Practice Packet: Oxidation Reduction Regents Chemistry: Dr...
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PracticePacket:OxidationReduction
Regents Chemistry: Dr. Shanzer
PracticePacketChapter14:OxidationReduction&Electrochemistry
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Chapter 1 : Electrochemistry
Cathode – The electrode at which reaction occurs (positive)
Electrode – a conductor in a circuit that carries electrons to or from a substance other than a metal
Electrochemical Cell – any device that converts chemical energy into electrical energy or electrical energy into chemical energy
Electrolytic Cell – a cell that uses electricity from an outside source to force a nonsponstanous redox reaction to occur; Examples: recharging batteries, electroplating
Electroplating – an electrolytic process that involved oxidizing a source metal into a solution with the use of an external power source and then reducing the metal ion onto a metallic object that is to be plated (“silver plated”)
Half Reaction – a reaction that describes the change in oxidation number and subsequent gain or loss of electrons that occurs during oxidation or reduction
Oxidation – a process that involves complete or partial loss of electrons or gain of oxygen; results in an increase in the oxidation number
Oxidizing Agent – the species that is reduced and therefore removes the electrons from the species that was oxidized
Oxidation Number – the charge of an ion
Redox reaction – another name for an oxidation-reduction reaction; a reaction that involves the transfer of electrons between reactants
Reduction – a process that involves a complete or partial gain of electrons or the loss of oxygen; it results in a decrease in the oxidation number
Reducing Agent – the species that is oxidized and therefore gives electrons to the species that was reduced.
e the electrode at which oxidation occurs (negative)
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Salt Bridge – a tube containing a strong electrolyte used to separate the half-cells in a voltaic cell; it allows the passage of ions form one half-cell to the other but prevents the solutions from mixing
Species – the symbol and charge of an element or ion in a redox reaction
Voltaic Cell – an electrochemical cell that produces electric current as a result of a spontaneous redox reaction, used to make batteries. Consists of two half-cells connected by a salt bridge and two electrodes that connect to a load (device) that uses the electricity produced by the cell.
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Assigning Oxidation Numbers
Chemistry 200 Video Lesson 14.1
Objective:How do we assign atoms the correct oxidation number?
Oxidation & Reduction (Redox)Oxidation number• a number assigned to keep track of electron(s) gained
or lost in a redox rxns.
2. The Group 1 metals (Alkali Metals) in compoundsalways have an oxidation state of +1
3. The Group 2 metals (Alkali Earth Metals) incompounds always have an oxidation state of +2
4. The oxidation state for any simpleone-atom ion(monoatomic) is equalto its charge.
Rules for Assigning Oxidation Numbers (states)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.
In MgCl2, the Mg2+ ion has an oxidation number of +2.Each of the Cl- ions has an oxidation number of -1.
In FeCl2, the Fe2+ ion has an oxidation number of +2, while in FeCl3 the Fe3+ ion has an oxidation number of +3.5. Fluorine in compounds is always assigned an
oxidation state of -1.
6. Hydrogen in compounds is always assignedan oxidation number of +1. (HCl).If combined w/ a metal, Hydrogenhas an oxidation # of -1. (LiH)
7. Oxygen in compounds is assigned an oxidation state of -2.
**When combined w/ Fluorine, Oxygen has an oxidation state of +2.**
8. The sum of the oxidation states of all the atoms in aspecies must be equal to the net charge on thespecies.
If the species is neutral, the sum of the oxidation states is zero.
If the species has a charge, the sum is equal to that charge.
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Determine the oxidation number of sulfur in H2SO4
H2SO4+1 -2+6
(-8)(+2) =0+6
Determine the oxidation number of nitrogen in NO3
-1
NO3-2+5
-1
(-6)= -1+5
Redox Reactions
Chemistry 200 Video Lesson 14.2
Objective: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 ?
RedoxRedox 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 )
Reduction• gain of electron(s) by an atom or ion & a
decrease in oxidation #( Mn+7 à Mn+2)
**Oxidation & Reduction occur simultaneously, they cannot occur separately**
+ 2e-
5e- +
Easy way to remember!!!
LEO says GERLEO = Loss of Electrons is OxidationGER = Gain of Electrons is Reduction
GER!!!!!Chemistry Yum Yum
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Oxidizing Agent
• the substance that causes the oxidation of othersubstances. They accept electron(s) easily &therefore are reduced
ex1: 5e- + Mn+7 à Mn+2
(gain of electrons, oxidation # reduced)
Reducing Agent
• the substance that allows another substance to bereduced. They lose electron(s) & therefore are oxidized
ex: Ca à Ca+2 + 2e- (loss of electrons, oxidation # increases)
**The species oxidized, the species reduced, the oxidizing agent or reducing agent must always be a reactant!!**
Gains Electrons
Oxidizing Agent
Reduced
Loses Electrons
Reducing Agent
Oxidized
Writing Half Reactions
• They show either the oxidation or reduction portion of aredox rxn, including electrons gained or lost
Half rxn for oxidation --> electrons are productsHalf rxn for reduction --> electrons are reactants
**Electronsgoonthesidew/themorepositiveoxid.#**
THERE’S AN EASIER WAY TO REMEMBER!!!
