Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 8: Problem 77

A new compound is made that has a \(\mathrm{C}-\mathrm{O}\) bond length of $120 \mathrm{pm}$. Is this bond likely to be a single, double, or triple C-O bond?

Short Answer

Expert verified
The given bond length of the C-O bond in the new compound is \(120 \: pm\). Comparing it with the approximate bond lengths of single, double, and triple C-O bonds (\(143 \: pm\), \(123 \: pm\), and \(113 \: pm\) respectively), we find that the bond length is closest to the double C-O bond length with a difference of only \(3 \: pm\). Therefore, it is most likely that the new compound contains a double C-O bond.

Step by step solution

01

Identify the bond lengths of single, double, and triple C-O bonds

To determine the type of bond present in the new compound, we need to know the typical bond lengths of single, double, and triple C-O bonds. Here are the approximate bond lengths for each type of bond: - Single C-O bond: \(143 \: pm\) - Double C-O bond: \(123 \: pm\) - Triple C-O bond: \(113 \: pm\)
02

Compare the given bond length with the known bond lengths

The given bond length for the new compound is \(120 \: pm\). We will compare this value with the bond lengths of the single, double, and triple C-O bonds: - For the single C-O bond: \(|120 - 143| = 23 \: pm\) - For the double C-O bond: \(|120 - 123| = 3 \: pm\) - For the triple C-O bond: \(|120 - 113| = 7 \: pm\)
03

Determine the most likely bond type

To determine the most likely C-O bond in the new compound, we will look at the smallest difference between the given bond length and the known bond lengths for single, double, and triple bonds. In this case, the smallest difference is between the given bond length and the known bond length for a double C-O bond (\(3 \: pm\)). Therefore, it is most likely that the new compound contains a double C-O bond.

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

Although \(\mathrm{I}_{3}^{-}\) is a known ion, \(\mathrm{F}_{3}^{-}\) is not. \((\mathbf{a})\) Draw the Lewis structure for \(I_{3}^{-}\) (it is linear, not a triangle). (b) One of your classmates says that \(\mathrm{F}_{3}^{-}\) does not exist because \(\mathrm{F}\) is too electronegative to make bonds with another atom. Give an example that proves your classmate is wrong. (c) Another classmate says \(\mathrm{F}_{3}^{-}\) does not exist because it would violate the octet rule. Is this classmate possibly correct? (d) Yet another classmate says \(\mathrm{F}_{3}^{-}\) does not exist because \(\mathrm{F}\) is too small to make bonds to more than one atom. Is this classmate possibly correct?

Calculate the formal charge on the indicated atom in each of the following molecules or ions: (a) the central oxygen atom in \(\mathrm{O}_{3},(\mathbf{b})\) phosphorus in \(\mathrm{PF}_{6}^{-},(\mathbf{c})\) nitrogen in \(\mathrm{NO}_{2}\), (d) iodine in ICl \(_{3}\), (e) chlorine in \(\mathrm{HClO}_{4}\) (hydrogen is bonded to \(\mathrm{O}\) ).

Consider the hypothetical molecule \(\mathrm{A}-\mathrm{A}=\mathrm{A}\) with a bent shape. Are the following statements true or false? (a) This molecule cannot exist. (b) If this molecule exists, it must possess an odd electron.

(a) What is the trend in electronegativity going from left to right in a row of the periodic table? (b) How do electronegativity values generally vary going down a column in the periodic table? (c) True or false: The most easily ionizable elements are the most electronegative.

The \(\mathrm{Ti}^{2+}\) ion is isoelectronic with the Ca atom. (a) Write the electron configurations of \(\mathrm{Ti}^{2+}\) and Ca. (b) Calculate the number of unpaired electrons for Ca and for \(\mathrm{Ti}^{2+}\). (c) What charge would Ti have to be isoelectronic with \(\mathrm{Ca}^{2+}\) ?
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Reactions

Read Explanation

Chemistry Branches

Read Explanation

Making Measurements

Read Explanation

Nuclear Chemistry

Read Explanation

Organic Chemistry

Read Explanation

The Earths Atmosphere

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