1. Chapter 6 The mole

2. Measuring Matter What do you ask for when you buy: 2 shoes 12 eggs 48 doughnuts 500 sheets of paper 1 pair 1 dozen 4 dozen 1 ream

3. Pair, Dozen, Ream These are all ways to batch a group of objects to make them easier to count! The object may change Eggs to Doughnuts But the number they represent is always constant!

4. What do eggs have to do with Chemistry? How many carbon atoms are in a teaspoon of carbon? 200,666,666,666,666,666,666,667 atoms!!! Can you even pronounce this?

5. 200,666,666,666,666,666,666,667 atoms!!! It would be nice if chemists had a batch like a dozen (but muchhhhhhh bigger) to handle this kind of number!

6. Meet the Mole! He is the Chemist’s “dozen”!

7. The chemist’s “dozen” is called the: MOLE (or the unit mol) 1 dozen atoms = 12 atoms 1 mole atoms = 602213670000000000000000 atoms How many moles are in 1 teaspoon of carbon atoms?.33 moles Or 1 mole = 6.02  10 23 What is a mole?

8. Measuring Matter – Moles and Avogadro’s number Mole (mol) – the amount of a substance that contains the same number of particles as the number of atoms in 12 g of carbon-12. Like doughnuts are counted in dozens, the mole is a SI unit for counting the amount of a substance. –1 dozen pencils have the same number of units as 1 dozen doughnuts –1 mole of carbon atoms have the same number of particles as 1 mole of water molecules This does not mean they both weigh the same, only that they have the same number of units or particles.

9. Measuring Matter – Moles and Avogadro’s number Avogadro’s Number – the number of particles (6.02  10 23 ) in exactly one mole of a pure substance. –1 mole pencils = 6.02  10 23 pencils –1 mole water molecules = 6.02  10 23 molecules of water

10. Measuring Matter – Moles and Avogadro’s number If Avogadro’s number is the number of particles in 1 mole, how do you know what kind of particle you have? Remember… Particles can be an atom, molecule, or formula unit?

11. What kind of particle? Particles can be an atom, molecule, or formula unit? Atom – one atom Molecule – more than one nonmetal atom Formula unit - compound with a metal or NH 4 +

12. Measuring Matter – Moles and Avogadro’s number How do you know what kind of particle you have? Examples 1.NaCl 2.H 2 O 3.H 2 4.Na Formula unit molecule atom

13. Measuring Matter – Moles and Avogadro’s number Avogadro’s number is really an equality! 1 mole C = 6.02  10 23 atoms C What can you use equalities to do? Equalities are conversion factors in Dimensional Analysis problems!

14. Measuring Matter – Moles and Avogadro’s number How many atoms are in 3.2 mol of C? = atoms C mol C atoms C 1 6.02  10 23 1.9  10 24

15. Measuring Matter – Moles and Avogadro’s number How many moles of water molecules are in 3.7  10 21 molecules of H 2 O? = mol H 2 O mol H 2 O Molecules H 2 O 1 6.02  10 23.0061 3.7  10 21 molecules H 2 O

16. Mass and the Mole Molar mass – the mass, in grams, of one mole of a substance. How do you find this mass? The atomic mass printed on the periodic table has two meanings – it is the average mass of an atom in atomic mass units (u) and the mass of one mole of atoms of a given element in grams.

17. Mass and the Mole Finding molar mass –Atoms – the mass of 1 mole of any atom is the same as the atomic mass in grams. 1mole H atoms = 1.00794 g 1mole C = 12.0107 g 1mol Cu = 63.546 g

18. Mass and the Mole Molar mass continued –Compounds – the mass of 1 mole of a compound is the sum of the masses of the atoms. 1mole H 2 O = 2 H = 1 O = 2(1.00794g) = 2.01588g 15.9994g 2.01588g + 15.9994g = 18.0153g 18.0153g

19. Practice!! Find the molar mass of the following! CCl 4 CaO (NH 4 ) 2 SO 4

20. Mass and the Mole Molar mass is really an equality! For water: 1mole H 2 O = 18.0153 g What can you use equalities to do? Equalities are conversion factors in Dimensional Analysis problems!

21. Mass and the Mole How many moles are in 242 g of water? mol H 2 O g H 2 O 1 18.0153 13.4 242 g H 2 O = mol H 2 O

22. Mass and the Mole What is the mass of 3.77 mol of Au? g Au mol Au 196.96655 1 743 3.77 mol Au = g Au

23. Multi Step Problems What is the mass of 5.28 x 10 28 molecules of water? = 6.02x10 23 5.28x10 28 molecules g molecules mole1 g 1 18.0153 1.58x10 6

24. The Last Conversion Factor! What do you do if you are asked to find atoms and your representative particle is NOT an atom?

25. The Formula Conversion Factor Think about what a formula really tells you! 1 molecule of H 2 O Doesn’t this mean: 1 molecule H 2 O = 2 hydrogen atoms And …. In 1 mole of H 2 O there are 2 moles of Hydrogen The formula is a conversion factor between atoms and compounds!

26. The Formula Conversion Factor How many hydrogen atoms are in 234 molecule of water? atoms H molecules H 2 O 2 1 234 molecules H 2 O = atoms H 468

27. How many Hydrogen atoms are in 54.2g of H 2 O? = 1 18.0153 atoms 54.2 g g mol mol of H 2 O Atoms 1 6.02x10 23 mol of O2 1 3.62x10 24

28. Conversion Review Moles Mass Particles Molar mass Avogadro’s # Atoms Formula

29. Percent Composition How would you calculate the percent females in this room? All percents are calculated in the same way!

30. Percent Composition Percent Composition – the percent by mass of each element in a compound. molar mass

31. What is the percent composition of each element in water? Mass H = Mass O = 15.9994 g Percent Composition 2(1.0079 g) = 2.01588 g + 18.0153 g % H = 11.1898% O = 88.8101%

32. Using Percent Composition If a glass of water contains 648 g of water, how many grams of hydrogen would it hold? Remember, water is 11.1898% hydrogen What is 11.1898% of 648 g? 72.5099 g 72.5 g

33. C 3 H 8 O Isopropyl Alcohol

34. Find the % composition of the elements in rubbing alcohol Molar Mass = C? H? O? 59.9586% 13.4180% 26.6235% 60.0950g

35. Empirical Formula What does H 2 O mean? Does it mean 2 atoms of H for every atom of O? YES Does it mean 2 g of H for every 1 g of O? NEVER

36. Empirical Formula What does H 2 O mean? Does it mean 2 moles of H for every mole of O? Always! Formulas are not only ratios of atoms, they are also ratios of MOLES

37. Formulas are ratios of moles!

38. Empirical Formula Empirical Formula: simplest whole number ratio of moles of the atoms in a substance. Experimental method that is the first step in finding the formula of a compound. Circle the empirical formulas! H 2 SO 4 H2OH2O N2O4N2O4 C2H6C2H6 NO 2 C 6 H 12 O 6 NaCl

39. Empirical Formula Finding the empirical formula 1.Find the mass of each element in the compound. –Usually given –If given as %, then change % to g. 25% H and 75% C  25 g H and 75 g C 2.Convert masses to moles. –Use molar masses. 25 g H = mol H g H mol H1 1.00794 25

40. Empirical Formula 3.Find the smallest whole number ratio of moles. a. Write the results of step 2 like a formula. If C = 6.2 mol and H = 25 mol C 6.2 H 25 b. Divide by the smallest mole amount. C 6.2 H 25 c. If not all whole numbers, multiply by 2,3, or 4 … 6.2 CH 4

41. Empirical Formula Examples for step 3 X =.029 molX =.009 mol Y =.039 molY =.006 mol X.029 Y.039.029 X 1 Y 1.34 Multiply by 3 X3Y4X3Y4 X.009 Y.006.006.006 X 1.5 Y 1 Multiply by 2 X3Y2X3Y2

42. Empirical Formula More Examples for step 3 X = 1.47 molX = 2.4  10 -4 mol Y = 3.68 molY = 7.3  10 -4 mol X 1.47 Y 3.68 1.47 X 1 Y 2.5 Multiply by 2 X2Y5X2Y5 2.4  10 -4 X 1 Y 3.04 X1Y3X1Y3

43. Empirical Formula - Example A sample of an unknown gas contains 43.2 g of carbon and 115.8 g of oxygen. What is the empirical formula? 1.Find Masses 43.2 g C115.8 g O 2.Change to moles 43.2 g C = mol C g C mol C1 12.0 3.60 115.8 g O = mol O g O mol O1 16.0 7.24

44. Empirical Formula - Example 3.Get whole numbers C 3.60 O 7.24 3.60 C 1 O 2.01 CO 2

45. Empirical Formula Find the empirical Formula of 52.8% Sn, 12.4% Fe, 16.0%C, & 18.8% N.

46. Molecular Formula Molecular formula - is some whole number multiple of the empirical formula. –HO is an empirical formula –H 2 O 2 is twice HO –(HO) X and X = 2 –For C 6 H 12 O 6, the empirical formula is CH 2 O and X=6 To convert an empirical formula to a molecular formula you must find X.

47. Molecular Formula - Example An unknown gas is found to have an empirical formula of NO 2 and a molar mass of 92.0 g/mol. What is the molecular formula? Molecular formula = (NO 2 ) X = (NO 2 ) 2 = N 2 O 4