Chemical formulas allow chemists to calculate characteristic values for a compound.
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1 Chemical Formulas Using Analytical Data to Calculate Chemical Formulas Chemical formulas allow chemists to calculate characteristic values for a compound. Calculation Types You Must be Able to Complete X Molar Mass (Formula Mass) X Percentage Composition by Mass X Using Percentage Composition Data to Calculate Empirical Formulas New: Using Data to Calculate Molecular Formulas For Ionic Compounds There is only 1 type of chemical formula: The Empirical Formula The Empirical Formula Gives the simplest whole number ratio of ions that produces a neutral arrangement Gives the simplest whole number ratio of moles Molecular Compounds are Different Molecular Formula C 6 H 12 O 6 For each element this is the: Actual number of atoms Actual number of moles This is the blueprint for drawing the Lewis Structure This is the formula written from the name Additional examples: Molecular Formula H 2 O H 2 O 2 Empirical Formula C H 2 O This is the simplest whole number ratio For each element this is the reduced : number of atoms number of moles This is the backbone Not used to write a name Empirical Formula H 2 O HO N 2 O 4 NO 2 ICl 3 ICl 3 In general, for molecular compounds, the molecular formula will be the same as the empirical formula or the molecular formula will be larger.
2 Answer the Following Sample Concept Questions 1) The molecular formula for vitamin C is C 6 H 8 O 6. What is the empirical formula? a. CHO c. C 3 H 4 O 3 b. CH 2 O d. C 2 H 4 O 2 2) Which of the following could be an empirical formula? a. N 2 O 4 b. b. N 2 H 6 c. c. N 2 O 5 d. d. More than one could be an empirical formula. e. None of these are empirical formulas. 3) If the empirical formula of a compound is CH 2 what is a possible molecular formula for the compound? a. CH 2 b. C 2 H 6 c. C 4 H 8 d. More than one could be a molecular formula for CH 2. e. None of these could be a molecular formula for CH 2. In summary, sometimes the Molecular Formula = Empirical Formula Other times the Molecular Formula > Empirical Formula It is larger by X where X is a whole number Never is the Molecular formula smaller than the empirical formula Not sure what the difference is between Molecular and Empirical Formulas for Covalent Compounds? Watch this video: All set then move on to molecular formula calculations notes, videos and problems
3 How to Calculate Molecular Formula Problem Types Given % composition data or the empirical formula and The molecular formula mass To solve problems Use the relationships given in these two formulas you must memorize 1st Formula 2nd Formula X (Empirical Formula) = Molecular Formula Where X is a whole-number multiple found by X = Molecular Formula Mass What will vary, problem to problem, is the information you are given and what you have to do to find X.
4 Problem Type 1 Given: Empirical Formula and Molar Mass of the Molecular Formula Video: Watch and take notes
5 Problem Type Given: Empirical Formula and Molecular Formula Mass Step 1 Calculate the Step 2 Solve for X X = Molecular Formula Mass Step 3 Apply X X (Empirical Formula) = Molecular Formula Step 4 Write the Molecular Formula After watching the video solve the following problem on a separate sheet of paper. You must show all work A compound was analyzed. The empirical formula of the compound is C4H4O and the molar mass of the molecule is 136 g/1mole.
6 Problem Type #2 Given percentage composition data and the molecular formula mass Video: Watch and take notes.
7 Problem Type 2 Given: % Composition and Molecular Formula Mass Step 1 Calculate the Empirical Formula % to mass Grams to Moles etc. Step 2 Calculate the Step 3 Solve for X X = Molecular Formula Mass Step 4 Apply X X (Empirical Formula) = Molecular Formula Step 5 Write the Molecular Formula After watching the video solve the following problem on a separate sheet of paper. You must show all work A compound was analyzed and found to have 65.5% carbon, 5.5% hydrogen and 29.0% oxygen? If the molar mass of this molecule is 110.g/mole, what is the molecular formula?
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Reactions continued And chemical review!! Steps to find grams in chemical Balance the equation to get molar ratios Find molar mass of the substances in question Find moles of the one given in grams Set
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