May 17 - TOPIC 9 RB OXIDATION-REDUCTION Objective :To determine O.N. for atoms in elements and compounds.Objective :To determine O.N. for atoms in elements and compounds. HW : Review Book – Topic 9 page 160 questions 1 to 10 HW : Review Book – Topic 9 page 160 questions 1 to 10

DO NOW OBSERVATION SKILLS! In your notebook record the experiment in words and then describe the experiment like a chemist (with a CHEMICAL REACTION! )

Indicate the metal and the non metal How metals react? How non metals react? Review : draw the dot diagram for each element, and for the compound formed How many electrons and protons in each reactant? How many electrons and protons in each element in the product?

REDOX REACTIONS (electron transfer reactions) Whenever an atom loses an electron another atom has to gain one. Both reactions are simultaneous.Whenever an atom loses an electron another atom has to gain one. Both reactions are simultaneous. Mg + O 2  MgO Magnesium lost 2 electrons because oxygen took them. The metal LOST electrons, the NON METAL GAINED electrons

What happens to a car when the paint chips off?

LEO GER Losing Losing Electrons is Electrons is Oxidation. Oxidation. Gaining Electrons is Reduction

REDOX REACTIONS REDuction – OXidation reactions Electrons are transferred from the element that is being oxidized to the one that is being reduced.

Oxidation Number (O.N.) Chemist use the O.N. to determine how many electrons are either gained or lost by an atom or ion in a chemical reaction.Chemist use the O.N. to determine how many electrons are either gained or lost by an atom or ion in a chemical reaction. O.N. is the charge or partial charge of an atom in a compound or an ion. O.N. is the charge or partial charge of an atom in a compound or an ion.

RULES FOR ASSIGNING O.N. 1. For all uncombined elements O.N. = O (FREE ELEMENTS) 2. For monoatomic ions the charge equals O.N. 3. Metals of group 1 in compounds O.N.= +1. Metals of group 2 in compounds O.N.= +2 Metals of group 2 in compounds O.N.= +2

4. Fluorine in compounds is always – 1. Other halogens -1 in binary compounds with metals. Other halogens -1 in binary compounds with metals. 5. Hydrogen + 1 except in metal hydrides (combined with metals of group 1 or 2) 6. Oxygen is -2 except when combined with F (is =2) or in peroxides (-1).

7. THE SUM OF THE OXIDATION NUMBERS IN ALL COMPOUNDS MUST BE ZERO7. THE SUM OF THE OXIDATION NUMBERS IN ALL COMPOUNDS MUST BE ZERO 8. FOR POLYATOMIC IONS THE SUM OF THE O.N. IS EQUAL TO THE CHARGE OF THE ION8. FOR POLYATOMIC IONS THE SUM OF THE O.N. IS EQUAL TO THE CHARGE OF THE ION

May 18 Objective: to recognize redox reactionsObjective: to recognize redox reactions HW: review book topic 9 Page 162HW: review book topic 9 Page 162 Q 11 to 20Q 11 to 20

P 160 rb 1)1 2)2 3)4 4)4 5)3 6)1 7)4 8)2 9)1 10)2

Do Now Find the O.N. for each element Cl 2 K 2 S 2 O 3 NO 3 - PO 4 3- CaCr 2 O 7 KNO 2 OF 2 H 2 O 2 KH

To recognize redox reactions… Look for changes in the oxidation number or the atoms. If one element changed the O.N. then for SURE is redox reaction.Look for changes in the oxidation number or the atoms. If one element changed the O.N. then for SURE is redox reaction. All single replacement, synthesis, decomposition and combustion reactions are REDOX.All single replacement, synthesis, decomposition and combustion reactions are REDOX. Double replacement reactions are not redox.Double replacement reactions are not redox.

PRACTICE – your turn! Get in your group and answer question 1 to 4 and 7 from the handout labeled REDOX WORKSHEET 1 / (BACK OF UNIT NOTES)

ANSWERS TO REDOX WORKSHEET 1 1a) zero b) the charge of the ion c) zero d) the charge of the ion 2 a) +4 b) 0 c) +3 d) +5 e) +3 f)+5 3 a)S +3 O -2 b) Cl 0 c) C +4 O -2 d)N +6 O -2 e) K +1 Cl -1 f)He 0 g) N +4 O -2 h ) H +1 N -3

VOCABULARY SIMULTANEOUS = at the same time OXIDATION = to lose electrons REDUCTION = to gain electrons OXIDATION NUMBER = charge or partial charge over an element.

May 21 How to recognize oxidizing and reducing agents? HW Review Book p 163 –21 to 31HW Review Book p 163 –21 to 31

P )2 12)1 13)2 14)2 15)1 16)3 17)3 18)4 19)1 20)2

AGENTS They are always found in the reactants side.

REDUCING AGENT When a substance is oxidized it LOSES electrons. Its O.N. increases. It is being oxidized and is making the other substance in the reaction reduced. Then the one that gets oxidized is the REDUCING AGENT. Its O.N. increases. It is being oxidized and is making the other substance in the reaction reduced. Then the one that gets oxidized is the REDUCING AGENT. R.A. gets oxidized. Its O.N. increases Active metals are good RA

OXIDIZING AGENTS When a substance is reduced it GAINS electrons. Its O.N. decreases. It is being reduced, it takes electrons from the other specie, it makes the other specie to get oxidize.Its O.N. decreases. It is being reduced, it takes electrons from the other specie, it makes the other specie to get oxidize. The one that gets reduced is the OXIDIZING AGENTThe one that gets reduced is the OXIDIZING AGENT Oxidizing Agent : Gets reducedOxidizing Agent : Gets reduced Its ON decreases. Its ON decreases.

2Mg + O 2  MgO2Mg + O 2  MgO Mg: oxidation number changes from 0 to +2. It increased. Mg gets oxidized. Is the reducing agent. Oxygen: Oxidation number changes from 0 to -2, it decreases is the Oxidizing agent.

OIL RIG OxidationOxidation Is Is Loss. Loss. ReductionReduction IsIs Gain. Gain.

May 23 Half reactions

A redox reaction can always be broken down as 2 half reactions that show the atom or ion that is being oxidized and the one that is being reduced.A redox reaction can always be broken down as 2 half reactions that show the atom or ion that is being oxidized and the one that is being reduced. MASS AND CHARGE has to be conserved in a half reactionMASS AND CHARGE has to be conserved in a half reaction 1. find the o.n. of each element in the reaction. Determine which is being reduced an which is being oxidized1. find the o.n. of each element in the reaction. Determine which is being reduced an which is being oxidized

2. Balance the masses first2. Balance the masses first 3. Complete each half reaction with electrons.( LEO GER)3. Complete each half reaction with electrons.( LEO GER) 4. Verify that masses and charges are balanced.4. Verify that masses and charges are balanced.

May 23 Objetive: Spontaneous Redox ReactionObjetive: Spontaneous Redox Reaction To use table J to predict if a single replacement reaction will occurr.To use table J to predict if a single replacement reaction will occurr.

Activity series Spontaneous Reactions : happen without external help.Spontaneous Reactions : happen without external help. CuSO 4 + Zn  Zn SO 4 + Cu CuSO 4 + Zn  Zn SO 4 + Cu In a single replacement reaction the most active element replaces the other element from a compound. (TABLE J)In a single replacement reaction the most active element replaces the other element from a compound. (TABLE J)

Table J The metal above gets oxidized the one below will get reduced.The metal above gets oxidized the one below will get reduced. For non metals the one above gets reduced the one below gets oxidized.For non metals the one above gets reduced the one below gets oxidized.

Predict if the reaction will occur Ag (NO 3 ) + Cu Ag (NO 3 ) + Cu  Zn +2 + Co Zn +2 + Co  MgCl 2 + Ni MgCl 2 + Ni  K + FeCl 3 K + FeCl 3  Li + Mg 2+ Li + Mg 2+ 

F 2 + NaCl F 2 + NaCl  I 2 + NaCl I 2 + NaCl  Cl 2 + Na I Cl 2 + Na I 

METALS IN TABLE J The higher the metal is in table J, the most active it is, the more tendency to became oxidized (lose electrons)The higher the metal is in table J, the most active it is, the more tendency to became oxidized (lose electrons) On Top of table J best reducing agentsOn Top of table J best reducing agents Towards the bottom metals tend to gain electrons then they became reduced and are good reducing agentsTowards the bottom metals tend to gain electrons then they became reduced and are good reducing agents

Non Metals F 2 has the greatest tendency to gain electrons ( became reduced) is the BEST OXIDIZING AGENT.F 2 has the greatest tendency to gain electrons ( became reduced) is the BEST OXIDIZING AGENT.

May 24 ELECTROCHEMISTRY OBJECTIVE: To distinguish between electrochemical and electrolytic cells To identify the different parts of a cell and explain their purpose. HW: TOPIC 9 REVIEW QUESTIONS 37 TO 41HW: TOPIC 9 REVIEW QUESTIONS 37 TO 41

Do now What SPONTANEOUS reaction would occur if we haveWhat SPONTANEOUS reaction would occur if we have Cu, Cu 2+, Zn and Zn 2+ together.Cu, Cu 2+, Zn and Zn 2+ together. Hint USE TABLE JHint USE TABLE J Where the electrons flow? Which loses which gains?Where the electrons flow? Which loses which gains?

IDEA! If we can place the two metals in two different containers and connect them with a wire the electrons will flow from the Zn to the Cu and we will have an electric current – ELECTRICITYIf we can place the two metals in two different containers and connect them with a wire the electrons will flow from the Zn to the Cu and we will have an electric current – ELECTRICITY But it does not work if we do not close the circuit – USE A SALT BRIDGEBut it does not work if we do not close the circuit – USE A SALT BRIDGE

ELECTROCHEMISTRY Electrode : where the oxidation or the reduction takes place.Electrode : where the oxidation or the reduction takes place. *Anode: where the oxidation occurs.*Anode: where the oxidation occurs. *Cathode: where the reduction occurs.*Cathode: where the reduction occurs. Voltaic or galvanic cell: produce ELECTRICITY from an spontaneous chemical reaction.Voltaic or galvanic cell: produce ELECTRICITY from an spontaneous chemical reaction.

ELECTRON FLOW. FROM THE ONE THAT GETS OXIDIZED TO THE ONE THAT GETS REDUCED.ELECTRON FLOW. FROM THE ONE THAT GETS OXIDIZED TO THE ONE THAT GETS REDUCED. POLARITIESPOLARITIES ANODE – NEGATIVE source of electronsANODE – NEGATIVE source of electrons CATHODE- POSITIVECATHODE- POSITIVE

A typical voltaic cell Cathode: the electrode at which reduction occurs Anode: the electrode at which oxidation occurs RED CAT REDuction at the cathode Salt bridge: a tube containing strong electrolyte, a pathway to allow the ions to move from one side to another. PERMIT THE MIGRATION OF IONS

Problems 1. A cell uses the reaction Mn + Ni 2+  Ni + Mn 2+ to produce electricity. a)Write the half-reaction that occurs at the anode. b) Write the half-reaction that occurs at the cathode. c) Which species in this cell loses electrons? d) As the cell produces electricity, which ion increases in concentration? Mn  Mn e - Ni e -  Ni Mn Mn 2+

1. Voltaic Cell A type of electrochemical cell that converts chemical energy to electrical energy by a spontaneous redox reaction. In 1800, Volta built the voltaic pile and discovered the first practical method of generating electricity. Constructed of alternating discs of zinc and copper, with pieces of cardboard soaked in salt water b/w the metals, the voltaic pile produced electrical current.

Electrochemical cell An apparatus that uses a redox reaction to produce electrical energy ( voltaic cell ) or uses electrical energy to cause a chemical reaction ( electrolytic cell ).

Electrolytic cell Uses electricity to force a reaction that is not spontaneous to occur.Uses electricity to force a reaction that is not spontaneous to occur. NOTICE THAT IN ELECTROLYTIC CELLS THERE IS A BATTERY OR A POWER SOURCE PRESENTNOTICE THAT IN ELECTROLYTIC CELLS THERE IS A BATTERY OR A POWER SOURCE PRESENT Electrolysis : to decompose a substance using electricityElectrolysis : to decompose a substance using electricity

Electroplating Is used to cover an object with metal using electricity. Is used to cover an object with metal using electricity. THE OBJECT TO BE COVERED GOES IN THE CATHODETHE OBJECT TO BE COVERED GOES IN THE CATHODE POLARITIES : ANODE – POSITIVEPOLARITIES : ANODE – POSITIVE CATHODE- NEGATIVE SOURCE OF ELECTRONS – CONNECTED TO NEGATIVECATHODE- NEGATIVE SOURCE OF ELECTRONS – CONNECTED TO NEGATIVE