Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 10: Problem 63

One of the following ions has a trigonal-planar shape: $\mathrm{SO}_{3}^{2-} ; \mathrm{PO}_{4}^{3-} ; \mathrm{PF}_{6}^{-} ; \mathrm{CO}_{3}^{2-} .$ Which ion is it? Explain.

Short Answer

Expert verified
The ion that has a trigonal planar shape is \(CO_{3}^{2-}\).

Step by step solution

01

Drawing Lewis Structure 1

Draw the Lewis structure of \(SO_{3}^{2-}\). It can be observed that sulphur (S) is the central atom bonded to three oxygen atoms and also carries a lone pair of electrons. This gives it a tetrahedral electronic geometry.
02

Drawing Lewis Structure 2

Next, draw the Lewis structure of \(PO_{4}^{3-}\). With phosphorus (P) as the central atom, it is bonded to four oxygen atoms, giving it a tetrahedral electronic geometry as well.
03

Drawing Lewis Structure 3

After that, draw the Lewis structure of \(PF_{6}^{-}\). Here, phosphorus (P) is the central atom and it is bonded to six fluorine atoms, resulting in an octahedral electronic geometry.
04

Drawing Lewis Structure 4

Finally, draw the Lewis structure of \(CO_{3}^{2-}\). In this case, carbon (C) is the central atom and is bonded to three oxygen atoms. This gives it three electron domains, meaning it has a trigonal planar electronic geometry.

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

The following polyatomic anions involve covalent bonds between O atoms and the central nonmetal atom. Propose an acceptable Lewis structure for each. (a) \(\mathrm{SO}_{3}^{2-} ;\) (b) \(\mathrm{NO}_{2}^{-} ;\) (c) \(\mathrm{CO}_{3}^{2-} ;\) (d) \(\mathrm{HO}_{2}^{-}\).

Suggest reasons why the following do not exist as stable molecules: (a) \(\mathrm{H}_{3} ;\) (b) \(\mathrm{HHe} ;\) (c) \(\mathrm{He}_{2}\); (d) \(\mathrm{H}_{3} \mathrm{O}\).

Briefly describe each of the following ideas: (a) formal charge; (b) resonance; (c) expanded valence shell; (d) bond energy.

Sodium azide, \(\mathrm{NaN}_{3}\), is the nitrogen gas-forming substance used in automobile air-bag systems. It is an ionic compound containing the azide ion, \(\mathrm{N}_{3}^{-}\). In this ion, the two nitrogen-to-nitrogen bond lengths are \(116 \mathrm{pm} .\) Describe the resonance hybrid Lewis structure of this ion.

Use the \(\mathrm{NH}_{3}\) molecule as an example to explain the difference between molecular geometry and electron-group geometry.
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Analysis

Read Explanation

Physical Chemistry

Read Explanation

Organic Chemistry

Read Explanation

Nuclear Chemistry

Read Explanation

Kinetics

Read Explanation

Chemical Reactions

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