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The Learning Goal for this assignment is: 1. Oxidation Numbers Redox Reactions Oxidation and reduction Every atom, ion or polyatomic ion has a formal oxidation number associated with it. This value compares the number of protons in an atom (positive charge) and the number of electrons assigned to that atom (negative charge). In many cases, the oxidation number reflects the actual charge on the atom, but there are many cases where it does not. Think of oxidation numbers as a bookkeeping exercise simply to keep track of where electrons go. 2. Reduction Reduction means what it says: the oxidation number is reduced in reduction. This is accomplished by adding electrons. The electrons, being negative, reduce the overall oxidation number of the atom receiving the electrons. 3. Oxidation Oxidation is the reverse process: the oxidation number of an atom is increased during oxidation. This is done by removing electrons. The electrons, being negative, make the atom that lost them more positive. I use this mnemonic to help me remember which is which: LEO the lion says GER. LEO = Loss of Electrons is Oxidation GER = Gain of Electrons is Reduction Another well-known mnemonic is this: OIL RIG OIL = Oxidation Is Loss (of Electrons) RIG = Reduction Is Gain (of Electrons) Another way is to simply remember that reduction is to reduce the oxidation number. Therefore, oxidation must increase the value. 4. Reduction-Oxidation Reactions There are many chemical reactions in which one substance gets reduced in oxidation number (reduction) while another participating substance gets increased in oxidation number (oxidation). Such a reaction is called called a REDOX reaction. The RED, of course, comes from REDuction and OX from OXidation. However, it is pronounced re-dox and not red-ox. Here is a simple example of a redox reaction:
Ag+ + Cu ---> Ag + Cu2+ I have deliberately not balanced it and I have also written it in net ionic form. I have found that kids studying redox get confused by net ionic form and how to change a full equation into net ionic form. Redox equations need to be balanced but, except for the simplest ones, it cannot be done by inspection (also called trial and error). I take that back, complex ones can be done by trial and error. It typically takes quite a bit of work, especially when compared to how long it takes when the proper technique is used. There is a technique used to balance redox reactions. It is called "balancing by half-reactions." The basic plan will be to split the full equation into two simpler parts (called half-reactions), balance them following several standard steps, then recombine the balanced half-reactions into the final answer. This is another technique called the "ion-electron method." I plan to ignore it. Notes: 5. Some Definitions Oxidizing Agent - that substance which oxidizes somebody else. It is reduced in the process. Reducing Agent - that substance which reduces somebody else. It is oxidized in the process. It helps me to remember these definitions by the opposite nature of what happens. By that, I mean the oxidizing agent gets reduced and the reducing agent gets oxidized. 6. Rules for Assigning Oxidation Numbers The Oxidation Number of an element corresponds to the number of electrons, e - , that an atom loses, gains, or appears to use when joining with other atoms in compounds. In determining the Oxidation Number of an atom, there are seven guidelines to follow: 1. The Oxidation Number of an individual atom is 0. This includes diatomic elements such as O2 or others like P4 and S8 2. The total Oxidation Number of all atoms in: a neutral species is 0 and in an ion is equal to the ion charge. 3. Group 1 metals have an Oxidation Number of +1 and Group 2 an Oxidation Number of +2 4. The Oxidation Number of fluorine is -1 in compounds 5. Hydrogen generally has an Oxidation Number of +1 in compounds, except hydrides 6. Oxygen generally has an Oxidation Number of -2 in compounds, except peroxides 7. In binary metal compounds, Group 17 elements have an Oxidation Number of -1, Group 16 of - 2, and Group 15 of -3. Note: The sum of the Oxidation Number s is equal to zero for neutral compounds and equal to the charge for polyatomic ion species. Now, some examples: 1. What is the oxidation number of Cl in HCl? Since H = +1, the Cl must be -1 (minus one).
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Enmanuel’s Chemistry Notebook
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Define Atomic Size: The size of the
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we can determine that 2 moles of HC
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