Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 4: Problem 143

Chlorine forms a number of oxides with the following oxidation numbers: \(+1,+3,+4,+6,\) and +7 . Write a formula for each of these compounds.

Short Answer

Expert verified
The formulas for the chlorides with oxidation states from +1 to +7 are: HClO (hypochlorous acid), HClO2 (chlorous acid), ClO2 (chlorine dioxide), HClO3 (chloric acid), and HClO4 (perchloric acid), respectively.

Step by step solution

01

Write Oxides with +1 Oxidation State

Chlorine with +1 oxidation state forms hypochlorous acid, symbolized as HClO, where oxygen has oxidation state -2 and hydrogen +1.
02

Write Oxides with +3 Oxidation State

Chlorine with +3 oxidation state forms chlorous acid, symbolized as HClO2, where oxygen again has oxidation state -2 and hydrogen +1.
03

Write Oxides with +4 Oxidation State

Chlorine with +4 oxidation state forms chlorine dioxide, symbolized as ClO2, where oxygen again has oxidation state -2.
04

Write Oxides with +6 Oxidation State

Chlorine with +6 oxidation state forms chloric acid, symbolized as HClO3, where oxygen again has oxidation state -2 and hydrogen +1.
05

Write Oxides with +7 Oxidation State

Chlorine with +7 oxidation state forms perchloric acid, symbolized as HClO4, where oxygen again has oxidation state -2 and hydrogen +1.

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

How many moles of \(\mathrm{MgCl}_{2}\) are present in \(60.0 \mathrm{~mL}\) of \(0.100 \mathrm{M} \mathrm{MgCl}_{2}\) solution?

What volume of a \(0.500 M\) HCl solution is needed to neutralize each of the following? (a) \(10.0 \mathrm{~mL}\) of a \(0.300 \mathrm{M} \mathrm{NaOH}\) solution (b) \(10.0 \mathrm{~mL}\) of a \(0.200 \mathrm{M} \mathrm{Ba}(\mathrm{OH})_{2}\) solution

Water is added to \(25.0 \mathrm{~mL}\) of a \(0.866 \mathrm{M} \mathrm{KNO}_{3}\) solution until the volume of the solution is exactly \(500 \mathrm{~mL}\). What is the concentration of the final solution?

A \(60.0-\mathrm{mL} 0.513 \mathrm{M}\) glucose \(\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right)\) solution is mixed with \(120.0 \mathrm{~mL}\) of \(2.33 \mathrm{M}\) glucose solution. What is the concentration of the final solution? Assume the volumes are additive.

A 3.664 -g sample of a monoprotic acid was dissolved in water. It took \(20.27 \mathrm{~mL}\) of a \(0.1578 \mathrm{M}\) \(\mathrm{NaOH}\) solution to neutralize the acid. Calculate the molar mass of the acid.
See all solutions

Recommended explanations on Chemistry Textbooks

Nuclear Chemistry

Read Explanation

Chemistry Branches

Read Explanation

Physical Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Inorganic Chemistry

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