Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 10: Problem 30

Write a plausible Lewis structure for \(\mathrm{C}_{3} \mathrm{O}_{2},\) a substance known as carbon suboxide.

Short Answer

Expert verified
The correct Lewis structure for \(C_{3}O_{2}\) or carbon suboxide has the skeletal structure O-C-C-C-O, with two single bonds linking the Oxygen and the Carbon atoms, and double bonds linking the Carbon atoms. 8 electrons are distributed around the Oxygen atoms, satisfying the 'octet rule'.

Step by step solution

01

Calculation of Total Valence Electrons

Calculate the total number of valence electrons. This is computed by adding the number of valence electrons from each atom. Since C (Carbon) has 4 valence electrons and there are 3 carbon atoms, the total valence electrons from carbon is \(4*3 = 12\). On the other hand, O (Oxygen) has 6 valence electrons and there are 2 oxygen atoms. The total valence electrons from oxygen is \(6*2 = 12\). Therefore, total valence electrons in the \(C_{3}O_{2}\) molecule is \(12 + 12 = 24\).
02

Construct the Skeletal Structure

Determine the skeletal structure of the molecule. In \(C_{3}O_{2}\), the carbon (C) atoms are usually in the center because oxygen (O) is more electronegative. Hence, the skeletal structure will look like O-C-C-C-O.
03

Distribute the Remaining Electrons

Start by placing two electrons (as a bond) between each pair of bonded atoms. Then add lone pairs of electrons around each atom until each atom (except Hydrogen) is surrounded by 8 electrons or until you have used all the electrons. Remember, each bond represents two electrons. After placing the first 8 electrons (4 bonds of 2 electrons each), 16 electrons are left. Place these around the oxygen atoms (8 electrons around each oxygen). Now, each atom is surrounded by 8 electrons, satisfying the octet rule.
04

Verify and Confirm Structure

Double-check the structure to confirm that the octet rule is obeyed for every atom (except Hydrogen) and that all the valence electrons have been used. If the octet rule has been violated, adjust the structure by converting lone pairs to bonding pairs for atoms violating the rule. For \(C_{3}O_{2}\), no such adjustments are necessary because the octet rule is obeyed for every atom and all 24 valence electrons are used. Hence, the Lewis structure is correct as it is.

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

Use the VSEPR theory to predict the shapes of the anions (a) \(\mathrm{ClO}_{4}^{-} ;\) (b) \(\mathrm{S}_{2} \mathrm{O}_{3}^{2-}\left(\text { that is, } \mathrm{SSO}_{3}^{2-}\right) ;\) (c) \(\mathrm{PF}_{6}^{-}\); (d) I \(_{3}^{-}\).

Draw Lewis structures for the following species, indicating formal charges and resonance where applicable: (a) \(\mathrm{HCO}_{2}=\) (b) \(\mathrm{HCO}_{3}^{-}\) (c) \(\mathrm{FSO}_{3}^{-}\) (d) \(\mathrm{N}_{2} \mathrm{O}_{3}^{2-}\) (the nitrogen atoms are joined centrally with one oxygen atom on one \(\mathrm{N}\) and two on the other)

Which molecule is nonpolar? (a) \(\mathrm{SO}_{3} ;\) (b) \(\mathrm{CH}_{2} \mathrm{Cl}_{2}\); (c) \(\mathrm{NH}_{3} ;\) (d) FNO.

One possibility for the electron-group geometry for seven electron groups is pentagonal-bipyramidal, as found in the IF \(_{7}\) molecule. Write the VSEPR notation for this molecule. Sketch the structure of the molecule, labeling all the bond angles.

Explain why it is not necessary to find the Lewis structure with the smallest formal charges to make a successful prediction of molecular geometry in the VSEPR theory. For example, write Lewis structures for \(S O_{2}\) having different formal charges, and predict the molecular geometry based on these structures.
See all solutions

Recommended explanations on Chemistry Textbooks

Making Measurements

Read Explanation

Kinetics

Read Explanation

Inorganic Chemistry

Read Explanation

Organic Chemistry

Read Explanation

Physical 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