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Slide 2 What is a Mole Chemists use the mole to count microscopic particles. How many socks come in a pair? 2 How many eggs are in a dozen? 12 How many eggs come in a gross? 144 How many pencils come in a ream? 500 Slide 3 So how many atoms come in a mole? 602,213,670,000,000,000,000,000. Seriously This number was created by an Italian physicist and lawyer named Amedeo Avogadro. Its called Avogadros Number. Is there an easier way to write it? 6.02 x 10 23 items = 1 mole Slide 4 Converting between moles and number of particles Think about eggs 1 dozen eggs = 12 eggs Conversion factor: 12 eggs/1 dozen eggs OR 1 dozen eggs/12 eggs So if you have 3.5 dozen eggs how many eggs do you have? 3.5 dozen x (12 eggs)/1 dozen = 42 eggs Slide 5 If you have 3.5 moles of sugar how many particles of sugar do you have? 1 mole of sugar = 6.02 x 10 23 particles of sugar. Set up the problem: 3.5 moles x (6.02 x 10 23 particles/1 mole) Solve: 2.107 x 10 24 Slide 6 Zinc (Zn) is used to form a corrosion-inhibiting surface on galvanized steel. Determine the number of Zn atoms in 2.50 moles of Zn. 1.51 x 10 24 atoms Calculate the number of molecules in 11.5 mol of water. 6.92 x 10 24 molecules Silver nitrate Ag(NO 3 ) 2 is used to make several different compounds used in photographic films. How many molecules of silver nitrate are there in 3.25 moles of Ag(NO 3 ) 2 ? 1.96 x 10 24 How many atoms of oxygen are there in 5.0 mol of oxygen gas? 6.02 x 10 24 atoms Slide 7 Converting from number of particles to moles Calculate the number of moles of Zinc that contains 4.50 x 10 24 atoms. 0.914 moles How many moles can be made up from 5.57 x 10 24 atoms of Al? 9.55 moles How many moles can be made up from 2.5 x 10 25 atoms of Fe? 41.5 moles Slide 8 Slide 9 What would have more mass a dozen eggs or a dozen elephants? Why would a dozen elephants have more mass? Just like elephants and eggs certain atoms are bigger than others. For example Neon is much bigger than Helium. Which would have more mass 1 mole of Neon or 1 mole of Helium? Slide 10 Molar Mass The molar mass of an element is the mass in grams of one mole of that element. Why is this important? Molar mass can be used to calculate the number of atoms with out using a microscope. Slide 11 Using molar mass If one dozen jelly beans has a mass of 35 g how much mass does 5 dozen jelly beans have? 175 g To convert from Moles to mass you multiply by the molar mass. What is the mass of 3.oo moles of copper? 191 g cu. To convert from mass to moles you divide by the molar mass. Slide 12 Example Problems Chromium (Cr), a transition element, is a component of chrome plating. Chrome plating is used on metals and steel alloys to control corrosion. Calculate the mass in grams of 0.045 moles of Cr. 2.34 g Cr Slide 13 Calcium (Ca), the fifth most abundant element on earth, is always found combined with other atoms because of its high reactivity. How many moles of calcium are in 525 g Ca? 13.1 moles Ca Slide 14 Converting between mass and atoms The next step is converting a given mass of an element into a number of atoms. If we have 550 g of jelly beans and there are 35 g of jelly beans in a dozen how many dozen jelly beans do we have? 16 dozen How many jelly beans are there in 16 dozen? 192 Slide 15 Mass-to-Atom Conversion Gold (Au) is one of a group of metals called the coinage metals. How many atoms of gold are there in a U.S. gold eagle coin with a mass of 31.1 g? 9.51 x 10 22 Slide 16 Atom-to-Mass Conversion Helium (He) is an unreactive noble gas found underground. A party balloon contains 5.5 x 10 22 atoms of helium gas. What is the mass, in grams, of the helium? 