Concept explainers
(a)
Interpretation: Assign oxidation numbers to all of the elements of the following:
Li3PO4
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 each of the following:
SO32-
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 each of the following:
Cr2S3
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 each of the following:
NO3-
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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Check out a sample textbook solutionChapter 15 Solutions
Basic Chemistry
- Balance each of the following oxidationreduction reactions by nsing the oxidation states method. a. Cl2(g) + Al(s) Al3+(aq) + Cl(aq) b. O2(g) + H2O(l) + Ph(s) Ph(OH)2(s) c. H+(aq) + MnO4(aq) + Fe2+(aq) Mn2+(aq) + Fe3+(aq) + H2O(l)arrow_forwardBalance each of the following oxidationreduction reactions by using the oxidation states method. a.C2H4(g) + O2(g) CO3(g) + H2O(g) b. Mg(s) + HCl(aq) Mg2+(aq) + Cl(aq) + H2(g) c.Co3+(aq) + Ni(s) Co2+(aq) + Ni2+(aq) d.Zn(s) + H2SO4(aq) ZnSo4(aq) + H2(g)arrow_forwardBalance each of the following oxidationreduction reactions by using the oxidation states method. a. C2H6(g) + O2(g) CO2(g) + H2O(g) b. Mg(s) + HCl(aq) Mg2+(aq) + Cl(aq) + H2(g) c. Co3+ (aq) + Ni(s) Co2+(aq) + Ni2+(aq) d. Zn(s) + H2SO4(aq) ZnSO4(aq) + H2(g)arrow_forward
- 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_forwardIdentify each of the blowing substances as a likely oxidizing or reducing agent: HNO3, Na, C12, O2, KMnO4.arrow_forwardFour metals, A, B, C, and D, exhibit the following properties: (a) Only A and C react with 1.0 M hydrochloric acid to give H2(g). (b) When C is added to solutions of the ions of the other metals, metallic B, D, and A are formed. (c) Metal D reduces Bn+ to give metallic B and Dn+. Based on this information, arrange the four metals in order of increasing ability to act as reducing agents.arrow_forward
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