Find the oxidation numbers of each element in a reaction and see which ones have changed.
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2 Find the oxidation numbers of each element in a reaction and see which ones have changed. Rules for oxidation numbers: An element that is not in a compound has an oxidation number of zero (0) Group 1 Metals are always 1+ Group 2 Metals are always 2+ Fluorine is always 1- Oxygen is always 2- except when combined with F (OF 2 ) or the peroxide ion (O 2 2- ) J Deutsch
3 An oxidation-reduction (redox) reaction involves the Sodium transfers its electrons to + The oxidation numbers of the atoms will change. one goes up (oxidation) and one goes down (reduction) J Deutsch
4 Reduction is the gain of electrons. Nonmetals The oxidation number goes (reduces) The element that is reduced is called the. J Deutsch
5 A can be written to represent reduction. Cu e- Cu 0 In reduction half reactions, electrons are written on the J Deutsch
6 Oxidation is the Metal atoms The oxidation numbers go (increases) The element that is oxidized is called the J Deutsch
7 A can be written to represent oxidation. Zn 0 Zn e - In oxidation half reactions, electrons are written on J Deutsch
8 LEO growls GER L G E E O R J Deutsch
9 Table J tells us if a redox reaction can occur between an atom and an ion. A more active metal will replace an ion on Table J. A more active nonmetal will replace an ion on Table J. The, the more readily the replacement will take place. J Deutsch
10 A metal will replace a metal from its compound. Zn + CuSO 4 Cu + ZnSO 4 Zinc replaces copper because zinc is more active than copper. Cu + ZnSO4 No Reaction Copper cannot replace zinc J Deutsch
11 Regents Question: 01/03 #46 According to Reference Table J, which of these metals will react most readily with 1.0 M HCl to produce H 2 (g)? (1) Ca (2) K (3) Mg (4) Zn J Deutsch
12 During redox, one atom is while another atom is. Reduction and oxidation happen together. The oxidation numbers of the atoms will change: one goes up (0 to +1) and one goes down (0 to -2) 0 0 2H 2 + O 2 Oxidation + 2H 2 O Reduction 2- J Deutsch
13 In a redox reaction the The number of electrons must be Al + O 2 Al 2 O 3 Al 0 Al e- oxidation - 3 electrons lost O e- 2O 2- reduction - 4 electrons gained Balance the electrons (Al 0 Al e-) multiply by 4 3(O e- 2O 2-( multiply by 3 12 electrons are transferred in this reaction J Deutsch
14 Regents Question: Given the reaction: Mg(s) + 2H + (aq) + 2Cl (aq) Mg 2+ (aq) + 2Cl (aq) + H 2 (g) Which species undergoes oxidation? (1) Mg(s) (2) H + (aq) LEO growls GER LEO (3) Cl (aq) (4) H 2 (g) J Deutsch
15 Regents Question: 06/03 #28 Given the equation: 2 Al + 3 Cu 2+ 2 Al Cu The reduction half-reaction is (1) Al Al e (2) Cu e Cu (3) Al + 3e Al 3+ (4) Cu 2+ Cu + 2e J Deutsch
16 Regents Question: Which particles are gained and lost during a redox reaction? (1) electrons (2) Protons (3) Neutrons (4) positrons J Deutsch
17 Regents Question: As a Ca atom undergoes oxidation to Ca 2+, the number of neutrons in its nucleus (1) decreases (2) increases (3) remains the same J Deutsch
18 Regents Question: 08/02 #22 In any redox reaction, the substance that undergoes reduction will (1) lose electrons and have a decrease in oxidation number (2) lose electrons and have an increase in oxidation number (3) gain electrons and have a decrease in oxidation number (4) gain electrons and have an increase in oxidation number J Deutsch
19 Regents Question: Which particles are gained and lost during a redox reaction? (1) electrons (2) Protons (3) Neutrons (4) positrons J Deutsch
20 Regents Question: As a Ca atom undergoes oxidation to Ca 2+, the number of neutrons in its nucleus (1) decreases (2) increases (3) remains the same J Deutsch
