PracticePacket:OxidationReduction
Regents Chemistry: Mrs. Mintz
PracticePacket
Chapter14:OxidationReduction&Electrochemistry
1
Assigning
Oxidation
Numbers
Objective:
How do we assign atoms the correct
oxidation number?
Chemistry 200
Video Lesson 14.1
Rules for Assigning Oxidation Numbers (states)
Oxidation & Reduction (Redox)
Oxidation number
1. Free elements are assigned an oxidation state of zero
The hydrogen in H2, the sodium in Na, and the sulfur in S8 all have oxidation numbers of zero.
2. The Group 1 metals (Alkali Metals) in compounds
always have an oxidation state of +1
• a number assigned to keep track of electron(s) gained
or lost in a redox rxns.
3. The Group 2 metals (Alkali Earth Metals) in
compounds always have an oxidation state of +2
4. The oxidation state for any simple
one-atom ion(monoatomic) is equal
to its charge.
7. Oxygen in compounds is assigned an oxidation state of -2.
**When combined w/ Fluorine, Oxygen has an oxidation
state of +2.**
In MgCl2, the Mg2+ ion has an oxidation number of +2.
Each of the Cl- ions has an oxidation number of -1.
Fe2+
ion has an oxidation number of +2, In FeCl2, the
while in FeCl3 the Fe3+ ion has an oxidation number of +3.
5.  Fluorine in compounds is always assigned an
oxidation state of -1.
8. The sum of the oxidation states of all the atoms in a
species must be equal to the net charge on the
species.
If the species is neutral, the sum of
the oxidation states is zero.
6.  Hydrogen in compounds is always assigned
an oxidation number of +1. (HCl).
If combined w/ a metal, Hydrogen
has an oxidation # of -1. (LiH)
If the species has a charge, the sum
is equal to that charge.
2
Determine the oxidation number of sulfur in H2SO4
(+2)+6(-8)=0
+1 +6-2
Determine the oxidation number of nitrogen in NO3-1
+5(-6)= -1
+5-2
-1
H2SO4
NO3
Objective:
Redox
Reactions
How do we identify substances being
oxidized or reduced and the oxidizing and
reducing agents. How do we use this information to create
half reactions ?
Chemistry 200
Video Lesson 14.2
Redox
Easy way to remember!!!
Redox reaction • a chemical rxn where electron(s) are transferred
from one atom to another
Oxidation
• loss of electron(s) by an atom or ion & an increase
)
in oxidation # (Ca à Ca+2 + 2e-
Chemistry
GER!!!!!
Yum Yum
LEO says GER
LEO = Loss of Electrons is Oxidation
Reduction
• gain of electron(s) by an atom or ion & a
decrease in oxidation #
( 5e - + Mn+7 à Mn+2)
GER = Gain of Electrons is Reduction
**Oxidation & Reduction occur simultaneously,
they cannot occur separately**
3
Oxidizing Agent
Reducing Agent
• the substance that allows another substance to be
reduced. They lose electron(s) & therefore are
oxidized
• the substance that causes the oxidation of other
substances. They accept electron(s) easily &
therefore are reduced
ex: Ca à Ca+2 + 2e-
ex1: 5e- + Mn+7 à Mn+2
(gain of electrons, oxidation # reduced)
(loss of electrons, oxidation # increases)
**The species oxidized, the species reduced, the oxidizing
agent or reducing agent must always be a reactant!!**
Writing Half Reactions
Gains Electrons Loses Electrons
Reduced Oxidized Oxidizing Agent
Reducing Agent
• They show either the oxidation or reduction portion of a
redox rxn, including electrons gained or lost
Half rxn for oxidation --> electrons are products
Half rxn for reduction --> electrons are reactants
THERE’S AN EASIER WAY TO REMEMBER!!!
**Electronsgoonthesidew/themorepositiveoxid.#**
Creating Half Reactions from a Redox Reaction
+1+5-6
+1+5-2
1.  Assign oxidation numbers to determine the
substance oxidized & the substance reduced.
+1-1
0
KClO3 --> KCl + O2
2.  Write each half reaction, balance by atom, then by
electrons. The ONLY exception is a half rxn the
contains a diatomic element.
Oxid:
2
O-2 à O2+ 4e- (reducing agent)
Red: 6e- +Cl+5 à Cl-1 (oxidizing agent)
3.  Identify the species oxidized, the species reduced
the oxidizing agent & the reducing agent.
4
Objectives
• Name the type of reactions involved in
electrochemical processes.
