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Assigning Oxidation Numbers Assigning Oxidation Numbers Ck12 Science Say Thanks to the Authors Click http://www.ck12.org/saythanks (No sign in required) AUTHOR Ck12 Science To access a customizable version of this book, as well as other interactive content, visit www.ck12.org CK-12 Foundation is a non-profit organization with a mission to reduce the cost of textbook materials for the K-12 market both in the U.S. and worldwide. Using an open-source, collaborative, and web-based compilation model, CK-12 pioneers and promotes the creation and distribution of high-quality, adaptive online textbooks that can be mixed, modified and printed (i.e., the FlexBook® textbooks). Copyright © 2016 CK-12 Foundation, www.ck12.org The names “CK-12” and “CK12” and associated logos and the terms “FlexBook®” and “FlexBook Platform®” (collectively “CK-12 Marks”) are trademarks and service marks of CK-12 Foundation and are protected by federal, state, and international laws. Any form of reproduction of this book in any format or medium, in whole or in sections must include the referral attribution link http://www.ck12.org/saythanks (placed in a visible location) in addition to the following terms. Except as otherwise noted, all CK-12 Content (including CK-12 Curriculum Material) is made available to Users in accordance with the Creative Commons Attribution-Non-Commercial 3.0 Unported (CC BY-NC 3.0) License (http://creativecommons.org/ licenses/by-nc/3.0/), as amended and updated by Creative Com- mons from time to time (the “CC License”), which is incorporated herein by this reference. Complete terms can be found at http://www.ck12.org/about/ terms-of-use. Printed: October 4, 2016 www.ck12.org Chapter 1. Assigning Oxidation Numbers CHAPTER 1 Assigning Oxidation Numbers • List the rules for determining oxidation numbers. • Use these rules to determine oxidation number in materials. Iron what? Once we move from the element iron to iron compounds, we need to be able to designate clearly the form of the iron ion. An example of this is iron that has been oxidized to form iron oxide during the process of rusting. Although Antoine Lavoisier first began the idea off oxidation as a concept, it was Wendell Latimer (1893-1955) who gave us the modern concept of oxidation numbers. His 1938 book The Oxidation States of the Elements and Their Potentials in Aqueous Solution laid out the concept in detail. Latimer was a well-known chemist who later became a member of the National Academy of Sciences. Not bad for a gentleman who started college planning on being a lawyer. Assigning Oxidation Numbers The oxidation number is a positive or negative number that is assigned to an atom to indicate its degree of oxidation or reduction. In oxidation-reduction processes, the driving force for chemical change is in the exchange of electrons between chemical species. A series of rules have been developed to help us: 1. For free elements (uncombined state), each atom has an oxidation number of zero. H2, Br2, Na, Be, K, O2, P4, all have oxidation number of 0. 1 www.ck12.org 2. Monatomic ions have oxidation number equal to charge. Li+ = +1, Ba2+ = +2, Fe3+ = +3, I− = −1, O2− = −2, etc. Alkali metal oxidation numbers = +1. Alkaline earth oxidation numbers = +2. Aluminum = +3 in all of its compounds. Oxygen’s oxidation number is -2 except when in hydrogen peroxide (H2O2), or a 2− peroxide ion (O2 ) where it is -1. 3. Hydrogen’s oxidation number is +1, except for when bonded to metals as the hydride ion forming binary compounds. In LiH, NaH, and CaH2, the oxidation number is -1. 4. Fluorine has an oxidation number of -1 in all of its compounds. 5. Halogens (Cl, Br, I) have negative oxidation numbers when they form halide compounds. When combined − with oxygen, they have positive numbers. In the chlorate ion (ClO3 ), the oxidation number of Cl +5, and the oxidation number of O is -2. 6. In a neutral atom or molecule, the sum of the oxidation numbers must be 0. In a polyatomic ion, the sum of the oxidation numbers of all the atoms in the ion must equal the charge on the ion. Sample Problem: What is the oxidation number for Mn in the compound KMnO4? The oxidation number for K is +1 (rule 2) The oxidation number for O is -2 (rule 2) Since this is a compound (there is no charge indicated on the molecule), the net charge on the molecule is zero (rule 6) So we have +1 + Mn + 4(−2) = 0 Mn − 7 = 0 Mn = +7 When dealing with oxidation numbers, we must always include the charge on the atom. Another way to determine the oxidation number of Mn in this compound is to recall that the permanganate anion (MnO4) has a charge of -1. In this case: Mn + 4(−2) = −1 Mn − 8 = −1 Mn = +7 Sample Problem: What is the oxidation number for iron in Fe2O3? O is − 2 (rule 2) 2Fe + 3(−2) = 0 2Fe = 6 Fe = 3: If we have the compound FeO, then Fe + (−2) = 0 and Fe = 2. Iron is one of those materials that can have more than one oxidation number. The halogens (except for fluorine) can also have more than one number. In the compound NaCl, we know that Na is +1, so Cl must be -1. But what about NaClO3? 2 www.ck12.org Chapter 1. Assigning Oxidation Numbers Na = 1 O = −2 1 +Cl + 3(−2) = 0 1 +Cl − 6 = 0: Cl − 5 = 0 Cl = +5: Not quite what we expected, but Cl, Br, and I will exhibit multiple oxidation numbers in compounds. MEDIA Click image to the left or use the URL below. URL: https://www.ck12.org/flx/render/embeddedobject/185708 Review 1. What is the oxidation number for the element zinc? 2. Nitrogen can exist in several oxide forms. What is the oxidation number of N in NO? in N2O? in NO2? 3. What is the oxidation number of H in HCl? in NaH? • oxidation number: A positive or negative number that is assigned to an atom to indicate its degree of oxidation or reduction. References 1. Courtesy of Boyd Norton, US Environmental Protection Agency. http://commons.wikimedia.org/wiki/File:T RACES_OF_IRON_OXIDE_GIVE_REDDISH_HUE_TO_THIS_ROCK_FORMATION_-_NARA_-_544899. tif. 3.
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