Guided Practice: Determine the OXIDATION...
Transcript of Guided Practice: Determine the OXIDATION...
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Section 4.9
Oxidation–Reduction Reactions
Return to TOC
Guided Practice: Determine the OXIDATION NUMBERS!
NH3 N =
ClO- Cl =
H3PO4 P =
MnO4- Mn =
Oxidation
number of F in
HF?
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Section 4.9
Oxidation–Reduction Reactions
Return to TOC
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Independent Practice:
Find the oxidation states for each of the
elements in each of the following
compounds:
• K2Cr2O7
• CO32-
• MnO2
• PCl5
• SF4
K = +1; Cr = +6; O = –2
C = +4; O = –2
Mn = +4; O = –2
P = +5; Cl = –1
S = +4; F = –1
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Section 4.9
Oxidation–Reduction Reactions
Return to TOC
Copyright © Cengage Learning. All rights reserved 3
• Reactions that are concerned with the transfer
of electrons.
• Also called ‘Redox’ reactions because oxidation
and reduction occur at the same time.
Oxidation-Reduction Reactions
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Section 4.9
Oxidation–Reduction Reactions
Return to TOC
• The atom that undergoes oxidation is called the
‘reducing agent’
• The atom that undergoes reduction is called the
‘oxidizing agent’
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Section 4.9
Oxidation–Reduction Reactions
Return to TOC
Why Study Redox Reactions
Manufacturing metals
Energy from
food!
Batteries
Corrosion
Rusting
Green color
on the copper
due to
Redox!
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Section 4.9
Oxidation–Reduction Reactions
Return to TOC
• Oxidation is the loss of electrons.
• Reduction is the gain of electrons.
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General, Organic, and Biological Chemistry Copyright © 2010 Pearson Education, Inc.
9
In light-sensitive sunglasses, UV light initiates an
oxidation-reduction reaction.
uv light
2Ag+ + 2Cl− 2Ag + Cl2
A. Which reactant is oxidized?
Cl − 2Cl− Cl + 2e−
B. Which reactant is reduced?
Ag+ 2Ag+ + 2e− 2Ag
Problem
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Not All Reactions are Redox Reactions
- Reactions in which there has been no
change in oxidation number are NOT redox reactions.
Example: silver nitrate and sodium
chloride solutions combine
)()()()( 3
2511111
3
251
aqONNasClAgaqClNaaqONAg
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Section 4.9
Oxidation–Reduction Reactions
Return to TOC
Example:
Zinc foil is added to a copper(II)nitrate solution.
Zn+ Cu(NO3)2 Cu + Zn(NO3)2
The net ionic for this reaction is:
Zn + Cu2+ Cu + Zn2+
The copper ion is being reduced: Cu2+ + 2e- Cu
The zinc atom is being oxidized: Zn Zn2+ + 2e-
The number of electrons gain / lost must be equal!
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General, Organic, and Biological Chemistry Copyright © 2010 Pearson Education, Inc.
12
Zn replaces Cu2+
zinc undergoes oxidation
Zn(s) Zn2+(aq) + 2e-
Cu2+ undergoes reduction
Cu2+(aq) + 2e- Cu(s)
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General, Organic, and Biological Chemistry Copyright © 2010 Pearson Education, Inc.
Zn Transfers Electrons to Cu2+
OIL Oxidation is losing electrons.
RIG Reduction is gaining electrons.
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General, Organic, and Biological Chemistry Copyright © 2010 Pearson Education, Inc.
14
Identify each of the following as (O) Oxidation or
(R) Reduction
__A. Sn(s) Sn4+(aq) + 4e−
__B. Fe3+(aq) + 1e− Fe2+(aq)
__C. Cl2(g) + 2e− 2Cl−(aq)
Learning Check
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General, Organic, and Biological Chemistry Copyright © 2010 Pearson Education, Inc.
15
Identify each of the following as (O) Oxidation or
(R) Reduction
O A. Sn(s) Sn4+(aq) + 4e−
R B. Fe3+(aq) + 1e− Fe2+(aq)
R C. Cl2(g) + 2e− 2Cl−(aq)
Solution
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Section 4.9
Oxidation–Reduction Reactions
Return to TOC
Example:
1. Write the molecular formula when Iron(III)oxide
and carbon monoxide react to form iron metal
and carbon dioxide.
2. Use oxidation numbers to determine which
atoms are becoming oxidized and reduced
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Section 4.10
Balancing Oxidation–Reduction Equations
Return to TOC
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Problem:
1. Write the balanced equation for the reaction that
occurs when zinc metal is placed in hydrochloric acid.
2. Write the oxidation states for each atom below.
Zn(s) + 2HCl(aq) ZnCl2 (aq) + H2(g)
0 +1 –1 +2 –1 0
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Section 4.10
Balancing Oxidation–Reduction Equations
Return to TOC
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1 e– gained (each atom)(Reduced)
• Zn(s) + HCl(aq) ZnCl2 (aq) + H2(g)
0 +1 –1 +2 –1 0
2 e– lost (Oxidized)
• The oxidation state of chlorine remains unchanged.
3. Connect the atoms that are being oxidized or reduced.
How many electrons are gained and lost? What compound is
being oxidized? Reduced?
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Section 4.10
Balancing Oxidation–Reduction Equations
Return to TOC
Balancing Oxidation reactions using half reactions will
be covered in a later chapter.
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