• Describe how a voltaic cell produces
electrical energy.
Electrochemical
Cells
Video Lesson 14.4
Electrochemical Process
Voltaic Cells
• An electrochemical process is any
conversion between chemical and and
electrical energy (charged particles).
• All electrochemical processes involve redox
reactions.
• The two half reactions must be physically
separated to be used as a source of
electrical energy.
• To obtain a useful current, we separate the oxidizing
and reducing agents so that electron transfer
occurs thru an external wire.
• What is needed – Spontaneous Reaction
o Salt Bridge
• connects the 2 containers & provides a
passage for ions from one solution to another
o Electrodes
• one of 2 surfaces that conduct electricity, the
site of oxidation & reduction rxns
Since Zn is higher on Table J, It will be Oxidized!
Anode
5
Cathode
Flow of Electrons
Voltaic Cell
Zn(s)
anode -
Overall Redox Rxn
Reduction occurs at the
cathode
Oxidation occurs at the
anode
From Anode to Cathode
e- -->
Zn(s) + Cu+2(aq) --> Zn+2(aq) + Cu(s)
Oxid: Zn(s) --> Zn+2(aq)+ 2e-
Red: 2e- + Cu+2(aq) --> Cu(s)
Zn Species oxidized_____
Cu+2 Species reduced_____
Zn
Anode_______
6
Cu(s)
cathode +
Cu
Zn
Zn+2
Cu+2
Zn
Reducing agent______
Cu Oxidizing agent_____
+2
Cu
Cathode_______
PracticePacket:Redox
Video14.1:OxidationNumbers
DeterminetheoxidationnumberofEACHelementineachofthefollowingsubstances:
1. KMnO4
6. PO4-3
7. zincoxide
2. S8
3. Na2Cr2O7
8. water
9. calciumhydride
4. CuCl2
10.
5. H2SO4
carbondioxide
Video14.2:RedoxReactions
WritingHalfReactions
Step1:Balancethehalfreactionbyatomusingcoefficients
Step2:Balancethehalfreactionbychargeusingelectrons(e-)
Electronsalwaysgoonthesidewiththemorepositiveoxidation#
**Halfrxnsarewrittenonaperatombasis.Theonlyexceptionisifthehalfrxncontainsadiatomic
element**
MgàMg+2
N-3àN2
O2àO-2
S+6àS-2
Cl+5àCl-1
3Cu+1à3Cu
Mn+2àMn+5
6H+1à3H2
7
14.1 Oxidation Numbers
Name:
1. What is the oxidation state of nitrogen in
the compound NH 4 Br?
1) –1
2) +2
3) –3
8. Given the reaction that occurs in an
electrochemical cell:
4) +4
Zn(s) + CuSO 4 (aq) ® ZnSO 4 (aq) +
Cu(s)
During this reaction, the oxidation number of Zn
changes from
2. What is the oxidation number of sulfur in
Na2S2O3 ?
1) –1
2) +2
3) +6
1) 0 to +2
2) 0 to –2
4) +4
3. Given the balanced equation representing
a reaction:
9. In which substance does hydrogen have
an oxidation number of zero?
1) LiH
2) H 2 O
2KClO 3 (s) ® 2KCl(s) + 3O 2 (g)
The oxidation state of chlorine in this reaction
changes from
1) –1 to +1
2) –1 to +5
3) + l to –1
4) +5 to –1
2) +2
3) +3
1) CO
2) CO 2
4) +8
5. What is the oxidation number assigned to
manganese in KMnO 4 ?
1) +7
2) +2
3) +3
4) +4
6. What is the oxidation state of nitrogen in
NaNO 2 ?
1) +1
2) +2
3) +3
4) +4
7. What is the oxidation number of chromium
in K 2 Cr 2 O 7 ?
1) +12 2) +2
3) +3
3) H 2 S
4) H 2
10. In which compound does carbon have an
oxidation state of –4?
4. What is the oxidation number of chromium
in the chromate ion, CrO 4 2– ?