0.366 g Slide 17 Homework Textbook (sorry) P. 328 # 15(a&b), 16(a&b) P. 329 # 17(a&b), 18(a&b) P. 331 # 19(a&b), 20(a&b) Slide 18 Slide 19 Chemical Formulas and the Mole In the compound CCl 2 F 2 how many atoms do we have? C: 1 Cl: 2 F: 2 So if we have one mole of CCl 2 F 2 we have one mole of carbon, two moles of Chlorine and one mole of Fluorine. Slide 20 Molar Mass of a Compound Determine the molar mass of each of the following compounds: NaOH CaCl 2 KC 2 H 3 O 2 C 2 H 5 OH HCN CCl 4 (NH 4 ) 3 PO 4 Slide 21 Converting moles to mass The characteristic odor of garlic is due to allyl sulfide (C 3 H 5 ) 2 S. What is the mass of 2.5 moles of allyl sulfide? What is the mass of 3.25 mol of H 2 SO 4 ? Slide 22 Converting Mass to Moles Calculate the number of moles in 325 g of Calcium hydroxide Ca(OH) 2 ? Calculate the number of moles in 22.6 g of AgNO 3. Slide 23 Mass to Number of Particles Aluminum chloride (AlCl 3 ) is used in refining petroleum and manufacturing rubber. How many Aluminum Chloride molecules are present in 35.6 g of AlCl 3 How many Al atoms are there? How many Cl atoms are there? Slide 24 Example Aluminum oxide (Al 2 O 3 ) when dissolved in water breaks apart into ions (Al 3+ and O 2- ) how many moles of Al 3+ will be produced when 1.5 moles of Al 2 O 3 are dissolved in water? Slide 25 Examples 1. What is the molar mass of ethanol C 2 H 5 OH? How many ethanol molecules are present in 45.6 g? How many carbon atoms are there in 45.6 g of ethanol? How many hydrogen atoms are there in 45.6 g of ethanol? How many oxygen atoms are there in 45.6 g of ethanol? 2. A sample of sodium sulfite Na 2 SO 3 has a mass of 2.25 g How many molecules of sodium sulfite are there? How many atoms of sodium are there? How many atoms of Sulfur are there? How many atoms of oxygen are there? Slide 26 Slide 27 Percent Composition A compound is made up of one or more atoms bonded together. Each of the atoms contributes mass to the compound. Example: The molar mass of NaOH is Na 22.98 g/mol O 16 g/mol H 1 g/mol Total: 39.98 g/mol Slide 28 Calculating Percent Composition Percent composition is calculated by dividing the mass of an individual element by the mass of the whole compound and then multiplying by 100. NaOH: Percent Composition of Na: (22.98/39.98) x 100 = 57.5% Percent Composition of O: (16/39.98) x 100 = 40% Percent Composition of H: (1/39.98) x 100 = 2.5% Slide 29 Compounds with multiple atoms of the same element NaHCO 3 Molar Mass: 84.01 g/mol Percent Composition of Na: (22.98/84.01) x 100 = 27.37% Percent Composition of H: (1/84.o1) x 100 = 1.2% Percent Composition of C: (12.01/84.01) x 100 = 14.3% Percent Composition of O: (48/84.01) x 100 = 57.14% Slide 30 Empirical Formula When we know a compounds percent composition we can determine its formula. The empirical formula of a compound is the formula with the smallest whole-number ratio of elements. Find the empirical formula for a compound that is 40.05% S and 59.95% O. If we assume that we have 100 g of this compound: How many grams of Sulfur do we have? 40.05 g How many grams of Oxygen do we have? 59.95 g Convert from grams to moles: 40.05 g S x 1 mol S/32.07 g S = 1.249 mol 59.95 g O x 1 mol O/16.00 g O = 3.747 mol Slide 31 S 1.249 O 3.747 SO 3 Sometimes the empirical formula is not the actual formula for the compound. Find the empirical formula for hydrogen peroxide which has a molar mass of 34 g/mol and is 5.9% Hydrogen and 94.1% Oxygen Slide 32 Molecular Formula A compounds molecular formula is its actual formula (not always the same as empirical formula) To determine the true molecular formula for a compound its molar mass must be known (either looked up or found experimentally). Once we know the molar mass and the empirical formula we can find the true formula of the compound. Slide 33 Example: Acetylene is a highly flammable compound used in blow torches. Acetylene has a molar mass of 26.04 g/mol. It is 92.2% Carbon and 7.8% Hydrogen. What is the chemical formula of Acetylene? Step 1: Find empirical formula: CH Step 2: Calculate molar mass of empirical formula. (If the molar mass is the same as the actual molar mass then the empirical formula is the true formula.) 13.02 g/mol Step 3: Divide real molar mass by the molar mass of the empirical formula. 26.04/13.02 = 2.000 Step 4: Multiply all atoms in the empirical formula by the answer to the true formula. C 2 H 2