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““Oxidation-Reduction Reactions”Oxidation-Reduction Reactions”
LEO SAYS GER
Pre-AP Chemistry
Charles Page High School
Stephen L. Cotton
Oxidation and Reduction (Redox)Oxidation and Reduction (Redox)
A process called “reduction” is the opposite of oxidation, and originally meant the loss of oxygen from a compound Oxidation and reduction always occur
simultaneously The substance gaining oxygen (or
losing electrons) is oxidized, while the substance losing oxygen (or gaining electrons) is reduced.
Oxidation and Reduction (Redox)Oxidation and Reduction (Redox) Today, many of these reactions may
not even involve oxygen Redox currently says that electrons
are transferred between reactants
Mg + S → Mg2+ + S2-
•The magnesium atom (which has zero charge) changes to a magnesium ion by losing 2 electrons, and is oxidized to Mg2+
•The sulfur atom (which has no charge) is changed to a sulfide ion by gaining 2 electrons, and is reduced to S2-
(MgS)
Leo the Lion!
• LEO the lion says GER– Loss of electrons is oxidation, gain of electrons
is reduction
LET'S LOOK AT
HALF REACTIONS
Oxidation and Reduction (Redox)Oxidation and Reduction (Redox)11
2
00
22
ClNaClNa
Each sodium atom loses one electron:
Each chlorine atom gains one electron:
eNaNa10
10 CleCl
LEO says GER :LEO says GER :
eNaNa10
Lose Electrons = Oxidation
Sodium is oxidized
Gain Electrons = Reduction
10 CleCl Chlorine is reduced
General, Organic, and Biological Chemistry Copyright © 2010 Pearson Education, Inc.
7
Identify each of the following half reactions as:
1) oxidation or 2) reduction
__A. Sn(s) Sn4+(aq) + 4e−
__B. Fe3+(aq) + 1e− Fe2+(aq)
__C. Cl2(g) + 2e− 2Cl−(aq)
Learning Check
General, Organic, and Biological Chemistry Copyright © 2010 Pearson Education, Inc.
8
Identify each of the following as:
1) oxidation or 2) reduction
1 A. Sn(s) Sn4+(aq) + 4e−
2 B. Fe3+(aq) + 1e− Fe2+(aq)
2 C. Cl2(g) + 2e− 2Cl−(aq)
Solution
LEO says GER :LEO says GER : - Losing electrons is oxidation, and the substance that loses the electrons is called the reducing agent. - Gaining electrons is reduction, and the substance that gains the electrons is called the oxidizing agent.
Mg(s) + S(s) → MgS(s)
Mg is oxidized: loses e-, becomes a Mg2+ ion
S is reduced: gains e- = S2- ion
Mg is the reducing
agent
S is the oxidizing agent
Oxidation and Reduction (Redox)Oxidation and Reduction (Redox) It is easy to see the loss and gain of electrons in ionic compounds, but what about covalent compounds?
Oxygen is highly electronegative, so, in water:
the oxygen gains electrons (is reduced and is the oxidizing agent), and the hydrogen loses electrons (is oxidized and is the reducing agent)
Other rules to remember:
• Flourine is ALWAYS -1.• Other halogens are going to be -1, EXC
EPT when bonding with oxygen.• Group I elements have an oxidation st
ate +1• Group II elements have an oxidation st
ate of +2
Water as a product
• If the H[+1] was taken from a reactant compound, it already had a +1 charge.
• If O[-2] was taken from a reactant compound, it already had -2 charge.
• Therefore, there will be no change in the oxidation number of the elements in H and O when water is made and the H2O will have a total oxidation number of zero.
Oxidation Reduction
Gains oxygen Lose Oxygen
Lose Hydrogen Gains hydrogen
Lose Electrons Gains electrons
Oxygen
Hydrogen
e-
Not All Reactions are Redox ReactionsNot All Reactions are Redox Reactions
- Reactions in which there has been no
change in oxidation number are NOT redox reactions.
Examples:
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3
251
aqONNasClAgaqClNaaqONAg
)()()()(22
2
1
4
26
2
1
4
26
2
1121
lOHaqOSNaaqOSHaqHONa