1) +6
3) +2 to 0
4) –2 to 0
4) +6
8
3) CCl 4
4) CH 4
PracticePacket:Redox
CreatingHalfReactionsfromRedoxReactions
Step1:Assignoxidationnumberstodeterminethesubstancesthathaveachangeinoxidationnumber
Step2:Identifythetwohalfreactions&balanceeachhalfreaction
Step3:Labeleachhalfreaction&identifythespeciesoxidized,thespeciesreduced,theoxidizing
agent&thereducingagent
Note:Thereactionprovidedtoyoumaybebalancedorunbalanced.Rememberthathalfreactionsaremadeonaperatom
basis.TheONLYexceptionisahalfreactionthatcontainsadiatomicelement
Speciesoxidized______________
Cu+2+MnàMn+4+Cu
Speciesreduced______________
Oxidation:
Speciesoxidized______________
ReducingAgent______________
Reduction:
3Ag+1+FeàFe+3+3Ag
Speciesreduced______________
Oxidation:
Speciesoxidized______________
OxidizingAgent______________
ReducingAgent______________
Reduction:
Na+Cl2àNaCl
Speciesreduced______________
Oxidation:
OxidizingAgent______________
OxidizingAgent______________
ReducingAgent______________
Reduction:
2H2+O2à2H2O
Speciesoxidized______________
OxidizingAgent______________
Speciesreduced______________
ReducingAgent______________
Oxidation:
Reduction:
9
PracticePacket:OxidationReduction
Speciesoxidized______________
2S+3O2à2SO3
Speciesreduced______________
Oxidation:
Speciesoxidized______________
ReducingAgent______________
Reduction:
2Fe+6HClà3H2+2FeCl3
Speciesreduced______________
Oxidation:
Speciesoxidized______________
OxidizingAgent______________
ReducingAgent______________
Reduction:
CH4+2O2àCO2+2H2O
Speciesreduced______________
Oxidation:
OxidizingAgent______________
OxidizingAgent______________
ReducingAgent______________
Reduction:
2KClO3à2KCl+3O2
Speciesoxidized______________
OxidizingAgent______________
Speciesreduced______________
ReducingAgent______________
Oxidation:
Reduction:
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10
14.2 Half Reactions
Name:
7. Which equation represents an oxidation-reduction
reaction?
1. An oxidation-reduction reaction involves the
1)
2)
3)
4)
sharing of electrons
sharing of protons
transfer of electrons
transfer of protons
1)
2)
3)
2. During which process does an atom gain one or
more electrons?
1) transmutation
2) reduction
4)
8. Which half-reaction shows conservation of charge?
3) oxidation
4) neutralization
1) Cu + e– ® Cu+
2) Cu2+ + 2e– ® Cu
3. Which half-reaction correctly represents reduction?
1)
2)
3)
4)
Mn 4+
Mn 4+
Mn 4+
Mn 4+
9. Which balanced equation represents an
oxidation-reduction reaction?
® Mn3+ + e –
® Mn7+ + 3e–
+ e – ® Mn3+
+ 3e– ® Mn7+
4. In a redox reaction, the total number of electrons lost
is
1) less than the total number of electrons gained
2) greater than the total number of electrons
gained
3) equal to the total number of electrons gained
4) equal to the total number of protons gained
2) Mg 2+ 3) Co2+
4) Ca2+
6. Given the balanced ionic equation representing a
reaction:
2Al(s) + 3Cu 2+(aq)
2Al3+(aq) + 3Cu(s)
Which half-reaction represents the reduction that
occurs?
1) Al
Al 3+ + 3e–
2) Al3+ + 3e–
Al
1)
2)
3)
4)
Ba(NO3) 2 + Na 2SO4 ®BaSO 4 + 2NaNO 3
H3PO4 + 3KOH ®K3PO4 + 3H2O
Fe(s) + S(s) ®FeS(s)
NH3(g) + HCl(g) ®NH4Cl(s)
10. Which expression correctly represents a balanced
reduction half-reaction?
1) Na+ + e – ® Na
2) Na ® Na+ + e –
5. Which ion is most easily reduced?
1) Zn 2+
3) Cu+ ® Cu + e –
4) Cu2+ ® Cu + 2e–
3) Cu
Cu2+ + 2e–
4) Cu2+ + 2e–
Cu
11
3) Cl 2 + 2e– ® Cl –
4) 2 Cl– ® Cl 2 + 2e–
PracticePacket:OxidationReduction
Lesson14.3:ActivitySeriesandSpontaneity
Table J: The table is arranged with the most reactive metals at the top of the
tableandtheleastreactivemetalsatthebottomofthetable.Whatthismeansis
thatametallistedonthetablewillreactwiththecompoundofametalthatis
below it. For example, Zn is above Cu on the table. This means that Zn will
replaceCuinacompound.ZnwillbeoxidizedbyacompoundcontainingCu.The
Cu+ionwillbereducedbyelementalZn0.MetalshigherontableJaremorelikely
tobeoxidized.
