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10.1 The Mole: A Measurement of Matter > Chapter 10 Chemical Quantities 10.1 The Mole: A Measurement of Matter 10.2 Mole-Mass and Mole-Volume Relationships 10.3 Percent Composition and Chemical Formulas 1 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. . 10.1 The Mole: A Measurement of Matter > What Is a Mole? Do Now Get an Activity sheet , go to the lab tables and get into your lab groups. Read the instructions on the sheet and be ready to begin the activities. 2 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. . What Is a Mole? 10.1 The Mole: A Measure> ment of Matter What ways can you quantify how much you have of something? 3 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. . 10.1 The Mole: A Measurement of Matter > What Is a Mole? Atomic Mass (AMU) • • • • The mass of a single atom We cannot measure something this small We use Molar Mass instead. Example: The atomic mass of lead is 207.2 amu. • If we weigh out 207.2 grams of lead we have the molar mass of lead. 4 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. . 10.1 The Mole: A Measurement of Matter > What Is a Mole? • The ‘mole’ is a unit of measurement used to count the number of particles found within a substance. • This is similar to using • • • • 5 Dozen (12) Pair (2) Ream (500) Gross (144) Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. . 10.1 The Mole: A Measurement of Matter 1 mole > What Is a Mole? = 6.02 × 1023 of ANYTHING 6.02 × 1023 is called Avogadro’s number in honor of the person who started working with it. http://ed.ted.com/lessons/daniel-dulek-how-big-is-a-mole-not-the-animal-the-other-one 6 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. . 10.1 The Mole: A Measurement of Matter > What Is a Mole? representative particle - species present in a substance, usually atoms, molecules, or formula units. Element Molecular Compound Ionic Compound 7 Representative particle Example Atom Copper Molecule H2O Formula Unit NaCl Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. . 10.1 The Mole: A Measurement of Matter > Interpret Data Representative Particles and Moles 8 Substance Representative particle Chemical formula Representative particles in 1.00 mol Copper Atom Cu 6.02 × 1023 Atomic nitrogen Atom N 6.02 × 1023 Nitrogen gas Molecule N2 6.02 × 1023 Water Molecule H2O 6.02 × 1023 Calcium ion Ion Ca2+ 6.02 × 1023 Calcium fluoride Formula unit CaF2 6.02 × 1023 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. . 10.1 The Mole: A Measurement of Matter > What Is a Mole? The mole can be used as a conversion factor 1 mole = 6.02 × 1023 representative particles 1 mole 6.02 × 1023 of something 9 6.02 × 1023 of something 1 mole Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. . 10.1 The Mole: A Measurement of Matter > Sample Problem 10.3 Converting Moles to Number of Molecules How many molecules are in 6.3 moles of methane (CH4)? 10 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. . 10.1 The Mole: A Measurement of Matter > Sample Problem 10.3 Converting Moles to Number of Molecules How many molecules are in 6.3 moles of methane (CH4)? 3.79 x 1024 molecules of CH4 11 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. . 10.1 The Mole: A Measurement of Matter > Sample Problem 10.3 Converting Moles to Atoms How many atoms are in 6.3 moles of methane (CH4)? 12 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. . 10.1 The Mole: A Measurement of Matter > Sample Problem 10.3 Converting Moles to Atoms How many atoms are in 6.3 moles of methane (CH4)? 1.89 x 1025 atoms 13 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. . 10.1 The Mole: A Measurement of Matter > Molar Mass Molar Mass • Mass of a mole of an element • For elements, this is the atomic mass given in the periodic table, expressed in grams. • Also called molecular weight or molecular mass(in case of molecules which is the sum of atomic masses of all the atoms they are composed of) Element Carbon Hydrogen Chlorine 14 Molar Mass 12.0 g 1.0 g 35.5 g Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. . 10.1 The Mole: A Measurement of Matter > Molar Mass The Mass of a Mole of an Element 1 mol of sulfur atoms = 32.1 g 1 mol of carbon atoms = 12.0 g 1 mol of iron atoms = 56.0 g This figure shows one mole of carbon, sulfur, and iron. 15 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. . 10.1 The Mole: A Measurement of Matter > Molar Mass The mass of a mole of a compound is the sum of the masses of all the atoms in the compound. Example Molar mass SO3 = molar mass S + molar mass O3 = 32.1g + 16.0g x 3 = 80.1 g 16 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. . 10.1 The Mole: A Measurement of Matter > Sample Problem 10.4 Finding the Molar Mass of a Compound Calculate the molar mass of the following compounds. a)NaCl b)N2O3 c)Fe(OH)2 d)Be3(PO4)2 17 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. . 10.1 The Mole: A Measurement of Matter > Sample Problem 10.4 Finding the Molar Mass of a Compound Calculate the molar mass of the following compounds. a)NaCl – 58.5g b)N2O3 – 76.0 g c)Fe(OH)2 – 89.8 g d)Be3(PO4)2 – 217 g 18 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. . 10.1 The Mole: A Measurement of Matter > END OF 10.1 19 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. .