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Redox Reactions I. Oxidation & Reduction -_________-_________ oxidation reduction ________, reactions or _____ redox ________, reactions are ________ reactions in which ________ electrons are __________ transferred from one atom another atom ____ to _______ ____ 2Na (s) + 1Cl2 (g) Synthesis 2NaCl (s) + Na Cl Cl Na + Cl Na - Cl + Na -when _______ Sodium reacts with Chlorine _______, each Sodium ______ _____ ___ atom ________ transfers one _______ electron to a _______ Chlorine _____ atom 2Na (s) + 1Cl2 (g) - 2Na1+ + 2Cl1- Redox Reactions I. Oxidation & Reduction -_________ oxidation is defined as the ____ loss of ________ _____ of a ________ electrons from the atoms substance -during its reaction with Chlorine _______, Sodium ______ _____ loses ________: electrons oxidation number is equal to the number of electrons lost or gained by an atom Reduction causes the numerical value of the oxidation number to be reduced Oxidation causes the numerical value of the oxidation number to increase 0 oxidized +1 Na Na1+ + eSodium is ________ oxidized -_______ reduction is defined as the gain -_________ ____ of electrons by the _____ atoms of a ________ substance ________ Sodium -during its reaction with _______, Chlorine _____ gains ________: electrons ________ 0 Cl2 + 2e- reduced -________ Chlorine is _______ reduced -1 2Cl1- Redox Reactions I. Oxidation & Reduction -a substance which ________ oxidizes another substance by ________ accepting its ________ electrons is called an ________ oxidizing _____, agent which is also reduced the substance that is _______ -a substance which _______ reduces another substance by ______ losing ________ electrons is reducing _____, agent which is also called an ________ oxidized the substance that is ________ oxidized 2K (s) + 1Br2 (g) 2KBr (s) reduced covalent compounds partially -________ _________ become _______ ________ oxidized and _______ partially _______ reduced by the _______ unequal _______ sharing of ________; electrons the more _____________ electronegative is considered to be reduced and the less _____________ electronegative is _______ oxidized considered to be ________ Redox Reactions I. Oxidation & Reduction oxidized 3H2 (g) + 1N2 (g) 2NH3 (g) reduced Identify each of the following changes as oxidation or reduction: I2 K 0 + 0 2e- oxidized +2 -1 reduced 2I1- Fe2+ +1 K1+ oxidized +1 + e- Ag1+ + e- +3 Fe3+ + ereduced Ag Identify what is oxidized and what is reduced in each of the following: 2Br1- + 1Cl2 1Br2 + 2Cl1oxidized reduced 2Ce + 3Cu2+ oxidized reduced 2Zn + 1O2 oxidized 3Cu + 2Ce3+ reduced 2ZnO 0 Redox Reactions I. Oxidation & Reduction Identify the oxidizing agent and the reducing agent in each of the following reactions: 1Mg + 1I2 reducing agent oxidizing agent 2Na + 2H1+ reducing agent 1MgI2 1H2 + 2Na1+ oxidizing agent 1H2S + 1Cl2 reducing agent oxidizing agent 1S + 2HCl Redox Reactions I. Oxidation & Reduction Determine the oxidation number of the boldface element in each of the chemical formulas below: +1+ 1(x) + 4(-2) = 0 NaClO4 +7 NH4Cl -3 Ca3N2 MgB4O7 -3 +3 AlPO4 +5 Li3AsO4 +5 HIO4 +7 Fe2O3 +3 HNO2 +3 K2CrO4 +6 KMnO4 +7 HNO3 +5 Redox Reactions I. Oxidation & Reduction Determine the oxidation number of the boldface element in each of the polyatomic ions below: 1(x) + 4(+1) = +1 NH41+ AsO43- CrO42- -3 +5 +6 +7 B4O72- NH21- ClO41- +3 -3 +7 SO42- NO21- +6 +3 MnO41+7 ClO31+5 IO41- CO32+4 Redox Reactions II. Balancing Redox Equations Use the oxidation-number method to balance the redox equation below: Cu (s) + HNO3 (aq) Cu(NO3)2 (aq) + NO2 (g) + H2O (l) 1. Assign oxidation numbers to all atoms in the equation. 0 Cu (s) + +1 +5 -2 +2 +5 -2 HNO3 (aq) Cu(NO3)2 (aq) + +4 -2 +1 -2 NO2 (g) + H2O (l) 2. Identify the atoms that are oxidized and the atoms that are reduced. oxidized 0 Cu (s) + +1 +5 -2 HNO3 (aq) +2 +5 -2 Cu(NO3)2 (aq) + reduced +4 -2 +1 -2 NO2 (g) + H2O (l) Redox Reactions II. Balancing Redox Equations 3. Determine the change in oxidation number for the atoms that are oxidized and for the atoms that are reduced. +2 oxidized 0 Cu (s) + +1 +5 -2 +2 HNO3 (aq) +5 -2 Cu(NO3)2 (aq) + +4 -2 +1 -2 NO2 (g) + H2O (l) reduced -1 4. Make the change in oxidation numbers equal in magnitude by adjusting coefficients in the equation. +2 oxidized 0 Cu (s) + +1 +5 -2 HNO3 (aq) +2 +5 -2 +4 -2 Cu(NO3)2 (aq) + 2 NO2 (g) + reduced -1(2) = -2 +1 -2 H2O (l) 5. If necessary, use the conventional method to balance the remainder of the equation. +2 oxidized 0 +1 +5 -2 +2 1 Cu (s) + 4 HNO3 (aq) +5 -2 +4 -2 +1 -2 1 Cu(NO3)2 (aq) + 2 NO2 (g) + 2 H2O (l) reduced -1(2) = -2 Use the oxidation-number method to balance the redox equations below: +2 (3) = +6 +1 -1 3 HCl +1 +5 -2 + +1 -2 +1 2 HNO3 3 HOCl +2 -2 + 2 NO -3 (2) = -6 +3 (2) = +6 3 SnCl4 + 2 Fe 3 SnCl2 + 2 FeCl3 -2 (3) = -6 +3 (4) = +12 8 4 NH3 (g) + 6 3 NO2 (g) -4 (3) = -12 7 N2 (g) + 12 H2O (l) +1 -2 + 1 H2O Redox Reactions II. Balancing Redox Equations Al (s) + NH4ClO4 (s) Al2O3 (g) + HCl (g) + N2 (g) + H2O (g) Use the oxidation-number method to balance the equation: 0 -3 +1 Al (s) + +7 -2 NH4ClO4 (s) oxidized +3 -2 +1 -1 0 +1 -2 Al2O3 (g) + HCl (g) + N2 (g) + H2O (g) +3 +3 oxidized reduced -8 (3) = -24 The _____ space ______ shuttle gains nearly ____ 72% of its ___ lift from its _____ solid ______ rocket _______ boosters (_____) SRB’s during the ____ first ___ two minutes of ______. launch The ______ SRB’s _______ contain _______ 495,000 ___ kg of a each _______ _______ mixture of __________ Aluminum and ___________ Ammonium __________ perchlorate http://alanrider.files.wordpress.com/2009/01/space_shuttle_launch.jpg Redox Reactions II. Balancing Redox Equations 10 Al(s)+ 6 3 NH4ClO4 (s) oxidized +3 5 Al2O3 (g) + 6 HCl (g) + 3 N2 (g) + 9 H2O (g) +3 oxidized reduced -8 (3) = -24 While in _____ orbit the _____ space _______ shuttle uses a ___________ spontaneous __________ propulsion _______ reaction to ________, maneuver which involves ___________________ monomethylhydrazine as the propellant and __________ Dinitrogen _________ tetroxide _________ as the_______ oxidizer https://secure.reservexl.net/wwwimg/img/tours/38-2.jpg Redox Reactions II. Balancing Redox Equations N2O4 + CH3N2H3 CO2 + N2 + H2O Use the oxidation-number method to balance the equation: +4 -2 -4 +1 -1 +1 +4 -2 0 +1 -2 4 4 9 12 5 2 N2O4 2 1 CO2 + 4 2 N2 + 6 H2O + 2 1 CH3N2H3 oxidized +8 oxidized +1 reduced -4 (2) = -8 http://www.arcadiastreet.com/cgvistas/spacexp/images/se_spaceshuttle_orbit_insert_600.jpg Redox Reactions II. Balancing Redox Equations Use the oxidation-number method to balance the following equations: HClO3 (aq) ClO2 (g) + HClO4 (aq) + H2O (l) H2O2 (aq) + H2SO4 (aq) + FeSO4 (aq) H2SeO3 (aq) + HClO3 (aq) Fe2(SO4)3 (aq) + H2O (1) H2SeO4 (aq) + Cl2 (g) + H2O (l) Redox Reactions II. Balancing Redox Equations 1. Hypothesis: How do you know if an oxidation-reduction reaction has occurred? 2. Prediction: 3. Gather Data: A. Safety: Copper(II) sulfate is mildly toxic, with an LD50 = 300mg/kg. Avoid ingestion (don’t eat or drink it). Wash hands thoroughly with soap and water before leaving lab. Goggles mandatory. Copper(II) sulfate is an environmental hazard, being extremely toxic to aquatic organisms like algae. B. Procedure: 1. Use a piece of sandpaper to polish the end of an iron nail. 3. Gather Data: B. Procedure: 2. Add about 3 mL of 1.0 M CuSO4 solution to a test tube. 3. Place the polished end of the nail in the CuSO4 solution. Let stand and observe for about 10 minutes. Record your observations. ___________________________________ 4. Analyze Data: 1. What is the substance found clinging to the nail? _______ 2. What happened to the color of the CuSO4 solution? _____ ______________________________________________ 3. Write the balanced chemical equation for the reaction you observed: ______________________________________ 4. What substance was oxidized? _____________________ 5. What substance was reduced? _____________________ Redox Reactions III. Half-Reactions -in the _________-_________ oxidation reduction _______ reaction ___ ____ ______, 2Fe + 3Cl 2FeCl3 each ____ iron 2 _____ ________ atom is ________ oxidized by ______ losing __ 3 electrons oxidation ____-_______ half reaction is: -the _________ Fe Fe3+ + 3e-each ________ ________ is _______ chlorine molecule reduced by gaining __ 2 ________ electrons _______ reduction ____-_______ half reaction is: -the _________ Cl2 + 2e- 2Cl- Redox Reactions III. Half-Reactions-in the _________-_________ oxidation reduction _______ reaction ___ ________ Cu + _______ AgNO3 Cu(NO3)2 + ___, Ag each copper ______ _____ atom is ________ oxidized by ______ losing __ 2 ________ electrons -the _________ oxidation ____-_______ half reaction is: Cu2+ + 2esilver ____ ion is _______ reduced by _______ gaining __ 1 -each ______ electron ________ Cu reduction ____-_______ half reaction is: -the _________ Ag1+ + 1e- Ag Redox Reactions III. Half-Reactions Write the oxidation and reduction half-reactions for the following oxidation-reduction equations: 0 +2 Pb (s) + Pd(NO3)2 (aq) Pd2+ + 2e- +5 -2 0 Pb(NO3)2 (aq) + Pd (s) Pd -2 KMnO4 (aq) + SO2 +2 Pb2+ + 2e- Pb +1 +7 +5 -2 +4 -2 +1 +6 -2 SO2 (g) K2SO4 (aq) SO42- + 2e- MnO41- + 5e- Mn2+ +2 +6 -2 + MnSO4 (aq) Redox Reactions III. Half-Reactions Write the oxidation and reduction half-reactions for the following oxidation-reduction equations: +2 -2 -3 +1 PbO (s) + 0 NH3 (g) PbO + 2e+2 +1 -2 N2 (g) + Pb (s) + H2O (l) N2 + 6e- 2NH3 +1 0 -2 Pb 0 +1 Na2S2O3 (aq) + I2 (s) S2O32I2 + 2e- S2O422I1- +3 -2 +1 -1 Na2S2O4 (aq) + NaI (aq) + 2e- Redox Reactions III. Half-Reactions Write the oxidation and reduction half-reactions for the following oxidation-reduction equations: +1 -2 +1 +4 -2 +1 +3 -2 NaOH (aq) + NO2 (g) NaNO2 (aq) + NaNO3 (aq) + H2O (l) NO2 NO31- NO2 + 1e+1 -1 + 1e- NO210 +2 HCl (aq) + Sn (s) Sn Sn2+ + 2e- 2H1+ + 2e- +1 +5 -2 -1 0 SnCl2 (aq) + H2 (g) H2 +1 -2 Redox Reactions III. Half-Reactions Write the oxidation and reduction half-reactions for the following oxidation-reduction equations: +1 +3 -2 +1 +5 -2 +1 +5 -2 H3PO3 (aq) + HNO3 (aq) H3PO4 (aq) PO33- PO43- NO31+1 -1 + 3e+1 NO (g) -2 + H2O (l) NO +7 -2 +1 -1 +2 -1 +1 -2 0 KCl (aq) + MnCl2 (aq) + H2O (l) + Cl2 (g) Cl2 + 2e- MnO41- + 5e- + +1 + 2e- HCl (aq) + KMnO4 (aq) 2Cl- +2 -2 Mn2+