/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 56 Give three examples of compounds... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 9: Problem 56

Give three examples of compounds that do not satisfy the octet rule. Write a Lewis structure for each.

Short Answer

Expert verified
Three examples of compounds that don't satisfy the octet rule are hydrogen (H2), boron trifluoride (BF3), and sulfur hexafluoride (SF6). The Lewis structures for these compounds are: H-H for H2, B single bonded to three F's for BF3, and S single bonded to six F's for SF6, respectively.

Step by step solution

01

Identifying Compounds That Don't Satisfy The Octet Rule

There are several compounds that do not follow the octet rule, they include: Hydrogen, Boron and Sulfur compounds. Hydrogen is satisfied with two electrons, Boron compounds often have six electrons in their valence shell, while Sulfur and Phosphorous can have more than eight electrons in their valence shell.
02

Drawing Lewis Structures Step 1: Hydrogen Compound

Hydrogen is the simplest element and it doesn't follow the octet rule. It only needs two electrons to fill its valence shell. An example of a hydrogen compound is \( H_2 \). The Lewis structure for \( H_2 \) is simply: H-H.
03

Drawing Lewis Structures Step 2: Boron Compound

Next, we look at Boron compounds. Boron often forms compounds in which it has fewer than 8 electrons. An example is Boron trifluoride, \( BF_3 \). The Lewis structure for \( BF_3 \) is as follows: B in the centre with three F atoms surrounding it and single bond connecting each F to the central B. There are also three lone pairs of electrons around each F atom, but none around B, resulting in only six electrons in the valence shell of Boron.
04

Drawing Lewis Structures Step 3: Sulfur Compound

Finally, let's look at Sulfur compounds. Sulfur is in period 3 of the periodic table and can have more than eight electrons. In sulfur hexafluoride, \( SF_6 \), sulfur has 12 electrons in its valence shell. The Lewis structure for \( SF_6 \) is S in the centre, surrounded by six F atoms. A single bond connects each F to the central S, resulting in a total of 12 electrons in the valence shell of Sulfur.

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.

Over 30 million students worldwide already upgrade their learning with 91影视!

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 only known argon-containing compound is HArF, which was prepared in \(2000 .\) Draw a Lewis structure of the compound.

An ionic bond is formed between a cation \(\mathrm{A}^{+}\) and an anion \(\mathrm{B}^{-}\). How would the energy of the ionic bond [see Equation (9.2)\(]\) be affected by the following changes? (a) doubling the radius of \(\mathrm{A}^{+},\) (b) tripling the charge on \(A^{+},(\mathrm{c})\) doubling the charges on \(\mathrm{A}^{+}\) and \(\mathrm{B}^{-},\) (d) decreasing the radii of \(\mathrm{A}^{+}\) and \(\mathrm{B}^{-}\) to half their original values.

Without referring to Figure 9.1 , write Lewis dot symbols for atoms of the following elements: (a) Be, (b) \(\mathrm{K},\) (c) \(\mathrm{Ca},\) (d) \(\mathrm{Ga},\) (e) \(\mathrm{O},\) (f) \(\mathrm{Br},(\mathrm{g}) \mathrm{N},(\mathrm{h}) \mathrm{I},\) (i) \(\mathrm{As}\), (j) F.

Specify which compound in the following pairs of ionic compounds has the higher lattice energy: (a) \(\mathrm{KCl}\) or \(\mathrm{MgO},\) (b) \(\mathrm{LiF}\) or \(\mathrm{LiBr}\) (c) \(\mathrm{Mg}_{3} \mathrm{~N}_{2}\) or \(\mathrm{NaCl}\). Explain your choice.

Distinguish among single, double, and triple bonds in a molecule, and give an example of each.
See all solutions

Recommended explanations on Chemistry Textbooks

Kinetics

Read Explanation

Chemistry Branches

Read Explanation

Chemical Analysis

Read Explanation

Physical Chemistry

Read Explanation

Nuclear 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.