Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 7: Problem 8

Radioastronomers have detected the isoformyl ion, \(\mathrm{HCO}^{\top}\), in outer space. Write the Lewis structure for this ion.

Short Answer

Expert verified
Answer: The Lewis structure for the isoformyl ion, HCO+, is H-C=O with two lone pairs on the oxygen atom.

Step by step solution

01

Count the valence electrons

First, we have to determine the total number of valence electrons in the isoformyl ion, HCO+: Hydrogen (H) has 1 valence electron, Carbon (C) has 4 valence electrons, Oxygen (O) has 6 valence electrons, and there is a +1 charge, which means we have to subtract 1 electron. Adding all the electrons, we have: \(1 + 4 + 6 - 1 = 10\) valence electrons.
02

Arrange the atoms

We arrange the atoms and create the basic molecule structure. Here, carbon is typically the central atom due to its affinity for bonding, and we place hydrogen and oxygen atoms around the central carbon atom: H-C-O.
03

Distribute the valence electrons

Now we need to share the valence electrons among the atoms to satisfy their octet (or duet for hydrogen). Starting with the H-C bond, assign 2 electrons to create a single bond. Assign remaining electrons to the oxygen atom to complete its octet: - Add 4 electrons to the O (two lone pairs) to give the oxygen six electrons. - Next, share 2 electrons between the C and O atom to create a double bond.
04

Check extra electrons

Check if there are any extra electrons left to distribute. In this case, we've used all 10 valence electrons. Now you have the Lewis structure for the isoformyl ion, \(\mathrm{HCO}^{\top}\): H-C=O with two lone pairs on the oxygen atom.

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

Consider the following molecules: \(\mathrm{SiH}_{4}, \mathrm{PH}_{3}, \mathrm{H}_{2} \mathrm{~S}\). In each case, a central atom is surrounded by four electron pairs. In which of these molecules would you expect the bond angle to be less than \(109.5^{\circ}\) ? Explain your reasoning.

Phosphoryl chloride, \(\mathrm{POCl}_{3}\), has the skeleton structure Write (a) a Lewis structure for \(\mathrm{POCl}_{3}\) following the octet rule. Calculate the formal charges in this structure. (b) a Lewis structure in which all the formal charges are zero. (The octet rule need not be followed.)

In which of the following molecules does the sulfur have an expanded octet? For those that do, write the Lewis structure. (a) \(\mathrm{SO}_{2}\) (b) \(\mathrm{SF}_{4}\) (c) \(\mathrm{SO}_{2} \mathrm{Cl}_{2}\) (d) \(\mathrm{SF}_{6}\)

The Lewis structure for hydrazoic acid may be written as (a) Draw two other resonance forms for this molecule. (b) Is

Borazine, \(\mathrm{B}_{3} \mathrm{~N}_{3} \mathrm{H}_{6}\), has the skeleton Draw the resonance forms of the molecule.
See all solutions

Recommended explanations on Chemistry Textbooks

Nuclear Chemistry

Read Explanation

Kinetics

Read Explanation

Making Measurements

Read Explanation

Chemical Analysis

Read Explanation

The Earths Atmosphere

Read Explanation

Chemistry Branches

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