\hline, So now we'll work on problem six from Chapter 20. Accessibility StatementFor more information contact us atinfo@libretexts.org. \text { Half-Reactions } & \boldsymbol{E}^{\ci, so in this problem, were given with four reduction reactions and their standard reduction part in shell. The strongest elemental reducing agent is lithium, which is not the least electronegative element. How do you optimize the selectivity of solid phase extraction (SPE)? The zinc causes the sulfur to gain electrons and become reduced and so the zinc is called the reducing agent. Break the reaction down into a net ionic equation and then into half-reactions. A) F2 B)F- C)Li+ D)Li GIVEN THE TABLE ON THE OTHER SIDE OF THIS CARD. Reduction Half-Reaction E' (V) ++ - A 0.80 B2+ + 2e - B 0.38 C2 + 2e -> 20 0.17 D3+ + 3e =D -1.36 Part A Which substance is the strongest oxidizing agent? Which equation is correctly labeled oxidation or reduction? One of the reactants of an oxidation-reduction process is a reducing agent, which decreases the other reactant by discharging electrons to it. I highly recommend you use this site! The more active an element is, the more likely it is to lose electrons and be a reducing agent. Some molecules such as carbon monoxide (CO) are also used in. Plus, get practice tests, quizzes, and personalized coaching to help you How To Find The Oxidizing and Reducing Agent - YouTube Practice Problem 9: Arrange the following oxidizing and reducing agents in order of increasing strength: Reducing agents: Cl - , Cu, H 2, H -, HF, Pb, and Zn Since the activity of a metal is judged by how readily it loses electrons, metals in this activity series progressively become less active and more stable as you go down the electrochemical series. b. the weakest reducing agent, A: Oxidizing agent: Thus, hydrogen peroxide is the stronger oxidizing agent. It explains how to determine which reactant is oxidized and which substance is reduced.My Website: https://www.video-tutor.netPatreon: https://www.patreon.com/MathScienceTutorAmazon Store: https://www.amazon.com/shop/theorganicchemistrytutorDisclaimer: Some of the links associated with this video may generate affiliate commissions on my behalf. In this series of reactions, water is converted to oxygen gas, and we have something to sustain our lives. Diana Pearson, Connie Xu, Luvleen Brar (UCD). Of course, it is oxidized in the process. Reducing Agents - Examples, Strong and Weak Reducing Agents - Vedantu In a typical Zn - Fe bimetallic system , Zn with electrode potential of -0.763 v compared to Fe having electrode potential of -0.44 v with potential difference of about 0.32 v between Zn and Fe will drive corrosion. (a) The strongest reducing agent is the one with the lowest (most negative) standard reduction potential, while the strongest oxidizing agent is the one with the highest (most positive) standard reduction potential. A: Explanation to the correct answer is given below, A: Metals are the chemical elements having the following physical properties: The substance that loses electrons is being oxidized and is the reducing agent. A 2 D Previous Answers Correct An oxidizing agent can oxidize any substance that is a weaker oxidizer than itself. What is the oxidation number of, A: Redox reaction: The electrochemical reaction in which gain of electrons is called reduction and loss, A: Identify : A reducing agent is one of the reactants of an oxidation-reduction reaction which reduces the other reactant by giving out electrons to the reactant. Oxidizing Agent | Definition, Applications & Examples, Acid & Base Anhydrides | Definition, Formation & Examples, Cell Potential | Definition, Chart & Calculation, Industrial Production of Sodium Hydroxide: Processes & Equations. And as we know that the lowered reduction important shell, the Lord that tendency off assistance to reduced so the substance with the lowest reduction part shield should be the strongest reducing agent. Which of these substances is the best reducing agent - BYJU'S We can also say, as you go down the electrochemical series ability of elements to lose electron reduces. Check all that apply. The simplest way to think of this is that the oxidizing agent is the substance that is reduced, while the reducing agent is the substance that is oxidized as shown in Figure \(\PageIndex{1}\) and summarized in Table \(\PageIndex{1}\). On moving down the group, the atomic size increases. Try refreshing the page, or contact customer support. Light striking a plant pigment known as chlorophyll initiates a complex series of reactions, many of which involve redox processes complete with movement of electrons. She has taught science at the high school and college levels. BA B2 C2 B. 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Reducing Agent (Reductant) - Definition & Examples With Videos - BYJU'S Mr Nikhilesh , very interesting and easy way for interpretation. Both the oxidizing and reducing agents are the reactants and therefore appear on the left-hand side of an equation. Zn + 2H(+) Zn(2+) + H2, See all questions in Oxidation and Reduction Reactions. Examples of how to identify oxidizing and reducing agents are shown. On the product side, the six oxygen atoms needed for balance are divided between the SO2 and the H2 O. If one reagent in a reaction removes oxygen, contributes hydrogen, or contributes electrons, it is said to be a reducing agent. Which is weakest? B The strongest oxidizing agent is A D The strongest reducing agent is D D31 C B2 ! The LibreTexts libraries arePowered by NICE CXone Expertand are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. The oxidizing agent is a substance that causes oxidation by accepting electrons; therefore, its oxidation state decreases. In galvanic cells, A: Sacrificial anode - In this technique, the metal to be protected is made cathode and is connected to, A: Electrochemical series is series of elements arranged in increasing order of reduction potentials.. Standard reduction potentials (video) | Khan Academy How do you determine which oxidizing agent is stronger? The strongest reducing agents are the alkali metals (Group 1) as they have low electronegativities and lose electrons very easily. To summarize, electrochemical series tells us , the stronger the reduction potential, the more difficult is oxidation and weaker the reduction potential, the easier is oxidation. The reducing agent is stronger when it has a more negative reduction potential and weaker when it has a more positive reduction potential. Here's a list of steps to help you balance a redox equation. \(S\) is the reducing agent and \(Mn\) is the oxidizing agent. Na, Al, Mg etc. 2003-2023 Chegg Inc. All rights reserved. Which is weakest? On the other hand, a substance with higher (more positive) reduction potential tend to accept electrons and thus are oxidizing agents . How many coulombs arc required? Which can be reduced by $\mathrm{C}$ ? Step 2/3 This voltage difference drives the current flow to accelerate corrosion of the anodic metal. The examples below show how to analyze a redox reaction and identify oxidizing and reducing agents. The substance that is reduced in a reaction is the oxidizing agent because it gains electrons. Balancing Redox Reactions and Identifying Oxidizing and Reducing Agents Anodic metal corrosion is more rapid and more damaging as the voltage difference between two electrodes increases. -2 + (-4) = -6. Answered: Which substance is the strongest | bartleby y Part B Which substances can be oxidized by B27 Check all that apply. How many faradays are required for each of the following processes? Added both side 4OH-ion Try it in the Numerade app? Here. The higher the electronegativity the greater the pull an oxidizing agent has for electrons. Lithium metal is therefore the strongest reductant (most easily oxidized) of the alkali metals in aqueous solution. How do you choose the best equipment and process for dry or wet separation methods. It is difficult to reduce lithium. In basic medium, Note: MarisaAlviar-Agnew(Sacramento City College). Verified by Toppr. 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Explanation for the correct options: Metals are generally good reducing agents. Identify the reactants and the products and assign oxidation numbers. Cl 2 gains one electron; it is reduced from Cl 2 to 2 Cl -; thus, Cl 2 is the oxidizing agent. [Sections 20.4 and 20.5] Answer (a)see for solution (b)see for solution (c) see for solution Upgrade to View Answer Discussion You must be signed in to discuss. The substance that has the capability to cause the loss of electrons named an, A: Oxidation number of Fluorine is always negative than other bromine, Chlorine and Oxygen because it, A: Reduction may be defined as the process in which addition of hydrogen or an electropositive element, A: Oxidation To unlock this lesson you must be a