Wednesday, October 17th
Today:
 Review
 Quiz
 Continue Chapter 6
1
© 2013 Pearson Education, Inc.
Chapter 6, Section 1
1
Review: Formation of Magnesium Ion,
Mg2+
Magnesium achieves an octet by losing its two
valence electrons.
© 2013 Pearson Education, Inc.
Chapter 6, Section 1
2
Group Numbers for Some Positive and
Negative Ions
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Chapter 6, Section 1
3
Polyatomic Ions
A polyatomic ion
 is a group of atoms.
 has an overall ionic charge.
Examples:
NH4+
ammonium
SO42−
sulfate
PO43−
phosphate
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Chapter 6, Section 1
OH−
hydroxide
CO32− carbonate
4
Guide to Drawing Electron-Dot
Formulas
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Chapter 6, Section 1
5
Learning Check
Draw the electron-dot formula for PF3.
© 2013 Pearson Education, Inc.
Chapter 6, Section 1
6
Names of Covalent Compounds
When naming a covalent
compound,
 the first nonmetal in the formula
is named by its element name,
and
 the second nonmetal is named
using the first syllable of its
element name, followed by ide.
Prefixes are used
 to indicate the number of atoms
present for each element in the
compound, and
 because two nonmetals can
form two or more different
compounds
© 2013 Pearson Education, Inc.
Chapter 6, Section 1
7
Learning Check
Name the covalent compound N2S5.
© 2013 Pearson Education, Inc.
Chapter 6, Section 1
8
Writing a Chemical Equation
A chemical equation tells us what substances react
(reactants) and what substances are formed
(products).
C(s) + O2(g)
reactants
CO2(g)
product
(+) used when there is two or more products or reactants
heat is used to start the reaction
(s) the compound is a solid
(l) the compound is a liquid
(g) the compound is a gas
(aq) aqueous, the compound is dissolved in water
© 2013 Pearson Education, Inc.
Chapter 6, Section 1
9
Summary Reaction Types
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Chapter 6, Section 1
10
Quiz Time
11
© 2013 Pearson Education, Inc.
Chapter 6, Section 1
11
Oxidation and Reduction,
Formation of CaS
In the reaction:
 the reactant, Ca has a charge of 0 and the
product, CaS contains a Ca2+ ion.
 calcium loses two electrons, meaning
oxidation has taken place.
 the reactant, S has a charge of 0 and the
product, CaS contains an S2− ion.
 sulfur gains two electrons, meaning
reduction has taken place.
© 2013 Pearson Education, Inc.
Chapter 6, Section 1
12
© 2013 Pearson Education, Inc.
Chapter 6, Section 1
13
Counting Units
Counting terms are used to describe specific
quantities.
 1 dozen donuts
= 12 donuts
 1 ream of paper
= 500 sheets
 1 case = 24 cans
© 2013 Pearson Education, Inc.
Chapter 6, Section 1
14
A Mole of Atoms
A mole is a counting unit that contains
 the same number of particles as there are
carbon atoms in 12.0 g of carbon 12C.
 6.02 x 1023 atoms of an element (Avogadro’s
number).
© 2013 Pearson Education, Inc.
Chapter 6, Section 1
15
A Mole of Sulfur
1 mole of sulfur contains Avogadro’s number of
atoms.
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Chapter 6, Section 1
16
A Mole of a Compound
A mole
 of a covalent compound has Avogadro’s
number of molecules.
 of an ionic compound contains Avogadro’s
number of formula units.
© 2013 Pearson Education, Inc.
Chapter 6, Section 1
17
Number of Particles in One Mole
© 2013 Pearson Education, Inc.
Chapter 6, Section 1
18
Avogadro’s Number as an
Equality
Avogadro’s number (6.02 x 1023) can be written
as an
equality and two conversion factors.
Equality:
Conversion Factors:
© 2013 Pearson Education, Inc.
Chapter 6, Section 1
19
Learning Check
How many moles of CO2 are in 2.50 x 1024
molecules of CO2?
© 2013 Pearson Education, Inc.
Chapter 6, Section 1
20
Solution
How many moles of CO2 are in 2.50 x 1024
molecules of CO2?
Step 1 State the given and needed
quantities.
