1. NOTEBOOK SET UP FIRST PAGE IS A TABLE OF CONTENTS NUMBER THE PAGES AS YOU GO. In the beginning if you have pages you need to glue/tape/staple in, write “STAPLED” under the page number, EVERY MONDAY, SET ASIDE 2 PAGES, BACK AND FRONT, FOR THE WEEKLY BELL WORKS. EVERY TIME WE DO NOTES, WRITE THE TITLE OF THE NOTES IN THE BEGINNING OF THE SECTION, WRITE A PAGE NUMBER, AND WHATEVER NOTES WE ARE DOING. DATEBELL WORK/NOTES TITLEPAGE NUMBER 02/08/2016BELL WORKS- WEEK 2PAGE 2 02/08/2016MOLE RATIOS NOTESPAGE 4

2. NOTEBOOK RUBRIC

3. THE MOLE A MEASUREMENT OF MATTER

4. THINK ABOUT THIS… IS IT PRACTICAL TO COUNT EACH GRAIN OF SAND? HOW ELSE MIGHT YOU MEASURE, OR QUANTIFY, THE SAND?

5. MEASURING MATTER  How might you measure some forms of matter?  Pepsi?  Potatoes?  Songs on Your Playlist?

6. MEASURING MATTER  How might you measure some forms of matter? Typically there are three methods for measuring matter: 1.Count 2.Mass 3.Volume

7. MEASURING MATTER  There are some common units for measuring items using a specific number:  A Pair  A Dozen  A Ream = 2 = 12 = 500

8. MEASURING MATTER  Skittles© can be measured in three different ways. 1.Count – 50 Skittles in a bag 2.Mass – 1 Skittle is 1 gram 3.Volume – 2.17 Ounces in a bag

9. MEASURING MATTER  Each of the different ways to measure Skittles© can be equated to a dozen skittles. 1.Count: 1 dozen = 2.Mass: 1 dozen =  1 Skittle© is 1 gram  12 Skittles© are 12 x 1 Gram = 12 Grams 12 Skittles 12 Grams

10. THE MOLE  Imagine trying to count individual grains of sand.  Units like a dozen or a pair would not be helpful.

11. THE MOLE RECALL Matter is anything that has mass and takes ups space; it is composed of atoms, molecules and ions.

12. THE MOLE  Particles, like atoms and molecules, are even smaller than grains of sand.  A large number of particles exist in even the smallest amounts of samples.

13. THE MOLE  Chemists use a unit that is a specified number of particles.  This unit is called a mole.  Just like a dozen means 12 things, a mole represents 6.02 x 10 23 things.

14. THE MOLE  A mole is a new S.I. Unit to measure the amount of a substance.  The number of things it represents, 6.02 x 10 23, is known as Avogadro’s Number.  A mole of any substance contains Avogadro’s number of particles, or 6.02 x 10 23 particles.

15. THE MOLE Let’s Make Sure We Get This: 1.1 mole of pens = ________________ pens 2.1 mole of paper = _________________paper 3.1 mole of Skittles© = _______________Skittles©

16. THE MOLE Let’s Make Sure We Get This: 1.1 mole of pens = 6.02 x 10 23 pens 2.1 mole of paper = 6.02 x 10 23 paper 3.1 mole of Skittles© = 6.02 x 10 23 Skittles©

17. THE MOLE

19.  We can also interchange between the number of atoms and the number of moles given each.  Remember —1 mole of atoms = 6.02 x 10 23 atoms.  What if we had 2 moles of atoms?  2 x (6.02 x 10 23 atoms) = 1.20 x 10 24 atoms

20. THE MOLE  What if we had 3.01 x 10 23 of atoms …how many moles ?  Use the analogy of the dozen.  What if we had 24 eggs …how many dozen ?  1 Dozen = 12 eggs  24 eggs/ 12 eggs = 2 Dozen

21. THE MOLE  What if we had 3.01 x 10 23 of atoms …how many moles ?  1 mole = 6.02 x 10 23 atoms  3.01 x 10 23 atoms / 6.02 x 10 23 atoms = 0.5 moles [NOT GOING TO STRESS THIS TOO MUCH NOW]

22. THE MASS OF A MOLE OF AN ELEMENT  When we used to calculate the mass of an element, we counted the protons and neutrons.  The unit for this mass was the atomic mass unit or amu. Example: Mass of Carbon is 12 amu. Mass of Hydrogen is 1.01 amu

23. THE MASS OF A MOLE OF AN ELEMENT  Chemists have converted the unit of amu to the convenient metric unit of gram.  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 known as the MOLAR MASS. (Unit for molar mass is g/mol)

24. THE MASS OF A MOLE OF AN ELEMENT  Using the Periodic Table now, we can define the masses given as the MOLAR MASSES. Example: Carbon is 12.00 g Hydrogen is 1.01 g

25. THE MASS OF A MOLE OF AN ELEMENT PRACTICE Use the Periodic Table to determine the Molar Masses (in g/mol) of each element. 1.Magnesium _________________ 2.Fluorine _______________ 3.Osmium __________________

26. THE MASS OF A MOLE OF AN ELEMENT PRACTICE Use the Periodic Table to determine the Molar Masses (in g/mol) of each element. 1.Magnesium 24.305 g/mol 2.Fluorine 18.998 g/mol 3.Osmium 190.23 g/mol

27. THE MASS OF A MOLE OF AN ELEMENT RECALL The mass of 1 mole of an element is known as the molar mass. We can use the Periodic Table to determine these masses. 1 mole of Nitrogen is 1 mole of Potassium is

28. THE MASS OF A MOLE OF AN ELEMENT RECALL The mass of 1 mole of an element is known as the molar mass. We can use the Periodic Table to determine these masses. 1 mole of Nitrogen is 14.00674 grams. 1 mole of Potassium is

29. THE MASS OF A MOLE OF AN ELEMENT RECALL The mass of 1 mole of an element is known as the molar mass. We can use the Periodic Table to determine these masses. 1 mole of Nitrogen is 14.00674 grams. Molar Mass = 14.00674 g/mol 1 mole of Potassium is

30. THE MASS OF A MOLE OF AN ELEMENT RECALL The mass of 1 mole of an element is known as the molar mass. We can use the Periodic Table to determine these masses. 1 mole of Nitrogen is 14.00674 grams. Molar Mass = 14.00674 g/mol 1 mole of Potassium is 39.0983 g

31. THE MASS OF A MOLE OF AN ELEMENT RECALL The mass of 1 mole of an element is known as the molar mass. We can use the Periodic Table to determine these masses. 1 mole of Nitrogen is 14.00674 grams. Molar Mass = 14.00674 g/mol 1 mole of Potassium is 39.0983 g Molar Mass = 39.0983 g/mol

32. THE MASS OF A MOLE OF A COMPOUND We can also use the molar masses of the elements to determine the molar masses of compounds. The mass of a mole of a compound is the molar mass (g/mol) of the compound.

33. THE MASS OF A MOLE OF A COMPOUND RECALL-COUNTING ATOMS IN FORMULA SO 3  MOLAR MASS OF SULFUR _________________  MOLAR MASS OF OXYGEN _________________ 1 S atom3 O atoms

34. THE MASS OF A MOLE OF A COMPOUND RECALL-COUNTING ATOMS IN FORMULA SO 3  MOLAR MASS OF SULFUR 32.065 g/mol  MOLAR MASS OF OXYGEN 15.9994 g/mol 1 S atom3 O atoms

35. THE MASS OF A MOLE OF A COMPOUND To calculate the molar mass of a compound,: 1.Determine the number of each atom in the formula (this corresponds to 1 mole of compound) 2.Find the molar mass of each element in the compound 3.Add the molar masses of the elements in the compound.

36. THE MASS OF A MOLE OF A COMPOUND RECALL-COUNTING ATOMS IN FORMULA SO 3  MOLAR MASS OF SULFUR 32.065 g/mol  MOLAR MASS OF OXYGEN 15.9994 g/mol  MOLAR MASS OF SO 3 ( 1 S x 32.065 g/mol ) + ( 3 O x 15.9994 g/mol) = 80.06 g/mol 1 S atom 3 O atoms