Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 4: Problem 80

Assign oxidation states for all atoms in each of the following compounds. a. \(\mathrm{UO}_{2}^{2+}\) b. \(\mathrm{As}_{2} \mathrm{O}_{3}\) c. \(\mathrm{NaBiO}_{3}\) d. As \(_{4}\) e. \(\mathrm{HAsO}_{2}\) f. \(\mathrm{Mg}_{2} \mathrm{P}_{2} \mathrm{O}_{7}\) g. \(\mathrm{Na}_{2} \mathrm{~S}_{2} \mathrm{O}_{3}\) h. \(\mathrm{Hg}_{2} \mathrm{Cl}_{2}\) i. \(\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\)

Short Answer

Expert verified
a. U: +6, O: -2 b. As: +3, O: -2 c. Na: +1, Bi: +5, O: -2 d. As: 0 e. H: +1, As: +3, O: -2 f. Mg: +2, P: +5, O: -2 g. Na: +1, S: +2, O: -2 h. Hg: +1, Cl: -1 i. Ca: +2, N: +5, O: -2

Step by step solution

01

a. Assigning oxidation states for \(\mathrm{UO}_{2}^{2+}\)

We know that the overall charge of the compound is +2 and the oxidation state of oxygen is usually -2. Since there are two oxygen atoms, their combined oxidation state is -4. Thus, the uranium atom must have an oxidation state of +6 to balance the overall charge to +2. Uranium: +6 Oxygen: -2
02

b. Assigning oxidation states for \(\mathrm{As}_{2} \mathrm{O}_{3}\)

In this compound, the overall charge is 0. Assuming oxygen has an oxidation state of -2, the total oxidation state of the three oxygen atoms is -6. To balance it, the two arsenic atoms must have a combined oxidation state of +6. Therefore, each arsenic atom has an oxidation state of +3. Arsenic: +3 Oxygen: -2
03

c. Assigning oxidation states for \(\mathrm{NaBiO}_{3}\)

The overall charge of the compound is 0. Sodium is an alkali metal with an oxidation state of +1, and oxygen usually has an oxidation state of -2. With one sodium and three oxygen atoms, their combined oxidation state is +1 - 6 = -5. Thus, the bismuth atom must have an oxidation state of +5 to balance the overall charge. Sodium: +1 Bismuth: +5 Oxygen: -2
04

d. Assigning oxidation states for As\(_{4}\)

As this is an uncombined element, each arsenic atom has an oxidation state of 0. Arsenic: 0
05

e. Assigning oxidation states for \(\mathrm{HAsO}_{2}\)

The overall charge of the compound is 0. We know that hydrogen has an oxidation state of +1, and oxygen has an oxidation state of -2. With one hydrogen and two oxygen atoms, their combined oxidation state is +1 - 4 = -3. Thus, the arsenic atom must have an oxidation state of +3 to balance the overall charge. Hydrogen: +1 Arsenic: +3 Oxygen: -2
06

f. Assigning oxidation states for \(\mathrm{Mg}_{2} \mathrm{P}_{2} \mathrm{O}_{7}\)

The overall charge of the compound is 0. We know that magnesium has an oxidation state of +2, and oxygen has an oxidation state of -2. With two magnesium atoms and seven oxygen atoms, their combined oxidation state is 2(+2) - 7(2) = +4 - 14 = -10. Thus, the two phosphorus atoms must have a combined oxidation state of +10. Therefore, each phosphorus atom has an oxidation state of +5. Magnesium: +2 Phosphorus: +5 Oxygen: -2
07

g. Assigning oxidation states for \(\mathrm{Na}_{2} \mathrm{~S}_{2} \mathrm{O}_{3}\)

We know that sodium has an oxidation state of +1, oxygen has an oxidation state of -2, and the overall charge of the compound is 0. With two sodium and three oxygen atoms, their combined oxidation state is 2(+1) - 3(2) = +2 - 6 = -4. Thus, the two sulfur atoms must have a combined oxidation state of +4. Therefore, each sulfur atom has an oxidation state of +2. Sodium: +1 Sulfur: +2 Oxygen: -2
08

h. Assigning oxidation states for \(\mathrm{Hg}_{2} \mathrm{Cl}_{2}\)

The overall charge of the compound is 0. We know that chlorine has an oxidation state of -1. With two chlorine atoms, their combined oxidation state is -2. So, the two mercury atoms must have a combined oxidation state of +2. Therefore, each mercury atom has an oxidation state of +1. Mercury: +1 Chlorine: -1
09

i. Assigning oxidation states for \(\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\)

Identify that the compound is made up of calcium and two nitrates. Calcium has an oxidation state of +2, and the overall charge of the compound is 0. Now we need to find the oxidation state of nitrogen and oxygen in the nitrate ion. The nitrate ion, \(\mathrm{NO}_{3}^{-}\), has an overall charge of -1. Oxygen has an oxidation state of -2. In the nitrate ion, the combined oxidation state of the three oxygen atoms is -6. Thus, nitrogen must have an oxidation state of +5 to balance the charge of the nitrate ion. Calcium: +2 Nitrogen: +5 Oxygen: -2

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Write the balanced formula, complete ionic, and net ionic equations for each of the following acid-base reactions. a. \(\mathrm{HNO}_{3}(a q)+\mathrm{Al}(\mathrm{OH})_{3}(s) \rightarrow\) b. \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)+\mathrm{KOH}(a q) \rightarrow\) c. \(\mathrm{Ca}(\mathrm{OH})_{2}(a q)+\mathrm{HCl}(a q) \rightarrow\)

A \(10.00-\mathrm{mL}\) sample of vinegar, an aqueous solution of acetic acid \(\left(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)\), is titrated with \(0.5062 \mathrm{M} \mathrm{NaOH}\), and \(16.58 \mathrm{~mL}\) is required to reach the equivalence point. a. What is the molarity of the acetic acid? b. If the density of the vinegar is \(1.006 \mathrm{~g} / \mathrm{cm}^{3}\), what is the mass percent of acetic acid in the vinegar?

When hydrochloric acid reacts with magnesium metal, hydrogen gas and aqueous magnesium chloride are produced. What volume of \(5.0 \mathrm{M} \mathrm{HCl}\) is required to react completely with \(3.00 \mathrm{~g}\) of magnesium?

Which of the following solutions of strong electrolytes contains the largest number of moles of chloride ions: \(100.0 \mathrm{~mL}\) of \(0.30 \mathrm{M} \mathrm{AlCl}_{3}, 50.0 \mathrm{~mL}\) of \(0.60 \mathrm{M} \mathrm{MgCl}_{2}\), or \(200.0 \mathrm{~mL}\) of \(0.40 \mathrm{M} \mathrm{NaCl} ?\)

The zinc in a \(1.343-g\) sample of a foot powder was precipitated as \(\mathrm{ZnNH}_{4} \mathrm{PO}_{4} .\) Strong heating of the precipitate yielded \(0.4089 \mathrm{~g} \mathrm{Zn}_{2} \mathrm{P}_{2} \mathrm{O}_{7} .\) Calculate the mass percent of zinc in the sample of foot powder.
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Reactions

Read Explanation

Chemistry Branches

Read Explanation

Organic Chemistry

Read Explanation

Kinetics

Read Explanation

Making Measurements

Read Explanation

Ionic and Molecular Compounds

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free