Concept explainers
Give the oxidation numbers for the underlined atoms in the following molecules and ions:
Interpretation:
The oxidation number of the underlined atoms isto be determined.
Concept introduction:
The oxidation number can be assigned using the following rules:
In free state, an element is always in
For a neutral compound, oxidation numbers of atoms add upto
In a polyatomic ion, oxidation number of atoms add up to the charge on the ion.
The oxidation number of monoatomic ions is same as its charge.
Oxygen is usually in
Hydrogen is usually in
Group 1 elements are always in
Answer to Problem 45QP
Solution:
(a)
(b) +7
(c)
(d)
(e)
(f)
(g)
(h)
(i)
(j)
(k)
(l)
(m)
(n)
Explanation of Solution
(a)
Let the oxidation number of Clbe
Hence, the oxidation number ofCl can be calculated as follows:
Thus, the oxidation number of Clis
(b)
In
Hence, the oxidation number ofiodine can be calculated as follows:
Thus, the oxidation number of iodine is
(c)
Let the oxidation number of carbonbe
Hence, the oxidation number ofcarbon can be calculated as follows:
Thus, the oxidation number of carbonis
(d)
Let the oxidation number of carbonbe
Hence, the oxidation number ofcarbon can be calculated as follows:
Thus, the oxidation number of carbon is
(e)
Let the oxidation number of carbonbe
Hence, the oxidation number ofcarbon can be calculated as follows:
Thus, the oxidation number of carbon is
(f)
Let the oxidation number of chromium (Cr)be
Hence, the oxidation number ofchromium can be calculated as follows:
Thus, the oxidation number of chromium is
(g)
Let the oxidation number of chromium be
Hence, the oxidation number ofchromium can be calculated as follows:
Thus, the oxidation number of chromium is
(h)
Let the oxidation number of manganese be
Hence, the oxidation number ofmanganese can be calculated as follows:
Thus, the oxidation number of manganese is
(i)
Let the oxidation number of carbonbe
Hence, the oxidation number ofcarbon can be calculated as follows:
Thus, the oxidation number of carbon is
(j)
The oxidation number of any atom in its elemental form is zero.
Hence, the oxidation number of lithiumis
(k)
Let the oxidation number of iodinebe
Hence, the oxidation number ofiodine can be calculated as follows:
Thus, the oxidation number of iodine is
(l)
Let the oxidation number of oxygenbe
Hence, the oxidation number ofoxygen can be calculated as follows:
Thus, the oxidation number of oxygen is
(m)
Let the oxidation number of phosphorus be
Hence, the oxidation number ofphosphorus can be calculated as follows:
Thus, the oxidation number of phosphorus is
(n)
Let the oxidation number of Aube
Hence, the oxidation number of Au can be calculated as follows:
Thus, the oxidation number of Au is
Want to see more full solutions like this?
Chapter 4 Solutions
Chemistry
Additional Science Textbook Solutions
General, Organic, & Biological Chemistry
Organic Chemistry As a Second Language: Second Semester Topics
Chemistry & Chemical Reactivity
Essential Organic Chemistry (3rd Edition)
Basic Chemistry (5th Edition)
- 1. Sometimes a reaction can fall in more than one category. Into what category (or categories) does the reaction of Ba(OH)2(aq) + H+PO4(aq) fit? acid-base and oxidation-reduction oxidation-reduction acid-base and precipitation precipitationarrow_forwardElemental bromine is the source of bromine compounds. The element is produced from certain brine solutions that occur naturally. These brines are essentially solutions of calcium bromide that, when treated with chlorine gas, yield bromine in a displacement reaction. What are the molecular equation and net ionic equation for the reaction? A solution containing 40.0 g of calcium bromide requires 14.2 g of chlorine to react completely with it, and 22.2 g of calcium chloride is produced in addition to whatever bromine is obtained. How many grams of calcium bromide are required to produce 10.0 pounds of bromine?arrow_forwardArsenic acid, H3AsO4, is a poisonous acid that has been used in the treatment of wood to prevent insect damage. Arsenic acid has three acidic protons. Say you take a 25.00-mL sample of arsenic acid and prepare it for titration with NaOH by adding 25.00 mL of water. The complete neutralization of this solution requires the addition of 53.07 mL of 0.6441 M NaOH solution. Write the balanced chemical reaction for the titration, and calculate the molarity of the arsenic acid sample.arrow_forward
- One way of determining blood alcohol levels is by performing a titration on a sample of blood. In this process, the alcohol from the blood is oxidized by dichromate ions (Cr2O72-) according to the following net ionic equation: C2H5OH+2Cr2O72+16H+2CO2+4Cr3++11H2O A 10.00-g sample of blood was drawn from a patient, and 13.77 mL of 0.02538 M K2Cr2O7 was required to titrate the alcohol. What was the patient’s blood alcohol level? (See the previous problem for definition of blood alcohol level. K2Cr2O7 is a strong electrolyte, so it dissociates completely in solution.)arrow_forwardTriiodide ions are generated in solution by the following (unbalanced) reaction in acidic solution: IO3(aq) + I(aq) I3(aq) Triiodide ion concentration is determined by titration with a sodium thiosulfate (Na2S2O3) solution. The products are iodide ion and tetrathionate ion (S4O6). a. Balance the equation for the reaction of IO3 with I ions. b. A sample of 0.6013 g of potassium iodate was dissolved in water. Hydrochloric acid and solid potassium iodide were then added. What is the minimum mass of solid KI and the minimum volume of 3.00 M HQ required to convert all of the IO3 ions to I ions? c. Write and balance the equation for the reaction of S2O32 with I3 in acidic solution. d. A 25.00-mL sample of a 0.0100 M solution of KIO. is reacted with an excess of KI. It requires 32.04 mL of Na2S2O3 solution to titrate the I3 ions present. What is the molarity of the Na2S2O3 solution? e. How would you prepare 500.0 mL of the KIO3 solution in part d using solid KIO3?arrow_forwardWhat volume of 0.0521 M Ba(OH)2 is required to neutralize exactly 14.20 mL of 0.141 M H3PO4? Phosphoric acid contains three acidic hydrogens.arrow_forward
- Describe in words how you would prepare pure crystalline AgCl and NaNO3 from solid AgNO3 and solid NaCl.arrow_forwardA solution of hydrogen peroxide, H2O2, is titrated with a solution of potassium permanganate, KMnO4. The reaction is 5H2O2(aq)+2KMnO4(aq)+3H2SO4(aq)5O2(g)+2MnSO4(aq)+K2SO4(aq)+8H2O(l) It requires 51.7 mL of 0.145 M KMnO4 to titrate 20.0 g of the solution of hydrogen peroxide. What is the mass percentage of H2O2 in the solution?arrow_forwardCalcium in blood or urine can be determined by precipitation as calcium oxalate, CaC2O4. The precipitate is dissolved in strong acid and titrated with potassium permanganate. The equation for reaction is 2MnO4(aq)+6H+(aq)+5H2C2O4(aq)2Mn2+(aq)+10CO2(g)+8H2O A 24-hour urine sample is collected from an adult patient, reduced to a small volume, and titrated with 26.2 mL of 0.0946 M KMnO4. How many grams of calcium oxalate are in the sample? Normal range for Ca2+ output for an adult is 100 to 300 mg per 24 hour. Is the sample within the normal range?arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry: 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
- Introduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage LearningGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning