Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 22: Problem 31

Write the chemical formula for each of the following, and indicate the oxidation state of the halogen or noble-gas atom in each: (a) xenon trioxide difluoride, \((\mathbf{b})\) chlorine dioxide, \((\mathbf{c})\) molybdenum hexafluoride, \((\mathbf{d})\) iodic acid, (e) sodium hypobromite, \((\mathbf{f})\) magnesium iodite.

Short Answer

Expert verified
The chemical formulas and oxidation states for the given compounds are: a) Xenon trioxide difluoride: XeO₃F₂, oxidation state of Xe is +8. b) Chlorine dioxide: ClO₂, oxidation state of Cl is +4. c) Molybdenum hexafluoride: MoF₆, oxidation state of Mo is +6. d) Iodic acid: HIO₃, oxidation state of I is +5. e) Sodium hypobromite: NaBrO, oxidation state of Br is +1. f) Magnesium iodite: Mg(IO₂)₂, oxidation state of I is +3.

Step by step solution

01

a) Xenon trioxide difluoride

First, we need to identify the elements involved: xenon (Xe), oxygen (O), and fluorine (F). The prefixes 'tri' and 'di' tell us there are three oxygen atoms and two fluorine atoms. The chemical formula is XeO₃F₂. To find the oxidation state of Xe, we can set up an equation based on the oxidation state of oxygen (-2) and fluorine (-1), and then solve for Xe: \(x + 3(-2) + 2(-1) = 0 \Rightarrow x = +8\). The oxidation state of xenon in the compound is +8.
02

b) Chlorine dioxide

Chlorine (Cl) and oxygen (O) are the elements involved. In chlorine dioxide, there is one chlorine and two oxygen atoms. The chemical formula is ClO₂. The oxidation state of oxygen is -2, so to find the oxidation state of chlorine, we set up the equation: \(x + 2(-2) = 0 \Rightarrow x = +4\). The oxidation state of chlorine in the compound is +4.
03

c) Molybdenum hexafluoride

The elements in this compound are molybdenum (Mo) and fluorine (F). The prefix 'hexa' indicates that there are six fluorine atoms. The chemical formula is MoF₆. The oxidation state of fluorine is -1. To find the oxidation state of Mo, we set up an equation: \(x + 6(-1) = 0 \Rightarrow x = +6\). The oxidation state of molybdenum in the compound is +6.
04

d) Iodic acid

In iodic acid, the elements involved are iodine (I), hydrogen (H), and oxygen (O). The chemical formula is HIO₃. The oxidation state of hydrogen is +1 and for oxygen is -2. To find the oxidation state of iodine, we set up an equation: \((+1) + x + 3(-2) = 0 \Rightarrow x = +5\). The oxidation state of iodine in the compound is +5.
05

e) Sodium hypobromite

The elements in the sodium hypobromite are sodium (Na), bromine (Br), and oxygen (O). The chemical formula is NaBrO. The oxidation state of sodium is +1 and for oxygen is -2. To find the oxidation state of bromine, we set up an equation: \( (+1) + x + (-2) = 0 \Rightarrow x = +1\). The oxidation state of bromine in the compound is +1.
06

f) Magnesium iodite

Magnesium (Mg) and iodine (I) are the elements in magnesium iodite. This compound contains the iodite ion (IO₂⁻). The chemical formula is Mg(IO₂)₂. The magnesium ion (Mg²⁺) has an oxidation state of +2 and each iodite ion has a charge of -1. The oxidation state of iodine in the iodite ion is found by setting up an equation: \(x + 2(-2) = -1 \Rightarrow x = +3\). The oxidation state of iodine in the compound is +3.

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

(a) Determine the number of sodium ions in the chemical formula of albite, \(\mathrm{Na}_{x} \mathrm{AlSi}_{3} \mathrm{O}_{8} .(\mathbf{b})\) Determine the number of hydroxide ions in the chemical formula of tremolite, $\mathrm{Ca}_{2} \mathrm{Mg}_{5}\left(\mathrm{Si}_{4} \mathrm{O}_{11}\right)_{2}(\mathrm{OH})_{x}$.

Write a balanced equation for each of the following reactions: (a) hydrolysis of \(\mathrm{PCl}_{5},(\mathbf{b})\) dehydration of phosphoric acid (also called orthophosphoric acid) to form pyrophosphoric acid, \((\mathbf{c})\) reaction of \(\mathrm{P}_{4} \mathrm{O}_{10}\) with water.

The maximum allowable concentration of \(\mathrm{H}_{2} \mathrm{~S}(g)\) in air is \(20 \mathrm{mg}\) per kilogram of air ( 20 ppm by mass). How many grams of FeS would be required to react with hydrochloric acid to produce this concentration at \(101.3 \mathrm{kPa}\) and \(25^{\circ} \mathrm{C}\) in an average room measuring $3.5 \mathrm{~m} \times 6.0 \mathrm{~m} \times 2.5 \mathrm{~m} ?\( (Under these conditions, the average molar mass of air is \)29.0 \mathrm{~g} / \mathrm{mol} .)$

Write the chemical formula for each of the following, and indicate the oxidation state of the halogen or noble-gas atom in each: (a) krypton tetrafluoride, (b) hexafluoroantimonate ion, \((\mathbf{c})\) sodium hypoiodite, \((\mathbf{d})\) perbromic acid, (e) aluminum perchlorate, (f) iron(II) iodite.

Explain the following observations: (a) For a given oxidation state, the acid strength of the oxyacid in aqueous solution decreases in the order chlorine \(>\) bromine \(>\) iodine. (b) Hydrofluoric acid cannot be stored in glass bottles. (c) HI cannot be prepared by treating NaI with sulfuric acid. (d) The interhalogen \(\mathrm{ICl}_{3}\) is known, but \(\mathrm{BrCl}_{3}\) is not.
See all solutions

Recommended explanations on Chemistry Textbooks

Nuclear Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Physical Chemistry

Read Explanation

Inorganic Chemistry

Read Explanation

Kinetics

Read Explanation

Chemical Analysis

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