Given
Need
2.50 x 1024 molecules of CO2
moles of CO2
Step 2 Write a plan to convert moles to
atoms or molecules.
molecules of CO2 → moles of CO2
© 2013 Pearson Education, Inc.
Chapter 6, Section 1
21
Solution
How many moles of CO2 are in 2.50 x 1024
molecules of CO2?
Step 3 Use Avogadro’s number to write
conversion factors.
© 2013 Pearson Education, Inc.
Chapter 6, Section 1
22
Solution
How many moles of CO2 are in 2.50 x 1024
molecules of CO2?
Step 4 Set up the problem to calculate the
number of particles.
© 2013 Pearson Education, Inc.
Chapter 6, Section 1
23
Subscripts State Atoms and
Moles
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Chapter 6, Section 1
24
Moles of Elements in a Formula
The subscripts in a formula give
 the relationship of atoms in the formula and
 the moles of each element in 1 mole of a
compound.
Glucose
C6H12O6
© 2013 Pearson Education, Inc.
Chapter 6, Section 1
25
Conversion Factors from
Subscripts
Subscripts used for conversion factors relate
moles of each element in 1 mole of a compound
For aspirin, C9H8O4, can be written as:
© 2013 Pearson Education, Inc.
Chapter 6, Section 1
26
Guide to Calculating Moles
© 2013 Pearson Education, Inc.
Chapter 6, Section 1
27
Learning Check
How many O atoms are in 0.150 mole of aspirin,
C9H8O4?
© 2013 Pearson Education, Inc.
Chapter 6, Section 1
28
Molar Mass
Molar mass is
 the mass of one mole
of a substance.
 the number of grams
that equals the atomic
mass of that element.
Molar mass is rounded to
the tenths (0.1 g) place
for use in this text.
© 2013 Pearson Education, Inc.
Chapter 6, Section 1
29
Guide to Calculating Molar Mass
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Chapter 6, Section 1
30
Molar Mass of CaCl2
We calculate the molar mass of CaCl2 to the nearest
0.1 g as follows.
Analyze the Problem.
Given
Need
formula unit CaCl2 molar mass of Ca, Cl; CaCl2
Step 1 Obtain the molar mass of each element.
© 2013 Pearson Education, Inc.
Chapter 6, Section 1
31
Molar Mass of CaCl2
We calculate the molar mass of CaCl2 to the nearest
0.1 g as follows.
Step 2 Multiply each molar mass by the number of
moles (subscript) in the formula.
Grams from 1 mole of Ca
Grams from 2 moles of Cl
© 2013 Pearson Education, Inc.
Chapter 6, Section 1
32
Molar Mass of CaCl2
We calculate the molar mass of CaCl2 to the nearest 0.1 g
as follows.
Step 3 Calculate the molar mass by adding the
masses of the elements.
© 2013 Pearson Education, Inc.
Chapter 6, Section 1
33
Learning Check
Determine the molar mass of K3PO4 to 0.1 g.
© 2013 Pearson Education, Inc.
Chapter 6, Section 1
34
Solution
Determine the molar mass of K3PO4 to 0.1 g.
Analyze the Problem.
Given
Need
formula unit K3PO4
molar mass of K, P, O;
molar mass of K3PO4
Step 1 Obtain the molar mass of each element.
© 2013 Pearson Education, Inc.
Chapter 6, Section 1
35
Solution
Determine the molar mass of K3PO4 to 0.1 g.
Step 2 Multiply each molar mass by the number
of moles (subscript) in the formula.
Grams from 3 moles of K
© 2013 Pearson Education, Inc.
Chapter 6, Section 1
36
Solution
Determine the molar mass of K3PO4 to 0.1 g.
Step 3 Calculate the molar mass by adding the
masses of the elements.
© 2013 Pearson Education, Inc.
Chapter 6, Section 1
37
One-Mole Quantities
32.1 g
© 2013 Pearson Education, Inc.
55.9 g
58.5 g
Chapter 6, Section 1
294.2 g
342.3 g
38
Chemistry and Cooking
 Bisquick
2 Cups Mix
2 Eggs
1 Cup Milk
8 Pancakes
39
© 2013 Pearson Education, Inc.
Chapter 6, Section 1
39
Friday
More Chapter 6
Group Assignment
40
© 2013 Pearson Education, Inc.
Chapter 6, Section 1
40