific inquiry
B.2 Structure ad properties of matter
E.2 Understandings about science and technology
G.1 Science as a human endeavor

47. Objectives – Section 4 Review Vocabulary:
Explain what is meant by the percent composition of a compound.
Determine the empirical and molecular formulas for a compound from mass percent and actual mass data.
Review Vocabulary:
percent by mass: the ratio of the mass of each element to the total mass of the compound expressed as a percent

48. New Vocabulary
percent composition empirical formula molecular formula A molecular formula of a compound is a whole-number multiple of its empirical formula.

49. Percent Composition
The percent by mass of any element in a compound can be found by dividing the mass of the element by the mass of the compound and multiplying by 100.

50. Percent Composition
The percent by mass of each element in a compound is the percent composition of a compound.
Percent composition of a compound can also be determined from its chemical formula.

51. Mini-Lab: Analyze Chewing Gum, pg. 342

52. Percent Composition
Practice Problems #54-57, page 344

53. Empirical Formula
The empirical formula for a compound is the smallest whole-number mole ratio of the elements.
You can calculate the empirical formula from percent by mass by assuming you have g of the compound. Then, convert the mass of each element to moles.
The empirical formula may or may not be the same as the molecular formula.
Molecular formula of hydrogen peroxide = H2O2
Empirical formula of hydrogen peroxide = HO

54. Empirical Formula
Practice Problems #58-61, page 346

55. Molecular Formula
The molecular formula specifies the actual number of atoms of each element in one molecule or formula unit of the substance.
Molecular formula is always a whole-number multiple of the empirical formula.

56. Molecular Formula

57. Molecular Formula
Practice Problems #62-66, page 350

58. Lab: Mole Ratios

59. Molecular Formula
Worksheet: Supplemental Problems

60. Homework, Section 4 SECTION 4 REVIEW, Page 350 Questions #67-73
Answer with complete sentences
Due tomorrow

61. Section 5: Formulas of Hydrates
National Standards:
UCP.1 Systems, order, and organization
A.1 Abilities necessary to do scientific inquiry
A.2 Understandings about scientific inquiry
B.2 Structure ad properties of matter
B.3 Chemical reactions
B.6 Interactions of energy and matter
E.1 Abilities of technological design
E.2 Understandings about science and technology
F.5 Natural and human-induced hazards
F.6 Science and technology in local, national, and global challenges

62. Objectives – Section 5
Explain what a hydrate is and relate the name of the hydrate to its composition.
Determine the formula of a hydrate from laboratory data.
Review Vocabulary:
crystal lattice: a three-dimensional geometric arrangement of particles

63. New Vocabulary
hydrate Hydrates are solid ionic compounds in which water molecules are trapped.

64. Naming Hydrates
A hydrate is a compound that has a specific number of water molecules bound to its atoms.
The number of water molecules associated with each formula unit of the compound is written following a dot.
Sodium carbonate decahydrate = Na2CO3 • 10H2O

65. Naming Hydrates

66. Analyzing a Hydrate
When heated, water molecules are released from a hydrate leaving an anhydrous compound.
To determine the formula of a hydrate, find the number of moles of water associated with 1 mole of hydrate.

67. Analyzing a Hydrate Weigh hydrate. Heat to drive off the water.
Weigh the anhydrous compound.
Subtract and convert the difference to moles.
The ratio of moles of water to moles of anhydrous compound is the coefficient for water in the hydrate.

68. Analyzing a Hydrate
Practice Problems #74-75, page 353

69. Lab: Determine the Formula of a Hydrate, page 356

70. Use of Hydrates
Anhydrous forms of hydrates are often used to absorb water, particularly during shipment of electronic and optical equipment.
In chemistry labs, anhydrous forms of hydrates are used to remove moisture from the air and keep other substances dry.

71. Homework, Section 5 SECTION 5 REVIEW, Page 354 Questions #76-82
Answer with complete sentences
Due tomorrow

72. Key Concepts
The mole is a unit used to count particles of matter indirectly. One mole of a pure substance contains Avogadro’s number of particles.
Representative particles include atoms, ions, molecules, formula units, electrons, and other similar particles.
One mole of carbon-12 atoms has a mass of exactly 12 g.
Conversion factors written from Avogadro’s relationship can be used to convert between moles and number of representative particles.

73. Key Concepts
The mass in grams of 1 mol of any pure substance is called its molar mass.
The molar mass of an element is numerically equal to its atomic mass.
The molar mass of any substance is the mass in grams of Avogadro’s number of representative particles of the substance.
Molar mass is used to convert from moles to mass. The inverse of molar mass is used to convert from mass to moles.

74. Key Concepts
Subscripts in a chemical formula indicate how many moles of each element are present in 1 mol of the compound.
The molar mass of a compound is calculated from the molar masses of all of the elements in the compound.
Conversion factors based on a compound’s molar mass are used to convert between moles and mass of a compound.

75. Key Concepts
The percent by mass of an element in a compound gives the percentage of the compound’s total mass due to that element.
The subscripts in an empirical formula give the smallest whole-number ratio of moles of elements in the compound.
The molecular formula gives the actual number of atoms of each element in a molecule or formula unit of a substance.
The molecular formula is a whole-number multiple of the empirical formula.

76. Key Concepts
The formula of a hydrate consists of the formula of the ionic compound and the number of water molecules associated with one formula unit.
The name of a hydrate consists of the compound name and the word hydrate with a prefix indicating the number of water molecules in 1 mol of the compound.
Anhydrous compounds are formed when hydrates are heated.