1 / 73

Chapter Menu

The Mole. Section 10.1 Measuring Matter Section 10.2 Mass and the Mole Section 10.3 Moles of Compounds Section 10.4 Empirical and Molecular Formulas Section 10.5 Formulas of Hydrates. Click a hyperlink or folder tab to view the corresponding slides. Exit. Chapter Menu.

orla-simmons
Download Presentation

Chapter Menu

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. The Mole Section 10.1Measuring Matter Section 10.2Mass and the Mole Section 10.3Moles of Compounds Section 10.4Empirical and Molecular Formulas Section 10.5 Formulas of Hydrates Click a hyperlink or folder tab to view the corresponding slides. Exit Chapter Menu

  2. Section 10.1 Measuring Matter Explain how a mole is used to indirectly count the number of particles of matter. molecule: two or more atoms that covalently bond together to form a unit Relate the mole to a common everyday counting unit. Convert between moles and number of representative particles. mole Avogadro’s number Chemists use the mole to count atoms, molecules, ions, and formula units. Section 10-1

  3. Counting Particles Chemists need a convenient method for accurately counting the number of atoms, molecules, or formula units of a substance. The mole is the SI base unit used to measure the amount of a substance. 1 mole is the amount of atoms in 12 g of pure carbon-12, or 6.02  1023 atoms. The number is called Avogadro’s number. Section 10-1

  4. Converting Between Moles and Particles Conversion factors must be used. Moles to particles Number of molecules in 3.50 mol of sucrose Section 10-1

  5. Converting Between Moles and Particles (cont.) Particles to moles Use the inverse of Avogadro’s number as the conversion factor. Section 10-1

  6. A B C D Section 10.1 Assessment What does the mole measure? A.mass of a substance B.amount of a substance C.volume of a gas D.density of a gas Section 10-1

  7. A B C D What is the conversion factor for determining the number of moles of a substance from a known number of particles? A. B. C.1 particle  6.02  1023 D.1 mol  6.02  1023particles Section 10.1 Assessment Section 10-1

  8. End of Section 10-1

  9. Section 10.2 Mass and the Mole Relate the mass of an atom to the mass of a mole of atoms. conversion factor: a ratio of equivalent values used to express the same quantity in different units Convert between number of moles and the mass of an element. Convert between number of moles and number of atoms of an element. molar mass A mole always contains the same number of particles; however, moles of different substances have different masses. Section 10-2

  10. The Mass of a Mole 1 mol of copper and 1 mol of carbon have different masses. One copper atom has a different mass than 1 carbon atom. Section 10-2

  11. The Mass of a Mole (cont.) Molar mass is the mass in grams of one mole of any pure substance. The molar mass of any element is numerically equivalent to its atomic mass and has the units g/mol. Section 10-2

  12. Using Molar Mass Moles to mass 3.00 moles of copper has a mass of 191 g. Section 10-2

  13. Using Molar Mass (cont.) Convert mass to moles with the inverse molar mass conversion factor. Convert moles to atoms with Avogadro’s number as the conversion factor. Section 10-2

  14. Using Molar Mass (cont.) This figure shows the steps to complete conversions between mass and atoms. Section 10-2

  15. A B C D Section 10.2 Assessment The mass in grams of 1 mol of any pure substance is: A.molar mass B.Avogadro’s number C.atomic mass D.1 g/mol Section 10-2

  16. A B C D Section 10.2 Assessment Molar mass is used to convert what? A.mass to moles B.moles to mass C.atomic weight D.particles Section 10-2

  17. End of Section 10-2

  18. Section 10.3 Moles of Compounds Recognize the mole relationships shown by a chemical formula. Calculate the molar mass of a compound. Convert between the number of moles and mass of a compound. Apply conversion factors to determine the number of atoms or ions in a known mass of a compound. representative particle: an atom, molecule, formula unit, or ion Section 10-3

  19. Section 10.3 Moles of Compounds (cont.) The molar mass of a compound can be calculated from its chemical formula and can be used to convert from mass to moles of that compound. Section 10-3

  20. Chemical Formulas and the Mole Chemical formulas indicate the numbers and types of atoms contained in one unit of the compound. One mole of CCl2F2 contains one mole of C atoms, two moles of Cl atoms,and two moles of F atoms. Section 10-3

  21. The Molar Mass of Compounds The molar mass of a compound equals the molar mass of each element, multiplied by the moles of that element in the chemical formula, added together. The molar mass of a compound demonstrates the law of conservation of mass. Section 10-3

  22. Converting Moles of a Compound to Mass For elements, the conversion factor is the molar mass of the compound. The procedure is the same for compounds, except that you must first calculate the molar mass of the compound. Section 10-3

  23. Converting the Mass of a Compound to Moles The conversion factor is the inverse of the molar mass of the compound. Section 10-3

  24. Converting the Mass of a Compound to Number of Particles Convert mass to moles of compound with the inverse of molar mass. Convert moles to particles with Avogadro’s number. Section 10-3

