Oxidation-Reduction Reactions LEO SAYS GER. Oxidation and Reduction (Redox) Electrons are...
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Transcript of Oxidation-Reduction Reactions LEO SAYS GER. Oxidation and Reduction (Redox) Electrons are...
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Oxidation-Reduction Reactions
LEO SAYS GER
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Oxidation and Reduction (Redox)
Electrons are transferred Spontaneous redox rxns can transfer energy
Electrons (electricity) Heat
Non-spontaneous redox rxns can be made to happen with electricity
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Oxidation Reduction Reactions(Redox)
Each sodium atom loses one electron:
Each chlorine atom gains one electron:
11
2
00
22
ClNaClNa
eNaNa10
10 CleCl
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LEO says GER :Lose Electrons = Oxidation
Sodium is oxidized
Gain Electrons = Reduction
Chlorine is reduced
eNaNa10
10 CleCl
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Not All Reactions are Redox Reactions
Reactions in which there has been no change in oxidation number are not redox rxns.
Examples:
1 5 2 1 1 1 1 1 5 2
3 3( ) ( ) ( ) ( )Ag N O aq NaCl aq AgCl s Na N O aq
1 2 1 1 6 2 1 6 2 1 2
2 24 2 42 ( ) ( ) ( ) ( )NaOH aq H S O aq Na S O aq H O l
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Rules for Assigning Oxidation Numbers
Rules 1 & 21. The oxidation number of any
uncombined element is zero
2. The oxidation number of a monatomic ion equals its charge
11
2
00
22
ClNaClNa
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Rules for Assigning Oxidation Numbers
Rules 3 & 4
3. The oxidation number of oxygen in compounds is -24. The oxidation number of hydrogen in compounds is +1
2
2
1
OH
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Rules for Assigning Oxidation Number Rule 5
5. The sum of the oxidation numbers in the formula of a compound is 0
2(+1) + (-2) = 0 H O
(+2) + 2(-2) + 2(+1) = 0 Ca O H
2
2
1
OH 2
122
)(
HOCa
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Rules for Assigning Oxidation Numbers
Rule 66. The sum of the oxidation numbers in the formula of a polyatomic ion is equal to its charge
X + 3(-2) = -1N O
X = +5 X = +6
X + 4(-2) = -2S O
3
2?
ON
24
2?
OS
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Reducing Agents and Oxidizing Agents
The substance reduced is the oxidizing agent The substance oxidized is the reducing agent
Sodium is oxidized – it is the reducing agent
Chlorine is reduced – it is the oxidizing agent
eNaNa10
10 CleCl
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Trends in Oxidation and Reduction
Active metals: Lose electrons easily Are easily oxidized Are strong reducing agents
Active nonmetals: Gain electrons easily Are easily reduced Are strong oxidizing agents
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Electrochemical Terminology
Half-cell: a metal electrode in contact with a solution of its own ions
Electrode: A conductor used to establish contact with a nonmetallic part of a circuit, such as an electrolyte
Anode: The electrode where oxidation takes place
Cathode: The electrode where reduction takes place
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Voltaic Cells
Voltaic cells: Electrochemical cells in which a spontaneous redox reaction can be harnessed to produce an electric current.
Anode: negative
Cathode: positive
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Zinc – Copper Battery
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Zinc-Carbon Dry Cell Battery
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Mercury Dry Cell Battery
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Lead Storage Automotive
Battery
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Electrolytic
Cells
Electrolytic cells: Electrochemical cell in which an electric current is used to drive a non-spontaneous process
Cathode: negative
Anode: positive
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Electrolysis of H2O
2H2O 2H2 + O2
Electrolyte is usually dilute sulfuric acid
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Electroplating
of SilverCathode is the object to be plated
Anode is a piece of the plating metal
Solution contains ions of the plating metal
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Standard Reduction Potentials
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Measuring Electrode Potential
1. H2 Electrode is assigned a potential of zero volts2. Second electrode is placed in a solution of its own ions
3. Reduction potential of second electrode is measured.