21 An oxidation-reduction (redox) reaction involves the transfer of electrons (e - ). Sodium transfers its electrons to chlorine + The oxidation numbers of the atoms will change. one goes up (oxidation) and one goes down (reduction) J Deutsch
22 Reduction is the gain of electrons. Nonmetals gain electrons to form ions The oxidation number goes down (reduces) The element that is reduced is called the oxidizing agent. J Deutsch
23 A half-reaction can be written to represent reduction. Cu e- Cu 0 In reduction half reactions, electrons are written on the left because electrons are gained J Deutsch
24 Oxidation is the loss of electrons. Metal atoms lose electrons to become + ions The oxidation numbers go up (increases) The element that is oxidized is called the reducing agent... J Deutsch
25 A half-reaction can be written to represent oxidation. Zn 0 Zn e - In oxidation half reactions, electrons are written on the right because electrons are lost J Deutsch
26 LEO growls GER Losing Electrons Gaining Electrons Oxidation Reduction J Deutsch
27 Regents Question: Given the reaction: Mg(s) + 2H + (aq) + 2Cl (aq) Mg 2+ (aq) + 2Cl (aq) + H 2 (g) Which species undergoes oxidation? (1) Mg(s) (2) H + (aq) LEO growls GER LEO (3) Cl (aq) (4) H 2 (g) J Deutsch
28 Regents Question: Given the equation: C(s) + H 2 O(g) CO(g) + H 2 (g) Which species undergoes reduction? (1) C(s) (2) H + LEO growls GER (3) C 2+ (4) H 2 (g) J Deutsch
29 Regents Question: 08/02 #22 In any redox reaction, the substance that undergoes reduction will (1) lose electrons and have a decrease in oxidation number (2) lose electrons and have an increase in oxidation number (3) gain electrons and have a decrease in oxidation number (4) gain electrons and have an increase in oxidation number J Deutsch
30 Regents Question: 06/03 #28 Given the equation: 2 Al + 3 Cu 2+ 2 Al Cu The reduction half-reaction is (1) Al Al e (2) Cu e Cu (3) Al + 3e Al 3+ (4) Cu 2+ Cu + 2e J Deutsch
31 Oxidation numbers can be assigned to atoms and ions. Changes in oxidation numbers indicate that oxidation and reduction have occurred Zn + Cu(NO 3 ) 2 Zn 0 Zn e - Oxidation Cu e - Cu 0 Reduction Zn(NO 3 ) 2 + Cu Find the oxidation numbers and see which ones change. J Deutsch
32 Regents Question: What is the oxidation number of chromium in K 2 Cr 2 O 7? (1) +12 (2) +2 (3) +3 (4) +6 J Deutsch
33 Regents Question: In which substance does chlorine have an oxidation number of +1? (1) Cl 2 (2) HCl (3) HClO (4) HClO 2 J Deutsch
34 During redox, one atom is oxidized while another atom is reduced. Reduction and oxidation happen together. The oxidation numbers of the atoms will change: one goes up (0 to +1) and one goes down (0 to -2) 0 0 2H 2 + O 2 Oxidation + 2H 2 O Reduction 2- J Deutsch
35 In a redox reaction the number of electrons lost is equal to the number of electrons gained. The number of electrons must be balanced! Al + O 2 Al 2 O 3 Al 0 Al e- oxidation - 3 electrons lost O e- 2O 2- reduction - 4 electrons gained Balance the electrons (Al 0 Al e-) multiply by 4 3(O e- 2O 2-( multiply by 3 12 electrons are transferred in this reaction J Deutsch
36 Table J tells us if a redox reaction can occur between an atom and an ion. A more active metal will replace an ion below it on Table J. A more active nonmetal will replace an ion below it on Table J. The higher up the table, the more readily the replacement will take place. J Deutsch
37 A more active metal will replace a less active metal from its compound. Zn + CuSO 4 Cu + ZnSO 4 Zinc replaces copper because zinc is more active than copper. Cu + ZnSO4 No Reaction Copper cannot replace zinc Oxidation is on top Reduction is on bottom J Deutsch
38 Regents Question: 01/03 #46 According to Reference Table J, which of these metals will react most readily with 1.0 M HCl to produce H 2 (g)? (1) Ca (2) K (3) Mg (4) Zn J Deutsch
39 An electrochemical cell can be either voltaic or electrolytic. J Deutsch 2003
40 J Deutsch
41 The Electrochemical Cell. In an electrochemical cell, oxidation occurs at the anode and reduction at the cathode. (3.2j) Red Cat An Ox Reduction at the Cathode Oxidation at the Anode J Deutsch
42 A voltaic cell spontaneously converts chemical energy to electrical energy. (3.2k) Batteries are voltaic cells J Deutsch
43 Electrons flow from the anode (- electrode) to the cathode (+ electrode) through the wire in a voltaic cell. An Ox -oxidation takes place electrons are lost. Red Cat -reduction takes place electrons are gained. Zn Zn e - e- e- e- e- Cu e - Cu e- e- e- e- Electrons released here by oxidation e- e- e- Electrons needed here for reduction J Deutsch
44 J Deutsch
45 ns/projectfolder/flashfiles/electrochem/voltaic CellEMF.swf x/voltaiccelll20.htm entialchemistry/flash/galvan5.swf per_and_zinc_electrodes J Deutsch
46 Regents Question: 06/03 #46 A diagram of a chemical cell and an equation are shown below. When the switch is closed, electrons will flow from (1) the Pb(s) to the Cu(s) (3) the Pb 2+ (aq) to the Pb(s) (2) the Cu(s) to the Pb(s) (4) the Cu 2+ (aq) to the J Deutsch
47 The salt bridge completes the circuit allows ions to flow from one ½ cell to the other ½ cell to maintain neutrality. Zn Zn e - Cu e - Cu J Deutsch
48 Regents Question: 06/03 #27 Which statement is true for any electrochemical cell? (1) Oxidation occurs at the anode, only. (2) Reduction occurs at the anode, only. (3) Oxidation occurs at both the anode and the cathode. (4) Reduction occurs at both the anode and the cathode. J Deutsch
49 An electrolytic cell requires electrical energy to produce chemical change. This process is known as electrolysis. (3.2l) J Deutsch
50 Regents Question: 06/02 #70-75 Base your answers to the next six questions on the following redox reaction, which occurs spontaneously in an electrochemical cell. Zn + Cr 3+ Zn 2+ + Cr Write the half-reaction for the reduction that occurs. Cr e- Cr 0 Write the half-reaction for the oxidation that occurs. Zn 0 Zn e- Balance the equation using the smallest wholenumber coefficients. The number of e-s gained = the number of e-s lost 3Zn + 2Cr 3+ 2Zn Cr J Deutsch
51 Regents Question: 06/02 #70-75 Base your answers to the next five questions on the following redox reaction, which occurs spontaneously in an electrochemical cell. Zn + Cr 3+ Zn 2+ + Cr Which species loses electrons and which species gains electrons? Zn 0 loses electrons, Cr 3+ gains electrons Which half-reaction occurs at the cathode? Cr e- Cr 0 Hint: Red Cat State what happens to the number of protons in a Zn atom when it changes to Zn 2+ as the redox reaction occurs. The number of protons remains the same. J Deutsch
52 Regents Question: 01/03 #53-55 Indicate with one or more arrows the direction of electron flow through the Hint: wire. Zinc is above copper on table J Write an equation for the half-reaction that occurs at the zinc electrode. Zn Zn e - so Zn is oxidized Explain the function of the salt bridge. The salt bridge completes the circuit and allows ions to flow from one ½ cell to the other. This keeps the ½ cells neutral. e- J Deutsch
53 Uses of Electrolytic cells Recharging a battery Electroplating During copper plating, Cu 2+ ions are reduced to Cu 0 metal at the cathode (Red Cat) which is the negative electrode Electrolysis The Hoffman apparatus uses electricity to break water apart into hydrogen + oxygen J Deutsch
54 Regents Question: 06/02 #22 Which process requires an external power source? (1) neutralization (2) synthesis (3) fermentation (4) electrolysis J Deutsch
55 The cathode is negative and is the site of reduction in an electrolytic cell. Cu 2+ ions are reduced to Cu 0 metal at the negative electrode. J Deutsch
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