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Title: Chemistry: Matter and Change


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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
3
Section 10-1
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 Avogadros number
Chemists use the mole to count atoms, molecules,
ions, and formula units.
4
Section 10-1
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 Avogadros number.

5
Section 10-1
Converting Between Moles and Particles
  • Conversion factors must be used.
  • Moles to particles

Number of molecules in 3.50 mol of sucrose
6
Section 10-1
Converting Between Moles and Particles (cont.)
  • Particles to moles
  • Use the inverse of Avogadros number as the
    conversion factor.

7
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
  1. A
  2. B
  3. C
  4. D

8
Section 10-1
Section 10.1 Assessment
  1. A
  2. B
  3. C
  4. D

9
End of Section 10-1
10
Section 10-2
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.
11
Section 10-2
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.

12
Section 10-2
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.

13
Section 10-2
Using Molar Mass
  • Moles to mass

3.00 moles of copper has a mass of 191 g.
14
Section 10-2
Using Molar Mass (cont.)
  • Convert mass to moles with the inverse molar mass
    conversion factor.
  • Convert moles to atoms with Avogadros number as
    the conversion factor.

15
Section 10-2
Using Molar Mass (cont.)
  • This figure shows the steps to complete
    conversions between mass and atoms.

16
Section 10-2
Section 10.2 Assessment
The mass in grams of 1 mol of any pure substance
is A. molar mass B. Avogadros number
C. atomic mass D. 1 g/mol
  1. A
  2. B
  3. C
  4. D

17
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
  1. A
  2. B
  3. C
  4. D

18
End of Section 10-2
19
Section 10-3
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
20
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.
21
Section 10-3
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.

22
Section 10-3
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.

23
Section 10-3
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.

24
Section 10-3
Converting the Mass of a Compound to Moles
  • The conversion factor is the inverse of the molar
    mass of the compound.

25
Section 10-3
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 Avogadros number.

26
Section 10-3
Converting the Mass of a Compound to Number of
Particles (cont.)
  • This figure summarizes the conversions between
    mass, moles, and particles.

27
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
  1. A
  2. B
  3. C
  4. D

28
Section 10-3
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
  1. A
  2. B
  3. C
  4. D

29
End of Section 10-3
30
Section 10-4
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.
31
Section 10-4
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.

32
Section 10-4
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.

33
Section 10-4
Empirical Formula
  • The empirical formula for 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

34
Section 10-4
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.

35
Section 10-4
Molecular Formula (cont.)
36
Section 10-4
Section 10.4 Assessment
What is the empirical formula for the compound
C6H12O6? A. CHO B. C2H3O2 C. CH2O D. CH3O
  1. A
  2. B
  3. C
  4. D

37
Section 10-4
Section 10.4 Assessment
Which is the empirical formula for hydrogen
peroxide? A. H2O2 B. H2O C. HO D. none of
the above
  1. A
  2. B
  3. C
  4. D

38
End of Section 10-4
39
Section 10-5
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.
40
Section 10-5
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

41
Section 10-5
Naming Hydrates (cont.)
42
Section 10-5
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.

43
Section 10-5
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.

44
Section 10-5
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.

45
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.
  1. A
  2. B
  3. C
  4. D

46
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
  1. A
  2. B
  3. C
  4. D

47
End of Section 10-5
48
Resources Menu
Chemistry Online Study Guide Chapter
Assessment Standardized Test Practice Image
Bank Concepts in Motion
49
Study Guide 1
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 Avogadros 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 Avogadros
    relationship can be used to convert between moles
    and number of representative particles.

50
Study Guide 2
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 Avogadros 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.

51
Study Guide 3
Section 10.3 Moles of Compounds
Key Concepts
  • Subscripts in a chemical formula indicate how
    many moles of each element are present in 1 mol
    of the compound.
  • The molar mass of a compound is calculated from
    the molar masses of all of the elements in the
    compound.
  • Conversion factors based on a compounds molar
    mass are used to convert between moles and mass
    of a compound.

52
Study Guide 4
Section 10.4 Empirical and Molecular Formulas
Key Concepts
  • The percent by mass of an element in a compound
    gives the percentage of the compounds total mass
    due to that element.
  • The subscripts in an empirical formula give the
    smallest whole-number ratio of moles of elements
    in the compound.
  • The molecular formula gives the actual number of
    atoms of each element in a molecule or formula
    unit of a substance.
  • The molecular formula is a whole-number multiple
    of the empirical formula.

53
Study Guide 5
Section 10.5 Formulas of Hydrates
Key Concepts
  • The formula of a hydrate consists of the formula
    of the ionic compound and the number of water
    molecules associated with one formula unit.
  • The name of a hydrate consists of the compound
    name and the word hydrate with a prefix
    indicating the number of water molecules in 1 mol
    of the compound.
  • Anhydrous compounds are formed when hydrates are
    heated.

54
Chapter Assessment 1
What does Avogadros 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
  1. A
  2. B
  3. C
  4. D

55
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
  1. A
  2. B
  3. C
  4. D

56
Chapter Assessment 3
How many moles of hydrogen atoms are in one mole
of H2O2? A. 1 B. 2 C. 3 D. 0.5
  1. A
  2. B
  3. C
  4. D

57
Chapter Assessment 4
What is the empirical formula of Al2Br3?
A. AlBr B. AlBr3 C. Al2Br D. Al2Br3
  1. A
  2. B
  3. C
  4. D

58
Chapter Assessment 5
What is an ionic solid with trapped water
molecules called? A. aqueous solution
B. anhydrous compound C. hydrate D. solute
  1. A
  2. B
  3. C
  4. D

59
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
  1. A
  2. B
  3. C
  4. D

60
STP 2
How many moles of Al are in 2.0 mol of Al2Br3?
A. 2 B. 4 C. 6 D. 1
  1. A
  2. B
  3. C
  4. D

61
STP 3
How many water molecules are associated with 3.0
mol of CoCl2 6H2O? A. 18 B. 1.1 ? 1025
C. 3.6 ? 1024 D. 1.8 ? 1024
  1. A
  2. B
  3. C
  4. D

62
STP 4
How many atoms of hydrogen are in 3.5 mol of
H2S? A. 7.0 ? 1023 B. 2.1 ? 1023 C. 6.0 ?
1023 D. 4.2 ? 1024
  1. A
  2. B
  3. C
  4. D

63
STP 5
Which is not the correct formula for an ionic
compound? A. CO2 B. NaCl C. Na2SO4 D. LiBr2
  1. A
  2. B
  3. C
  4. D

64
IB Menu
Click on an image to enlarge.
65
IB 1
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IB 2
67
IB 3
68
IB 4
69
IB 6
70
IB 7
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CIM
Figure 10.6 Molar Mass Table 10.1 Formulas of
Hydrates
72
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