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(a)
Interpretation: Assign oxidation numbers to all of the elements of the following:
KCl
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:
MnO2
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:
NO
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:
Mn2O3
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
EP BASIC CHEMISTRY-STANDALONE ACCESS
- 5 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_forwardThe oxidation number of chromium in sodium chromite, NaCrO2, is A. -1 B. -2 C. +2 D. +1 E. +3arrow_forwardIn 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_forward
- What is the oxidation number Ga in Ga(OH)3 ? a. +1 b. +3 c. -3 d. -1arrow_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_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
- 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. 12arrow_forwardWhat element is being reduced in the following redox reaction? C3H8O2(aq) + KMnO4(aq) ⟶⟶ C3H2O4K2(aq) + MnO2(aq) A. O B. Mn C. K D. C E. Harrow_forwardWhat is the oxidation number of element underlined in the following element, compound and ion? a. Al³+ b. C1037 c. 03 d. PCla e. Cr₂072-arrow_forward
- 9. What is the oxidation state of phosphorus (P) in sodium phosphate, ??,?? ,? A. +5 B. +3 C. 0 D. -3 E. -5arrow_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_forwardIdentify the oxidizing agent in the following reaction 2Na + 2H2O 2ÑAOH + H2 A. Na B. H2O C. NaOH D. H2arrow_forward
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