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Practice Packet: Oxidation Reduction Regents Chemistry: Mrs. Mintz Practice Packet Chapter 14: Oxidation Reduction & Electrochemistry 1

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Page 1: Practice Packet: Oxidation Reduction Regents Chemistry ...mintzchemistry.weebly.com/uploads/4/8/8/9/48892969/redox_packet.pdf · Practice Packet: Oxidation Reduction Regents Chemistry:

PracticePacket:OxidationReduction

Regents Chemistry: Mrs. Mintz

PracticePacketChapter14:OxidationReduction&Electrochemistry

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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 and 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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PracticePacket:Redox

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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Name: 14.1 Oxidation Numbers

1) –1 2) +2 3) –3 4) +4

1. What is the oxidation state of nitrogen inthe compound NH4Br?

1) –1 2) +2 3) +6 4) +4

2. What is the oxidation number of sulfur inNa2S2O3 ?

3. Given the balanced equation representinga reaction:

2KClO3(s) ® 2KCl(s) + 3O2(g)

1) –1 to +12) –1 to +5

3) + l to –14) +5 to –1

The oxidation state of chlorine in this reactionchanges from

1) +6 2) +2 3) +3 4) +8

4. What is the oxidation number of chromiumin the chromate ion, CrO42– ?

1) +7 2) +2 3) +3 4) +4

5. What is the oxidation number assigned tomanganese in KMnO4?

1) +1 2) +2 3) +3 4) +4

6. What is the oxidation state of nitrogen inNaNO2?

1) +12 2) +2 3) +3 4) +6

7. What is the oxidation number of chromiumin K2Cr2O7 ?

8. Given the reaction that occurs in anelectrochemical cell:

Zn(s) + CuSO4(aq) ® ZnSO4(aq) +Cu(s)

1) 0 to +22) 0 to –2

3) +2 to 04) –2 to 0

During this reaction, the oxidation number of Znchanges from

1) LiH2) H2O

3) H2S4) H2

9. In which substance does hydrogen havean oxidation number of zero?

1) CO2) CO2

3) CCl44) CH4

10. In which compound does carbon have anoxidation state of –4?

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PracticePacket:Redox

CreatingHalfReactionsfromRedoxReactionsStep1:AssignoxidationnumberstodeterminethesubstancesthathaveachangeinoxidationnumberStep2:Identifythetwohalfreactions&balanceeachhalfreactionStep3:Labeleachhalfreaction&identifythespeciesoxidized,thespeciesreduced,theoxidizingagent&thereducingagentNote:Thereactionprovidedtoyoumaybebalancedorunbalanced.Rememberthathalfreactionsaremadeonaperatombasis.TheONLYexceptionisahalfreactionthatcontainsadiatomicelement

Cu+2+MnàMn+4+CuSpeciesoxidized______________ OxidizingAgent______________

Speciesreduced______________ ReducingAgent______________

Oxidation: Reduction:

3Ag+1+FeàFe+3+3AgSpeciesoxidized______________ OxidizingAgent______________

Speciesreduced______________ ReducingAgent______________

Oxidation: Reduction:

Na+Cl2àNaClSpeciesoxidized______________ OxidizingAgent______________

Speciesreduced______________ ReducingAgent______________

Oxidation: Reduction:

2H2+O2à2H2O

Speciesoxidized______________ OxidizingAgent______________

Speciesreduced______________ ReducingAgent______________

Oxidation: Reduction:

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2S+3O2à2SO3Speciesoxidized______________ OxidizingAgent______________

Speciesreduced______________ ReducingAgent______________

Oxidation: Reduction:

2Fe+6HClà3H2+2FeCl3Speciesoxidized______________ OxidizingAgent______________

Speciesreduced______________ ReducingAgent______________

Oxidation: Reduction:

CH4+2O2àCO2+2H2OSpeciesoxidized______________ OxidizingAgent______________

Speciesreduced______________ ReducingAgent______________

Oxidation: Reduction:

