1. Chemical Composition

2. 8.1 Counting by Weighing Which method is more effective? Counting jelly beans vs. weighing jelly bean total mass Average mass = ------------------ number of samples

3. 8.2 Atomic Mass: Counting Atoms by Weighing Atomic mass unit (amu): unit of mass for an atom 1 amu = 1.66 x 10 -24 g

4. Example Calculate the mass in amu of a sample of aluminum contains 75 atoms Carbon contains 62 atoms Calculate the number of sodium atoms present in a sample that has 1172.49 amu Copper atoms present in a sample that has a mass of 1779.4 amu

5. 8.3 The Mole SI unit for an amount of substance Countable units Can be obtained from a balanced equation E.gC(s) + O 2 (g)  CO 2 (g) 1 atom of C reacts with 1 molecule O 2 to yield 1 molecule of CO 2 OR 1 mol of C reacts with 1 mole O 2 to yield 1 mole CO 2

6. 8.3 The Mole Described the number of objects present in a dozen Based on C-12 1 mol of anything = 6.02 x 10 23 units of that substance (atoms, molecules, particles, dollars etc..) Avogadro’s number 1 mol of an atom = atomic weight of an atom in grams Use as a conversion factor E.g Atomic weight of Na = 22.99 amu 1 mol Na = 22.99 g Na

7. Steps in determination the mole Determine the final unit Determine the atomic mass of an atom Write out an equivalence Express equivalence as a conversion factor

8. Example Calculate the number moles of atoms and the number of atoms in 2.50 g sample of calcium 57.7 g sample of sulfur

9. 8.4 Molar Mass Like density, it’s a ratio of two numbers. Mass per one mole of substance Unit => g/mol E.g if 0.400 mol of a compound has a mass of 17.6 g, what is the molar mass of the compound? Replaced with molecular weight because molar mass described the concept more accurately Formula weight is used for ionic compound

10. Example What is the molar mass of CH 4 ? Calculate molar mass of sulfur dioxide, a gas produced when sulfur containing fuels are burned. Calculate the molar mass for each of the substance below (record to two decimal places) Water Ammonia Barium hydroxide

11. Calculating the Mass from Moles Recall Molar mass is the mass per one mole of a substance 1 mol of substance = # g Use as a conversion factor E.gif the molar mass of NaCl = 58.44 g/mol

12. Example Calcium carbonate (also called as calcite), is the principal mineral found in limestone, marble, chalk, pearls and the shells of marine animals such as clams Calculate the molar mass of calcium carbonate A certain sample of calcium carbonate contains 4.86 mol. What is the mass in grams of this sample?

13. Example Calculate the mass of 4.85 mol of acetic acid, HC 2 H 3 O 2. Vinegar is a dilute solution of acetic acid Calculate the molar mass of sodium sulfate. A sample of sodium sulfate with a mass of 300.0 g represents what number mole of sodium sulfate? How many water molecules are in a 10.0g sample of water?

14. 8.5 Percent Composition Percent composition – the mass present of each element present in a compound % composition = To calculate the percent composition (percentage composition) of a compound Calculate the molar mass of the compound Calculate the total mass of each element present in the formula of the compound Calculate the percent composition (percentage composition): % by weight (mass) of element = (total mass of element present ÷ molecular mass) x 100

15. Example Carvone is a substance that occurs in two forms, both of which have the same molecular formula (C 10 H 14 O) and molar mass. One type of carvone gives caraway seeds their characteristic smell; the other is responsible for the smell of spearmint oil. Calculate the mass of percent of each element in carvone. Determine the mass percent of each element in sulfuric acid.

16. 8.6 Formula of Compounds Formula of a compound represents the relative numbers of various types of atoms present. E.g CO 2, H 2 O etc.. Empirical formula: simplest formula Molecular formula: the actual formula of a compound

17. 8.7 Calculation of Empirical Formula In each case below, the molecular formula for a compound is given. Determine the empirical formula for each compound C 6 H 6. This is the molecular for benzene; a liquid commonly used in industry as a starting material for many important products H 2 O 2. This is hydrogen peroxide, a substance commonly diluted with water and used as a disinfectant CCl 4. This is carbon tetrachloride, an organic solvent

18. 8.7 Calculation of Empirical Formula Step 1: Obtain the mass of each element present (in grams) Step 2: Determine the number of moles of each type of atom present Step 3: Divide the number of mole of each element by the smallest number of moles to convert the smallest number to 1. If all of the numbers so obtained are integers, these are the subscripts in the empirical formula. If one or more of these number are not integers, go on to step 4 Step 4: Multiply the numbers you derived in step 3 by the smallest integer that will convert all of them to whole numbers. This set of whole numbers represents the subscripts in the empirical formula

19. Example In a lab experiment it was observed that 0.6884 g of lead combines with 0.2356 g of chlorine to form a binary compound. Calculate the empirical formula of this compound When a 2.00 g sample of iron metal is heated in air, it reacts with oxygen to achieve a final mass of 2.573 g. Determine the empirical formula for this iron oxide

20. Calculating Empirical Formula from Percent Composition Cisplatin, the common name for a platinum compound that is used to treat cancerous tumors, has the composition (mass percent) 65.02% platinum, 9.34 % nitrogen, 2.02% hydrogen, and 23.63% chlorine. Calculate the empirical formula for csiplatin

21. 8.8 Calculation of Molecular Formulas Molecular formula – gives the actual numbers of atoms in a molecule Molecular formula = n x empirical formula may be the same as the empirical formula a multiple of the empirical formula (or # of empirical unit) is defined: Multiple ( # of empirical unit) or n =

22. Example A compound used as an additive for gasoline to help prevent engine knock shows the following percent composition 71.65 % Cl24.27 % C4.07 % H The molar mass is known to be 98.96 g/mol. Determine the empirical formula and the molecular formula for this compound  A compound containing carbon, hydrogen, and oxygen is found to be 40.00% C and 6.700% by mass. The molar mass of this compound is between 115 g/mol and 125 g/mol. Determine the molecular formula for this compound