Creating Half Reactions from a Redox Reaction1. Assign oxidation numbers to determine the
substance oxidized & the substance reduced.
2. Write each half reaction, balance by atom, then byelectrons. The ONLY exception is a half rxn thecontains a diatomic element.
3. Identify the species oxidized, the species reducedthe oxidizing agent & the reducing agent.
KClO3 --> KCl + O2+1 -2+5
-6+1+5+1-1 0
Oxid: Red:
O-2 à O22 + 4e-
Cl+5 à Cl-16e- +
(reducing agent)
(oxidizing agent)
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Electrochemical Cells
Video Lesson 14.4
Objectives• Name the type of reactions involved in
electrochemical processes.• Describe how a voltaic cell produces
electrical energy.
Electrochemical Process• An electrochemical process is any
conversion between chemical andelectrical energy (charged particles).
• All electrochemical processes involve redoxreactions.
• The two half reactions must be physicallyseparated to be used as a source ofelectrical energy.
Voltaic Cells• 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 Cathode
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Reduction occurs at the cathode
Oxidation occurs at the anode
From Anode to Cathode
Flow of Electrons Voltaic CellOverall Redox Rxn
Zn(s) + Cu+2(aq) --> Zn+2
(aq) + Cu(s)
Oxid:Red:
Zn(s) --> Zn+2(aq)+ 2e-
Cu+2(aq) --> Cu(s)2e- +
Species oxidized_____ Reducing agent______Species reduced_____ Oxidizing agent_____Anode_______ Cathode_______
Zn
Cu+2 Cu+2
Zn
Zn+2 Cu+2
Zn(s)anode -
Cu(s)cathode +
e- -->
Zn Cu
Zn Cu
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Sketch Notes
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Name:_____________________________________________________Date:_____________________Per:__________
Assigning Oxidation Numbers
Formula Element and Oxidation Number
1. NO2 N O
2. KCl K Cl
3. MnO2 Mn O
4. H2SO4 H S O
5. K3PO4 K P O
6. HNO3 H N O
7. Fe2O3 Fe O
8. CaCl2 Ca Cl
9. Na2S2O3 Na S O
10. CH4 C H
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PracticePacket:�����
Video14.1:OxidationNumbersDeterminetheoxidationnumberofEACHelementineachofthefollowingsubstances:
1. KMnO4
2. S8
3. Na2Cr2O7
4. CuCl2
5. H2SO4
6. PO4-3
7. zincoxide
8. water
9. calciumhydride
10. carbondioxide
Video14.2:RedoxReactionsWritingHalfReactions
Step1:BalancethehalfreactionbyatomusingcoefficientsStep2:Balancethehalfreactionbychargeusingelectrons(e-)
Electronsalwaysgoonthesidewiththemorepositiveoxidation#
**Halfrxnsarewrittenonaperatombasis.Theonlyexceptionisifthehalfrxncontainsadiatomicelement**
MgàMg+2
O2àO-2
Cl+5àCl-1
Mn+2àMn+5
N-3àN2
S+6àS-2
3Cu+1à3Cu
6H+1à3H2
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Practice Packet:Redox
Creating Half Reactions from Redox Reactions Step 1: Assign oxidation numbers to determine the substances that have a change in oxidation number Step 2: Identify the two half reactions & balance each half reaction Step 3: Label each half reaction & identify the species oxidized, the species reduced, the oxidizing agent & the reducing agent Note:Thereactionprovidedtoyoumaybebalancedorunbalanced.Rememberthathalfreactionsaremadeonaperatombasis.TheONLYexceptionisahalfreactionthatcontainsadiatomicelement
CuSO4 + Mn à Mn(SO4)2 + Cu Species oxidized ______________ Oxidizing Agent ______________
Species reduced ______________ Reducing Agent ______________
Oxidation: Reduction:
AgF + Fe à FeF3 + Ag Species oxidized ______________ Oxidizing Agent ______________
Species reduced ______________ Reducing Agent ______________
Oxidation: Reduction:
Na + Cl2 à NaCl Species oxidized ______________ Oxidizing Agent ______________
Species reduced ______________ Reducing Agent ______________
Oxidation: Reduction:
H2 + O2 à H2O Species oxidized ______________ Oxidizing Agent ______________
Species reduced ______________ Reducing Agent ______________
Oxidation: Reduction:
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Practice Packet: Oxidation Reduction
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S + O2 à SO3 Species oxidized ______________ Oxidizing Agent ______________
Species reduced ______________ Reducing Agent ______________
Oxidation: Reduction:
Fe + HCl à H2 + FeCl3 Species oxidized ______________ Oxidizing Agent ______________
Species reduced ______________ Reducing Agent ______________
Oxidation: Reduction:
CH4 + O2 à CO2 + H2O Species oxidized ______________ Oxidizing Agent ______________
Species reduced ______________ Reducing Agent ______________
Oxidation: Reduction:
KClO3 à KCl + O2 Species oxidized ______________ Oxidizing Agent ______________
Species reduced ______________ Reducing Agent ______________
Oxidation: Reduction:
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PracticePacket:OxidationReduction
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Lesson14.3:ActivitySeriesandSpontaneity
Table J:The table is arrangedwith themost reactivemetals at the topof thetableandtheleastreactivemetalsatthebottomofthetable.Whatthismeansisthatametal listedonthetablewillreactwiththecompoundofametal that isbelow it. For example, Zn is above Cu on the table. This means that Zn willreplaceCuinacompound.ZnwillbeoxidizedbyacompoundcontainingCu.TheCu+ionwillbereducedbyelementalZn0.MetalshigherontableJaremorelikelytobeoxidized.