2KClO3à2KCl+3O2

Speciesoxidized______________ OxidizingAgent______________

Speciesreduced______________ ReducingAgent______________

Oxidation: Reduction:

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Name: 14.2 Half Reactions

1) sharing of electrons2) sharing of protons3) transfer of electrons4) transfer of protons

1. An oxidation-reduction reaction involves the

1) transmutation2) reduction

3) oxidation4) neutralization

2. During which process does an atom gain one ormore electrons?

1) Mn4+ ® Mn3+ + e–

2) Mn4+ ® Mn7+ + 3e–

3) Mn4+ + e– ® Mn3+

4) Mn4+ + 3e– ® Mn7+

3. Which half-reaction correctly represents reduction?

1) less than the total number of electrons gained2) greater than the total number of electrons

gained3) equal to the total number of electrons gained4) equal to the total number of protons gained

4. In a redox reaction, the total number of electrons lostis

1) Zn2+ 2) Mg2+ 3) Co2+ 4) Ca2+

5. Which ion is most easily reduced?

1) Al Al3+ + 3e–

2) Al3+ + 3e– Al3) Cu Cu2+ + 2e–

4) Cu2+ + 2e– Cu

6. Given the balanced ionic equation representing areaction:

2Al(s) + 3Cu2+(aq) 2Al3+(aq) + 3Cu(s)Which half-reaction represents the reduction thatoccurs?

1)2)

3)4)

7. Which equation represents an oxidation-reductionreaction?

1) Cu + e– ® Cu+

2) Cu2+ + 2e– ® Cu3) Cu+ ® Cu + e–

4) Cu2+ ® Cu + 2e–

8. Which half-reaction shows conservation of charge?

1) Ba(NO3)2 + Na2SO4 ®BaSO4 + 2NaNO3

2) H3PO4 + 3KOH ®K3PO4 + 3H2O3) Fe(s) + S(s) ®FeS(s)4) NH3(g) + HCl(g) ®NH4Cl(s)

9. Which balanced equation represents anoxidation-reduction reaction?

1) Na+ + e– ® Na2) Na ® Na+ + e–

3) Cl2 + 2e– ® Cl–4) 2 Cl– ® Cl2 + 2e–

10. Which expression correctly represents a balancedreduction half-reaction?

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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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Video14.4:ElectrochemicalCellsAvoltaiccellisanelectrochemicalcell.(An

electrochemicalcellproduceselectriccurrentasaresultofaspontaneousredoxreaction,usedtomakebatteries.Theyconsistoftwohalf-cellsconnectedbyasaltbridgeandtwoelectrodesthatconnecttoaloadthatusestheelectricityproducedbythecell.)Anexampleanelectrochemicalcellisabattery.

OverallRedoxReaction:

Oxidation½Reaction: Reduction½Reaction:

SpeciesOxidized:_________________ Anode:______________

SpeciesReduced:_________________ Cathode:____________

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Anoperatingvoltaiccellhaszincandironelectrodes.Thecellandtheunbalancedionicequationrepresentingthereactionthatoccursinthecellareshownbelow.

1. Writethebalancedoxidationhalf-reactionforthiscell.

2. Writethebalancedreductionhalfreactionforthiscell.

3. If6molesofZnreact,howmanymolesofelectronswillbetransferred?

4. Explain,intermsofZnatomsandZnions,whythemassoftheZnelectrodedecreasesasthecelloperates.

5. Identifythesubatomicparticlesthatflowthroughthewireasthecelloperates.

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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 MoltenSalt ElectrolysisofWater

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Electroplating:

CompletethechartElectrochemicalCells

VoltaicCell ElectrolyticCellExample: Example:ElectroplatingRedoxReactions

2electrodesAnode=oxidationNegative(-) Anode=Cathode= Cathode=ReductionNegative(-)Electronsflowfromanodetocathode

Useelectricalenergyforforceanonspontaneousredoxreactiontooccur(chemical)

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