2Warm Up: Determine the name and molar mass of the following compounds. NaOHMnO2H2SO4
3Be sure you go back and review the basics… How did you do?NaOH g/mol, sodium hydroxideMnO g/mol, Manganese (IV) oxideH2SO g/mol, Sulfuric acidBe sure you go back and review the basics…
4Molecular Formula Activity This activity was designed to help you remember some of the content we learned last semester.You will also be learning about formulas (empirical and molecular) and percent composition.
5The Activity Work in groups of 3 or 4. Be sure that every word of the activity is read out loud…take turns.Every person needs to fill in their sheet.The bags containing LEGO molecules are on my desk, come get one when you are ready. Balances are out.
6Warm Up- Write the formulas Calcium hydroxideCarbon monoxideIron (III) chlorideCopper (II) nitrateSulfur tetroxide
8What is Percent Composition? Two ways of describing the composition of a compound.HCl1. How many atoms of each element2. The mass of each element in the compound (percentage).
9How do I calculate Percent Composition? Calculate the molar massMass of element x 100= % composition Total Molar MassAdd all the %compositions to make sure they total 100%.
10Let’s find the percent composition of each element in water. H2O
11Find the percent composition of each element in these compounds Li3NBaSO3
12Li3N Molar mass Li 3moles x 6.94 g/mol = 20.82g N 1mol x g/mol = g20.82g g = 34.83g
13Mass percent Li20.82g x 100 = %34.83gMass percent N14.01g x 100 = %59.78% % = 100%
14BaSO3 Molar mass Ba 1mol x 137.3g/mol = 137.3g S 1mol x 32.07g/mol = 32.07gO 3mol x 16.00g/mol = 48.00gTotal =217.37g
15BaSO3 Mass percent Ba 137.3g x 100 = 63.16% 217.37g Mass percent S Mass percent O48.00g x 100 = %63.16% % % =99.99% Close enough!!
16K2Cr2O7 Molar mass K 2mol x 39.10g/mol = 78.20g Cr 2mol x 52.0g/mol = gO 7mol x 16.00g/mol = gTotal =294.2g
17K2Cr2O7 Mass percent K 78.20g x 100 = 26.58% 294.2g Mass percent Cr Mass percent O112g x 100 = %26.58% % % =100%
18Look at the Percent Comp WS You can do these no problem right?Look at the problems at the bottom!
19Once you determine the Percent composition you can do various calculations How much potassium can be obtained in the decomposition of 50.0 g of K2Cr2O7?Multiply the Total mass by the percent = g
20How did we determine the chemical formula of your LEGO compound? We take a known amount of the sample and take it apart.All the pieces are collected and weighed.This provides the mass of each type of element allowing us to determine the mass percent of each element.We use this information to determine the formula.13.29 g 9g
21ExampleSuppose we have a compound that contains the elements C, H and O.Total mass = g.C = gH = gO = g
22Convert grams to moles. (0.0806g C) x 1mol C = 0.0067mol C 12.01g ( g H) x 1mol H = mol H1.008g H(0.1074g O) x 1mol O = mol O16.00g O
23Now, look for the smallest number and divide! 0.0067mol Cmol Hmol OThis usually results in whole numbers-that tell us the ratio of atoms in the compound
24Warm Up- Jan 11, 2013Determine the percent composition of nitrogen in NO3.
25How did you do on % Comp HW? K=24.74%Mn=34.76%O = 40.50%Mg = 16.39%N = 18.89%O = 64.72%Al=15.77%S= 28.11%O= 56.12%g O2g Feg AgQuestions??
26Empirical FormulaSymbols of the elements with subscripts showing the smallest whole-number mole ratio of the different atoms in the compound.CH2O1:2:1 Mole ratio
27Empirical vs. Molecular formulas Empirical formula- smallest whole-number ratio of the atoms in a compound.Molecular formula- gives the actual number of atoms in the compound.
28What would be the empirical formulas? CH2OC2H4O2C3H6O3C4H8O4
29Example: Step 4An oxide of aluminum is formed by the reaction of 4.151g Al with 3.692g of Oxygen. Determine the empirical formula of the compound.
30K: Aluminum Oxide is formed- Al and O 4.151 g of Al3.692g of OUK: Empirical formula Al O
312. Determine the number of moles of each element. 4.151g Al x 1mol = mol Al26.98g Al3.692g O x 1mol = mol O16.00g O
323. Divide the number of moles of each element b the smallest number of moles mol Al= 1 mol Al0.1539mol O = 1.5 mol OBummer! Not whole numbers! You can’t have a half a mol! What can I multiply both numbers by and get whole numbers?
33Empirical formula- Al2 O3 = 1 mol Al x 2 = 20.1539= 1.5 mol O x 2 = 3Empirical formula- Al2 O3
34Warm UpIf the empirical formula is CO, write 3 molecular formulas that would be correct.Al2 O3Al4 O6Al6 O9
35Determining Molecular Formulas If you know the empirical formula… CH2 And are given the molar mass of the molecular formula… 42.09g/mol We want to figure out how many of the empirical formulas fit into the molecular formula.
36You try…A compound has a molar mass of g/mol. The compound has an empirical formula of NO. Determine the molecular formula.
37Sometimes you need to figure out the empirical formula first! A sample contains a compound that is 30.45% nitrogen and 69.55% Oxygen. The molar mass of the compound is 92.02g/mol. What is the molecular formula. a. Assume 100g- makes % into g b. Convert grams to moles c. Divide by the smallest # moles d. Write the Empirical formula and determine the molar mass. e. Divide the molar mass of the compound by the molar mass of the empirical formula.
38Work on the WS…Homework is the formula review… Major quiz Wed/Thurs…