Thereaction: Zn+Cu(NO3)2àCu+Zn(NO3)2willspontaneouslyoccur.
Foreachexamplebelow,ifareactionwilloccurspontaneouslybasedonthe
elementpositionsintheActivitySeries,completetheequationandbalance
it.Ifthereisnoreaction,writenoreaction.
1. Ag(s)+Cu(NO3)2(aq)à
2. Pb(s)+AuCl(aq)à
3. Au(s)+LiCl(aq)à
4. Mg(s)+Pb(NO3)2(aq)à
Determineifaspontaneousreactionwilloccur.Ifonewilloccur,write
thebalancedoxidationandreductionhalfreactions.
1. Zn+Pb(NO3)2àPb+Zn(NO3)2
•
Isthereactionspontaneous?________________
•
Ifyes,writetheoxidation½reaction:
•
Ifyes,writethereduction½reaction:
2. 3Zn+2Al(NO3)3à2Al+3Zn(NO3)2
•
Isthereactionspontaneous?________________
•
Ifyes,writetheoxidation½reaction:
•
Ifyes,writethereduction½reaction:
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12
PracticePacket:OxidationReduction
Video14.4:ElectrochemicalCells
Avoltaiccellisanelectrochemicalcell.(An
electrochemicalcellproduceselectriccurrentasaresultofa
spontaneousredoxreaction,usedtomakebatteries.They
consistoftwohalf-cellsconnectedbyasaltbridgeandtwo
electrodesthatconnecttoaloadthatusestheelectricity
producedbythecell.)Anexampleanelectrochemicalcellisa
battery.
OverallRedoxReaction:
Oxidation½Reaction:
Reduction½Reaction:
SpeciesOxidized:_________________
Anode:______________
SpeciesReduced:_________________
Cathode:____________
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13
PracticePacket:OxidationReduction
Anoperatingvoltaiccellhaszincandironelectrodes.Thecellandtheunbalancedionicequation
representingthereactionthatoccursinthecellareshownbelow.
1. Writethebalancedoxidationhalf-reactionforthiscell.
2. Writethebalancedreductionhalfreactionforthiscell.
3. If6molesofZnreact,howmanymolesofelectronswillbetransferred?
4. Explain,intermsofZnatomsandZnions,whythemassoftheZnelectrodedecreasesasthe
celloperates.
5. Identifythesubatomicparticlesthatflowthroughthewireasthecelloperates.
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14
PracticePacket:OxidationReduction
Astudentconstructsanelectrochemicalcellduringalaboratoryinvestigation.Whentheswitchis
closed,electronsflowthroughtheexternalcircuit.Thediagrambelowrepresentsthiscellandthe
reactionthatoccurs.
1. State,intermsofenergy,whythiscellisavoltaiccell.
______________________________________________________________________________________________________________
______________________________________________________________________________________________________________
2. DeterminethenumberofmolesofAlI(s)neededtocompletelyreactwith9.0molesofNi2+(aq)
ions.
3. Writethebalancedhalf-reactionequationfortheoxidationthatoccurswhentheswitchis
closed.
4. Statethedirectionofelectronflowthroughthewireandwhentheswitchisclosed.
______________________________________________________________________________________________________________
Lesson14.5:ElectrolyticCells.
Electrolyticcellsuseelectricalenergytoforceanonspontaneouschemicalreactiontooccur.
Reductionoccursatthecathode.Thecathodeistheelectrodewhereelectronsaresentandisthe
negativeelectrode.Oxidationoccursattheanode.Theanodeistheelectrodewhereelectronsare
drawnawayfromandisthepositiveelectrode.
Electroplating
MoltenSalt
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15
ElectrolysisofWater
PracticePacket:OxidationReduction
Electroplating:
Completethechart
ElectrochemicalCells
VoltaicCell
Example:
RedoxReactions
ElectrolyticCell
Example:Electroplating
2electrodes
Anode=
Cathode=ReductionNegative(-)
Anode=oxidationNegative(-)
Cathode=
Electronsflowfromanodetocathode
Useelectricalenergyforforceanonspontaneous
redoxreactiontooccur(chemical)
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16
1
14.5 Electrolytic Cells
3
on a nickel key. As the cell
operates, oxidation occurs at the silver electrode and the mass of the silver electrode decreases.
1
cell operates
2
3
4
5
4
5
17
6
8
6
7
8
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