Concept explainers
(a)
Interpretation: In the following reactions, identify the reactant that is oxidized and the reactant that is reduced:
Concept Introduction:
The rules for assigning oxidation number to elements are:
- For an element in its free state it is assigned an oxidation number of zero.
- Monatomic ions have oxidation number that is equal to charge of the monatomic ion.
- Alkali metals have +1 oxidation number, alkaline earth metals have +2 oxidation number and halogens are assigned -1 oxidation number.
- In most compounds H is assigned a +1 oxidation number and O is assigned a -2 oxidation number.
- For a neutral compound the summation of oxidation numbers of all elements in the compound is zero.
If the oxidation number of an element increases then it undergoes oxidation and if the oxidation number of the element decreases then it undergoes reduction.
(b)
Interpretation: In the following reactions, identify the reactant that is oxidized and the reactant that is reduced:
Concept Introduction:
The rules for assigning oxidation number to elements are:
- For an element in its free state it is assigned an oxidation number of zero.
- Monatomic ions have oxidation number that is equal to charge of the monatomic ion.
- Alkali metals have +1 oxidation number, alkaline earth metals have +2 oxidation number and halogens are assigned -1 oxidation number.
- In most compounds H is assigned a +1 oxidation number and O is assigned a -2 oxidation number.
- For a neutral compound the summation of oxidation numbers of all elements in the compound is zero.
If the oxidation number of an element increases then it undergoes oxidation and if the oxidation number of the element decreases then it undergoes reduction.
(c)
Interpretation: In the following reactions, identify the reactant that is oxidized and the reactant that is reduced:
Concept Introduction:
The rules for assigning oxidation number to elements are:
- For an element in its free state it is assigned an oxidation number of zero.
- Monatomic ions have oxidation number that is equal to charge of the monatomic ion.
- Alkali metals have +1 oxidation number, alkaline earth metals have +2 oxidation number and halogens are assigned -1 oxidation number.
- In most compounds H is assigned a +1 oxidation number and O is assigned a -2 oxidation number.
- For a neutral compound the summation of oxidation numbers of all elements in the compound is zero.
If the oxidation number of an element increases then it undergoes oxidation and if the oxidation number of the element decreases then it undergoes reduction.
(d)
Interpretation: In the following reactions, identify the reactant that is oxidized and the reactant that is reduced:
Concept Introduction:
The rules for assigning oxidation number to elements are:
- For an element in its free state it is assigned an oxidation number of zero.
- Monatomic ions have oxidation number that is equal to charge of the monatomic ion.
- Alkali metals have +1 oxidation number, alkaline earth metals have +2 oxidation number and halogens are assigned -1 oxidation number.
- In most compounds H is assigned a +1 oxidation number and O is assigned a -2 oxidation number.
- For a neutral compound the summation of oxidation numbers of all elements in the compound is zero.
If the oxidation number of an element increases then it undergoes oxidation and if the oxidation number of the element decreases then it undergoes reduction.
Want to see the full answer?
Check out a sample textbook solutionChapter 8 Solutions
EP BASIC CHEMISTRY-MODIFIED MASTERING
- For each reaction, indicate which elements are oxidized and which are reduced: a.2Al+3CU2+2Al3++3Cub.2H++NiNi2++H2c.2I-+Cl2I2+2Cl-arrow_forwardIdentify the atoms that are oxidized and reduced, the change in oxidation state for each, and the oxidizing and reducing agents in each of the following equations: (a) Mg(s)+NiCl2(aq)MgCl2(aq)+Ni(s) (b) PCl3(l)+Cl2(g)PCl5(s) (c) C2H4(g)+3O2(g)2CO2(g)+2H2O(g) (d) Zn(s)+H2SO4(aq)ZnSO4(aq)+H2(g) (e) 2K2S2O3(s)+I2(s)K2S4O6(s)+2KI(s) (f) 3Cu(s)+8HNO3(aq)3Cu( NO3)2(aq)+2NO(g)+4H2O(l)arrow_forwardWrite equations for respiration and photosynthesis. For each reaction, label the substances that are oxidized and reduced. Why are these reactions important?arrow_forward
- Oxidation of 1.00 g of carbon monoxide, CO, produces 1.57 g of carbon dioxide, CO2. How many grams of oxygen were required in this reaction?arrow_forwardConsider the reaction between oxygen (O2) gas and magnesium metal to form magnesium oxide. Using oxidation states, how many electrons would each oxygen atom gain, and how many electrons would each magnesium atom lose? How many magnesium atoms are needed to react with one oxygen molecule? Write a balanced equation for this reaction.arrow_forwardOne of the few industrial-scale processes that produce organic compounds electrochemically is used by the Monsanto Company to produce1,4-dicyanobutane. The reduction reaction is 2CH2CHCH+2H++2eNC(CH2)4CN The NC(CH2)4CN is then chemically reduced using hydrogen gas to H2N(CH2)6NH2, which is used in the production of nylon. What current must be used to produce 150.kg NC(CH2)4CN per hour?arrow_forward
- . For each of the following oxidation-reduction reactions of metals with nonmetals, identify which element is oxidized and which is reduced. a.4Na(s)+O2(g)2Na2O(s)b.Fe(s)+H2SO4(aq)FeSO4(aq)+H2(g)c.2Al2O3(s)4Al(s)+3O2(g)d.3Mg(s)+N2(g)Mg3N2(s)arrow_forwardIndicate what type, or types, of reaction each of the following represents: (a) Ca(s)+Br2(l)CaBr2(s) (b) Ca(OH)2(aq)+2HBr(aq)CaBr2(aq)+2H2O(l) (c) C6H12(l)+9O2(g)6CO2(g)+6H2O(g)arrow_forwardBromine is obtained from sea water by the following redox reaction: Cl2(g) + 2 NaBr(aq) 2 NaCl(aq) + Br2() (a) What has been oxidized? What has been reduced? (b) Identify the oxidizing and reducing agents.arrow_forward
- Write balanced chemical equations for the reactions used to prepare each of the following compounds from the given starting material(s). In some cases, additional reactants may be required. (a) solid ammonium nitrate from gaseous molecular nitrogen via a two-step process (first reduce the nitrogen to ammonia, then neutralize the ammonia with an appropriate acid) (b) gaseous hydrogen bromide from liquid molecular bromine via a one-step redox reaction (c) gaseous H2S from solid Zn and S via a two-step process (first a redox reaction between the starting materials, then reaction of the product with a strong acid)arrow_forward5. For the following combustion reactions, identify the species that is oxidized, the species that is reduced, the oxidizing agent, and the reducing agent. a. 2 C₂H₂ +50₂ → 4 CO₂ + 2 H₂O b. 2 C4H10+ 13 0₂8 CO₂ + 10 H₂Oarrow_forwardWhat is oxidized and what is reduced, respectively, in the following reaction? 2Al(s) + 3Br₂(g) → 2AlBr3(s) Select one: a. Al is oxidized and Br₂ is reduced. 2Al(s) + 3Br2(g) → 2AlBr3(s) Ob. Al is reduced and Br₂ is oxidized. Oc. AlBr3 is reduced and Al is oxidized. Od. AlBr3 is reduced and Br₂ is oxidized. Clear my choice Search lijı ******arrow_forward
- Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningWorld of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
- Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning