Concept explainers
(a)
Interpretation: Assign oxidation numbers to all of the elements in C2H3O2-
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 in AlCl3
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 in NH4+
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 in HBrO4
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. 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_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_forward
- Vitamin C has the formula C6H8O6. Besides being an acid, it is a reducing agent. One method for determining the amount of vitamin C in a sample is to titrate it with a solution of bromine, Br2, an oxidizing agent. C6H8O6(aq) + Br2(aq) 2 HBr(aq) + C6H6O6(aq) A 1.00-g "chewable" vitamin C tablet requires 27.85 ml of 0.102 M Br2 for titration to the equivalence point. What is the mass of vitamin C in the tablet?arrow_forwardClassify each of the following reactions as a precipitation, acid-base, or gas forming reaction. Show states for the products (s, , g aq), and then balance the completed equation. Write the net ionic equation. (a) MnCl2(aq) + Na2S(aq) MnS + NaCl (b) K2CO3(aq) + ZnCl2(aq) ZnCO3 + Kaarrow_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
- MCQ 8: Oxidation state +2 of a compound have greater ionic character than oxidation state of A. +1 B. +3 C. +4 D. +5arrow_forward4. Give the oxidation number of the underlined atoms in the following molecules and ions: a. ClFb. IF7 c. CH4 d. C2H2e. C2H4f. K2CrO4g. K2Cr2O7h. KMnO4i. NaHCO3j. O2k. NaIO3l. K2O m. PF6n. AuCl4arrow_forwardDetermine the Oxidation number in the given chemical reaction below: a. Ti →Ti O2 b. C → C2 O4 2 c. N → HNO3arrow_forward
- Identify the oxidation number of the atom/s 1. NaCl2. Cu2O 3. CaH2 4. S8 5. H2O2arrow_forwardAssigning Oxidation Numbers Use these rules in order. The sum of all oxidation numbers of all elements = charge on substance. Oxidation Number: Examples: 1. Atoms in their elemental state Fe, H2, O2 2. Monatomic ions = charge F, Fe3+ IN COMPOUNDS NaCl, KNο 3. Group 1A 4. Group 2A 5. Fluorine +1 +2 MgO -1 HF, CIF 6. Hydrogen 7. Oxygen 8. Group 7A +1 H20 -2 SO2, HCIO4 -1 HCI 9. Group 6A -2 PbS,arrow_forwardWhat is the oxidation number for P within the polyatomic ion: Be2P2O7 a. +2 b. +6 c. -3 d. +5arrow_forward
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