Thereaction: Zn+Cu(NO3)2àCu+Zn(NO3)2willspontaneouslyoccur.
Foreachexamplebelow,ifareactionwilloccurspontaneouslybasedontheelementpositionsintheActivitySeries,completetheequationandbalanceit.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,writethebalancedoxidationandreductionhalfreactions.
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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PracticePacket:OxidationReduction
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Video14.4:ElectrochemicalCellsAvoltaiccellisanelectrochemicalcell. Avoltaic
cellproduceselectriccurrentasaresultofaspontaneousredoxreaction,usedtomakebatteries.Theyconsistoftwohalf-cellsconnectedbyasaltbridgeandtwoelectrodesthatconnecttoaloadthatusestheelectricityproducedbythecell.)Anexampleof anelectrochemicalcellisabattery.
OverallRedoxReaction:
Oxidation½Reaction: Reduction½Reaction:
SpeciesOxidized:_________________ Anode:______________
SpeciesReduced:_________________ Cathode:____________
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PracticePacket:OxidationReduction
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Anoperatingvoltaiccellhaszincandironelectrodes.Thecellandtheunbalancedionicequationrepresentingthereactionthatoccursinthecellareshownbelow.
1. Writethebalancedoxidationhalf-reactionforthiscell.
2. Writethebalancedreductionhalfreactionforthiscell.
3. If6molesofZnreact,howmanymolesofelectronswillbetransferred?
4. Explain,intermsofZnatomsandZnions,whythemassoftheZnelectrodedecreasesasthecelloperates.
5. Identifythesubatomicparticlesthatflowthroughthewireasthecelloperates.
+ +
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PRACTICE PACKET: ELECTROCHEMISTRY
LESSON 14.4: Electrochemical Cells
Voltaic Cells (batteries) Directions: In each of the following, determine which element oxidized easier on table J (higher up on table J). Then label the anode, cathode, direction of e- flow, (remember electrons flow from high to low), which electrode increases and decreases in mass and then write the half reactions in the spaces provided.
1. 2.
ox: ox: red: red:
3. 4.
ox: ox: red: red:
Objective:x Determine the flow of electrons in a battery (voltaic cell) x Identify the anode and cathode in a voltaic cell
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PracticePacket:OxidationReduction
MoltenSalt
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Astudentconstructsanelectrochemicalcellduringalaboratoryinvestigation.Whentheswitchisclosed,electronsflowthroughtheexternalcircuit.Thediagrambelowrepresentsthiscellandthereactionthatoccurs.
1. State,intermsofenergy,whythiscellisavoltaiccell.____________________________________________________________________________________________________________________________________________________________________________________________________________________________
2. DeterminethenumberofmolesofAlI(s)neededtocompletelyreactwith9.0molesofNi2+(aq)ions.
3. Writethebalancedhalf-reactionequationfortheoxidationthatoccurswhentheswitchisclosed.
4. Statethedirectionofelectronflowthroughthewireandwhentheswitchisclosed.______________________________________________________________________________________________________________
Lesson14.5:ElectrolyticCells.Electrolyticcellsuseelectricalenergytoforceanonspontaneouschemicalreactiontooccur.Reductionoccursatthecathode.Thecathodeistheelectrodewhereelectronsaresentandisthenegativeelectrode.Oxidationoccursattheanode.Theanodeistheelectrodewhereelectronsaredrawnawayfromandisthepositiveelectrode.
Electroplating ElectrolysisofWater
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PracticePacket:OxidationReduction
http://drshanzerchemistry.weebly.com
Electroplating:
CompletethechartElectrochemicalCells
VoltaicCell ElectrolyticCellExample: Example:ElectroplatingRedoxReactions
2electrodesAnode=oxidationNegative(-) Anode=Cathode= Cathode=ReductionNegative(-)Electronsflowfromanodetocathode
Useelectricalenergyforforceanonspontaneousredoxreactiontooccur(chemical)
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