Organic Chemistry Study Guide and Solutions
Organic Chemistry Study Guide and Solutions
6th Edition
ISBN: 9781936221868
Author: Marc Loudon, Jim Parise
Publisher: W. H. Freeman
bartleby

Concept explainers

bartleby

Videos

Question
Book Icon
Chapter 1, Problem 1.3P
Interpretation Introduction

(a)

Interpretation:

The Lewis structure for HCCl3 is to be drawn with unshared pairs and the formal charges.

Concept introduction:

The Lewis structure shows the connectivity between atoms by identifying the lone pairs of electrons in a compound. Lewis structures are also called Lewis dot structures. The valence electrons around an atom are shown by dots. Bonds between atoms are shown by lines and the lone pair of electrons is shown by a pair of dots.

The rules to draw Lewis structure are given as,

• Determine the electronegativity and the number of valence electrons contributed by each atom.

• Generally, the lowest electronegativity atom is the central atom.

• Write the skeleton structure of the molecule.

• Two valence electrons are used to form a bond in skeleton structure between the central and outer atoms.

• Satisfy the octets of each atom by distributing the valence electrons as nonbonding electrons. It is better to start with the outermost atoms.

Interpretation Introduction

(b)

Interpretation:

The Lewis structure for NH3 is to be drawn is to be drawn with unshared pairs and the formal charges.

Concept introduction:

The Lewis structure shows the connectivity between atoms by identifying the lone pairs of electrons in a compound. Lewis structures are also called Lewis dot structures. The valence electrons around an atom are shown by dots. Bonds between atoms are shown by lines and the lone pair of electrons is shown by a pair of dots.

The rules to draw Lewis structure are given as,

• Determine the electronegativity and the number of valence electrons contributed by each atom.

• Generally, the lowest electronegativity atom is the central atom.

• Write the skeleton structure of the molecule.

• Two valence electrons are used to form a bond in skeleton structure between the central and outer atoms.

• Satisfy the octets of each atom by distributing the valence electrons as nonbonding electrons. It is better to start with the outermost atoms.

Interpretation Introduction

(c)

Interpretation:

The Lewis structure for [NH4]+ is to be drawn is to be drawn with unshared pairs and the formal charges.

Concept introduction:

The Lewis structure shows the connectivity between atoms by identifying the lone pairs of electrons in a compound. Lewis structures are also called Lewis dot structures. The valence electrons around an atom are shown by dots. Bonds between atoms are shown by lines and the lone pair of electrons is shown by a pair of dots.

The rules to draw Lewis structure are given as,

• Determine the electronegativity and the number of valence electrons contributed by each atom.

• Generally, the lowest electronegativity atom is the central atom.

• Write the skeleton structure of the molecule.

• Two valence electrons are used to form a bond in skeleton structure between the central and outer atoms.

• Satisfy the octets of each atom by distributing the valence electrons as nonbonding electrons. It is better to start with the outermost atoms.

Interpretation Introduction

(d)

Interpretation:

The Lewis structure for [H3O]+ is to be drawn is to be drawn with unshared pairs and the formal charges.

Concept introduction:

The Lewis structure shows the connectivity between atoms by identifying the lone pairs of electrons in a compound. Lewis structures are also called Lewis dot structures. The valence electrons around an atom are shown by dots. Bonds between atoms are shown by lines and the lone pair of electrons is shown by a pair of dots.

The rules to draw Lewis structure are given as,

• Determine the electronegativity and the number of valence electrons contributed by each atom.

• Generally, the lowest electronegativity atom is the central atom.

• Write the skeleton structure of the molecule.

• Two valence electrons are used to form a bond in skeleton structure between the central and outer atoms.

• Satisfy the octets of each atom by distributing the valence electrons as nonbonding electrons. It is better to start with the outermost atoms.

Blurred answer
Students have asked these similar questions
Cyanogen (CN)2 is known as pseodohalogen because it has some properties like halogens. It is composed of two CN’s joined together.(i) Draw the Lewis structure for all the possible combination for (CN)2.(ii) Calculate the formal charge and determine which one of the structures that you have drawn is most stable.(iii) For the stable structure, determine the geometry around the two central atoms.(iv) For the stable structure, draw the dipole arrows for the bonds.(v) Base on the stable structure, determine the polarity of molecule and state your reason.
Write the Lewis structures for the following, and include resonance structures where appropriate. Indicate which has the strongest carbon-oxygen bond.(a) CO2(b) CO
Write Lewis structures for these compounds. Show all valence electrons. None of them contains a ring of atoms. (a) Hydrogen peroxide, H2O2 (b) Hydrazine, N2H4 (c) Methanol, CH3OH
Knowledge Booster
Background pattern image
Chemistry
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
SEE MORE QUESTIONS
Recommended textbooks for you
Text book image
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Text book image
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Text book image
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Text book image
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Text book image
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Text book image
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY
Stoichiometry - Chemistry for Massive Creatures: Crash Course Chemistry #6; Author: Crash Course;https://www.youtube.com/watch?v=UL1jmJaUkaQ;License: Standard YouTube License, CC-BY
Bonding (Ionic, Covalent & Metallic) - GCSE Chemistry; Author: Science Shorts;https://www.youtube.com/watch?v=p9MA6Od-zBA;License: Standard YouTube License, CC-BY
General Chemistry 1A. Lecture 12. Two Theories of Bonding.; Author: UCI Open;https://www.youtube.com/watch?v=dLTlL9Z1bh0;License: CC-BY