![Pearson eText Basic Chemistry -- Instant Access (Pearson+)](https://www.bartleby.com/isbn_cover_images/9780135765982/9780135765982_largeCoverImage.gif)
Concept explainers
(a)
Interpretation: Assign oxidation numbers to all of the elements in the following:
N2O
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 each of the following:
LiOH
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 each of the following:
SbO2-
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 each of the following:
IO4-
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.
![Check Mark](/static/check-mark.png)
Want to see the full answer?
Check out a sample textbook solution![Blurred answer](/static/blurred-answer.jpg)
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_forwardBalance 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_forward
- Balance 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_forwardAssign oxidation numbers to each atom in the following: a. P4O6 b. BiO3 − c. N2H4 d. Mg(BrO4)2 e. MnSO4 f. Mn(SO4)2arrow_forwardThe oxidation number of S in SO32- is Select one: a. +6 b. +2 С. О d. +4 e. -1arrow_forward
- The oxidation number of chromium in sodium chromite, NaCrO2, is A. -1 B. -2 C. +2 D. +1 E. +3arrow_forwardAssign oxidation numbers to the elements in the following compounds: 1. NH4HCO3 2. F2 3. Ca3(PO4)2arrow_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
- In the following reaction, the oxidation number of Fe changes from ____ to ____. Fe2O3 + 3CO → 2Fe + 3CO2 a. doesn't change (tidak berubah) b. +2, 0 c. 0, +2 d. +3, 0 e. 0, +3arrow_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 of chromium in the chromate ion, CrO42-? a. +2 O b. +6 O c. +8 O d. +3arrow_forward
- Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningIntroductory Chemistry: A FoundationChemistryISBN:9781285199030Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
![Text book image](https://www.bartleby.com/isbn_cover_images/9781337399425/9781337399425_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781305079373/9781305079373_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781285199030/9781285199030_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781305079243/9781305079243_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781133611097/9781133611097_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781285199047/9781285199047_smallCoverImage.gif)