1. Slide 1 of 43 Chemistry10.1

2. © Copyright Pearson Prentice Hall Slide 2 of 43 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. 10.1

3. Slide 3 of 43 © Copyright Pearson Prentice Hall The Mole: A Measurement of Matter > Measuring Matter You often measure the amount of something by one of three different methods—by count, by mass, and by volume. 10.1

4. © Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 4 of 43 10.1

5. © Copyright Pearson Prentice Hall Slide 5 of 43 Practice Problems for Sample Problem 10.1 Problem Solving 10.1 Solve Problem 1 with the help of an interactive guided tutorial.

6. Slide 6 of 43 © Copyright Pearson Prentice Hall The Mole: A Measurement of Matter > What is a mole? We are familiar with terms that represent a number: 1 dozen a bakers dozen 1 gross 1 ream a gaggle of geese

7. Slide 7 of 43 © Copyright Pearson Prentice Hall The Mole: A Measurement of Matter > What is a mole? A mole is also a term that represents a number. This number is know as Avogadro’s number and is: 6.02 x 10 23 particles, students, grains of sand, etc.

8. Slide 8 of 43 © Copyright Pearson Prentice Hall The Mole: A Measurement of Matter > 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. 10.1

9. Slide 9 of 43 © Copyright Pearson Prentice Hall The Mole: A Measurement of Matter > What is a Mole? 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. Representative particles 1 mole 6.02 x 10 23 representative particles moles 10.1

10. Slide 10 of 43 © Copyright Pearson Prentice Hall The Mole: A Measurement of Matter > What is a Mole? 10.1

11. © Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 11 of 43 10.2

12. © Copyright Pearson Prentice Hall Slide 12 of 43 Practice Problems for Sample Problem 10.2 Problem Solving 10.4 Solve Problem 4 with the help of an interactive guided tutorial.

13. Slide 13 of 43 © Copyright Pearson Prentice Hall The Mole: A Measurement of Matter > What is a Mole? Converting Moles to Number of Particles Moles 6.02 x 10 23 representative particles 1 mole representative particles 10.1

14. © Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 14 of 43 10.3 Propane is a gas used for cooking and heating. How many molecules of propane are in 2.12 mol of propane (C 3 H 8 )? How many total atoms are there in 2.12 mol of propane? Converting Moles to Number of Atoms

15. © Copyright Pearson Prentice Hall Slide 15 of 43 Practice Problems for Sample Problem 10.3 Problem Solving 10.5 Solve Problem 5 with the help of an interactive guided tutorial.

16. Slide 16 of 43 © Copyright Pearson Prentice Hall The Mole: A Measurement of Matter > 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 atomic mass or molar mass. The atomic mass or molar mass of an element should always be expressed to 2 decimal places. 10.1

17. Slide 17 of 43 © Copyright Pearson Prentice Hall The Mole: A Measurement of Matter > The Mass of a Mole of an Element One molar mass of carbon, sulfur, mercury, and iron are shown. 10.1 12.01 g/mol 32.07 g/mol 200.59 g/mol 55.85 g/mol

18. © Copyright Pearson Prentice Hall Slide 18 of 43 The Mole: A Measurement of Matter > 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. 10.1

19. Slide 19 of 43 © Copyright Pearson Prentice Hall The Mole: A Measurement of Matter > 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 80.07 g. 10.1 32.07 g/mol +48.00 g/mol = 80.07 g/mol

20. © Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 20 of 43 10.4

21. © Copyright Pearson Prentice Hall Slide 21 of 43 Practice Problems for Sample Problem 10.4 Problem Solving 10.7 Solve Problem 7 with the help of an interactive guided tutorial.

22. © Copyright Pearson Prentice Hall Slide 22 of 43 Section Quiz -or- Continue to: Launch: Assess students’ understanding of the concepts in Section 10.1 Section Quiz. 10.1.

23. © Copyright Pearson Prentice Hall Slide 23 of 43 1. Three common ways of measuring the amount of something are by count, by mass, and a.by temperature. b.by volume. c.by area. d.by density. 10.1 Section Quiz.

24. © Copyright Pearson Prentice Hall Slide 24 of 43 2. A mole of hydrogen gas, H 2 (g), contains 6.02 x 10 23 a.molecules. b.atoms. c.amu. d.grams. 10.1 Section Quiz.

25. © Copyright Pearson Prentice Hall Slide 25 of 43 3. 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. 10.1 Section Quiz.

26. © Copyright Pearson Prentice Hall Slide 26 of 43 4. Calculate the molar mass of ammonium nitrate. a.45.02 g b.80.05 g c.60.06 g d.48.05 g 10.1 Section Quiz.

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