rules for assigning oxidation #’s
DESCRIPTION
Rules for Assigning Oxidation #’s. Elements by themselves are neutral Ox # = 0 Ex: Na 0 , O 2 0 , Mg 0 Monoatomic Ions show their oxidation # as their written charge Ex: H +1 , Cl -1 , Al +3. Group #1 Elements in compounds: Ox # = +1Ex: LiBr, NaCl Group #2 Elements in compounds: - PowerPoint PPT PresentationTRANSCRIPT
Rules for Assigning Rules for Assigning Oxidation #’sOxidation #’s
Elements by themselves are neutralElements by themselves are neutral
Ox # = 0Ox # = 0
Ex: NaEx: Na00, O, O2200, Mg, Mg00
Monoatomic Ions show their oxidation # as Monoatomic Ions show their oxidation # as their written chargetheir written charge
Ex: HEx: H+1+1, Cl, Cl-1-1, Al, Al+3+3
Group #1 ElementsGroup #1 Elements in compounds: in compounds:
Ox # = +1Ox # = +1 Ex: LiBr, NaClEx: LiBr, NaCl
Group #2 ElementsGroup #2 Elements in compounds: in compounds:
Ox # = +2Ox # = +2 Ex: MgBrEx: MgBr22, CaCl, CaCl22
AluminumAluminum in compounds: in compounds:
Ox # = +3Ox # = +3 Ex: AlClEx: AlCl33
FluorineFluorine in compounds in compounds
Ox # = -1Ox # = -1 Ex: LiF, MgFEx: LiF, MgF22
HydrogenHydrogen: :
Ox # = +1 (most common)Ox # = +1 (most common)when combined with nonmetalswhen combined with nonmetals
Ex: HCl, HEx: HCl, H22SOSO44, H, H22SS
Ox # = -1Ox # = -1When combined with metals (metal hydrides)When combined with metals (metal hydrides)
Ex: LiH, MgHEx: LiH, MgH22
OxygenOxygen:: Oxidation # = -2 (usually) Oxidation # = -2 (usually)Ex: COEx: CO22, H, H22OO
Special Cases:Special Cases:Peroxides: Oxygen is a diatomic ion (OPeroxides: Oxygen is a diatomic ion (O22))-2-2 with with
total charge of -2, each oxygen has -1 chargetotal charge of -2, each oxygen has -1 chargeEx: HEx: H22OO22, BaO, BaO22
When bonded with Fluorine: Ox # = +2When bonded with Fluorine: Ox # = +2Ex: OFEx: OF22
How to Find Charges If No “Rule”?How to Find Charges If No “Rule”?
Sum of Individual Ox # of all the elements Sum of Individual Ox # of all the elements in a compound = 0in a compound = 0All compounds are NEUTRALAll compounds are NEUTRAL
Ex: NaClOEx: NaClO33
What is the ox # for each element?What is the ox # for each element?
Draw your Lines….Draw your Lines….
How to Find Charges If No “Rule”?How to Find Charges If No “Rule”?
Sum of Ox # of all atoms in a polyatomic Sum of Ox # of all atoms in a polyatomic ion is equal to the charge of that ion.ion is equal to the charge of that ion.
Ex: POEx: PO44-3-3
What is the charge of each element?What is the charge of each element?
Let’s PracticeLet’s Practice
What is the oxidation number of sulfur in What is the oxidation number of sulfur in NaNa22SS22OO33??
(1) -1 (1) -1
(2) +6(2) +6
(3) +2 (3) +2
(4) +4 (4) +4
What is the oxidation number of chromium What is the oxidation number of chromium in the chromate ion, CrOin the chromate ion, CrO4 4
2–2– ? ?
(1) +6 (1) +6
(2) +3(2) +3
(3) +2 (3) +2
(4) +8 (4) +8
In which compound does chlorine have the In which compound does chlorine have the highest oxidation number? highest oxidation number?
(1) NaClO (1) NaClO
(2) NaClO(2) NaClO33
(3) NaClO(3) NaClO22
(4) NaClO(4) NaClO44
What is the oxidation number assigned to What is the oxidation number assigned to manganese in KMnOmanganese in KMnO44??
(1) +7 (1) +7
(2) +3(2) +3
(3) +2 (3) +2
(4) +4 (4) +4
Mahjong Oxidation # Game:Mahjong Oxidation # Game:http://www2.stetson.edu/mahjongchem/http://www2.stetson.edu/mahjongchem/
Oxidation and Reduction Oxidation and Reduction ReactionsReactions
Oxidation (Read only)Oxidation (Read only)
Original definition:Original definition:When substances combined with oxygenWhen substances combined with oxygen..
