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Empirical and Molecular Formulas INFORMATION (P See book pages 343 – 351 Name: _____________________ Empirical and Molecular Formulas INFORMATION (p. 348 – 349): An empirical formula is a “lowest common denominator” molecular formula for covalent molecules. It represents the ratio in which atoms (or MOLES of atoms) combine to form compounds, but not the actual numbers of atoms in the compound. Multiple compounds can have the same empirical formula. Glucose, C6H12O6, contains carbon, hydrogen, and oxygen. The ratio of carbon to hydrogen to oxygen is 1:2:1. CH2O is the empirical formula for glucose. Since the percent composition of each element in an empirical formula represents the ratio in which they occur, the percent composition can be used, in conjunction with the molar masses of the elements, to determine the empirical formula of a compound. It is generally prudent to assume a 100.0 gram sample of the compound for the purpose of simplifying the calculations. Example 1: Caffeine has the following percent composition: carbon, 49.48%; hydrogen 5.19%; oxygen, 16.48%; and nitrogen, 28.85%. What is its empirical formula? (see page 349) INFORMATION (p. 350 – 351): A molecular formula is a formula that represents the actual number of each atom in a compound. Whereas CH2O is the empirical formula for glucose, C6H12O6 is the molecular formula. An actual molecule of glucose contains six carbon atoms, twelve hydrogen atoms, and six oxygen atoms. (Or six moles of carbon atoms, 12 moles of hydrogen atoms, and six moles of oxygen atoms). Since an empirical formula indicates the ratios of the elements in the compound, it can be used, along with the molar mass of the compound, to determine the molecular formula. As with empirical formulas, assume a 100.0 gram sample to simplify the calculations. Example 2: The molar mass of caffeine is 194.19 g/mol. What is its molecular formula? (See page 351) Example 3: What is the empirical formula for a compound that contains 0.0134 grams of iron, 0.00769 grams of sulfur, and 0.0115 grams of oxygen? (Two steps: (1) See page 344 AND (2) See Example 1 OR page 349) 1 Hint for determining EF (Empirical Formula): % to mass, mass to mole, divide by small, multiply till whole Here are the steps to follow to work Empirical Formula problems: 1. Take either the GRAMS of each element given or the PERCENTAGE of each element given and divide it by the atomic mass of that element. Leave the result of each division in AT LEAST 4 SIG FIGS. 2. Compare all the results from Step 1 by selecting the SMALLEST value and dividing ALL values by this smallest one. 3. The results of Step 2 will either be VERY close to whole numbers or will be recognizable mixed number fractions (decimals such as 1.5, 2.333, 6.67, etc). a. If any result from Step 3 is a mixed number, you must multiply ALL values by some number to make it a whole number. Ex: 1.33 x 3, 2.25 x 4, 2.50 x 2, etc. 4. Use these whole number results as SUBSCRIPTS and write the empirical formula, listing the elements in the order they are given in the problem. (HINT: don’t be surprised if the subscripts in some formulas are VERY large-many organic molecules are huge) _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ __ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ Hint for determining MF (Molecular Formula): MF=(EF)n n=MF molar mass (given in problem) EF molar mass How to find the molecular formula: 1. Calculate the mass of the empirical formula (which you have already found or it will be given to you ) 2. Divide the known molar mass by the mass of the empirical formula. 3. Multiply that number by the subscripts of the empirical formula to get the subscripts for the molecular formula. _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ __ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ How to find the percent composition of a compound: 1. Write a correct formula for the compound 2. Find the molar mass of the compound 3. Divide the total atomic mass of EACH ELEMENT by the molar mass 4. Multiply by 100 to convert your results to a percent 5. Since you have no significant figures to go by, express your answer to TWO decimal places with the % sign. _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ __ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ Empirical or Molecular Formula Problems: Be sure to show ALL work!!! 1. Find the empirical formula for a compound that contains 32.8% chromium and 67.2% chlorine. (See Example 1 OR page 349) 2 2. What is the empirical formula for a compound that contains 67.1% zinc and the rest oxygen? (See Example 1 OR page 349) 3. The percent composition of a binary compound is 92.3% carbon and 7.7% hydrogen. If the actual molar mass is 78.0grams/mol, find the molecular formula? (Two steps: (1) See Example 1 OR page 349 AND (2) See Example 2 OR page 351) 4. What is the molecular formula of dichloracetic acid if the empirical formula is CHOCl and the actual molar mass is 129.0 grams/mol? (See Example 2 OR page 351) 5. An empirical formula is found to contain three atoms of carbon, four atoms of hydrogen, and two atoms of oxygen. The actual molar mass is 288.0 grams/mol. Find the molecular formula. 6. Find the empirical formula of a compound that contains l5.8 g of Al, 28.1 g of S, and 56.1 g of oxygen. 3 7. The empirical formula for a hydrocarbon is CH2. Its actual molar mass is 294 g/mol. What is its molecular formula? 8. 500. grams of a compound are found to contain 133 grams of potassium, l76.5 grams of chromium and the rest is oxygen. What is the empirical formula for the compound? _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ __ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ NOMENCLATURE REVIEW: (SEE PAGES 281 – 302, 308 – 310) SEE PAGES 308 - 310 Determining the formula for Magnesium Fluoride? 1. Identify the charges = Mg2+ F1 2+ 1 2. Cross the Charges, Mg F = Mg1F2 3. If the subscript is a 1 it does not need to be written. 4. If there is a common subscript such as 2 as in Mg2O2, reduce it to Mg1O1 which is also MgO. 4 9. Write the formulas for the following ionic (p. 288 – 289, 292-293, or Acids – p. 301) compounds: a. Sodium chloride i. Calcium sulfate 1+ 1- Na 1Cl 1 = NaCl b. Strontium phosphide j. Lithium phosphate c. Iron (III) bromide k. Magnesium nitrate d. Aluminum sulfide l. Potassium chlorate e. Copper (II) iodide m. Hydrobromic acid f. Indium oxide n. Hydrochloric acid g. Rubidium arsenide o. Nitric acid h. Lead (IV) nitride p. Nitrous acid 10. Write the names for the following ionic (BIC, TIC, or Acids) compounds (p. 290-291, 294): q. KBr w. CuO cc. FeCO3 r. Fe3N2 x. Ba3P2 dd. CuSO4 s. SrBr2 y. Ca3(PO4)2 ee. H2SO4 t. AlCl3 z. LiNO3 ff. H2SO3 u. Sn3P2 aa. MgSO4 v. CaI2 bb. Al2(CO3)3 11. Write the names or formulas for the following covalent (BMC) compounds (p. 296 – 298): If only two elements are combining, the compound is said to be binary. The element which is less electronegative (closer to the metals in the periodic table) is named first, followed by the other element’s name with an –ide suffix. Number 1 2 3 4 5 6 7 8 9 10 Prefix mono di tri tetra penta hexa hepta octa nona deca a. Dicarbon Tetrahydride i. CH4 b. Carbon Tetrafluoride j. C3H8 c. Nitrogen Trichloride k. CI4 d. Carbon Monoxide l. NF3 e. Carbon Dioxide m. PF3 f. Sulfur Dichloride n.
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