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Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.. Chapter 10 Chemical Quantities 10.1 The Mole: A Measurement of Matter 10.2.

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Presentation on theme: "Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.. Chapter 10 Chemical Quantities 10.1 The Mole: A Measurement of Matter 10.2."— Presentation transcript:

1 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.. 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

2 The Mole Concept Avogadro’s Number = 6.022 x 10 23

3  How can you quantify the amount of sand in a sand sculpture? Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.. CHEMISTRY & YOU You could measure the amount of sand in a sculpture by counting the grains of sand. Is there an easier way to measure the amount of sand?

4  There are terms used to equate a certain quantity of matter o For example 1 dozen = 12, 1 Ton = 2,000 LBs and 1 gross = 144.  Before we get to the chemical terms lets convert between units we already know

5  For example – let’s say you want to buy some Bazooka Gum o You could buy it by the piece from the deli o You could buy it by the box from ShopRite o You could buy it by mass from the candy store

6  So, the different ways to measure Bazooka gum o 1 dozen = 12 pieces o 1 dozen = 1.75 boxes o 1 dozen = 168 grams

7  Based on those conversions, I can determine how much Bazooka gum I have, regardless of how it is measured.  I have 95 pieces of Bazooka gum, how many grams do I have?

8  I have 95 pieces of Bazooka gum, how many grams to I have?

9  If I have 2 stadiums how many baseball bats do I want to purchase? 2 baseball players = 4 baseball bats 1 stadium = 18 baseball players 18 baseball players = 52 corn dogs

10  What Is a Mole? ◦ How do chemists count the number of atoms, molecules, or formula units in a substance? Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved..

11 These particles are much, much smaller than grains of sand, and an extremely large number of them are in a small sample of a substance. Obviously, counting particles one by one is not practical. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.. Recall that matter is composed of atoms, molecules, and ions.

12  In chemistry, there are many way to measure the amount of substance o The count (quantity) o The volume (how much space it takes up) o The mass (the amount of matter)  Knowing how the count, mass, and volume of an item relate to a common unit allows you to convert among these units.

13  In chemistry, we do not use a dozen. o Since atoms are so small, we need a quantity with a larger amount  We use the mole (mol) o 1 mole = 6.022 X 10 23 representative particles (atoms, molecules, formula units) o It is known as Avogadro’s number

14  An Italian chemist whose important contributions was his resolution of the confusion surrounding atoms and molecules. Avogadro believed that particles could be composed of molecules and that molecules could be composed of still simpler units, atoms. The number of molecules in a mole (one gram molecular weight) was termed Avogadro's number

15  We usually are dealing with three types of representative particles o Molecules  H 2 O and H 2 are molecules, covalently bonded o Atoms  Al and Na are atoms, not bonded o Formula units  CaCl 2 and NaOH are formula units, ionicly bonded

16  1 mole of any representative particle is always 6.02 X 10 23  Using this value we can convert between moles and atoms/ molecules/ formula units

17  For example: If a sample contains 0.476 mol of O 2, how many representative particles are present?

18  For example: If a sample contains 5.2 X 10 21 atoms of aluminum, how many moles are present?

19  Magnesium is a light metal used in the manufacture of aircraft, automobile wheels, and tools. How many moles of magnesium is 1.25 × 10 23 atoms of magnesium? Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.. Sample Problem 10.2 Converting Number of Atoms to Moles

20  We can determine the molar mass of representative particles o Molar mass is the mass of 1 mole of that substance  The atomic mass is equal to the molar mass for an element o 1 mol Na = 22.99 g Na

21  For molecules and formula units, we must calculate the molar mass  Let’s calculate the molar mass of SO 3 S = 1 X 32.07 = 32.07 O = 3 X 16.00 = 48.00 = 80.07 g/mol

22  We can use the molar mass of a substance to convert from moles to mass o Remember the molar mass is the mass of 1 mole of that substance o SO 3 = 80.07 g/mol = 80.07 g SO 3 1 mol SO 3

23  Using this relationship, we can easily convert a mole amount to a mass amount  How many grams is there in a 0.750 mole sample of SO 3 ?

24  We can also convert a mass amount to a mole amount  How many moles is there in a 28.5 gram sample of SO 3 ?

25 ◦ The mole allows chemists to count the number of representative particles in a substance. ◦ The atomic mass of an element expressed in grams is the mass of a mole of the element. ◦ 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. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved..


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