Ex:Ex:All combustion (burning) reactionsAll combustion (burning) reactions
CHCH44(g) + 2O(g) + 2O22(g) (g) COCO22(g) + 2H(g) + 2H22O(l)O(l)
All “rusting” reactionsAll “rusting” reactions
4Fe(s) + 3O4Fe(s) + 3O22(g)(g) 2Fe2Fe22OO33(s)(s)
Reduction (Read Only)Reduction (Read Only)
Original Definition:Original Definition:
Reaction where a substance “gave up” oxygen.Reaction where a substance “gave up” oxygen.
Called “reductions” because they producedCalled “reductions” because they produced
products that were “reduced” in mass becauseproducts that were “reduced” in mass because
gas escaped.gas escaped.
Ex:Ex:
2Fe2Fe22OO33(l) + 3C(s)(l) + 3C(s) 4Fe(l) + 3CO 4Fe(l) + 3CO22(g)(g)
Oxidation/Reduction ReactionsOxidation/Reduction Reactions
Oxidation:Oxidation: LOSS of one or more electrons. LOSS of one or more electrons.
Reduction:Reduction: GAIN of one or more electrons GAIN of one or more electrons
Oxidation & reduction always occur together.Oxidation & reduction always occur together.
• Deal with a movement of Deal with a movement of ELECTRONSELECTRONS
between atoms during a reaction.between atoms during a reaction.
• Electrons travel from what is oxidizedElectrons travel from what is oxidized
towards what is reduced.towards what is reduced.
One atom loses e-, One atom loses e-,
the other gains e-the other gains e-
This is called This is called “electron transfer”“electron transfer”
Remember!!Remember!!
Or…RememberOr…Remember
Redox ReactionsRedox Reactions:: ALWAYSALWAYS involve changes in charge involve changes in charge
If charges don’t change it’s NOT a Redox rxn.If charges don’t change it’s NOT a Redox rxn.
Conservation of “Charge”Conservation of “Charge”
Total electrons lost = Total electrons gainedTotal electrons lost = Total electrons gained
Redox Reactions must balance electrons as well as atoms!
Let’s PracticeLet’s Practice
Which changes occur when PtWhich changes occur when Pt2+2+ is reduced? is reduced?
(1) Pt(1) Pt2+2+ gains electrons and its oxidation number increases. gains electrons and its oxidation number increases.
(2) Pt(2) Pt2+2+ gains electrons and its oxidation number decreases. gains electrons and its oxidation number decreases.
(3) Pt(3) Pt2+2+ loses electrons and its oxidation number increases. loses electrons and its oxidation number increases.
(4) Pt(4) Pt2+2+ loses electrons and its oxidation number decreases. loses electrons and its oxidation number decreases.
Answer: 1Answer: 1
Given the balanced equation representing a redox Given the balanced equation representing a redox reaction:reaction:
2Al + 3Cu2Al + 3Cu2+2+ →→ 2Al 2Al3+3+ + 3Cu + 3Cu
Which statement is true about this reaction?Which statement is true about this reaction?
(1) Each Al loses 2e- and each Cu(1) Each Al loses 2e- and each Cu2+2+ gains 3e- gains 3e-
(2) Each Al loses 3e- and each Cu(2) Each Al loses 3e- and each Cu2+2+ gains 2e- gains 2e-
(3) Each Al(3) Each Al3+3+ gains 2e- and each Cu loses 3e- gains 2e- and each Cu loses 3e-
(4) Each Al(4) Each Al3+3+ gains 3e- and each Cu loses 2e- gains 3e- and each Cu loses 2e-
Answer: 2Answer: 2
In an oxidation-reduction reaction, reduction In an oxidation-reduction reaction, reduction is defined as theis defined as the
(1) loss of protons (1) loss of protons
(2) loss of electrons(2) loss of electrons
(3) gain of protons (3) gain of protons
(4) gain of electrons (4) gain of electrons
Which change in oxidation number indicates Which change in oxidation number indicates oxidation?oxidation?
