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Thank you for your purchase! I would love to hear specific feedback how the product worked with your students. If you have any questions or concerns about the product, please email me so I can assist you to ensure your satisfaction with the product. Additionally, please check back periodically as I usually make updates to the product either based on questions submitted, feedback, or my desire to enhance the quality of the product. Table of Contents Page 3 Terms of Purchase & Copyright Pages 4-5 Procedures for class set-up Page 6 Customization for resizing IGOs Pages 7-8 Instructions for Note Pages Pages 9-20 Student Note Pages Pages 21-26 Student Notes Pages Key Pages 27-28 Hexagon Mole Fold Pages 29-30 Mole Pyramid Pages 31-33 Empirical & Molecular Formula Fold Pages 34-35 Empirical Formula Layer Pyramid Pages 36-41 The Mole-dable (6-Flap) Upload or distribution prohibited Connect with me by clicking any of the social media icons below for products, instructional tips, and innovative ways to teach K-12 science. Sikumus prime was here

TERMS OF PURCHASE AND COPYRIGHT NOTICE The copyright for this product will be strictly enforced. Please thoroughly read and contact me if you have any questions. [A] A single purchase of this product is for individual classroom use by the purchaser only. Additional licenses may be purchased for multiple classrooms. **Wide-use licenses, such as a campus or district purchase, will receive an amended version of the product indicating wide-use approval with the campus or district name** [B] Scanning, electronic copying, file sharing, redistributing, editing, selling, or posting this item (or any part thereof) on the Internet, or with others, is strictly prohibited. This includes sharing and/or distribution across a campus, school district, region, or conference workshop. [C] You may not recreate any part(s) of this product to create items to use, sell, or share with others [this also includes translating the product from English to another language]. [D] All copyrights of clip art images used belong to their respective owners [as acknowledge in this product] and are not being sold. I do not claim ownership over the clip art used in my products. Disregarding the copyright of this product will subject you to the penalties of the Digital Millennium Copyright Act and legal action. Violations may also result in the immediate contact of school, district, school board, and/or state service center representatives to inform them of your disregard of the Terms of Purchase and copyright [which is stated in its entirety on the product page]. Additional clip art was purchased through and/or granted use through a. This product may include images available through Public Domain; however, all source sites were contacted prior to use. Purchase of this product does not grant you the right to copy and use the photographs and/or clip art.

Interactive Graphic Organizers (IGOs) All of my Interactive Graphic Organizers (IGOs) have the same basic format for teacher/student prep: = cut on dotted line(s) only = fold on solid black line(s) fold on solid black line(s) cut on dotted lines only

Interactive Graphic Organizers (IGOs) Determine which version works for you. [composition book, spiral notebook, and/or lapbook]

Did you print an IGO and it did not fit inside your notebook or lapbook? Interactive Graphic Organizers (IGOs) You should be able to resize the document prior to printing [depending on your PDF software]. Look for the Custom Scale option in Adobe software [boxed in black above] I used a mixture of 75%, 85%, and 100% for the IGOs. Play around with the customization to determine what size works for your class.

Half Sheet Notes IGOs Student Notes (pgs. 9-20) / Answer Key (pgs. 21-26) The IGO notes come in half sheets (1 page per 2 students). There are a total of 12 note/activity sheets for students covering the following topics: The Mole Concept Percent Composition Empirical Formula Molecular Formula The following topics have been cycled into the notes as well for review purposes: Ionic Nomenclature Covalent Nomenclature Students should fill in the blanks as the teacher is lecturing. The teacher may decide to cover 1 sheet at a time and incorporate one or more of the IGOs found in this product; although, it is not required. Answer keys are provided.

Half Sheet Notes IGOs Supplemental Activities (pgs. 13, 14, and 16) This activity is not required; however, it is one that I have done prior to teaching moles. Please refer to my blog post by clicking here. You may use any object for this activity. The first two scenarios will vary per class. The teacher may decide the numbers/ratios for these activities. Therefore, a key is not provided. This activity is not required; however, it is one that I have done while teaching Percent Composition. I normally use Dubble Bubble gum (cheap $$$). You may also talk about potential errors concerning this lab (e.g. weighing chewed gum with saliva)

