CHEM 101 1nd Edition Lecture 14Outline of Last Lecture I. Acid-Base ReactionsII. Oxides of NonmetalsIII. Gas Forming ReactionsIV. Oxidation and ReductionOutline of Current Lecture I. Assigning Oxidation StatesII. Oxidation State ReactionsCurrent LectureI. Assigning Oxidation Statesa. MEMORIZEb. Flourine always has an oxidation of -1c. The oxidation state Of oxygen is -2i. Except when with F, it take on positive numberii. Except in Peroxide and Superperoxidesd. Cl, Br, and I have an oxidation of -1i. Except when combined with O and Fe. Oxidation state of H is +1 in most compoundsi. Except when H is bound to a metal, where it is given a -1 charge f. The algebraic sum of the oxidation number for the atom in a neutral compound must be zero; in a polyatomic ion, the sum must be equal to the ion chargeg. Examples:i. Kh2PO41. 0 = 1 (ox # K) + 2 (ox # H) + 1(ox # P) + 4(ox # O)2. 0 = +1 + 2(+1) + 1(ox #P) + 4(-2)3. 0 = 4 + 1(ox # P) -84. -4 = 1(ox # P) -85. 4 = 1(ox # P)6. P has +4 oxidation numberii. Fe2O31. 0 = 2(ox # Fe) + 3(ox # O)2. 0 = 2(ox # Fe) + 3(-2)3. 0 = 2(ox # Fe) - 6These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.4. 6 = 2(ox # Fe)5. Fe has +3 oxidation numberII. Oxidation State Reactionsa. The species being reduced is the oxidizing agent and the species being oxidized isthe reducing agentb. Problemi. Write the net ionic equation for the following reaction. Is it a redox reaction? If so, label the element(s) being oxidized and reduced the oxidizing agent and the reducing agent.1. 2 Cr (s) + 3 Cu(NO3)2 (aq) --> 2 Cr(NO3)3 (aq) + 3 Cu (s)2. Cu2+ (aq) + 2 NO3- (aq) --> 2 Cr3+ (aq) + 3 NO3- (aq) + 3 Cu (s)3. 2 Cr (s) + 3 Cu2+ (aq) --> 2 Cr3+ (aq) + 3 Cu (s)4. Cr is reducing agent5. Cu is oxidizing
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