(1) –1 to +2(1) –1 to +2 (2) +2 to –3(2) +2 to –3
(3) –1 to –2 (3) –1 to –2 (4) +3 to +2 (4) +3 to +2
When a neutral atom undergoes oxidation, When a neutral atom undergoes oxidation, the atom’s oxidation statethe atom’s oxidation state
(1) decreases as it gains electrons(1) decreases as it gains electrons
(2) decreases as it loses electrons(2) decreases as it loses electrons
(3) increases as it gains electrons(3) increases as it gains electrons
(4) increases as it loses electrons(4) increases as it loses electrons
Oxidizing/Reducing AgentsOxidizing/Reducing Agents
Oxidizing AgentOxidizing Agent::substance reducedsubstance reduced Gains electronsGains electrons
Reducing Agent:Reducing Agent: substance oxidizedsubstance oxidized Loses electronsLoses electrons
The “Agent” is the “opposite”The “Agent” is the “opposite”
Identify What is Changing in Identify What is Changing in ChargeCharge
What is oxidized and reduced?What is oxidized and reduced?
What are the oxidizing and reducing agents?What are the oxidizing and reducing agents?
Ex:Ex:
3Br3Br22 + 2AlI + 2AlI33 2AlBr2AlBr33 + 3I + 3I22
00 +3 -1 +3 -1 +3 -1 0 +3 -1 0
3Br3Br22 + 2AlI + 2AlI33 2AlBr2AlBr33 + 3I + 3I22
BrBr22 is reduced and is the oxidizing agent is reduced and is the oxidizing agent
II-1-1 is oxidized and is the reducing agent is oxidized and is the reducing agent
What is oxidized and reduced?What is oxidized and reduced?What are the oxidizing and reducing agents?What are the oxidizing and reducing agents?
Mg + CuSOMg + CuSO44 MgSOMgSO44 + Cu + Cu
2K + Br2K + Br22 2KBr2KBr
Cu + 2AgNOCu + 2AgNO33 Cu(NO Cu(NO33))22 + 2Ag + 2Ag
NOTE: NOTE: Atoms in a polyatomic ion DO NOT change in charge!Atoms in a polyatomic ion DO NOT change in charge!
0 +2 +2 00 +2 +2 0
Mg + CuSOMg + CuSO44 MgSOMgSO44 + Cu + CuMg oxidized (reducing agent)Mg oxidized (reducing agent)CuCu+2+2 reduced (oxidizing agent) reduced (oxidizing agent)
0 0 +1 -10 0 +1 -1
2K + Br2K + Br22 2KBr2KBrK oxidized (reducing agent)K oxidized (reducing agent)
BrBr2 2 reduced (oxidizing agent)reduced (oxidizing agent)
00 +1 +1 +2 0+2 0
Cu + 2AgNOCu + 2AgNO33 Cu(NO Cu(NO33))22 + 2Ag + 2AgCu oxidized (reducing agent)Cu oxidized (reducing agent)AgAg+1+1 reduced (oxidizing agent) reduced (oxidizing agent)
Redox or Not Redox Redox or Not Redox (that is the question…)(that is the question…)
Redox Reactions:Redox Reactions: must have atoms changing in must have atoms changing incharge.charge.
Not all reactions are redox.Not all reactions are redox.
Easy way to spot a redox reaction!!!Easy way to spot a redox reaction!!!Look for elements entering and leavingLook for elements entering and leavingcompoundscompounds..
Is it Redox?Is it Redox?
Look for Changes in Charge! Look for Changes in Charge! Are elements entering and leaving compounds?Are elements entering and leaving compounds?
Synthesis:Synthesis:
Ex:Ex: 2H2H22 + O + O22 2H2H22OO
Decomposition:Decomposition:
Ex:Ex: 2KClO2KClO33 2KCl + 3O2KCl + 3O22
Is it Redox?Is it Redox?
SynthesisSynthesis: : YESYES
00 0 0 +1 -2 +1 -2
Ex:Ex: 2H2H22 + O + O22 2H2H22OO
DecompositionDecomposition: : YESYES
+1 +5 -2+1 +5 -2 +1 -1 0 +1 -1 0
Ex:Ex: 2KClO2KClO33 2KCl + 3O2KCl + 3O22
Is it Redox?Is it Redox?
Combustion:Combustion:
CHCH44 + 2O + 2O22 COCO22 + 2H + 2H2200
Single Replacement:Single Replacement:
Zn + CuClZn + CuCl22 ZnClZnCl22 + Cu + Cu
Is it Redox?Is it Redox?
Combustion:Combustion: YESYES-4 +1 0 +4 -2 +1 -2-4 +1 0 +4 -2 +1 -2
CHCH44 + 2O + 2O22 COCO22 + 2H + 2H2200
Single Replacement:Single Replacement:YESYES 0 +2 -1 +2 -1 00 +2 -1 +2 -1 0
Zn + CuClZn + CuCl22 ZnClZnCl22 + Cu + Cu
Is it Redox?Is it Redox?