The Mole When you hear or read the phrase, The Mole, you might be inclined to think of a small burrowing animal or a secret agent. However, a mole in chemistry is a very important term and your understanding of this concept will be critical to your success. Before, we talk about what a mole in chemistry means, let us complete a quick activity Fill in the blanks: A dozen pencils = pencils A dozen cars = cars Data Table: Object Set 1 Mass (grams) 2 dozen apples = apples 6 dozen birds = birds Set 2 Mass (grams) Set 3 Mass (grams) Directions & Questions: 1. One at a time, separate each object into three different groups of a dozen. 2. Weigh each set and record in the data table above. 3. Answer the following questions on the back of this page. a. In general, what could be said about the mass of a dozen? b. Could the same rule be applied to the other 3 objects? c. You had a dozen of each object. Did you have the same amount of each object? d. You had a dozen of each object. Did each set of objects have the same mass? The Mole When you hear or read the phrase, The Mole, you might be inclined to think of a small burrowing animal or a secret agent. However, a mole in chemistry is a very important term and your understanding of this concept will be critical to your success. Before, we talk about what a mole in chemistry means, let us complete a quick activity Fill in the blanks: A dozen pencils = pencils A dozen cars = cars Data Table: Object Set 1 Mass (grams) 2 dozen apples = apples 6 dozen birds = birds Set 2 Mass (grams) Set 3 Mass (grams) Directions & Questions: 1. One at a time, separate each object into three different groups of a dozen. 2. Weigh each set and record in the data table above. 3. Answer the following questions on the back of this page. a. In general, what could be said about the mass of a dozen? b. Could the same rule be applied to the other 3 objects? c. You had a dozen of each object. Did you have the same amount of each object? d. You had a dozen of each object. Did each set of objects have the same mass? Recreating, scanning, electronic copying, file sharing, redistributing, editing, selling, or posting this item (or any part thereof) on the Internet, or with others, is strictly prohibited. Violations are subject to the penalties of the Digital Millennium Copyright Act. James Lyas (Bond with James)

The Mole A mole is a unit. It is abbreviated and is a unit used in chemistry that allows us to deal with numbers of atoms, molecules, ions, or formula units in a sample of a substance. ***Chemists have define a mole as the number of carbon atoms in exactly 12g of pure carbon-12. Just like a dozen is equal to of something and a pair is equal to of something, chemists have established that a mole is equal to of something In chemistry, the something refers to particles (,,, or ). Just like the number 3.14159 has a name - pi (π), 6.02 x 10 23 has a name. It is called. Now, would you say a dozen pencils weigh the same as a dozen cars? Of course not! While the of both objects is the same, we would expect the of a dozen pencils and cars to be different. A mole of anything represents the same ( x 10 23 ) but it does NOT represent the for all substances. The mole is the link between and. The MASS of 1 mole is equal to the of a substance. Quick Check: Take 2-3 minutes to complete the table below. Substance 1 mole of a substance Mass (g) Oxygen (O) Bromine (Br) Gold (Au) Water (H 2O) Sodium carbonate (Na 2CO 3) The Mole A mole is a unit. It is abbreviated and is a unit used in chemistry that allows us to deal with numbers of atoms, molecules, ions, or formula units in a sample of a substance. ***Chemists have define a mole as the number of carbon atoms in exactly 12g of pure carbon-12. Just like a dozen is equal to of something and a pair is equal to of something, chemists have established that a mole is equal to of something In chemistry, the something refers to particles (,,, or ). Just like the number 3.14159 has a name - pi (π), 6.02 x 10 23 has a name. It is called. Now, would you say a dozen pencils weigh the same as a dozen cars? Of course not! While the of both objects is the same, we would expect the of a dozen pencils and cars to be different. A mole of anything represents the same ( x 10 23 ) but it does NOT represent the for all substances. The mole is the link between and. The MASS of 1 mole is equal to the of a substance. Quick Check: Take 2-3 minutes to complete the table below. Substance 1 mole of a substance Mass (g) Oxygen (O) Bromine (Br) Gold (Au) Water (H 2O) Sodium carbonate (Na 2CO 3) Recreating, scanning, electronic copying, file sharing, redistributing, editing, selling, or posting this item (or any part thereof) on the Internet, or with others, is strictly prohibited. Violations are subject to the penalties of the Digital Millennium Copyright Act. James Lyas (Bond with James)

Formula Weights You may see the following terms: Formula Mass Molecular Mass Molar Mass These terms all pretty much refer to the same thing in regard to doing calculations. For now, let us refer to this concept as because this term will be important when doing a specific type of calculation in chemistry. These problems are pretty easy. You need to know two things: 1. 2. (ex: C6H12O6) I Do: What is the molar mass of glucose, C6H12O6? Atom You Do: What is the molar mass of sodium sulfate, Na 2SO 4? Atom # of Each # of Each Periodic Table Atomic Mass x = x = x = Periodic Table Atomic Mass x = x = x = Total Total Formula Weights You may see the following terms: Formula Mass Molecular Mass Molar Mass These terms all pretty much refer to the same thing in regard to doing calculations. For now, let us refer to this concept as because this term will be important when doing a specific type of calculation in chemistry. These problems are pretty easy. You need to know two things: 1. 2. (ex: C6H12O6) I Do: What is the molar mass of glucose, C6H12O6? Atom # of Each Periodic Table Atomic Mass x = x = x = You Do: What is the molar mass of sodium sulfate, Na 2SO 4? Atom # of Each Periodic Table Atomic Mass x = x = x = Total Total Recreating, scanning, electronic copying, file sharing, redistributing, editing, selling, or posting this item (or any part thereof) on the Internet, or with others, is strictly prohibited. Violations are subject to the penalties of the Digital Millennium Copyright Act. James Lyas (Bond with James)