Study.com Member. A: Number of moles of electrons = 6 Lithium is the strongest reducing agent. Weve got your back. Compared to hydrogen, lithium at the top of the table has lowest reduction potential and fluorine at the bottom of the table has the highest reduction potential. An oxidation reaction is a reaction that takes an electron from one substance. a. Mn b. Al c. Ni d. Cr A: The reducing agents are said to be those substances or compounds which have lower ability to gain The value E) for B2+ is 0.38 V The value of E for Cis 0.17 V and for D the value is -1.36 V the E for B2t they can be oxidized by B2 Part C Which substances can be reduced by D? Match the words in the left column to the appropriate blanks in the sentences on the right. Balancing Redox Reactions and Identifying Oxidizing and Reducing Agents What is Oxidation and Reduction? How do you optimize the dye loading and injection efficiency in DSSCs? Also identify the oxidizing agent and the reducing agent in the overall reaction, \[\ce{Zn + 2Fe^{3+} -> Zn^{2+} +2Fe^{2+}} \nonumber \nonumber \], \(\ce{Zn -> Zn^{2+} + 2e^{-}}\) oxidationloss of electrons, \(\ce{2e^{-} + 2Fe^{3+} -> 2Fe^{2+}}\) reductiongain of electrons. And that means do plus will be the strongest reducing agent. On the other hand, it is a very strong oxidizing agent because it will easily and happily gain electrons. what can we say about reduction and oxidation in terms of oxidation number? A C D Which can be reduced by C? Educator app for Reason: A substance which helps in oxidation is known as reducing agent. Oxidizing and Reducing Agents - Division of Chemical Education, Purdue Opposite to this, the more readily a substance gains electrons , the more stronger it is as oxidizing agent. The weaker the reduction potential, the easier is oxidation- example is lithium. Solution Verified by Toppr Correct option is B) Among the elements of alkaline earth metals, barium is the strongest reducing agent. This is a reduction reaction. The \(\ce{Cl_2}\) is being reduced and is the oxidizing agent. Which is the strongest reducing agent? It is difficult to oxidize fluorine. A reducing agent is something that causes another substance to reduce. If we are reducing zinc 2+ to solid zinc, the standard reduction potential turns out to be -.76 volts. This chemistry video tutorial explains how to find the oxidizing agent and the reducing agent in a redox reaction. Application of electrochemical series in Galvanic corrosion -What makes metals electrodes in Galvaniccorrosion? 0 + (-2) = -2. Oxidizing and reducing strength of elements depends upon the atomic . From the table, we can see that A is the strongest reducing agent and D is the strongest oxidizing agent. Which is the best reducing agent? (a) Which substance is the strongest reducing agent? Which is the So the strongest oxidizing agent will be. These metals with different potential become two electrodes of a electrochemical cell with one supplying electrons to another as shown below. What balanced equation represents a redox reaction? 3. Which is stronger? Reduction is gain of electrons. How do you evaluate the performance and efficiency of gravity separation? Order the following oxidizing agents by increasing strength under standard-state conditions: Mg2+(aq), Hg2+(aq), Pb2+(aq). So before finding out that lives right down the reduction relation equations. Overview Br - loses an electron; it is oxidized from Br - to Br 2; thus, Br - is the reducing agent. Which is the strongest oxidizing agent? Lithium has the strongest ability to lose electron.. Galvanic corrosion is typically a two metal corrosion. Study with Quizlet and memorize flashcards containing terms like Which one of the following is not a redox reaction?, Consider the reaction CuO(s) + H2(g) Cu(s) + H2O(l) In this reaction, which substances are the oxidant (oxidizing agent) and reductant (reducing agent), respectively?, When the following redox equation is balanced with smallest whole number coefficients, the coefficient for . You can update your choices at any time in your settings. The reducing agent is a substance that causes reduction by losing electrons; therefore its oxidation state increases. If we are reducing copper 2+ to solid copper, the standard reduction potential is +.34 volts. Experts are tested by Chegg as specialists in their subject area. Split reaction into oxidation and reduction halves The strongest reducing agents will be found at the corner of the table where sodium and potassium metal are listed. First is three questions, which substances the strongest oxidizing agent and which is the weakest. reduction=decrease in oxidation number oxidation=increase in oxidation number Which of the following is the strongest oxidizing agent? The standard reduction potentials can be interpreted as a ranking of substances according to their oxidizing and reducing power. Maps Practical Geometry Separation of Substances Playing With Numbers India: Climate, Vegetation and Wildlife. 