Double Replacement:Double Replacement:
AgNOAgNO33 + LiCl + LiCl AgCl + LiNO AgCl + LiNO33
Is it Redox?Is it Redox?
Double Replacement:Double Replacement: NO!!!!NO!!!!
Ions switch partners, but don’t change in chargeIons switch partners, but don’t change in charge
+1 +5 -2 +1 -1 +1 -1 +1 +5 -2+1 +5 -2 +1 -1 +1 -1 +1 +5 -2
AgNOAgNO33 + LiCl + LiCl AgCl + LiNO AgCl + LiNO33
Remember charges of atoms inside polyatomicRemember charges of atoms inside polyatomic
Ions do not change!Ions do not change!
Let’s PracticeLet’s Practice
Which equation represents an oxidationWhich equation represents an oxidationreduction reaction?reduction reaction?
(1) CH(1) CH44 + 2O + 2O22 →→ CO CO22 + 2H + 2H22OO
(2) H(2) H22SOSO44 + Ca(OH) + Ca(OH)22 →→ CaSO CaSO44 + 2H + 2H22OO
(3) MgCrO(3) MgCrO44 + BaCl + BaCl22 →→ MgCl MgCl22 + BaCrO + BaCrO44
(4) Zn(NO(4) Zn(NO33))22 + Na + Na22COCO33 →→ 2NaNO 2NaNO33 + ZnCO + ZnCO33
Which reaction is an example of anWhich reaction is an example of anoxidation reduction reaction?oxidation reduction reaction?
(1) AgNO(1) AgNO33 + KI + KI →→AgI + KNOAgI + KNO33
(2) Cu + 2 AgNO(2) Cu + 2 AgNO33 →→ Cu(NO Cu(NO33))22 + 2 Ag + 2 Ag
(3) 2 KOH + H(3) 2 KOH + H22SOSO44 →→ K K22SOSO44 + 2H + 2H22OO
(4) Ba(OH)(4) Ba(OH)22 + 2HCl + 2HCl →→ BaCl BaCl22 + 2H + 2H22OO
Writing Half ReactionsWriting Half Reactions
Redox Reactions are composed of two partsRedox Reactions are composed of two parts
or half reactions.or half reactions.
Half Reactions Show:Half Reactions Show:
Element being oxidized or reduced.Element being oxidized or reduced.
Change in chargeChange in charge
# of moles of e# of moles of e-- being lost or gained being lost or gained
http://www.kentchemistry.com/links/Redox/flash/RedoxOxNumbers.swf
Writing Half ReactionsWriting Half Reactions
0 00 0 +1 -1 +1 -1
2Na + F2Na + F22 2NaF2NaF
Oxidation:Oxidation: NaNa Na Na+1+1 + 1e- + 1e-oror 2Na2Na 2Na 2Na+1 +1 + 2e- + 2e-
Note: e- are “lost” (on the right of arrow)Note: e- are “lost” (on the right of arrow)
Reduction:Reduction: F + 1e-F + 1e- F F-1-1
oror FF22 + 2e- + 2e- 2F 2F-1-1
Note: e- are “gained” (on the left of arrow)Note: e- are “gained” (on the left of arrow)
Ox’s Have Tails!!Ox’s Have Tails!!
Oxidation Half reactions always have Oxidation Half reactions always have “tails” of electrons“tails” of electrons
NaNa Na Na+1+1 + 1e- + 1e-
00 +2 -1 +2 -1 +2 -1 0+2 -1 0
Zn + CuClZn + CuCl22 ZnClZnCl22 + Cu + Cu
Ox:Ox: ZnZn ZnZn+2+2 + 2e- + 2e-
Red:Red: CuCu+2+2 + 2e- + 2e- CuCu
https://www.youtube.com/watch?v=-wvnX1f7yRYTutorial on Writing Half Reactions
Balancing Simple Redox RxnsBalancing Simple Redox Rxns
Must be:Must be:
Balanced for MassBalanced for Mass
ATOMS balanceATOMS balance
Balanced for ChargeBalanced for Charge
Total e- Lost = Total e- GainedTotal e- Lost = Total e- Gained
Applications of Redox ReactionsApplications of Redox Reactions
Corrosion of MetalsCorrosion of Metals
Metals gets oxidized byMetals gets oxidized by
oxygen in the air formingoxygen in the air forming
metal oxides (rust)metal oxides (rust)
4Fe(s) + 3O4Fe(s) + 3O22(g) (g) →→ 2Fe 2Fe22OO33(s)(s)
Prevention:Prevention: Use paint, oil, Use paint, oil,
““Plating” or attach to negativePlating” or attach to negative
terminal of a battery.terminal of a battery. Gold doesn’t rust…Why?
Ships or pipes made of Fe will “rust Ships or pipes made of Fe will “rust away” into Feaway” into Fe+2 +2 ions when oxidized.ions when oxidized.
Blocks of more reactive metals (see Blocks of more reactive metals (see Table J) like Mg or Zn are attached to Table J) like Mg or Zn are attached to ships or underground pipes.ships or underground pipes.
Electrons travel from more reactive Electrons travel from more reactive metal to less reactive iron preventing it metal to less reactive iron preventing it from oxidizing.from oxidizing.
Aluminum forms an oxide coating that Aluminum forms an oxide coating that protects the metal from further corrosion.protects the metal from further corrosion.
Photograph DevelopmentPhotograph Development involves oxidation and involves oxidation and
reduction of silver atoms and ionsreduction of silver atoms and ions
BleachBleach acts on acts on
stains by oxidizingstains by oxidizing
them, getting reduced them, getting reduced
in the processin the process
ExplosivesExplosives form gases like form gases like
NN22 from nitrogen compounds! from nitrogen compounds!
Car BatteriesCar BatteriesLead/Acid BatteryLead/Acid BatteryLead is both oxidized and reducedLead is both oxidized and reduced
Pb(s) + PbOPb(s) + PbO22(s) + 2H(s) + 2H22SOSO44(aq) → 2PbSO(aq) → 2PbSO44(s) + (s) +
2H2H22O(l)O(l)
http://www.youtube.com/watch?v=jW_KkEhCy68&safe=active
Reactivity of MetalsReactivity of Metals
Reference Table JReference Table J
Metals Higher on Table J Metals Higher on Table J
are more ‘active” are more ‘active”
““Active” metals are Active” metals are
easily oxidized (easily oxidized (loselose electrons), electrons),
and good “reducing agents”and good “reducing agents”
Copper replaces silver!
Single Replacement Reactions:Single Replacement Reactions:Elements higher on Table J “replace” elements that are lower.Elements higher on Table J “replace” elements that are lower.
Cu0(s) + AgNO3(aq) Ag0(s) + CuNO3(aq)
Ag0(s) + CuNO3(aq) wouldn’t happen!!!
Reactivity of NonmetalsReactivity of Nonmetals
Reference Table JReference Table JNonmetals higher on Table J Nonmetals higher on Table J are more “active” are more “active”
““Active” nonmetals Active” nonmetals are more easily reducedare more easily reduced((gaingain electrons), and electrons), and good “oxidizing agents”good “oxidizing agents”
Balancing Harder Balancing Harder Redox ReactionsRedox Reactions
(Honors)(Honors)
Oxidation Number MethodOxidation Number Method(Balancing in Acid Solution)(Balancing in Acid Solution)
• Find ox #’s and use brackets to connect elementsFind ox #’s and use brackets to connect elements
changing in charge.changing in charge.• Balance atoms changing in chargeBalance atoms changing in charge• Find total e- involved in each changeFind total e- involved in each change• If necessary balance e- by multiplicationIf necessary balance e- by multiplication• Balance all other atoms except H and OBalance all other atoms except H and O• Balance oxygen by adding HBalance oxygen by adding H22O to side deficientO to side deficient
• Balance hydrogen by adding HBalance hydrogen by adding H+1+1 to side deficient to side deficient• Check for balance with respect to atoms and charge.Check for balance with respect to atoms and charge.
Half Reaction Method Half Reaction Method (Ion/Electron Method)(Ion/Electron Method)
(In acid solution)(In acid solution)
Separate equation into two “basic” half reactionsSeparate equation into two “basic” half reactions Balance all atoms except H and OBalance all atoms except H and O Balance oxygen by adding HBalance oxygen by adding H22OO Balance hydrogen by adding HBalance hydrogen by adding H+1+1
Balance charge by adding electrons to more Balance charge by adding electrons to more positive sidepositive side
If necessary balance e- by multiplicationIf necessary balance e- by multiplication Add together half reactions and simplifyAdd together half reactions and simplify Check for balance of atoms and chargeCheck for balance of atoms and charge
Crash Course Chemistry: RedoxCrash Course Chemistry: Redoxhttps://www.youtube.com/watch?v=lQ6FBhttps://www.youtube.com/watch?v=lQ6FB
A1HM3s&index=11&list=PL8dPuuaLjXtPHA1HM3s&index=11&list=PL8dPuuaLjXtPHzzYuWy6fYEaX9mQQ8oGrzzYuWy6fYEaX9mQQ8oGr