Moles in my Signature Purpose: Materials: Procedure: Data: 1. Obtain a piece of chalk and measure its mass on the triple beam balance. Record the mass in your data table. 2. Write your signature on a piece of paper (or you may be asked to write your signature outside on the concrete). 3. Measure the mass of your unused chalk on the triple beam balance. Chalk (CaCO 3) Calculations: Initial Mass Final Mass Mass of chalk used Molar Mass Based on the mass of the chalk used and its molar mass, determine the number of moles of chalk you used to write your signature. Show your work in the space provide below. Moles in my Signature Purpose: Materials: Procedure: Data: 1. Obtain a piece of chalk and measure its mass on the triple beam balance. Record the mass in your data table. 2. Write your signature on a piece of paper (or you may be asked to write your signature outside on the concrete). 3. Measure the mass of your unused chalk on the triple beam balance. Chalk (CaCO 3) Calculations: Initial Mass Final Mass Mass of chalk used Molar Mass Based on the mass of the chalk used and its molar mass, determine the number of moles of chalk you used to write your signature. Show your work in the space provide below. Recreating, scanning, electronic copying, file sharing, redistributing, editing, selling, or posting this item (or any part thereof) on the Internet, or with others, is strictly prohibited. Violations are subject to the penalties of the Digital Millennium Copyright Act. James Lyas (Bond with James)

Percent Composition The tells us the of a certain component an item. Imaginary Pizza Scenario If you ate out of slices, what percentage of the pizza did you eat? Explain how you developed your answer? Real-Time Scenario (Male to Female Class Ratio) Count your classmates. Total: Male count Female count % of males % of females Code the appropriate number of boxes in the graphic on the right to illustrate this. Educational Scenario (Grade Calculation) You take a quiz that has 10 problems. You miss 3. What is your grade? You take a test that has 36 problems. You miss s 8. What is your grade? How did you come up with your answers? Percent Formula Percent Composition The tells us the of a certain component an item. Imaginary Pizza Scenario If you ate out of slices, what percentage of the pizza did you eat? Explain how you developed your answer? Real-Time Scenario (Male to Female Class Ratio) Count your classmates. Total: Male count Female count % of males % of females Code the appropriate number of boxes in the graphic on the right to illustrate this. Educational Scenario (Grade Calculation) You take a quiz that has 10 problems. You miss 3. What is your grade? You take a test that has 36 problems. You miss s 8. What is your grade? How did you come up with your answers? Percent Formula Recreating, scanning, electronic copying, file sharing, redistributing, editing, selling, or posting this item (or any part thereof) on the Internet, or with others, is strictly prohibited. Violations are subject to the penalties of the Digital Millennium Copyright Act. James Lyas (Bond with James)

Percent Composition Information needed to calculate the percent composition of a substance: I Do: Calculate the percent composition of tetraphosphorus pentoxide. We Do: Calculate the percent composition of potassium sulfate. You Do: Calculate the percent composition of iron (III) oxide. Review the previous three examples. Which is a better source of oxygen? Explain why. P O K S O Fe O Percent Composition Information needed to calculate the percent composition of a substance: I Do: Calculate the percent composition of tetraphosphorus pentoxide. We Do: Calculate the percent composition of potassium sulfate. You Do: Calculate the percent composition of iron (III) oxide. Review the previous three examples. Which is a better source of oxygen? Explain why. P O K S O Fe O Recreating, scanning, electronic copying, file sharing, redistributing, editing, selling, or posting this item (or any part thereof) on the Internet, or with others, is strictly prohibited. Violations are subject to the penalties of the Digital Millennium Copyright Act. James Lyas (Bond with James)

Percent Composition Activity OBJECTIVE: To determine the percent of sugar in an ordinary piece of bubble gum. PURPOSE: - Why are you doing this lab (in 1 to 2 sentences) - Must be stated in your own words MATERIALS: - List of all the materials used in your experiment PROCEDURE: - A step-by-step account of how you carried out your experiment. DATA: - Include a data table to showcase the data collected during the lab. CALCULATIONS: - Show all calculations that you did using the data collected during the lab. ANALYSIS: Show ALL work!!! 1. What is the percent sugar in your gum? 2. How many moles of sugar, C 6H 12O 6, did you chew? 3. How many molecules of sugar were in your gum? CONCLUSION: - Summarize the results of the lab activity Percent Composition Activity OBJECTIVE: To determine the percent of sugar in an ordinary piece of bubble gum. PURPOSE: - Why are you doing this lab (in 1 to 2 sentences) - Must be stated in your own words MATERIALS: - List of all the materials used in your experiment PROCEDURE: - A step-by-step account of how you carried out your experiment. DATA: - Include a data table to showcase the data collected during the lab. CALCULATIONS: - Show all calculations that you did using the data collected during the lab. ANALYSIS: Show ALL work!!! 4. What is the percent sugar in your gum? 5. How many moles of sugar, C 6H 12O 6, did you chew? 6. How many molecules of sugar were in your gum? CONCLUSION: - Summarize the results of the lab activity Recreating, scanning, electronic copying, file sharing, redistributing, editing, selling, or posting this item (or any part thereof) on the Internet, or with others, is strictly prohibited. Violations are subject to the penalties of the Digital Millennium Copyright Act. James Lyas (Bond with James)

Emperical Formula What is an empirical formula? The of a compound, in simple terms, is a formula which has been to the lowest terms. Scientists can use the of a compound to calculate and determine the formula for that compound. Empirical Formula Calculation Steps 1. to Assume that you have a 100-gram sample of the compound. Therefore, convert the into. 2. to Convert grams to. 3. by Divide all the values calculated in # by the value calculated. 4. til Multiply all values from # by a number until each set produces a number. Begin with a small number and increase until you are able to get whole numbers 5. Use as and place. Use the whole numbers obtained in # as subscripts in order to write the empirical formula. List the elements in the order that. Don t be surprise if you have large subscripts as some molecules are very large. Emperical Formula What is an empirical formula? The of a compound, in simple terms, is a formula which has been to the lowest terms. Scientists can use the of a compound to calculate and determine the formula for that compound. Empirical Formula Calculation Steps 1. to Assume that you have a 100-gram sample of the compound. Therefore, convert the into. 2. to Convert grams to. 3. by Divide all the values calculated in # by the value calculated. 4. til Multiply all values from # by a number until each set produces a number. Begin with a small number and increase until you are able to get whole numbers 5. Use as and place. Use the whole numbers obtained in # as subscripts in order to write the empirical formula. List the elements in the order that. Don t be surprise if you have large subscripts as some molecules are very large. Recreating, scanning, electronic copying, file sharing, redistributing, editing, selling, or posting this item (or any part thereof) on the Internet, or with others, is strictly prohibited. Violations are subject to the penalties of the Digital Millennium Copyright Act. James Lyas (Bond with James)

Emperical Formula We do: Find the empirical formula for a compound which contains 26.8% Sn, 16.0% Cl and 57.2% I. You Do: NutraSweet is 57.14% C, 6.16% H, 9.52% N, and 27.18% O. Calculate the empirical formula of NutraSweet. Emperical Formula We do: Find the empirical formula for a compound which contains 26.8% Sn, 16.0% Cl and 57.2% I. You Do: NutraSweet is 57.14% C, 6.16% H, 9.52% N, and 27.18% O. Calculate the empirical formula of NutraSweet. Recreating, scanning, electronic copying, file sharing, redistributing, editing, selling, or posting this item (or any part thereof) on the Internet, or with others, is strictly prohibited. Violations are subject to the penalties of the Digital Millennium Copyright Act. James Lyas (Bond with James)

Molecular Formula What is a molecular formula? A molecular formula is the formula of a compound. Let us review some common empirical and molecular formulas below: Name Name Empirical Formula Molecular Formula Water H2O H2O Hydrogen peroxide HO H2O2 Glucose CH2O C6H12O6 Dinitrogen monoxide NO N2O4 Caffeine C4H5N2O C8H10N4O2 Based on the table above, how is the molecular formula different from the empirical formula? Based on the table above, can the molecular formula be identical (the same) as the empirical formula? Definition: The molecular formula may be the formula or it may a of the formula. Molecular Formula What is a molecular formula? A molecular formula is the formula of a compound. Let us review some common empirical and molecular formulas below: Name Empirical Formula Molecular Formula Water H2O H2O Hydrogen peroxide HO H2O2 Glucose CH2O C6H12O6 Dinitrogen monoxide NO N2O4 Caffeine C4H5N2O C8H10N4O2 Based on the table above, how is the molecular formula different from the empirical formula? Based on the table above, can the molecular formula be identical (the same) as the empirical formula? Definition: The molecular formula may be the formula or it may a of the formula. Recreating, scanning, electronic copying, file sharing, redistributing, editing, selling, or posting this item (or any part thereof) on the Internet, or with others, is strictly prohibited. Violations are subject to the penalties of the Digital Millennium Copyright Act. James Lyas (Bond with James)

Molecular Formula How do you determine the molecular formula? To determine the molecular formula of a compound, you must know the compound s formula and the of the compound. Molecular Formula Calculation Steps: 1. Determine the empirical formula IF it has NOT be given [review your empirical formula calculation notes]. 2. Calculate the of the empirical formula. 3. Use the molecular formula mass (usually given in the problem) and divide it by the empirical formula mass (calculated in Step 2). Molecular formula mass Empirical formula mass 4. Using the number calculated in Step 3, that number by the subscripts in the empirical formula to obtain the subscripts for the molecular formula. Practice Time! We Do: The empirical formula of a compound is C 4H 9. What is the molecular formula of this compound if the molar mass is 114 g/mol? You Do: What is the molecular formula of Nutrasweet if the molar mass of NutraSweet is 294.30 g/mol? **Review the You Do section of your Empirical Formula notes for the empirical formula of Nutrasweet (as this was calculated there). **Complete your work on the back of this sheet. =??? Molecular Formula How do you determine the molecular formula? To determine the molecular formula of a compound, you must know the compound s formula and the of the compound. Molecular Formula Calculation Steps: 5. Determine the empirical formula IF it has NOT be given [review your empirical formula calculation notes]. 6. Calculate the of the empirical formula. 7. Use the molecular formula mass (usually given in the problem) and divide it by the empirical formula mass (calculated in Step 2). Molecular formula mass Empirical formula mass 8. Using the number calculated in Step 3, that number by the subscripts in the empirical formula to obtain the subscripts for the molecular formula. Practice Time! We Do: The empirical formula of a compound is C 4H 9. What is the molecular formula of this compound if the molar mass is 114 g/mol? You Do: What is the molecular formula of Nutrasweet if the molar mass of NutraSweet is 294.30 g/mol? **Review the You Do section of your Empirical Formula notes for the empirical formula of Nutrasweet (as this was calculated there). **Complete your work on the back of this sheet. =??? Recreating, scanning, electronic copying, file sharing, redistributing, editing, selling, or posting this item (or any part thereof) on the Internet, or with others, is strictly prohibited. Violations are subject to the penalties of the Digital Millennium Copyright Act. James Lyas (Bond with James)

The Mole When you hear or read the phrase, The Mole, you might be inclined to think of a small burrowing animal or a secret agent. However, a mole in chemistry is a very important term and your understanding of this concept will be critical to your success. Before, we talk about what a mole in chemistry means, let us complete a quick activity Fill in the blanks: A dozen pencils = _12_ pencils A dozen cars = _12_ cars Data Table: Object Your choice Your choice Your choice Your choice Set 1 Mass (grams) 2 dozen apples = _24_apples 6 dozen birds = _72_birds Set 2 Mass (grams) Set 3 Mass (grams) Directions & Questions: 1. One at a time, separate each object into three different groups of a dozen. 2. Weigh each set and record in the data table above. 3. Answer the following questions on the back of this page. a. In general, what could be said about the mass of a dozen (select one of the choices from above to place here) b. Could the same rule be applied to the other 3 objects? Yes c. You had a dozen of each object. Did you have the same amount of each object? Yes, a dozen = 12 d. You had a dozen of each object. Did each set of objects have the same mass? No, the mass varied The Mole A mole is a counting unit. It is abbreviated mol and is a unit used in chemistry that allows us to deal with numbers of atoms, molecules, ions, or formula units in a sample of a substance. ***Chemists have define a mole as the number of carbon atoms in exactly 12g of pure carbon-12. Just like a dozen is equal to 12 of something and a pair is equal to 2 of something, chemists have established that a mole is equal to 6.02 x 10 23 of something In chemistry, the something refers to particles ( atoms, molecules, ions, or formula units) Just like the number 3.14159 has a name - pi (π), 6.02 x 10 23 has a name. It is called Avogadro s number. Now, would you say a dozen pencils weigh the same as a dozen cars? Of course not! While the amount of both objects is the same, we would expect the mass of a dozen pencils and cars to be different. A mole of anything represents the same amount (6.02 x 10 23 ) but it does NOT represent the same mass for all substances. The mole is the link between particles and grams. The MASS of 1 mole is equal to the molar mass of a substance. Quick Check: Take 2-3 minutes to complete the table below. Substance 1 mole of a substance Mass (g) Oxygen (O) 6.02 x 10 23 16.00 Bromine (Br) 6.02 x 10 23 79.90 Gold (Au) 6.02 x 10 23 196.97 Water (H 2O) 6.02 x 10 23 18.02 Sodium carbonate (Na 2CO 3) 6.02 x 10 23 105.99 Recreating, scanning, electronic copying, file sharing, redistributing, editing, selling, or posting this item (or any part thereof) on the Internet, or with others, is strictly prohibited. Violations are subject to the penalties of the Digital Millennium Copyright Act. James Lyas (Bond with James)

Useful conversion factors The Mole 1 mole = 6.02 x 10 23 particles (atoms, molecules, ions, formula units) 1 mole = grams (molar mass) of a substance We can write each conversion factor two ways the way in which one is used over another will depend on the dimensional analysis setup. 1 mole 6.02 x 10 23 particles 6.02 x 10 23 particles 1 mole 1 mole??? molar mass (g)??? molar mass (g) 1 mole Practice Problems I Do: How many grams are in 2.00 mol of NaCl? 2.00 mol NaCl 58.45 g NaCl = 116.88 g = 117 g NaCl 1 mole NaCl We Do: How many grams are in 4.95 mol of Na 3PO 4? 4.95 mol Na 3PO 4 163.94 g Na 3PO 4 = 811.503 g Na 3PO 4 1 mol Na 3PO 4 = 812 g Na 3PO 4 We Do: How many moles are in 7.14 grams of H 2O? 7.14 g H 2O 1 mol H 2O = 0.396 mol H 2O 18.02 g H 2O Formula Weights You may see the following terms: Formula Mass Molecular Mass Molar Mass These terms all pretty much refer to the same thing in regard to doing calculations. For now, let us refer to this concept as molar mass because this term will be important when doing a specific type of calculation in chemistry. These problems are pretty easy. You need to know two things: 1. How to find the mass of an element on the Periodic Table 2. How to count atoms in a chemical formula (ex: C6H12O6) I Do: What is the molar mass of glucose, C6H12O6? Atom # of Each Periodic Table Atomic Mass C 6 x 12.01 = H 12 x 1.01 = O 6 x 16.00 = Total 72.06 12.12 96.00 = 180.18 g/mol You Do: What is the molar mass of sodium sulfate, Na 2SO 4? Atom # of Each Periodic Table Atomic Mass Na 2 X 23.00 = S 1 X 32.01 = O 4 X 16.00 = Total 46.00 32.01 64.00 = 142.01 g/mol Recreating, scanning, electronic copying, file sharing, redistributing, editing, selling, or posting this item (or any part thereof) on the Internet, or with others, is strictly prohibited. Violations are subject to the penalties of the Digital Millennium Copyright Act. James Lyas (Bond with James)

Moles in my Signature Purpose: to determine the number of moles used to write my signature Materials: chalk, triple beam balance, other materials as needed Procedure: Data: 1. Obtain a piece of chalk and measure its mass on the triple beam balance. Record the mass in your data table. 2. Write your signature on a piece of paper (or you may be asked to write your signature outside on the concrete). 3. Measure the mass of your unused chalk on the triple beam balance. Chalk (CaCO 3) Calculations: Initial Mass Final Mass Mass of chalk used Molar Mass Based on the mass of the chalk used and its molar mass, determine the number of moles of chalk you used to write your signature. Show your work in the space provide below. This will vary depending on how you conduct the activity. Students may each receive a piece of chalk or work in pairs. You may also take them outside to write on the concrete or use a sheet of paper instead. Percent Composition The percent composition tells us the amount of a certain component within an item. Imaginary Pizza Scenario If you ate out of slices, what percentage of the pizza did you eat? Explain how you developed your answer? Real-Time Scenario (Male to Female Class Ratio) Count your classmates. Total: Male count Female count % of males % of females Code the appropriate number of boxes in the graphic on the right to illustrate this. Educational Scenario (Grade Calculation) You take a quiz that has 10 problems. You miss 3. What is your grade? 70% You take a test that has 36 problems. You miss s 8. What is your grade? 78% How did you come up with your answers? Percent Formula Part x 100 Whole Recreating, scanning, electronic copying, file sharing, redistributing, editing, selling, or posting this item (or any part thereof) on the Internet, or with others, is strictly prohibited. Violations are subject to the penalties of the Digital Millennium Copyright Act. James Lyas (Bond with James)

Percent Composition Information needed to calculate the percent composition of a substance: The total mass (may need to calculate the molar mass) The number of each type of atom The mass of each type of atom I Do: Calculate the percent composition of tetraphosphorus pentoxide. We Do: Calculate the percent composition of potassium sulfate. James Lyas (Bond with James) You Do: Calculate the percent composition of iron (III) oxide. James Lyas (Bond with James) Review the previous three examples. Which is a better source of oxygen? Explain why. P 4O 5 because it contains a higher % of oxygen per compound compared to K 2SO 4 and Fe 2O 3 Percent Composition Activity OBJECTIVE: To determine the percent of sugar in an ordinary piece of bubble gum. PURPOSE: - Why are you doing this lab (in 1 to 2 sentences) - Must be stated in your own words MATERIALS: - List of all the materials used in your experiment PROCEDURE: - A step-by-step account of how you carried out your experiment. DATA: - Include a data table to showcase the data collected during the lab. CALCULATIONS: - Show all calculations that you did using the data collected during the lab. ANALYSIS: Show ALL work!!! 1. What is the percent sugar in your gum? 2. How many moles of sugar, C 6H 12O 6, did you chew? 3. How many molecules of sugar were in your gum? CONCLUSION: - Summarize the results of the lab activity Recreating, scanning, electronic copying, file sharing, redistributing, editing, selling, or posting this item (or any part thereof) on the Internet, or with others, is strictly prohibited. Violations are subject to the penalties of the Digital Millennium Copyright Act. James Lyas (Bond with James)

Emperical Formula What is an empirical formula? The empirical formula of a compound, in simple terms, is a formula which has been reduced to the lowest terms. Scientists can use the empirical formula of a compound to calculate and determine the formula for that compound. Empirical Formula Calculation Steps 1. Percent to mass Assume that you have a 100-gram sample of the compound. Therefore, convert the percent into grams. 2. Mass to mole Convert grams to moles. 3. Divide by small Divide all the values calculated in # 2 by the smallest value calculated. 4. Multiply til whole Multiply all values from # 3 by a number until each set produces a whole number. Begin with a small number and increase until you are able to get whole numbers 5. Use as subscripts and place below. Use the whole numbers obtained in #4 as subscripts in order to write the empirical formula. List the elements in the order that they appear in the problem (in most cases). Don t be surprise if you have large subscripts as some molecules are very large. Emperical Formula We do: Find the empirical formula for a compound which contains 26.8% Sn, 16.0% Cl and 57.2% I. James Lyas (Bond with James) You Do: NutraSweet is 57.14% C, 6.16% H, 9.52% N, and 27.18% O. Calculate the empirical formula of NutraSweet. James Lyas (Bond with James) Recreating, scanning, electronic copying, file sharing, redistributing, editing, selling, or posting this item (or any part thereof) on the Internet, or with others, is strictly prohibited. Violations are subject to the penalties of the Digital Millennium Copyright Act. James Lyas (Bond with James)

Molecular Formula What is a molecular formula? A molecular formula is the actual formula of a compound. Let us review some common empirical and molecular formulas below: Name Empirical Formula Molecular Formula Water H2O H2O Hydrogen peroxide HO H2O2 Glucose CH2O C6H12O6 Dinitrogen monoxide NO N2O4 Caffeine C4H5N2O C8H10N4O2 Based on the table above, how is the molecular formula different from the empirical formula? From the table above, the molecular formulas, for most of the compounds are a whole number multiple (of the subscripts) of the empirical formula. Based on the table above, can the molecular formula be identical (the same) as the empirical formula? The molecular and empirical formulas may be identical for some compounds. Definition: The molecular formula may be the actual formula or it may a whole number multiple of the empirical formula. Molecular Formula How do you determine the molecular formula? To determine the molecular formula of a compound, you must know the compound s empirical formula and the molar mass of the compound. Molecular Formula Calculation Steps: 1. Determine the empirical formula IF it has NOT be given [review your empirical formula calculation notes]. 2. Calculate the molar mass of the empirical formula. 3. Use the molecular formula mass (usually given in the problem) and divide it by the empirical formula mass (calculated in Step 2). Molecular formula mass Empirical formula mass 4. Using the number calculated in Step 3, multiply that number by the subscripts in the empirical formula to obtain the subscripts for the molecular formula. Practice Time! We Do: The empirical formula of a compound is C 4H 9. What is the molecular formula of this compound if the molar mass is 114 g/mol? James Lyas (Bond with James) =??? You Do: What is the molecular formula of Nutrasweet if the molar mass of NutraSweet is 294.30 g/mol? James Lyas (Bond with James) Recreating, scanning, electronic copying, file sharing, redistributing, editing, selling, or posting this item (or any part thereof) on the Internet, or with others, is strictly prohibited. Violations are subject to the penalties of the Digital Millennium Copyright Act. James Lyas (Bond with James)

Hexagon Mole Fold IGO (pg. 28) This IGO comes 1 page per 2 students. It is also pre-filled with information, unless you wish to add more to it. Students may use this to assist them during 1 or 2 step mole conversions Tape or glue bottom here

1-2 Step Mole Conversions (?) molar mass (must calculate for each substance) 1 mole 6.02 x 10 23 (particles, atoms, molecules, formula units, ions) Tape/glue behind here 1-2 Step Mole Conversions (?) molar mass (must calculate for each substance) 1 mole 6.02 x 10 23 (particles, atoms, molecules, formula units, ions) Tape/glue behind here Recreating, scanning, electronic copying, file sharing, redistributing, editing, selling, or posting this item (or any part thereof) on the Internet, or with others, is strictly prohibited. Violations are subject to the penalties of the Digital Millennium Copyright Act. James Lyas (Bond with James)

Mole Pyramid IGO (pg. 30) This IGO comes 1 page per 2 students. The directions are also included on the page for students to follow. Pictures A and B: Fold section #1 behind section #2. Picture C: Fold section #2 behind section #3. Pictures D and E: Fold section #3 behind section #4. Picture F: Finally, unfold the organizer and place section #1 directly behind section #4 to form a pyramid. Tape or glue the tab The Mole Concept into the notebook.

