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The purpose of the laboratory is to provide students with conce and theoretical knowledge to help them learn scientific concep- through scientific methods, to understand the nature of science. The purpose of this experiment is to develop a metal oxide figure out its empirical formula. This experiment will also d the formula of metal oxide. Data: (9 points) The sajandilevisado muoy moogt bris List all data that was collected from this experiment to help you determine the molecular formula oxide that you formed. Be sure to include the correct significant figures and units. Show all your c in the boxes. ob way enne vlajelgmos rti riw eldiouno art Example: Mass of the dry crucible = 5.983 g Mass of crucible and lid bro099 30.5579 Mass of crucible, lid and metal 0.0299 Mass of metal 30.5869 30.5869-30-5579.
30.0179 = 0.069 Mass of metal-oxygen compound 0.0319 Mass of oxygen in compound 24.305 Molar mass of metal 0.0298 x Imol 24.3058 Mole of metal in compoun Molar mass of oxygen atom 1200 16.00 packenwon 16.00g x Imol Mole of oxygen in compound -30.557g 0.0318 = 0.0012 mol S = 0.66m01
Discussion: (28 points) 1. Based on what you know about the unknown metal sample propose a balanced chemical equation for a. the formation of the Group 1 metal oxide (3 points) 4 MLS) + 0₂ (9) — 2M ₂0 (5) Group 1 metal charged a oxide a is -2 charged. the ox formed will be MO V b. the formation of the Group 2 metal oxide (3 points) group 2 has ta charge forms MO oxide 2M (5) + O₂(g) → 2MO(S) 2. Using the experimental data that you collected, determine the mass of the metal and oxygen in your final sample. (6 points) Mass 10 metale 36. $868 3. Using the mass of the metal found in Question 2 above and the known quantity of moles in the sample us calculate the molar mass of the metal. (3 points) 4. Using the molar mass, what metal is the unknown expected to be? (3 points) 5. Now that you have identified the metal, using the molar mass reported on the periodic table, calculate the number of moles in your sample using the experimental mass of the metal. (3 points)
6. Convert the mass of the oxygen found in Question 2 into the number of moles of oxygen. (3 points) 7. Using the values calculated in Questions 5 and 6, show the remaining steps to solve for the empirical form (You may complete these by hand. Be sure that all numbers are labeled with the correct units and your m shown in a logical order down the page.) (4 points) Conclusions: (6 points) 1. Based on the identification of the unknown metal, what is the expected ionic (empirical) formula? (4 poir 2. Is the expected ionic formula for this metal oxide consistent with the calculated empirical formula? Suppo your answers with the appropriate scientific reasoning. (4 points)