Chapter 7 Chemical Formulas and Chemical Compounds Table of Contents Section 3 Using Chemical Formulas Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Section 3 Using Chemical Formulas Objectives • Calculate the formula mass or molar mass of any given compound. • Use molar mass to convert between mass in grams and amount in moles of a chemical compound. • Calculate the number of molecules, formula units, or ions in a given molar amount of a chemical compound. • Calculate the percentage composition of a given chemical compound. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Section 3 Using Chemical Formulas • A chemical formula indicates: • the elements present in a compound • the relative number of atoms or ions of each element present in a compound • Chemical formulas also allow chemists to calculate a number of other characteristic values for a compound: • formula mass • molar mass • percentage composition Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Section 3 Using Chemical Formulas Formula Masses • The formula mass of any molecule, formula unit, or ion is the sum of the average atomic masses of all atoms represented in its formula. • example: formula mass of water, H2O average atomic mass of H: 1.01 amu average atomic mass of O: 16.00 amu average mass of H2O molecule: 18.02 amu Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Section 3 Using Chemical Formulas Formula Masses • The mass of a water molecule can be referred to as a molecular mass. • The mass of one formula unit of an ionic compound, such as NaCl, is not a molecular mass. • The mass of any unit represented by a chemical formula (H2O, NaCl) can be referred to as the formula mass. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Visual Concepts Formula Mass Click below to watch the Visual Concept. http://my.hrw.com/sh/hc6_003036809x/student/ch0 Visual Concept 7/sec03/vc00/hc607_03_v00fs.htm Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Section 3 Using Chemical Formulas Formula Masses, continued Sample Problem F Find the formula mass of potassium chlorate, KClO3. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Section 3 Using Chemical Formulas Formula Masses, continued Sample Problem F Solution The mass of a formula unit of KClO3 is found by adding the masses of one K atom, one Cl atom, and three O atoms. Atomic masses can be found in the periodic table in the back of your book. In your calculations, round each atomic mass to two decimal places. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Section 3 Using Chemical Formulas Formula Masses, continued Sample Problem F Solution, continued formula mass of KClO3 = 122.55 amu Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Visual Concepts Formula Mass Problem Calculation Click below to watch the PROBLEM ACTIVITY. PROBLEM ACTIVITY Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Practice Problems pg. 238 • Complete the following problems. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Visual Concepts The Mole Click below to watch the Visual Concept. http://my.hrw.com/sh/hc6_003036809x/stude Visual Concept nt/ch07/sec03/vc01/hc607_03_v01fs.htm Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Section 3 Using Chemical Formulas Molar Masses • The molar mass of a substance is equal to the mass in grams of one mole, or approximately 6.022 1023 particles, of the substance. • example: the molar mass of pure calcium, Ca, is 40.08 g/mol because one mole of calcium atoms has a mass of 40.08 g. • The molar mass of a compound is calculated by adding the masses of the elements present in a mole of the molecules or formula units that make up the compound. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Section 3 Using Chemical Formulas Molar Masses, continued • One mole of water molecules contains exactly two moles of H atoms and one mole of O atoms. The molar mass of water is calculated as follows. molar mass of H2O molecule: 18.02 g/mol • A compound’s molar mass is numerically equal to its formula mass. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Visual Concepts Molar Mass Click below to watch the Visual Concept. http://my.hrw.com/sh/hc6_003036809x/student/ch Visual Concept 07/sec03/vc02/hc607_03_v02fs.htm Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Section 3 Using Chemical Formulas Calculating Molar Masses for Ionic Compounds Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Section 3 Using Chemical Formulas Molar Masses, continued Sample Problem G What is the molar mass of barium nitrate, Ba(NO3)2? Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Section 3 Using Chemical Formulas Molar Masses, continued Sample Problem G Solution One mole of barium nitrate, contains one mole of Ba, two moles of N (1 2), and six moles of O (3 2). molar mass of Ba(NO3)2 = 261.35 g/mol Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Visual Concepts Molar Mass Calculation Click below to watch the Problem Activity. PROBLEM ACTIVITY Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Practice Problems pg. 239 Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Section 3 Using Chemical Formulas Molar Mass as a Conversion Factor • The molar mass of a compound can be used as a conversion factor to relate an amount in moles to a mass in grams for a given substance. • To convert moles to grams, multiply the amount in moles by the molar mass: Amount in moles molar mass (g/mol) = mass in grams Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Section 3 Using Chemical Formulas Mole-Mass Calculations Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Visual Concepts Molar Mass as a Conversion Factor Click below to watch the Visual Concept. http://my.hrw.com/sh/hc6_003036809x/s Visual Concept tudent/ch07/sec03/vc03/hc607_03_v03fs .htm Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Section 3 Using Chemical Formulas Molar Mass as a Conversion Factor, continued Sample Problem H What is the mass in grams of 2.50 mol of oxygen gas? Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Section 3 Using Chemical Formulas Molar Mass as a Conversion Factor, continued Sample Problem H Solution Given: 2.50 mol O2 Unknown: mass of O2 in grams Solution: moles O2 grams O2 amount of O2 (mol) molar mass of O2 (g/mol) = mass of O2 (g) Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Section 3 Using Chemical Formulas Molar Mass as a Conversion Factor, continued Sample Problem H Solution, continued Calculate the molar mass of O2. Use the molar mass of O2 to convert moles to mass. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Section 3 Using Chemical Formulas Converting Between Amount in Moles and Number of Particles Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Section 3 Using Chemical Formulas Molar Mass as a Conversion Factor, continued Sample Problem I Ibuprofen, C13H18O2, is the active ingredient in many nonprescription pain relievers. Its molar mass is 206.31 g/mol. a. If the tablets in a bottle contain a total of 33 g of ibuprofen, how many moles of ibuprofen are in the bottle? b. How many molecules of ibuprofen are in the bottle? c. What is the total mass in grams of carbon in 33 g of ibuprofen? Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Section 3 Using Chemical Formulas Molar Mass as a Conversion Factor, continued Sample Problem I Solution Given: 33 g of C13H18O2 molar mass 206.31 g/mol Unknown: a. moles C13H18O2 b. molecules C13H18O2 c. total mass of C Solution: a. grams moles Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Section 3 Using Chemical Formulas Molar Mass as a Conversion Factor, continued Sample Problem I Solution, continued b. moles c. moles C13H18O2 molecules moles C Chapter menu grams C Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Section 3 Using Chemical Formulas Molar Mass as a Conversion Factor, continued Sample Problem I Solution, continued a. b. c. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Practice Problems pg. 242 • Complete the practice problems in your notes before going to the next slide. Show ALL work as always! Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 ANSWERS pg. 242 • Be sure you have shown all of your work before checking answers. Note values may be rounded to significant figures, so your answer may be slightly different. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Visual Concepts Molecular Mass Problem Calculation Do this problem if you still need help. Click below to watch the PROBLEM ACTIVITY. PROBLEM ACTIVITY Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. 7.3 Percent Composition and Chemical Formulas It helps to know the percents of the components in a shirt because they affect how warm it is, whether it will need to be ironed, and how it should be cleaned. You will learn how the percents of the elements in a compound are important in chemistry. Slide of 40 35 © Copyright Pearson Prentice Hall End Show 7.3 Percent Composition and Chemical Formulas > The Percent Composition of a Compound The Percent Composition of a Compound How do you calculate the percent by mass of an element in a compound? Slide of 40 36 © Copyright Pearson Prentice Hall End Show Chapter 7 Section 3 Using Chemical Formulas Percentage Composition • It is often useful to know the percentage by mass of a particular element in a chemical compound. • To find the mass percentage of an element in a compound, the following equation can be used. • The mass percentage of an element in a compound is the same regardless of the sample’s size. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Section 3 Using Chemical Formulas Percentage Composition, continued • The percentage of an element in a compound can be calculated by determining how many grams of the element are present in one mole of the compound. • The percentage by mass of each element in a compound is known as the percentage composition of the compound. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. 7.3 Percent Composition and Chemical Formulas > The Percent Composition of a Compound The percent by mass of an element in a compound is the number of grams of the element divided by the mass in grams of the compound, multiplied by 100%. Slide of 40 39 © Copyright Pearson Prentice Hall End Show Chapter 7 Section 3 Using Chemical Formulas Percentage Composition of Iron Oxides Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Visual Concepts Percentage Composition Click below to watch the Visual Concept. http://my.hrw.com/sh/hc6_003036809x/student/ch Visual Concept 07/sec03/vc04/hc607_03_v04fs.htm Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. 7.3 Percent Composition and Chemical Formulas > The Percent Composition of a Compound Percent Composition from Mass Data The relative amounts of the elements in a compound are expressed as the percent composition or the percent by mass of each element in the compound. Slide of 40 42 © Copyright Pearson Prentice Hall End Show Chapter 7 BUBBLICIOUS SONG AND BUBBLEGUM LAB • PLAY THE BUBBLICIOUS SONG AND COMPLETE THE BUBBLEGUM LAB FOR PERCENTAGE COMPOSITION. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Visual Concepts Percentage Composition PROBLEM ACTIVITY Click below to watch the PROBLEM ACTIVITY. PROBLEM ACTIVITY Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Section 3 Using Chemical Formulas Percentage Composition Calculations Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Section 3 Using Chemical Formulas Percentage Composition, continued Sample Problem J Find the percentage composition of copper(I) sulfide, Cu2S. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Section 3 Using Chemical Formulas Percentage Composition, continued Sample Problem J Solution Given: formula, Cu2S Unknown: percentage composition of Cu2S Solution: formula molar mass mass percentage of each element Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Section 3 Using Chemical Formulas Percentage Composition, continued Sample Problem J Solution, continued Molar mass of Cu2S = 159.2 g Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Section 3 Using Chemical Formulas Percentage Composition, continued Sample Problem J Solution, continued Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 Practice Problems pg. 244 • Complete practice problems pg. 244 #1-2 only in your notes. Show all of your work before checking answers on the next slide. You must show work to get any credit also. Rounding might cause answers to be slightly off. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 7 ANSWERS pg. 244 Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Online Self-Check Quiz Complete the online Quiz and record answers. Ask if you have any questions about your answers. click here for online Quiz 7.3 (7 questions) You must be in the “Play mode” for the slideshow for hyperlink to work. Slide of 25 © Copyright Pearson Prentice Hall End Show VIDEOS FOR ADDITIONAL INSTRUCTION Additional Videos for Section 7.3: Using Chemical Formulas Molar Mass Slide of 28 © Copyright Pearson Prentice Hall End Show End of Chapter 7.3 Show Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved.