Skyler Wild - Final Chemistry Notebook

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+1 0 0 +2 Ag+ --> Ag Reduction Cu --> Cu2+ Oxidation 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: During reduction, it is losing electrons and during oxidization it is gaining electrons. When something is reduced, it becomes the oxidization agent, vice versa. 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).
2. What is the oxidation number of Na in Na2O? Since O = -2, the two Na must each be +1. 3. What is the oxidation number of Cl in ClO¯? The O is -2, but since a -1 must be left over, then the Cl is +1. 4. What is the oxidation number for each element in KMnO4? K = +1 because KCl exists. We know the Cl = -1 because HCl exists. O = -2 by definition Mn = +7. There are 4 oxygens for a total of -8, K is +1, so Mn must be the rest. 5. What is the oxidation number of S in SO4 2¯ O = -2. There are four oxygens for -8 total. Since -2 must be left over, the S must = +6. Please note that, if there is no charge indicated on a formula, the total charge is taken to be zero. Practice Problems Find oxidation numbers 1. N in NO3¯ N = +5 2. C in CO3 2¯ N = +4 3. Cr in CrO4 2¯ Cr = +6 4. Cr in Cr2O7 2¯ Cr = +6 5. Fe in Fe2O3 Fe = +3 6. Pb in PbOH + Pb = +2 7. V in VO2 + V = +3 8. V in VO 2+ V = 4 9. Mn in MnO4¯ Mn = 7 10. Mn in MnO4 2¯ Mn = 6 Notes: The objective is to balance the equation and get the charge that it is asking for, if there is no charge on an element, than its charge is automatically equal to 0. - Follow the 7 steps (Rules for Oxidation Numbers) and the examples given and practiced. Example: Cr in Cr2O72- : O has a charge equal to -2, 7 times -2 is -14, and the aim is to get negative two. In order to get -2, the 2 in Cr2 must be multiplied by 6. Therefore, Cr in Cr2O52- is 6.
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Reference Tables for Physical Setti
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150. 140. Table G Solubility Curves
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Table I Heats of Reaction at 101.3
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Table O Symbols Used in Nuclear Che
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0 6.941 +1 Li 3 2-1 Na 39.0983 K +1
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First Atomic Symbol Name Ionization
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Collier County CHEMISTRY EXAM FORMU
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CHEMISTRY EXAM FORMULA AND RESOURCE
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Honors Chemistry Class Policies and
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Unit 1 (22 days) Chapter 1 Introduc
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4 Lorenzo Walker Technical High Sch
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MUSTANG LABORATORIES COMMITMENT TO
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Chapter 1 Unit 1 Introduction to Ch
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The Learning Goal for this assignme
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2. One cereal bar has a mass of 37
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1. How many meters are in one kilom
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RULE #3: To add/subtract in scienti
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Rule 3: A final zero or trailing ze
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24 For addition and subtraction, lo
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Dimensional Analysis This is a way
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Chapter 4 Unit 2 Atomic Structure T
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Looking at Ions We haven’t talked
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Neutron Madness We have already lea
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Create groups for these Scientist a
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38
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In the space below, write the unabb
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Skyler Wild Name __________________
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The Learning Goal for this Assignme
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Atomic Size Define Atomic Size: The
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Define Electronegativity: Electrone
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Learning Goal for this section: Exp
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Beta Particle Decay Beta decay is a
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Inside the sun, fusion reactions ta
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58 Chapter 7 Unit 3 Ionic and Metal
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Ion Charge? What is the charge on f
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Here are some examples for you: Zn
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C 2 H 6 O Ethanol CH 3 CH 2 O Step
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Name Formula Charge Dichromate Cr
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Name Skyler Wild Date Example: Xeno
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Trioxygen Chemical Name O 3 Chemica
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Phosphorus Pentafluoride Chemical N
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78 Finding Bond Angles, Shapes, and
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case, we count two things stuck to
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Unit 4 Chapter 22 Hydrocarbon Compo
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84 https://www.bbc.co.uk/education/
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Introduction to Organic Chemistry T
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Carbon Prefix Alkane Name Chemical
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Unit 5 Chapter 10 Chemical Quantiti
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Learning Goal for this section: Des
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Example: Converting between mass an
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Step 5 Balance the hydrogen atoms n
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6) ___ 1 Mn(NO2)2 + ___ 1 BeCl2 __
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Single Disp ----------> A+BC x BOTH
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Stoichiometry and Balanced Equation
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Step 1: 200g C3H8 is equal to 4.54
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Stoichiometry and balanced equation
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Skyler Wild - Final Chemistry Notebook

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