redox chemistry oxidation and reduction electrochemistry
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Redox Chemistry Oxidation and Reduction Electrochemistry . Syllabus Statements, First Exams 2009. 9.1.1 Define oxidation and reduction in terms of electron loss and gain. 9.1.2 Deduce the oxidation number of an element in a compound. - PowerPoint PPT PresentationTRANSCRIPT
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•Redox ChemistryOxidation and ReductionElectrochemistry
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Syllabus Statements, First Exams 20099.1.1 Define oxidation and reduction in terms of electron
loss and gain. 9.1.2 Deduce the oxidation number of an element in a
compound. 9.1.3 State the names of compounds using oxidation
numbers. 9.1.4 Deduce whether an element undergoes oxidation or
reduction in reactions using oxidation numbers.9.2.1 Deduce simple oxidation and reduction half-equations
given the species involved in a redox reaction. 9.2.2 Deduce redox equations using half equations.9.2.3 Define the terms oxidizing agent and reducing agent.
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ReactionsPrecipitation: cations and anions come together to
form insoluble ionic compounds.
Equation2 KI (aq) + Pb(NO3)2 (aq) PbI2 (s) + 2 KNO3 (aq)
Complete Ionic Equation2 K+ (aq) + 2 I- (aq) + Pb2+ (aq) + 2 NO3
- (aq) PbI2 (s) + 2 K+ (aq) + 2 NO3- (aq)
Net Ionic Equation 2 I- (aq) + Pb2+ (aq) + PbI2 (s)
Did the charge on any of the species in this reaction change?e.g. What charge did K start with? Finish with?What charge did Pb start with? Finish with?
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ReactionsSingle-replacement reactions: One metallic element
replaces another metallic element in a salt.Equation
3 CuCl2 (aq) + 2 Al (s) 2 AlCl3 (aq) + 3 Cu (s)
Complete Ionic Equation 3 Cu2+ (aq) + 6 Cl- (aq) + 2 Al (s) 2 Al3+
(aq) + 6 Cl- (aq) + 3 Cu (s)
Net Ionic Equation3 Cu2+ (aq) + 2 Al (s) 2 Al3+ + 3 Cu (s)
Did the charge on any of the species in this reaction change?
YES!
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Electrochemical Reactions
In electrochemical reactions, electrons are transferred from one species to another.
Translation: Redox reactions involve the gaining and losing of electrons.
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Oxidation Numbers
In order to keep track of what loses electrons and what gains them, we assign oxidation numbers.
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Assigning Oxidation Numbers
Use the chart given and identify the oxidation state of nitrogen in each of the compounds/ions given.
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Examples…
NH3 N2H4 N2 N2O NO NO2 NO3-
-3 -2 0 +1 +2 +4 +5
How’d you do?Any questions?
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Oxidation
• A species is oxidized when it loses electrons.• Here, zinc loses two electrons to go from neutral
zinc metal to the Zn2+ ion.
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Oxidation and Reduction
• A species is reduced when it gains electrons.• Here, each of the H+ gains an electron and they
combine to form H2.
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LEO the lion goes GER
Loss of Electrons is Oxidation
Gain of Electrons is Reduction
Mnemonic Device
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OIL RIG
Oxidation Is Loss (of electrons)Reduction Is Gain (of electrons)
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King Phillip Came Over For Great SupperKingdomPhylumClassOrderFamilyGenusSpecies
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Oxidation and Reduction
• What is reduced is the oxidizing agent.– H+ oxidizes Zn by taking electrons from the zinc, being reduced
in the process.• What is oxidized is the reducing agent.
– Zn reduces H+ by giving it electrons, being oxidized in the process.
