Molecular vs. Empirical Formula Chemistry H 2 O H 2 O 2. NaCl
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1 Molecular vs Empirical Formula Chemistry Name Block Read the information below and then answer the questions that follow Definitions: Molecular formula the total number of atoms of each element in a compound Empirical formula the simplest/smallest ratio of each element in a compound Examples: Substance Molecular Formula Simplifying the Ratio Empirical Formula Sugar C 6 H 12 O 6 Water Hydrogen Peroxide Salt (Sodium Chloride) H 2 O H 2 O 2 NaCl Ribose C 5 H 10 O 5 Molecular & Empirical Formulas Part 1 Calculate the Molar Masses and % composition for both the empirical and molecular formula below Then, determine a similarity and difference between the two Substance Molecular Formula (MF) Empirical Formula (EF) Sugar C 6 H 12 O 6 CH 2 O Molar Mass %Composition % C: % H: % O: % C: % H: % O: Similarity between MF & EF Difference between MF & EF
2 Molecular & Empirical Formulas Part 2 Substance Molecular Formula Empirical Formula Water H 2 O H 2 O Salt (Sodium Chloride) NaCl NaCl You should have noticed that for both substances, the Molecular & Empirical Formulas are the same Explain why it is possible for both the Molecular & Empirical Formulas to be the same Molecular & Empirical Formulas Part 3 Substance Molecular Formula Empirical Formula Glucose C 6 H 12 O 6 CH 2 O Ribose C 5 H 10 O 5 CH 2 O You should have noticed that both substances have the same empirical formula Explain why it is possible for two different MFs and have the same EF
3 Molecular & Empirical Formulas Part 4 Substance Molecular Formula (MF) Empirical Formula (EF) Hydrogen Peroxide H 2 O 2 = Molar Mass 3402 g/mol 1701 g/mol The MF subscripts has a common divisible number, 2 Therefore, each subscript was divided by 2 in order to obtain the EF Calculate the ratio of the molar masses: = = What do you notice about the ratio of the molar mass and common divisible number? Critical Thinking: If you knew the empirical formula and molar mass of your molecular formula, how would you try to find the Molecular formula?
4 Practice: 1 Complete the table below by writing the empirical formula for each molecular formula Molecular Formula Empirical Formula P 4 O 10 N 2 O 5 C 12 H 27 C 20 H 25 O 10 2 A compound has an empirical formula of CH 2 and a molecular mass of 420g/mol Determine its molecular formula 3 The empirical formula was determined to be PBr 5 What is the molecular formula if the molar mass of the molecular formula was found to be 431 g/mol 4 A combustion analysis gives the following empirical formula of C2H4O Determine the molecular formula knowing that the molecular mass = 13216g/mol 5 Naphthalene is a carbon and hydrogen containing compound often used in moth balls The empirical formula is C 5 H 4 and its molar mass is 12816g/mol Find the molecular formula
5 Determining Empirical Formulas from Mass Data Ex: Assume you have a sample that is 0504 g hydrogen and 400 g oxygen 1 Convert grams moles for each element 2 Simplify the mole ratio for each element by dividing each number (of moles) by the smallest # of moles 3 Use the smallest whole-number mole ratio as the subscripts for the empirical formula Practice: 1 A 5325 g sample of methyl benzoate, a compound used in the manufacture of perfumes, is found to contain 3758 g of carbon, 0316 g of hydrogen and 1251 g of oxygen What is the empirical formula of methyl benzoate? 2 A 2498g sample of an unknown compound was analyzed and found to contain 135 g Ca, 108 g O, and 0675 g H What is the empirical formula of the compound?
6 Determining Empirical Formulas from Percent Composition Data: 2 Methods Ex: Determine the empirical formula for a compound containing 740% carbon (C), 865% hydrogen (H), and 173% nitrogen (N) by mass 1 Assume a 100 gram sample for the compound The percent composition of each element will then be equal to the mass of the element found in the 100 g sample Assume a 100 g sample: C: 740 % 74 g C in 100 g sample H: 865 % 865 g H in 100 g sample N: 173% 173 g N in 100 g sample 3 Simplify the mole ratio for each element by dividing each number (of moles) by the smallest # of moles C: H: = = Convert grams moles for each element C: 74 = H: 865 = N: 173 = 4 Use the smallest whole-number mole ratio as the subscripts for the empirical formula C: 5 H: 7 C5H7N N: = 100 N: 1 Note: If the simplified mole ratios are not all whole numbers, multiply by the smallest factor that will produce whole number subscripts Practice: 1 A compound is found to contain 6352% iron and 3648% sulfur Determine the empirical formula
7 2 Ascorbic Acid (vitamin C) is 4092% Carbon, 458% Hydrogen and 5450% Oxygen by mass Calculate the empirical formula of Ascorbic Acid ~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~ Mixed Practice: 1 Determine the empirical formula of the given molecular formulas below Molecular Formula HgBr2 Empirical Formula Molecular Formula C8H14 Empirical Formula C2H6O C3H6 2 A compound has an empirical formula of CF3 and a molar mass of g/mol What is the molecular formula of the compound? 3 A compound has an empirical formula of CaCl2 Determine the molecular formula of the substance if its molar mass is g/mol
8 4 A 100 gram sample of a compound contains 722 grams of magnesium and 278 grams of nitrogen The molar mass of this compound is g/mol a What is the empirical formula of the compound? b What is the molecular formula? 5 Fat makes up a major portion of all soaps A fat used in many soaps is 765% carbon, 122% hydrogen, and 113% oxygen a What is its empirical formula? b What is the molecular formula of a fat with a molar mass of 705 g/mol?
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CHEMICAL QUANTITIES Chapter Six Introducing the Mole The dozen is a unit of quantity If I have a dozen atoms, I have 12 atoms by definition. The mole(mol) is a very important unit of quantity in chemistry.
The Mole Concept. It is easily converted to grams, no of particles or in the case of gas volume.
The Mole Concept The mole is a convenient unit A mole is the number of atoms present in exactly 12 g of the isotope carbon-12. In 12 g of carbon-12 there are 6.022 x 10 23 carbon atoms It is easily converted