Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 10: Problem 110

A few years ago the synthesis of a salt containing the \(\mathrm{N}_{5}^{+}\) ion was reported. What is the likely shape of this ion-linear, bent, zigzag, tetrahedral, seesaw, or square-planar? Explain your choice.

Short Answer

Expert verified
The likely shape of the \(\mathrm{N}_{5}^{+}\) ion is tetrahedral.

Step by step solution

01

Determine the Lewis Structure

We first determine the Lewis structure of the \(\mathrm{N}_{5}^{+}\) ion. The Lewis structure is a simple depiction of covalent bonds and valence electrons in a molecule. With the N5+ ion, nitrogen has 5 valence electrons and it forms bonds with other 4 nitrogen atoms. This leaves it with a positive charge due to loss of an electron during bond formation.
02

Identify the central atom

From the Lewis structure, identify the central atom. Here, the central atom is Nitrogen.
03

Count valence electron pairs

Count the atoms attached to the central atom and lone pairs. The central Nitrogen is surrounded by four other Nitrogens and has no lone pairs.
04

Applying VSEPR theory

Use the VSEPR theory concept which states that electron pairs around an atom arrange themselves in such a way to minimize repulsion. Here, With 4 bonding pairs of electrons around the central nitrogen, it leads to a tetrahedral arrangement to minimize the repulsion between these electron pairs.
05

Predict the shape

Based on the VSEPR theory, the predicted shape of this molecule is tetrahedral as it minimizes the repulsion between the bonding pairs of electrons.

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

Describe the carbon-to-sulfur bond in \(\mathrm{H}_{2} \mathrm{CSF}_{4}\). That is, is it most likely a single, double, or triple bond?

Draw a plausible Lewis structure for the following series of molecules and ions: \((a) \operatorname{SiF}_{6}^{2-} ;\) (b) \(\mathrm{PF}_{5} ;\) (c) \(\mathrm{SF}_{4}\); (d) \(\mathrm{XeF}_{4}\). Describe the electron group geometry and molecular structure of these species.

Comment on the similarities and differences in the molecular structure of the following four-atom species: \(\mathrm{NO}_{3}^{-}, \mathrm{CO}_{3}^{2-}, \mathrm{SO}_{3}^{2-},\) and \(\mathrm{ClO}_{3}^{-}\).

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.

Construct a concept map illustrating the connections between Lewis dot structures, the shapes of molecules, and polarity.
See all solutions

Recommended explanations on Chemistry Textbooks

The Earths Atmosphere

Read Explanation

Physical Chemistry

Read Explanation

Organic Chemistry

Read Explanation

Chemistry Branches

Read Explanation

Inorganic Chemistry

Read Explanation

Ionic and Molecular Compounds

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