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Example ReactionIdentify the following:
Element oxidizedElement reducedOxidizing agentReducing agent
2 PbS (s) + 3 O2 (g) 2 PbO (s) + 2 SO2 (g)
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Example ReactionIdentify the following:
Element oxidized SulfurElement reducedOxidizing agentReducing agent
2 PbS (s) + 3 O2 (g) 2 PbO (s) + 2 SO2 (g)
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Example ReactionIdentify the following:
Element oxidized SulfurElement reduced OxygenOxidizing agentReducing agent
2 PbS (s) + 3 O2 (g) 2 PbO (s) + 2 SO2 (g)
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Example ReactionIdentify the following:
Element oxidized SulfurElement reduced OxygenOxidizing agent O2 (g)Reducing agent
2 PbS (s) + 3 O2 (g) 2 PbO (s) + 2 SO2 (g)
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Example ReactionIdentify the following:
Element oxidized SulfurElement reduced OxygenOxidizing agent O2 (g)Reducing agent PbS (s)
2 PbS (s) + 3 O2 (g) 2 PbO (s) + 2 SO2 (g)
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Example ReactionIdentify the following:
Element oxidizedElement reducedOxidizing agentReducing agent
Mg (s) + CuSO4 (aq) MgSO4 (aq) + Cu (s)
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Example ReactionIdentify the following:
Element oxidized MagnesiumElement reducedOxidizing agentReducing agent
Mg (s) + CuSO4 (aq) MgSO4 (aq) + Cu (s)
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Example ReactionIdentify the following:
Element oxidized MagnesiumElement reduced CopperOxidizing agentReducing agent
Mg (s) + CuSO4 (aq) MgSO4 (aq) + Cu (s)
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Example ReactionIdentify the following:
Element oxidized MagnesiumElement reduced CopperOxidizing agent CuSO4 (aq)Reducing agent
Mg (s) + CuSO4 (aq) MgSO4 (aq) + Cu (s)
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Example ReactionIdentify the following:
Element oxidized MagnesiumElement reduced CopperOxidizing agent CuSO4 (aq)Reducing agent Mg (s)
Mg (s) + CuSO4 (aq) MgSO4 (aq) + Cu (s)
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Another Example Reaction
5Fe2+(aq) +MnO4- (aq) +8H+(aq) → 5Fe3+(aq) + Mn2+(aq) + 4H2O(l)
Identify the following:Element oxidizedElement reducedOxidizing agentReducing agent
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Another Example Reaction
5Fe2+(aq) +MnO4- (aq) +8H+(aq) → 5Fe3+(aq) + Mn2+(aq) + 4H2O(l)
Identify the following:Element oxidized Fe2+
Element reducedOxidizing agentReducing agent
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Another Example Reaction
5Fe2+(aq) +MnO4- (aq) +8H+(aq) → 5Fe3+(aq) + Mn2+(aq) + 4H2O(l)
Identify the following:Element oxidized Fe2+
Element reduced MnOxidizing agentReducing agent
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Another Example Reaction
5Fe2+(aq) +MnO4- (aq) +8H+(aq) → 5Fe3+(aq) + Mn2+(aq) + 4H2O(l)
Identify the following:Element oxidized Fe2+
Element reduced MnOxidizing agent MnO4
- (aq)Reducing agent
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Another Example Reaction
5Fe2+(aq) +MnO4- (aq) +8H+(aq) → 5Fe3+(aq) + Mn2+(aq) + 4H2O(l)
Identify the following:Element oxidized Fe2+
Element reduced MnOxidizing agent MnO4
-
Reducing agent Fe2+
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Reactivity Series
Some metals make better reducing agents than other metals. (In other words, some metals are oxidized easier.)
Let’s look at two reactions:
Mg (s) + CuCl2 (aq) ???
Mg (s) + NaCl (aq) ???
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Reactivity Series
Mg (s) + CuCl2 (aq) MgCl2 (aq) + Cu (s)
Mg (s) + NaCl (aq) ???
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Reactivity Series
Mg (s) + CuCl2 (aq) MgCl2 (aq) + Cu (s)
Mg (s) + NaCl (aq) NR
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Reactivity Series
Mg (s) + CuCl2 (aq) MgCl2 (aq) + Cu (s)
Mg (s) + NaCl (aq) NR
Activity Series:
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Reactivity Series
Mg (s) + CuCl2 (aq) MgCl2 (aq) + Cu (s)
Mg (s) + NaCl (aq) NR
Activity Series: Na > Mg > Cu
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Reactivity Series
Some halogens make better reducing agents than other halogens. (In other words, some halogens are oxidized easier.)
Let’s look at two reactions:
F2 (g) + NaCl (aq) ???
Br2 (l) + NaCl (aq) ???
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Reactivity Series
Let’s look at two reactions:
F2 (s) + 2 NaCl (aq) 2 NaF + Cl2
Br2 (s) + NaCl (aq) ???
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Reactivity Series
Let’s look at two reactions:
F2 (s) + 2 NaCl (aq) 2 NaF + Cl2
Br2 (s) + NaCl (aq) NR
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Reactivity Series
Let’s look at two reactions:
F2 (s) + 2 NaCl (aq) 2 NaF + Cl2
Br2 (s) + NaCl (aq) NR
Activity Series:
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Reactivity Series
Let’s look at two reactions:
F2 (s) + 2 NaCl (aq) 2 NaF + Cl2
Br2 (s) + NaCl (aq) NR
Activity Series: F > Cl > Br
What does that resemble?
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Halogens
FClBrI
Most Reactive
Least Reactive