/*! 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 81 Describe how formal charges are ... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 8: Problem 81

Describe how formal charges are used to choose between possible molecular structures.

Short Answer

Expert verified
Question: Explain how to use formal charges to choose between multiple possible molecular structures in a compound. Answer: To use formal charges to choose between multiple possible molecular structures in a compound, follow these steps: 1. Understand the concept of formal charges, which are the apparent charges on individual atoms in a molecule, assuming complete electron transfer in ionic bonds and equal electron sharing in covalent bonds. 2. Calculate the formal charges for each atom in each possible molecular structure using the formula: Formal Charge = (Valence Electrons) - (Non-bonding Electrons + 1/2 Bonding Electrons) 3. Analyze the overall formal charges of the different possible structures. 4. Determine the most stable structure(s) based on the lowest overall formal charge and the presence of negative formal charges on the more electronegative elements. 5. Choose the most stable molecular structure(s) based on the analysis of formal charges and electronegativity.

Step by step solution

01

Understand the concept of formal charges

Formal charges are calculated for each atom within a molecule to help us determine the apparent charge on that atom, based on the assumption that electrons in ionic bonds are completely transferred and that electrons in covalent bonds are equally shared.
02

Calculate the formal charges for each atom in a molecule

To calculate the formal charge of an atom in a molecule, follow this formula: Formal Charge = (Valence Electrons) - (Non-bonding Electrons + 1/2 Bonding Electrons) Valence electrons are the number of electrons in the outer shell of the atom, non-bonding electrons are those that are not involved in any bond, and bonding electrons are those that are shared between atoms in a bond.
03

Analyze multiple possible molecular structures

When given multiple possible molecular structures for a compound, calculate the formal charges for each atom in each structure.
04

Determine the most stable structure(s)

The most stable structures will be those with the lowest overall formal charge, as they are the ones with the electrons distributed most evenly among the atoms. In general, a structure with formal charges closer to zero and with negative formal charges on the more electronegative elements will be more stable.
05

Use formal charges to choose between possible molecular structures

Compare the overall formal charges of the various structures, taking into account the electronegativity of the elements involved, to choose the most stable molecular structure(s).

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!

Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Calculating Formal Charges
Understanding the formal charge of an atom within a molecule is essential in predicting the molecular geometry and stability. To calculate the formal charge on an atom, use the formula:

\[ \text{Formal Charge} = (\text{Valence Electrons}) - (\text{Non-bonding Electrons} + \frac{1}{2} \times \text{Bonding Electrons}) \]

Valence electrons are the electrons in the atom's outermost shell, while non-bonding electrons are those not participating in bonds, often found in lone pairs. Bonding electrons are divided by two since they are shared with another atom. The formal charge is a hypothetical charge assuming equal sharing in covalent bonds, an important concept when distinguishing between multiple possible molecular structures. The goal is to have formal charges as close to zero as possible across the molecule, indicating an even distribution of electron density.
Valence Electrons
Valence electrons play a pivotal role in chemical bonding and molecular structure. They are the outermost electrons of an atom and are involved in forming chemical bonds. The number of valence electrons an atom has corresponds to its group number on the periodic table for Group 1 and 2 elements, and 13 through 18 for other elements, minus 10.

For example, carbon is in Group 14, so it has four valence electrons. These valence electrons are used to form covalent bonds with other atoms or exist as lone pairs on an atom. When we study formal charge and molecular stability, it's the valence electrons that we're really focusing on, as they can either be shared in bonds or exist as non-bonding pairs.
Molecular Stability
Molecular stability is influenced by the distribution of electrons across a molecule. A stable molecule typically has a full valence shell for all the atoms involved and minimal strain from bond angles or repulsion between electrons. When calculating formal charges, structures that result in formal charges closest to zero are generally more stable.

Molecular Symmetry and Stability

A symmetrical distribution of electrons leads to a more stable structure as it minimizes the repulsion between negatively charged electrons. Another crucial factor is assigning negative formal charges to more electronegative atoms and positive formal charges to less electronegative ones, which is more natural and leads to a lower energy and more stable configuration.
Electronegativity
Electronegativity refers to the ability of an atom to attract and hold onto electrons. In the context of formal charges, electronegativity helps determine the most stable molecular structure. Atoms with higher electronegativity are better at attracting electrons and will more likely hold a negative formal charge in a stable molecule.

Role in Stability

When comparing possible molecular structures, those with negative formal charges on the more electronegative atoms and positive charges on the less electronegative atoms are generally preferred. The concept of electronegativity allows chemists to predict which atoms within a molecule will remain neutral, which will gain a partial negative charge, and which may end up with a partial positive charge based on their ability to attract electrons.

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

Which is the least polar bond: \(C-S e, C=O, C 1-B r\) \(\mathrm{O}=\mathrm{O}, \mathrm{N}-\mathrm{H}, \mathrm{C}-\mathrm{H} ?\)

The heavier group 16 elements can expand their valence shell. The \(\mathrm{TeOF}_{6}^{2-}\) anion was first prepared in \(1993 .\) Draw the Lewis structure for \(\operatorname{Te} \mathrm{OF}_{6}^{2-}\).

Use average bond energies to estimate the enthalpy changes of the following reactions: a. \(\mathrm{CO}_{2}(g)+\mathrm{H}_{2}(g) \rightarrow \mathrm{H}_{2} \mathrm{O}(g)+\mathrm{CO}(g)\) b. \(\mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \rightarrow 2 \mathrm{NO}(g)\) c.\(\mathrm{C}(s)+\mathrm{CO}_{2}(g) \rightarrow 2 \mathrm{CO}(g)\)

When left at room temperature, mixtures of \(\mathrm{BF}_{3}\) and \(\mathrm{BCl}_{3}\) are found to contain significant amounts of \(\mathrm{BF}_{2} \mathrm{Cl}\) and BFCl \(_{2} .\) Using Lewis structures, explain the origin of the latter two compounds..

How do the electronegativities of the elements change across a period and down a group?
See all solutions

Recommended explanations on Chemistry Textbooks

Chemistry Branches

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Chemical Reactions

Read Explanation

Physical Chemistry

Read Explanation

Making Measurements

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.