Directions: Cut along the dotted lines only. 1 st : Fold section #1 behind section #2. 2 nd : Fold section #2 behind section #3. 3 rd : Fold section #3 behind section #4. Finally, unfold the organizer and place section #1 directly behind section #4 to form a pyramid. Tape or glue the tab The Mole Concept into your notebook. Recreating, scanning, electronic copying, file sharing, redistributing, editing, selling, or posting this item (or any part thereof) on the Internet, or with others, is strictly prohibited. Violations are subject to the penalties of the Digital Millennium Copyright Act. James Lyas (Bond with James) Directions: Cut along the dotted lines only. 1 st : Fold section #1 behind section #2. 2 nd : Fold section #2 behind section #3. 3 rd : Fold section #3 behind section #4. Finally, unfold the organizer and place section #1 directly behind section #4 to form a pyramid. Tape or glue the tab The Mole Concept into your notebook. Recreating, scanning, electronic copying, file sharing, redistributing, editing, selling, or posting this item (or any part thereof) on the Internet, or with others, is strictly prohibited. Violations are subject to the penalties of the Digital Millennium Copyright Act. James Lyas (Bond with James)

Empirical Formula & Molecular Formula Fold IGO (pg. 32-33) Use the Steps provided in the Half-sheet notes to fill in the blanks on both tabs. The information on the front face could be used to write the definitions of the empirical and molecular formulas. Make sure to cut along the small dotted line shown here in order for the IGO to properly fold in.

C 6 H 12 O 6 Molecular Formula Glue within the 4 circles or as instructed by your teacher. James Lyas (Bond with James) Empirical Formula CH 2 O Recreating, scanning, electronic copying, file sharing, redistributing, editing, selling, or posting this item (or any part thereof) on the Internet, or with others, is strictly prohibited. Violations are subject to the penalties of the Digital Millennium Copyright Act. James Lyas (Bond with James)

Recreating, scanning, electronic copying, file sharing, redistributing, editing, selling, or posting this item (or any part thereof) on the Internet, or with others, is strictly prohibited. Violations are subject to the penalties of the Digital Millennium Copyright Act. James Lyas (Bond with James) Empirical Formula Step 1: Step 2: Step 3: Step 4: Step 5: Example: Automobile antifreeze is composed of 38.7% carbon, 9.7% hydrogen, and 51.6% oxygen. The molar mass of this compound is 62.1 g/mol. Determine the empirical and molecular formulas of this compound. Step 1: Step 2: Step 3: Step 4: Molecular Formula

Empirical Formula Layered Pyramid IGO (pg. 35) This IGO comes 1 page per student. Place the largest piece into the notebook first and then layer until the smallest piece is on top. You may glue the bottom piece in or tape it at the bottom to create a layering effect. You will need to do this for each piece. Students may write notes concerning each step on the backside of each layer. They may even work a short empirical formula problem behind the last layer as students should have space to write directly on the back of the layer and on the notebook paper.

x 4 x 3 x 2 Multiple til Whole James Lyas (Bond with James) Percent to Mass Recreating, scanning, electronic copying, file sharing, redistributing, editing, selling, or posting this item (or any part thereof) on the Internet, or with others, is strictly prohibited. Violations are subject to the penalties of the Digital Millennium Copyright Act. James Lyas (Bond with James)

Mole Flaps IGO (pgs. 40-41) Cut along the dotted lines only this is important to create the small tab shown at the very top. You may label the top: Start with and End with as shown in the picture. You may print this sheet front and back; or you may print out the side with MOLES written on it and have students write on the 3 units on the outside flap instead. This IGO prints 1 page per student regardless of the method in which you decide to print the sheet.

Example problem: How many liters are represented in 150.0 g CO 2 at STP? Step 1: The problem starts with mass (150.0 g CO 2 ). Therefore, select the Mass (grams) tab under the Start with column Step 2: While not indicated, these are all equalities equaling 1 mole of a substance How does this work? Step 3: Problem asks for liters. Therefore, select the Volume of a Gas tab under the End With column

Example #2: How many atoms are in 10.0 grams of Aluminum? Step 1: The problem starts with mass (10.0 g Al). Therefore, select the Mass (grams) tab under the Start with column Step 2: While not indicated, these are all equalities equaling 1 mole of a substance How does this work? Step 3: Problem asks for atoms. Therefore, select the Representative Particles tab under the End With column

Will not work for these types of questions: The IGO does not account for problems such as these. Only specific to the units on the foldable. How many oxygen atoms are present in 0.714 mole of SO 3 How many atoms are in 0.010 g CaCO 3?

Divide by M Multiply by x P R I N T O N F R O N T 22.4 L/mol Divide by 6.02 x 10 23 (Avogadro s number) Divide by Molar mass (g/mol) O L E S 22.4 L/mol Multiply by x 6.02 x 10 23 (Avogadro s number) Multiply by x Molar mass (g/mol) P R I N T O N F R O N T

Volume of a gas at STP (liters) Volume of a gas at STP (liters) P R I N T O N B A C K Representative Particles (atoms, molecules, formula units) Representative Particles (atoms, molecules, formula units) P R I N T O N B A C K Mass (grams) Mass (grams)