1. Unit 3: Atomic Theory

2. Law of Conservation of Mass Mass is neither created nor destroyed during chemical or physical changes The total mass in the reactants has to be equal to the total mass of the products Atoms are rearranged

3. John Dalton 1808- proposed an explanation for the law of conservation of mass

4. Dalton’s Atomic Theory: (p 66) 1. All matter is composed of extremely small particles called atoms. 2. Atoms of a given element are identical in size, mass and other properties: atoms of different elements differ in size, mass and other properties 3. Atoms cannot be subdivided, created or destroyed

5. Dalton’s Atomic Theory: (con’td) 4. Atoms of different elements combine in simple whole number ratios to form chemical compounds 5. In chemical reactions, atoms are combined, separated and rearranged.

6. Which aspects of Dalton’s theory are incorrect? Atoms are divisible into smaller particles The same element can have different masses ( isotopes) The Modern Atomic Theory maintains Dalton’s points and accounts for the corrections stated above.

7. Law of Definite Proportions a chemical compound contains the same elements in exactly the same proportion by mass regardless of size of the sample Ex. NaCl 39.34% Na and 60.66% Cl ALWAYS! C. Johannesson

8. Law of Multiple Proportions If two or more different compounds are formed of the same two elements, the ratio of the masses of the second element combined with a certain mass of the first is always a ratio of small whole numbers Ex. CO 1.0g C to 1.33 g O CO 2 = 1.0 g C to 2.66 g O Ratio between the 2 oxygens is two! C. Johannesson

9. Law of Multiple proportions continued….. C. Johannesson

10. The Mole SI unit for the amount of substance It’s a counting unit –1 dozen = 12 units –1 pair = 2 unit –1 gross = 144 units –1 MOLE = Avogadro’s # = 6.02 x 10 23 Why do we need such a huge number in chemistry?

11. The Mole in perspective If you have a mole of pennies, and distribute them equally among every person on Earth, how much $$ would everyone get?

12. The Mole in perspective If you have a mole of pennies, and distribute them equally among every person on Earth, how much $$ would everyone get?

13. The Mole in perspective 1. One mole of paper would make a stack that would reach to the moon more than 80 billion times 2. One mole of grains of sand would be more than all of the sand on Miami Beach 3. One mole of blood cells would be more than the total number of blood cells found in every human on earth

14. 4. A one liter bottle of water contains 55.5 moles of water 5. One mole of seconds is about 19 quadrillion years, 4,240,666 times the age of the earth, or 954,150 times the age of the universe itself 6. One mole of cents could repay the United States National Debt 86 million times

15. Avogadro’s Number: Italian scientist, Amadeo Avogadro Number of particles in a mole is known as Avogadro’s number = 6.02 X10 23

16. Molar Mass: The mass of one mole of pure substance Ex. Lithium = 6.94 g/mol

17. Molar conversions:

18. Calculate the molar mass of: Cu NaCl Ca 2 SO 4 Al(NO 3 ) 3 C. Johannesson

19. Moles & Mass For Calculations - Use Dimensional Analysis – Set up What is the mass of 3.0 mols of NaCl? How many mols are in 30.0 g of H 2 O? C. Johannesson

20. Moles & Particles How many atoms are in 3.0 mols of H 2 O? How many moles of Aluminum, are in 4.02 x 10 23 atoms of Al? C. Johannesson

21. Moles & Particles & Mass Calculate the mass of 3.7 x 10 24 molecules of MgCl 2. How many atoms are in 100.0g of Silver? C. Johannesson

22. Do Now How many particles are in 200g of Gold? C. Johannesson

23. Molarity (M) Number of moles of solute in one liter of solution Molarity = (moles of solute/ L of solvent) C. Johannesson

24. Percent Composition Percent by mass of each element in a compound. % composition of any pure substance is always constant, whatever the source or sample size. Useful in identifying the characteristic of any substance. Used by investigators from many fields, Analytical chemistry, forensics etc. to determine the identity of unknown materials.

25. Sample Problems Calculate the percentage composition of each element in NaNO 3. C. Johannesson

26. Answer 27.05%Na, 16.48% N, 56.47% O C. Johannesson

27. Sample Problem 2 Calculate the percentage composition of Oxygen in Ag 2 SO 4. C. Johannesson

28. Answer 69.19% Ag, 10.28% S, 20.52% O C. Johannesson

29. Water in a hydrate What is the mass percentage of water in the hydrate CuSO 4 ●5H 2 O? 36.08% C. Johannesson

30. Determining Chemical Formulas Empirical formulas – consists of the symbols for the elements combined in a compound, with subscripts showing the smallest whole-number ratio of the different atoms in the compound. Molecular Formulas – a multiple of the empirical formula. C. Johannesson

31. Guidelines Determine the mass of each element Convert into moles Divide by the smallest mole or the elements present Determine the ratio Write the formula (Usually elements are listed from left to right on the PTOE) C. Johannesson

32. Sample Problems A compound is analyzed and found to contain 36.70% K, 33.27% Cl, and 30.03% O. What is the empirical formula of the compound? A 60.00 g sample of tetramethyllead, a gasoline additive, is found to contain 38.43 g of lead, 17.83 of carbon, and hydrogen. Find its empirical formula. C. Johannesson