1. Chapter 6 Mathematics & Chemical Formulas Unit 7 – The Mole

2. Atoms are too small/light Atoms are too small and too light to count or mass as individuals – One Carbon-12 atom = 1.99 x 10 -23 grams We use this as the basis for atomic mass units 1 Carbon atom is 12 amu. – 6 protons + 6 neutrons = 12 things that make up the mass of a carbon atom

3. Atomic Mass & Molecular Mass Atomic mass - the mass of 1 mole of atoms (also known as molar mass) Molecular Mass – the masses of all of the atoms in a chemical compound. – Ex: CH 4 – Ex: CaCl 2

4. Molecular Mass – Example So, the formula weight of calcium chloride, CaCl 2, would be Ca: 1(40.1 amu) + Cl: 2(35.5 amu) 111.1 amu To convert to molar mass, change amus to g/mol. 1 amu = 1 g/mol

5. Molecular Mass – Example For the molecule methane, CH 4, the molecular weight would be C: 1(12.0 amu) 16.0 amu + H: 4(1.0 amu) The molar mass of methane would be 16.0 g/mol

6. 1 mole - different physical states Moles provide a bridge from the molecular scale to the real-world scale.

7. Examples of Molar Mass List the molar masses of the following: – Zn – CuSO 4 – NaCl – H 2 O – Al 2 (SO 4 ) 3

8. The Mole – a word that means a # Other words that mean #s: One dozen = 12 One gross = 144 One score = 20 One ream = 500 One MOLE = 6.02 x 10 23 602000000000000000000000

9. Avogadros Number Avogadros Number - 6.02 x 10 23 particles in 1 mole 1 mole of 12 C has a mass of 12 g.

10. Mole Conversions Moles tell you how many atoms you have, AND how much mass in grams you have. We use moles to convert from atoms and grams.

11. Mole Conversion Factors There are 4 possible conversion factors for mole conversions: – Show your work -use a conversion factor every time

12. Using your calculator To Enter 6.02 x 10 23 into your calculator, use the EE button, so it would appear as 6.02E23. Practice with the two following examples

13. Examples: If you have 4.25 x 10 22 atoms of Al, how many moles do you have? If you have 0.37 moles of Al, how many atoms do you have?

14. Mole Diagram

15. Mole Examples If you have 8.64g of Mg, how many moles do you have? If you have 1.23 moles of Phosphorous, how many grams do you have?

16. Mole Relationships One mole of: – atoms – ions – molecules contains Avogadros number of those particles. One mole of: – molecules or formula units contains Avogadros number times the number of atoms or ions of each element in the compound.

18. Formula mass and % composition Percent Composition = All of the parts should add up to 100% !! Example: What is the mass percent of each element in carvone (C 10 H 14 O) ?

19. C 10 H 14 O 1. To find % composition you must 1 st find the mass of the whole thing! 2. Then find the mass of each part (you kind of already did that) and divide it by the mass of the whole thing x 100 to find % mass of each part.

20. Empirical and Molecular Formulas Unit 7 - 2009

21. Empirical and Molecular Formulas An empirical formula shows the simplest whole number ratio of atoms of each element in a compound A molecular formula shows the actual number of atoms of each element in a compound

22. Example: Glucose Glucose has a molecular formula of: – C 6 H 12 O 6 It has an empirical formula of: – CH 2 O

23. Formulas contd A molecular formula is always a multiple of empirical formula A compound has ONE molecular formula Many compounds have the same empirical formula

24. Example 0.18 grams of magnesium react with 0.12 grams of oxygen to form magnesium oxide Convert all grams to moles Divide all numbers of moles by the smallest # present (do a ratio!) Multiply all numbers by the smallest # that will make them WHOLE NUMBERS

25. Example An oxide of aluminum is formed with 4.151 g of Aluminum and 3.692 g of Oxygen. Calculate the empirical formula of the compound: 1. Convert all grams to moles 2. Divide all numbers of moles by the smallest # present (do a ratio!) 3. Multiply all numbers by the smallest # that will make them WHOLE NUMBERS

26. Find molecular formulas from empirical formulas A white powder is analyzed and found to have an empirical formula of P 2 O 5. It has a molar mass of 283.88 g/mol. What is the molecular formula for this compound?

27. Hydrated compounds Sometimes, compounds contain water molecules within their crystal structure If a compound contains water molecules, we write it like this: MgSO 4 7H 2 O

28. Hydrates MgSO 4 7H 2 O The little dot between the MgSO 4 and the H 2 O is NOT a multiplication symbol – the H 2 O is just attached How many atoms of each element are in the compound above? How about in Na 3 PO 4 6H 2 O?

29. Lab 9: Percent Comp of a Hydrate If you know the mass of hydrate (what you start with) and you know the mass after you cook it, what have you lost? That is the mass of the H 2 O you lost If you know mass H 2 O and you know mass whole thing….you can calculate % of H 2 O in the compound!!