Cmc chapter 10

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 Exit Click a hyperlink or folder tab to view the corresponding slides.

Section 10-1 Section 10.1 Measuring Matter ,[object Object],molecule: two or more atoms that covalently bond together to form a unit mole Avogadro’s number ,[object Object],[object Object],Chemists use the mole to count atoms, molecules, ions, and formula units.

Section 10-1 Counting Particles ,[object Object],[object Object],[object Object],[object Object]

Section 10-1 Converting Between Moles and Particles ,[object Object],[object Object],Number of molecules in 3.50 mol of sucrose

Section 10-1 Converting Between Moles and Particles (cont.) ,[object Object],[object Object]

[object Object],[object Object],[object Object],[object Object],Section 10-1 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

[object Object],[object Object],[object Object],[object Object],Section 10-1 Section 10.1 Assessment 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  10 23 D. 1 mol  6.02  10 23 particles

Section 10-2 Section 10.2 Mass and the Mole ,[object Object],conversion factor: a ratio of equivalent values used to express the same quantity in different units molar mass ,[object Object],[object Object],A mole always contains the same number of particles; however, moles of different substances have different masses.

Section 10-2 The Mass of a Mole ,[object Object],[object Object]

Section 10-2 The Mass of a Mole (cont.) ,[object Object],[object Object]

Section 10-2 Using Molar Mass ,[object Object],3.00 moles of copper has a mass of 191 g.

Section 10-2 Using Molar Mass (cont.) ,[object Object],[object Object]

Section 10-2 Using Molar Mass (cont.) ,[object Object]

[object Object],[object Object],[object Object],[object Object],Section 10-2 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

[object Object],[object Object],[object Object],[object Object],Section 10-2 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 10-3 Section 10.3 Moles of Compounds ,[object Object],representative particle: an atom, molecule, formula unit, or ion ,[object Object],[object Object],[object Object]

Section 10-3 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 Chemical Formulas and the Mole ,[object Object],[object Object]

Section 10-3 The Molar Mass of Compounds ,[object Object],[object Object]

Section 10-3 Converting Moles of a Compound to Mass ,[object Object],[object Object]

Section 10-3 Converting the Mass of a Compound to Moles ,[object Object]

Section 10-3 Converting the Mass of a Compound to Number of Particles ,[object Object],[object Object]

Section 10-3 Converting the Mass of a Compound to Number of Particles (cont.) ,[object Object]

[object Object],[object Object],[object Object],[object Object],Section 10-3 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

[object Object],[object Object],[object Object],[object Object],Section 10-3 Section 10.3 Assessment How many particles of Mg are in 10 moles of MgBr 2 ? A. 6.02  10 23 B. 6.02  10 24 C. 1.20  10 24 D. 1.20  10 25

Section 10-4 Section 10.4 Empirical and Molecular Formulas ,[object Object],percent by mass: the ratio of the mass of each element to the total mass of the compound expressed as a percent percent composition empirical formula molecular formula ,[object Object],A molecular formula of a compound is a whole-number multiple of its empirical formula.

Section 10-4 Percent Composition ,[object Object]

Section 10-4 Percent Composition (cont.) ,[object Object],[object Object]

Section 10-4 Empirical Formula ,[object Object],[object Object],[object Object],[object Object],[object Object]

Section 10-4 Molecular Formula ,[object Object],[object Object]

Section 10-4 Molecular Formula (cont.)

[object Object],[object Object],[object Object],[object Object],Section 10-4 Section 10.4 Assessment What is the empirical formula for the compound C 6 H 12 O 6 ? A. CHO B. C 2 H 3 O 2 C. CH 2 O D. CH 3 O

[object Object],[object Object],[object Object],[object Object],Section 10-4 Section 10.4 Assessment Which is the empirical formula for hydrogen peroxide? A. H 2 O 2 B. H 2 O C. HO D. none of the above

Section 10-5 Section 10.5 Formulas of Hydrates ,[object Object],crystal lattice: a three-dimensional geometric arrangement of particles hydrate ,[object Object],Hydrates are solid ionic compounds in which water molecules are trapped.

Section 10-5 Naming Hydrates ,[object Object],[object Object],[object Object]

Section 10-5 Naming Hydrates (cont.)

Section 10-5 Analyzing a Hydrate ,[object Object],[object Object]

Section 10-5 Analyzing a Hydrate (cont.) ,[object Object],[object Object],[object Object],[object Object],[object Object]

Section 10-5 Use of Hydrates ,[object Object],[object Object]

[object Object],[object Object],[object Object],[object Object],Section 10-5 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.

[object Object],[object Object],[object Object],[object Object],Section 10-5 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

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

Study Guide 1 Section 10.1 Measuring Matter Key Concepts ,[object Object],[object Object],[object Object],[object Object]

Study Guide 2 Section 10.2 Mass and the Mole Key Concepts ,[object Object],[object Object],[object Object],[object Object]

Study Guide 3 Section 10.3 Moles of Compounds Key Concepts ,[object Object],[object Object],[object Object]

Study Guide 4 Section 10.4 Empirical and Molecular Formulas Key Concepts ,[object Object],[object Object],[object Object],[object Object]

Study Guide 5 Section 10.5 Formulas of Hydrates Key Concepts ,[object Object],[object Object],[object Object]

[object Object],[object Object],[object Object],[object Object],Chapter Assessment 1 What does Avogadro’s number represent? A. the number of atoms in 1 mol of an element B. the number of molecules in 1 mol of a compound C. the number of Na + ions in 1 mol of NaCl (aq) D. all of the above

[object Object],[object Object],[object Object],[object Object],Chapter Assessment 2 The molar mass of an element is numerically equivalent to what? A. 1 amu B. 1 mole C. its atomic mass D. its atomic number

[object Object],[object Object],[object Object],[object Object],Chapter Assessment 3 How many moles of hydrogen atoms are in one mole of H 2 O 2 ? A. 1 B. 2 C. 3 D. 0.5

[object Object],[object Object],[object Object],[object Object],Chapter Assessment 4 What is the empirical formula of Al 2 Br 3 ? A. AlBr B. AlBr 3 C. Al 2 Br D. Al 2 Br 3

[object Object],[object Object],[object Object],[object Object],Chapter Assessment 5 What is an ionic solid with trapped water molecules called? A. aqueous solution B. anhydrous compound C. hydrate D. solute

[object Object],[object Object],[object Object],[object Object],STP 1 Two substances have the same percent by mass composition, but very different properties. They must have the same ____. A. density B. empirical formula C. molecular formula D. molar mass

[object Object],[object Object],[object Object],[object Object],STP 2 How many moles of Al are in 2.0 mol of Al 2 Br 3 ? A. 2 B. 4 C. 6 D. 1

[object Object],[object Object],[object Object],[object Object],STP 3 How many water molecules are associated with 3.0 mol of CoCl 2 • 6H 2 O? A. 18 B. 1.1  10 25 C. 3.6  10 24 D. 1.8  10 24

[object Object],[object Object],[object Object],[object Object],STP 4 How many atoms of hydrogen are in 3.5 mol of H 2 S? A. 7.0  10 23 B. 2.1  10 23 C. 6.0  10 23 D. 4.2  10 24

[object Object],[object Object],[object Object],[object Object],STP 5 Which is not the correct formula for an ionic compound? A. CO 2 B. NaCl C. Na 2 SO 4 D. LiBr 2

IB Menu Click on an image to enlarge.

CIM Figure 10.6 Molar Mass Table 10.1 Formulas of Hydrates

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Cmc chapter 10

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