  25. Converting the Mass of a Compound to Number of Particles (cont.) This figure summarizes the conversions between mass, moles, and particles. Section 10-3

  26. A B C D Section 10.3 Assessment How many moles of OH— ions are in 2.50 moles of Ca(OH)2? A.2.00 B.2.50 C.4.00 D.5.00 Section 10-3

  27. A B C D Section 10.3 Assessment How many particles of Mg are in 10 moles of MgBr2? A.6.02  1023 B.6.02  1024 C.1.20  1024 D.1.20  1025 Section 10-3

  28. End of Section 10-3

  29. Section 10.4 Empirical and Molecular Formulas Explain what is meant by the percent composition of a compound. percent by mass: the ratio of the mass of each element to the total mass of the compound expressed as a percent Determine the empirical and molecular formulas for a compound from mass percent and actual mass data. percent composition empirical formula molecular formula A molecular formula of a compound is a whole-number multiple of its empirical formula. Section 10-4

  30. Percent Composition The percent by mass of any element in a compound can be found by dividing the mass of the element by the mass of the compound and multiplying by 100. Section 10-4

  31. Percent Composition (cont.) The percent by mass of each element in a compound is the percent composition of a compound. Percent composition of a compound can also be determined from its chemical formula. Section 10-4

  32. Empirical Formula The empirical formulafor a compound is the smallest whole-number mole ratio of the elements. • You can calculate the empirical formula from percent by mass by assuming you have 100.00 g of the compound. Then, convert the mass of each element to moles. • The empirical formula may or may not be the same as the molecular formula. Molecular formula of hydrogen peroxide = H2O2 Empirical formula of hydrogen peroxide = HO Section 10-4

  33. Molecular Formula The molecular formula specifies the actual number of atoms of each element in one molecule or formula unit of the substance. Molecular formula is always a whole-number multiple of the empirical formula. Section 10-4

  34. Molecular Formula (cont.) Section 10-4

  35. A B C D Section 10.4 Assessment What is the empirical formula for the compound C6H12O6? A.CHO B.C2H3O2 C.CH2O D.CH3O Section 10-4

  36. A B C D Section 10.4 Assessment Which is the empirical formula for hydrogen peroxide? A.H2O2 B.H2O C.HO D.none of the above Section 10-4

  37. End of Section 10-4

  38. Section 10.5 Formulas of Hydrates Explain what a hydrate is and relate the name of the hydrate to its composition. crystal lattice:a three-dimensional geometric arrangement of particles Determine the formula of a hydrate from laboratory data. hydrate Hydrates are solid ionic compounds in which water molecules are trapped. Section 10-5

  39. Naming Hydrates A hydrate is a compound that has a specific number of water molecules bound to its atoms. The number of water molecules associated with each formula unit of the compound is written following a dot. Sodium carbonate decahydrate = Na2CO3 • 10H2O Section 10-5

  40. Naming Hydrates (cont.) Section 10-5

  41. Analyzing a Hydrate When heated, water molecules are released from a hydrate leaving an anhydrous compound. To determine the formula of a hydrate, find the number of moles of water associated with 1 mole of hydrate. Section 10-5

  42. Analyzing a Hydrate (cont.) Weigh hydrate. Heat to drive off the water. Weigh the anhydrous compound. Subtract and convert the difference to moles. The ratio of moles of water to moles of anhydrous compound is the coefficient for water in the hydrate. Section 10-5

  43. Use of Hydrates Anhydrous forms of hydrates are often used to absorb water, particularly during shipment of electronic and optical equipment. In chemistry labs, anhydrous forms of hydrates are used to remove moisture from the air and keep other substances dry. Section 10-5

  44. A B C D Section 10.5 Assessment Heating a hydrate causes what to happen? A.Water is driven from the hydrate. B.The hydrate melts. C.The hydrate conducts electricity. D.There is no change in the hydrate. Section 10-5

  45. A B C D Section 10.5 Assessment A hydrate that has been heated and the water driven off is called: A.dehydrated compound B.antihydrated compound C.anhydrous compound D.hydrous compound Section 10-5

  46. End of Section 10-5

  47. Chemistry Online Study Guide Chapter Assessment Standardized Test Practice Image Bank Concepts in Motion Resources Menu

  48. Section 10.1 Measuring Matter Key Concepts The mole is a unit used to count particles of matter indirectly. One mole of a pure substance contains Avogadro’s number of particles. Representative particles include atoms, ions, molecules, formula units, electrons, and other similar particles. One mole of carbon-12 atoms has a mass of exactly 12 g. Conversion factors written from Avogadro’s relationship can be used to convert between moles and number of representative particles. Study Guide 1

  49. Section 10.2 Mass and the Mole Key Concepts The mass in grams of 1 mol of any pure substance is called its molar mass. The molar mass of an element is numerically equal to its atomic mass. The molar mass of any substance is the mass in grams of Avogadro’s number of representative particles of the substance. Molar mass is used to convert from moles to mass. The inverse of molar mass is used to convert from mass to moles. Study Guide 2

More Related