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(a)
Interpretation: Assign oxidation numbers to all of the elements of the following:
H2S
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: Assign oxidation numbers to all of the elements of the following:
NO2
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: Assign oxidation numbers to all of the elements of the following:
CCl4
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: Assign oxidation numbers to all of the elements of the following:
PCl3
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.
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Chapter 15 Solutions
Pearson eText Basic Chemistry -- Instant Access (Pearson+)
- What does it mean for a substance to be oxidized? The term “oxidation” originally came from substances reacting with oxygen gas. Explain why a substance that reacts with oxygen gas will always be oxidized.arrow_forward5 items multiple choice 35. What is the oxidation number of chlorine in HClO4? A. +1 B. +6 C. +7 D. -8 36. How many electrons were lost/gained in the following redox reaction 2K2Cr2O7 + 2H2O + 3S 4KOH + 2Cr2O3 + 3SO2? A. 2 B. 3 C. 6 D. 12 37. In the reaction, Fe2+ + Cr2O72- Fe3+ + Cr3+, which is involved in oxidation? A. Fe B. Cr2O7 C. Cr D. O 38. Which of the following half reactions in CORRECT? A. I2 + 1e- I- B. Cu2+ + 2e- Cu+ C. Zn2+ + 2e- Zn D. 2H+ + 2e- H2- 39. The following are examples of spontaneous reactions EXCEPT A. Water freezes spontaneously below 0ᵒC, and ice melts spontaneously above 0ᵒC. B. Heat flows from a colder one but reverse happens spontaneously. C. A waterfall runs downhill, but never up spontaneously. D. A lump of sugar spontaneously dissolves in a cup of coffee, but dissolved sugar does not spontaneously reappear in its original form. 40. For an equilibrium process, the free-energy change ∆G is A. less than zero. B. greater than zero. C. equal to…arrow_forwardWhat is the oxidation state of element X in the compound H3X30? a. +3 b. +2 с. +1 d. 0 е. -1 f. -2 g. -3arrow_forward
- In which two compounds does nitrogen have the same oxidation number? N₂O3 and HNO3 N₂O5 and HNO3 NO₂ and N₂03 N₂O4 and HNO2 HNO2 and NH3 A. B. C. D. E.arrow_forward6. Use the reaction below to answer the following questions. /8 points 3 Mg + N2 → Mg,N2 a. Which substance is losing electrons? b. Which substance is gaining electrons? c. Which substance is oxidized? d. Which substance is reduced? 7. Write the oxidation states of each element in the substances below. J6 points a. H,02 H b. Н.О H c. SF6 Farrow_forwardWhat is the oxidation number of the carbon indicated with the letter A? O Question 12 A What is the oxidation number of the carbon indicated with the letter D? :0: A B =o. B IIOII H :0: H E Earrow_forward
- the oxidation number of sulfur atoms in thiosulfate O a. 2 O b. 2, 8 O c. 0, 4 O d. -2, 8arrow_forwardAssign oxidation numbers to the elements in the following compounds: 1. NH4HCO3 2. F2 3. Ca3(PO4)2arrow_forwardIn the smelting of iron from iron oxide according to the equation what is the change in oxidation number for iron? Fe2O3(s) + 3CO(g) ------> 2Fe(s) + 3CO2(g) Select one: a. -3 b. +2 c. 0 d. +3 e. -2arrow_forward
- 4. For the reaction the product will be: a. 1 y 2 b. 2 c. 1 d. 4 e. 3arrow_forward9. What is the oxidation state of phosphorus (P) in sodium phosphate, ??,?? ,? A. +5 B. +3 C. 0 D. -3 E. -5arrow_forward10. In the reaction, Fe203(s) + 3CO(g) 2Fe(l) + 3C02(g) --- a. carbon monoxide is reduced c. carbon monoxide is the oxidizing agent L b. iron(III) oxide is oxidized d. iron(III) oxide is the oxidizing agentarrow_forward
- Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxIntroductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
- Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
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