1, 1,4, 1, 2 O c. 1, 1, 2, 1, 2 O d. 4, 1, 2, 1, 2 o e. 4, 1, 4, 4, 2. You can use the steps you used previously to balance other equations to start, but then you have to take into account the key ions and oxidation numbers. It is an electrochemical oxidation-reduction (redox) process, occurs when two metals different in terms of their potential, are in electrical contact while immersed in an electrically conducting liquid. The force which drive an element to acquire electrons and thereby be reduced is called Reduction potential of the element. The text book definition of Electrochemical series is " it is an arrangement of elements in order of increasing reduction potential values". Reduction Order the following oxidizing agents by increasing strength under standard-state conditions: Ag+(aq); Cd2+(aq); MnO4(aq) (in acidic solution). 2Cu(s)+O2(g)2CuO(s) b. Cl2(aq)+2KI(aq)2KCl(aq)+I2(aq) c. 3MnO2(s)+4Al(s)2Al2O3(s)+3Mn(s) d. 2H+(aq)+3SO32(aq)+2NO3(aq)2NO(g)+H2O(l)+3SO42(aq) e. Mg(s)+2HCl(aq)MgCl2(aq)+H2(g) f. 4NO2(g)+O2(g)2N2O5(g). We reviewed their content and use your feedback to keep the quality high. An error occurred trying to load this video. 40802 views a. (c) Write a balanced equation for the overall cell reaction that delivers the highest voltage, and calculate $E^{\circ}$ for the reaction. By adding water molecules. Chem 210 Chp 21 Flashcards | Quizlet First week only $4.99! (b) Which substances can be oxidized by $\mathrm{B}^{2+}$ ? A3+ B2+ C D Which is the strongest oxidizing agent? Solution Verified by Toppr Correct option is D) SbH 3 is the strongest reducing agent because sb 5+ is most stable in its respective group so it gets easily oxidised so its the strongest reducing agent. A substance with lower (more negative) reduction potential tends to donate electrons and hence is said to be a reducing agent. Reducing Agents, Strong | CAMEO Chemicals | NOAA I would definitely recommend Study.com to my colleagues. Learn more in our Cookie Policy. If an electode reaction has dssolved oxygen as a reactant, is the electrode an anode or a cathode? Get 5 free video unlocks on our app with code GOMOBILE. Consider the redox reaction (1) and Figure 1 below: . A reducing agent is a substance that, in a redox process, loses electrons to other substances and undergoes oxidation to a higher valency state. The reaction below is a redox reaction that produces zinc sulfide: \[\ce{Zn} + \ce{S} \rightarrow \ce{ZnS}\nonumber \], \[\begin{align*} &\text{Oxidation:} \: \ce{Zn} \rightarrow \ce{Zn^{2+}} + 2 \ce{e^-} \\ &\text{Reduction:} \: \ce{S} + 2 \ce{e^-} \rightarrow \ce{S^{2-}} \end{align*} \nonumber \]. Its like a teacher waved a magic wand and did the work for me. KI + KCrO + HCl CrCl + KCl + I + HO _Ag + -02 + 4H+ + Ag+ + - H20 Select one: O a. What are the reduced components in this reaction? Electrochemical series is a tool to predict relative power of oxidizing and reducing agents. So, we are explaining oxidation and reduction first in brief here. It helped me pass my exam and the test questions are very similar to the practice quizzes on Study.com. Lab 11 - Redox Reactions - WebAssign A3+ B2+ C D Consider the following table of standard reduction potentials: Which substances can be oxidized by B2+? And in first part of this question, we were asked to find out the substance, which is the strongest reducing agent and the substance, which is the strongest oxidizing agent. Metal having greater standard oxidation potential value will, A: When moisture present in air causes certain chemical reactions which tends to deteriorate a solid, A: The cell potential for the cell, which is formed by putting the hydrogen electrode at anode and Ni, A: In electrolytic cell the cathode are mark negative and anode are marked positive . As a member, you'll also get unlimited access to over 88,000 Reduction Half-Reaction EV) A+ + - + A 0.80 B2+ + 2e- B 0.38 C2 + 2e- 2C- 0.17 D3+ + 3e- D -1.36 a) Which substance is the strongest oxidizing agent in this table? Consider the following table of standard reduction potentials:(a) Which substance is the strongest reducing agent? Part A Which substance is the strongest oxidizing agent? 1, 1, 2, 1, 1 b. Write the following reaction in the form of half-equations. - Definition, Types & Examples, ACTH Stimulation Test: Protocol & Side Effects, How to Interpret the ACTH Stimulation Test, Renal & Biliary Drug Excretion: Definition & Process, Working Scholars Bringing Tuition-Free College to the Community. Check all that apply. In electrochemical series, the substances which are stronger reducing agents than hydrogen are placed above hydrogen in top half and have negative values of standard reduction potentials. Fluorine is at the bottom of the table has highest reduction potential. Order the following oxidizing agents by increasing strength under standard-state conditions: O2(g); MnO4(aq); NO3 (aq) (in acidic solution ). Hence, reducing power also increases from Be to Ba. Post any question and get expert help quickly. We find Half-ReactionmmmmmmmmmmmmmmmmmmmllE /V lH2O2(aq) + 2H+(aq) + 2e- 2H2O (l);mmmmmmml1.77 Reducing agents can be ranked by increasing strength by ranking their reduction potentials. _Ag + -02 + 4H+ + - Ag+ + - H20 Select one: O a. So the element with the highest electronegativity is the strongest oxidizing agent. I know it is strange that 'oxidation' means 'giving up' and 'reduction' means 'taking in,' but remember that an electron is negatively charged, so everything is kind of backwards. Which substance is the strongest reducing agent? Recap - An oxidizing agent is a substance which makes other to lose electrons and gains those electrons to get reduced. class 7. class 6. Reduction Half-Reaction E' (V) ++ - A 0.80 B2+ + 2e - B 0.38 C2 + 2e -> 20 0.17 D3+ + 3e =D -1.36 Lewis Base Overview & Examples | What is a Lewis Base? reduction ____________ is reduced in the following reaction: CrO+6SO+14H2Cr+3SO+7HO A. CrO b. SO c. H d. Cr e. SO CrO ___________ is the oxidizing agent in the reaction below. Select one: O a. I- 0 b. Ag O c. MnO2 d. H202 o e. NO When the following reaction is balanced, what are the stoichiometric coefficients for each substance? succeed. Generally, students get confused in redox reactions aboout which element is getting reduced and which is getting oxidized. 1, 1,4, 1, 2 O c. 1, 1, 2, 1, 2 O d. 4, 1, 2, 1, 2 o e. 4, 1, 4, 4, 2 1. The more positive value, the more likely the substance is to be reduced, so obviously +.34 is more positive than -.76. Oxidation Number Rules & Examples | What is an Oxidation Number? A reduction reaction is a reaction that gives an electron to a substance. The stronger the reduction potential, the more difficult is oxidation - example is fluorine. What are the key steps and assumptions for mass and energy balance in distillation column simulation? Zn will act as anode and oxidize and corrode because Zn is more active metal than Fe, Zn = Zn2+ + 2e- (corrosion of zinc). Balance the equation of hydrogen sulfide in air reacting to form sulfur dioxide and water. Snapsolve any problem by taking a picture. Hence, option B is correct. Oxidation is the removal of electrons from an atom or polyatomic ion. A reducing agent (also called a reductant or reducer) is the element or a compound in a redox (reduction-oxidation) reaction (see electrochemistry) that reduces another species.In doing so, it becomes oxidized, and is therefore the electron donor in the redox. So the best reducing agents are at the bottom of the table on the right side and have the most negative standard potentials. flashcard sets. The Fish Tale Across the Wall Tenths and Hundredths Parts and Whole Can you see the Pattern? To give up an electron means to become more positively charged. When the two metals in a galvanic couple are close on the series, their voltage ranges overlap, and either one can be the anode, depending on the exact exposure conditions. Identify the element which is the strongest reducing agent. Chem. Ch.20: Electrochemistry Flashcards | Quizlet Thus, the correct answer is option A. Zn (s) is the strongest reducing agent. 0 2 D A chemical reaction does not occur for this question Submit Request Answer. The table below is showing how oxidizing and reducing substances are arranged in an electrochemical series.
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