Practice Packet: Oxidation Reduction Regents Chemistry: Dr...

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Practice Packet: Oxidation Reduction Regents Chemistry: Dr. Shanzer Practice Packet Chapter 14: Oxidation Reduction & Electrochemistry 211

Transcript of 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

16

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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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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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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. Avoltaic

cellproduceselectriccurrentasaresultofaspontaneousredoxreaction,usedtomakebatteries.Theyconsistoftwohalf-cellsconnectedbyasaltbridgeandtwoelectrodesthatconnecttoaloadthatusestheelectricityproducedbythecell.)Anexampleof anelectrochemicalcellisabattery.

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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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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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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Electroplating:

CompletethechartElectrochemicalCells

VoltaicCell ElectrolyticCellExample: Example:ElectroplatingRedoxReactions

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

Useelectricalenergyforforceanonspontaneousredoxreactiontooccur(chemical)

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