EBK ORGANIC CHEMISTRY: PRINCIPLES AND M
EBK ORGANIC CHEMISTRY: PRINCIPLES AND M
2nd Edition
ISBN: 9780393630817
Author: KARTY
Publisher: W.W.NORTON+CO. (CC)
bartleby

Concept explainers

Types of Chemical Bonds
The attractive force which has the ability of holding various constituent elements like atoms, ions, molecules, etc. together in different chemical species is termed as a chemical bond. Chemical compounds are dependent on the strength of chemical bonds b…
Polarizability In Organic Chemistry
Polarizability refers to the ability of an atom/molecule to distort the electron cloud of neighboring species towards itself and the process of distortion of electron cloud is known as polarization.
Coordinate Covalent Bonds
A coordinate covalent bond is also known as a dative bond, which is a type of covalent bond. It is formed between two atoms, where the two electrons required to form the bond come from the same atom resulting in a semi-polar bond. The study of coordinate…
bartleby

Videos

Question
Book Icon
Chapter 1, Problem 1.46P
Interpretation Introduction

(a)

Interpretation:

Lewis structure for the given molecule is to be completed.

Concept introduction:

Lewis structures involve only valence electrons. When drawing a Lewis structure, the first step is to calculate the total number of valence electrons. For a complete Lewis structure of a molecule, the atoms must complete their normal valency by bond formation and lone pairs of electrons. Maximum number of covalent bonds formed by any neutral atom with maximum number of lone pairs is

Atom Number of bond Number of lone pairs
C 4 0
H 1 0
O 2 2
N 1 1
F 1 3

Expert Solution
Check Mark

Answer to Problem 1.46P

The complete Lewis structure for the given molecule is

EBK ORGANIC CHEMISTRY: PRINCIPLES AND M, Chapter 1, Problem 1.46P , additional homework tip 1

Explanation of Solution

The given structure is

EBK ORGANIC CHEMISTRY: PRINCIPLES AND M, Chapter 1, Problem 1.46P , additional homework tip 2

Total valence electron count for the given molecule is 54 valence electrons. In the given structure, there are, in all, 14 single bonds, which means 28 valence electrons are used. Two lone pairs are placed on the oxygen atom attached to the C and H as H-O-C and three lone pairs are placed on the fluorine atom. This means 4 + 6 = 10 more electrons are used. This leaves 16 electrons.

EBK ORGANIC CHEMISTRY: PRINCIPLES AND M, Chapter 1, Problem 1.46P , additional homework tip 3

The other oxygen atom has formed only one bond with carbon. This is converted to a double bond and two lone pairs are placed on the oxygen atom so that its octet is complete. A double bond is placed between C and N atom to complete the octet of carbon and a lone pair is placed in nitrogen to complete its octet.

A triple bond is placed between the other C and N to complete the octet of carbon and a lone pair is placed in the nitrogen to complete its octet.

EBK ORGANIC CHEMISTRY: PRINCIPLES AND M, Chapter 1, Problem 1.46P , additional homework tip 4

This structure now accounts for all 54 electrons and the octet of each atom, except hydrogen, is complete. The duet for all hydrogens is complete.

Conclusion

The Lewis structure for the given molecule is completed from total valence electron count.

Interpretation Introduction

(b)

Interpretation:

Lewis structure for the given molecule is to be completed.

Concept introduction:

Lewis structures involve only valence electrons. When drawing a Lewis structure, the first step is to calculate the total number of valence electrons. For a complete Lewis structure of a molecule, every carbon atom must form four covalent bonds whereas the hydrogen atom forms one bond.

Expert Solution
Check Mark

Answer to Problem 1.46P

The complete Lewis structure for the given molecule is

EBK ORGANIC CHEMISTRY: PRINCIPLES AND M, Chapter 1, Problem 1.46P , additional homework tip 5

Explanation of Solution

The given structure is

EBK ORGANIC CHEMISTRY: PRINCIPLES AND M, Chapter 1, Problem 1.46P , additional homework tip 6

Total valence electron count for the given molecule must be 38. In the given structure, there are, in all, 14 single bonds which means 28 valence electrons are used. A triple bond is placed between the carbon atoms outside the ring, so that the octet of both carbon atoms is complete. Alternate double bonds are placed in the ring so that each carbon atom in the ring has a complete octet.

EBK ORGANIC CHEMISTRY: PRINCIPLES AND M, Chapter 1, Problem 1.46P , additional homework tip 7

This structure now accounts for all 38 electrons and the octet of each atom, except hydrogen, is complete. The duet for all hydrogen atoms is complete.

Conclusion

The Lewis structure for the given molecule is completed from total valence electron count.

Interpretation Introduction

(c)

Interpretation:

Lewis structure for the given molecule is to be completed.

Concept introduction:

Lewis structures involve only valence electrons. When drawing a Lewis structure, the first step is to calculate the total number of valence electrons. For a complete Lewis structure of a molecule, the atoms must complete their normal valency by bond formation and lone pairs of electrons. Maximum numbers of covalent bonds formed by any neutral atom with maximum number of lone pair are

Atom Number of bond Number of lone pairs
C 4 0
H 1 0
O 2 2
N 1 1

Expert Solution
Check Mark

Answer to Problem 1.46P

The complete Lewis structure for the given molecule is

EBK ORGANIC CHEMISTRY: PRINCIPLES AND M, Chapter 1, Problem 1.46P , additional homework tip 8

Explanation of Solution

The given structure is

EBK ORGANIC CHEMISTRY: PRINCIPLES AND M, Chapter 1, Problem 1.46P , additional homework tip 9

Total valence electron count for the given molecule is 28 valence electrons. In the given structure, there are in all 9 single bonds which means 18 valence electrons are used.

The oxygen atom has formed only one bond with nitrogen. This is converted to a double bond and two lone pairs are placed on the oxygen atom so that its octet is complete. Another lone pair is placed on the nitrogen atom so that its octet is complete.

A double bond is placed between the C atoms attached to one hydrogen each. This completes the octet of both carbon atoms

EBK ORGANIC CHEMISTRY: PRINCIPLES AND M, Chapter 1, Problem 1.46P , additional homework tip 10

This structure now accounts for all the 28 electrons, and the octet of each atom, except hydrogen, is complete. The duet for all hydrogen atoms is complete.

Conclusion

The Lewis structure for the given molecule is completed from total valence electron count.

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!
Previous
Chapter 1, Problem 1.45P
Next
Chapter 1, Problem 1.47P
Students have asked these similar questions
I need help with this question.
< Complete the following structural formula for a neutral molecule by adding H atoms to complete the valence of each atom. Do not introduce any double or triple bonds. Then complete the Lewis diagram by adding any unshared electron pairs needed, so that each atom except H has a complete octet. [Review Topics] [References] Use the References to access important values if needed for this question. Br Br C—C— Write the molecular formula in the order CHX, where X stands for Cl or Br. Submit Answer The number of unshared pairs in the Lewis diagram unshared pair(s). Retry Entire Group 9 more group attempts remaining Previous Email Instructor Next Save and E
Would you help me, please? I struggled with my homework

Chapter 1 Solutions

EBK ORGANIC CHEMISTRY: PRINCIPLES AND M

Ch. 1 - Prob. 1.1PCh. 1 - Prob. 1.2PCh. 1 - Prob. 1.3PCh. 1 - Prob. 1.4PCh. 1 - Prob. 1.5PCh. 1 - Prob. 1.6PCh. 1 - Prob. 1.7PCh. 1 - Prob. 1.8PCh. 1 - Prob. 1.9PCh. 1 - Prob. 1.10P
Ch. 1 - Prob. 1.11PCh. 1 - Prob. 1.12PCh. 1 - Prob. 1.13PCh. 1 - Prob. 1.14PCh. 1 - Prob. 1.15PCh. 1 - Prob. 1.16PCh. 1 - Prob. 1.17PCh. 1 - Prob. 1.18PCh. 1 - Prob. 1.19PCh. 1 - Prob. 1.20PCh. 1 - Prob. 1.21PCh. 1 - Prob. 1.22PCh. 1 - Prob. 1.23PCh. 1 - Prob. 1.24PCh. 1 - Prob. 1.25PCh. 1 - Prob. 1.26PCh. 1 - Prob. 1.27PCh. 1 - Prob. 1.28PCh. 1 - Prob. 1.29PCh. 1 - Prob. 1.30PCh. 1 - Prob. 1.31PCh. 1 - Prob. 1.32PCh. 1 - Prob. 1.33PCh. 1 - Prob. 1.34PCh. 1 - Prob. 1.35PCh. 1 - Prob. 1.36PCh. 1 - Prob. 1.37PCh. 1 - Prob. 1.38PCh. 1 - Prob. 1.39PCh. 1 - