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Balancing Redox Equations
Balancing Redox Equations

... Oxidizing Agent - Causes oxidation; undergoes reduction (gains electrons). Reducing Agent - Causes reduction; undergoes oxidation (loses electrons). **In spontaneous redox reactions, stronger oxidizing and reducing agents are converted into weaker oxidizing and reducing agents. ...
Redox Reactions - KFUPM Faculty List
Redox Reactions - KFUPM Faculty List

... Oxidation-Reduction Reactions Oxidation is losing electrons: Zn(s) ...
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... Electroplating is an electrolytic process used to coat metal objects with a more expensive and less reactive metal. The diagram below shows an electroplating cell that includes a battery connected to a silver bar and a metal spoon. The bar and spoon are submerged in AgNO3(aq). ...
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... ____2. How many atoms of oxygen are there in 7 molecules of oxygen gas? II. Balancing Equations-Write balanced equations for each of the following reactions l. Mg + O2  magnesium oxide ...
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ALE 23. Balancing Redox Reactions

... The Model Oxidation-reduction or Redox reactions involve the transfer of one or more electrons from one chemical species to another. Redox reactions are involved in the corrosion of metals, the combustion of fuels, the generation of electricity from batteries and many biological processes including ...
Redox Reactions - hrsbstaff.ednet.ns.ca
Redox Reactions - hrsbstaff.ednet.ns.ca

... Oxidation and reduction reaction = redox rxn  Oxidation is loss of electrons and reduction is gain of electrons = transfer of electrons  Those 2 reactions are occurring simultaneously ...
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... A redox reaction is one involving oxidation and reduction, where there is always a change in the oxidation numbers of the elements involved. ...
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... a redox, identify what was oxidized, what was reduced, & the oxidizing and reducing agents. A. Cu2+(aq) + Zn(s) → Zn2+(aq) + Cu(s) B. 2H2O → 2H2 + O2 C. NaCl + AgF → AgCl + NaF D. Ca(s)+ 2HNO3(aq)→Ca(NO3)2(aq)+ H2(g) ...
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Notes
Notes

... This  table  is  used  to  predict  whether  a  chemical  species  will  spontaneously  give  electrons  to  or  take   electrons  from  another  species.   • Oxidizing  agents  (take  electrons)  are  on  the  ____________  side   ...
Chemistry B2A Chapter 18 Oxidation
Chemistry B2A Chapter 18 Oxidation

... Note: When the oxidizing or reducing agent is named, the whole compound is specified, not just the element that undergoes the change. Oxidation states (oxidation numbers): it lets us keep track of electrons in oxidationreduction reactions by assigning charges to the various atoms in a compound. Howe ...
Document
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... Which statement correctly describes what occurs when this reaction takes place in a closed system? (A) Atoms of Zn(s) lose electrons and are oxidized. (B) Atoms of Zn(s) gain electrons and are reduced. (C) There is a net loss of mass. (D) There is a net gain of mass. ...
Outline
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... 2. polyatomic ions do NOT separate into individual atoms 3. Table of solubilities a. how to tell if a reaction occurs using table 4. Equations a. molecular equation b. total ionic equation c. net ionic equation d. spectator ions B. Redox reactions 1. what is oxidation and reduction a. loss and gain ...
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... A redox reaction is one where one substance is _______________ while another substance is simultaneously _______________ ...
The five main types of redox reactions are combination
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... are those in which the oxidation states of the reactants change. This occurs because in such reactions, electrons are always transferred between species. Redox reactions take place through either a simple process, such as the burning of carbon in oxygen to yield carbon dioxide (CO2), or a more compl ...
Electrochemistry
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... b. balance O atoms by adding H2O as needed c. balance H atoms by adding H+ as needed d. balance charge by adding e- as needed 3. multiply half-reactions by as needed to make the # of e- lost in ox. equal to # of e- gained in red. 4. add half reactions, simplify by canceling 5. double check everythin ...
Oxidation and Reduction
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... 14. Recall that the same number of electrons that are lost by atoms during oxidation must be gained by atoms during reduction. Show how the half-reactions for Reactions C and D in Model 2 can be added together to give the overall redox reactions shown. ...
S8 + ___ F2 → ___ SF6 - Canvas by Instructure
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... called the reducing agent.  The species that is reduced is called the oxidizing agent.  In the above reaction, what is being oxidized?  What is being reduced?  What is the oxidizing agent?  What is the reducing agent? ...
A.P. Chemistry
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... Combination (synthesis), decomposition (analysis), combustion, and single replacement reactions are all types of Redox reactions. There is also a reaction type called disproportionation in which an element in one oxidative state is simultaneously oxidized and reduced.(p. 950) ...
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Chapter 19 part 1

... Oxidizing and reducing agents • Oxidation and reduction must occur simultaneously • The reactant that reduces an atom is called the reducing agent • the reducing agent contains the element that is oxidized • The reactant that oxidizes an atom is called the oxidizing agent • the oxidizing agent cont ...
Answers for Review Questions Exam 3
Answers for Review Questions Exam 3

... 12. First 2.47 Volts should be 2.47 Amperes. That gives 4.100g of Fe deposited. 13. Corrosion is the loss of metals to a solution of some form. The process that occurs is the oxidation of the metal and the reduction of water, followed by the formation of a metal hydroxide. 14. Because not all metals ...
Answers for Review Questions Exam 3
Answers for Review Questions Exam 3

... 12. First 2.47 Volts should be 2.47 Amperes. That gives 4.100g of Fe deposited. 13. Corrosion is the loss of metals to a solution of some form. The process that occurs is the oxidation of the metal and the reduction of water, followed by the formation of a metal hydroxide. 14. Because not all metals ...
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Redox



Redox reactions include all chemical reactions in which atoms have their oxidation state changed; in general, redox reactions involve the transfer of electrons between species. The term ""redox"" comes from two concepts involved with electron transfer: reduction and oxidation. It can be explained in simple terms: Oxidation is the loss of electrons or an increase in oxidation state by a molecule, atom, or ion. Reduction is the gain of electrons or a decrease in oxidation state by a molecule, atom, or ion.Although oxidation reactions are commonly associated with the formation of oxides from oxygen molecules, these are only specific examples of a more general concept of reactions involving electron transfer.Redox reactions, or oxidation-reduction reactions, have a number of similarities to acid–base reactions. Like acid–base reactions, redox reactions are a matched set, that is, there cannot be an oxidation reaction without a reduction reaction happening simultaneously. The oxidation alone and the reduction alone are each called a half-reaction, because two half-reactions always occur together to form a whole reaction. When writing half-reactions, the gained or lost electrons are typically included explicitly in order that the half-reaction be balanced with respect to electric charge.Though sufficient for many purposes, these descriptions are not precisely correct. Oxidation and reduction properly refer to a change in oxidation state — the actual transfer of electrons may never occur. The oxidation state of an atom is the fictitious charge that an atom would have if all bonds between atoms of different elements were 100% ionic. Thus, oxidation is better defined as an increase in oxidation state, and reduction as a decrease in oxidation state. In practice, the transfer of electrons will always cause a change in oxidation state, but there are many reactions that are classed as ""redox"" even though no electron transfer occurs (such as those involving covalent bonds).There are simple redox processes, such as the oxidation of carbon to yield carbon dioxide (CO2) or the reduction of carbon by hydrogen to yield methane (CH4), and more complex processes such as the oxidation of glucose (C6H12O6) in the human body through a series of complex electron transfer processes.
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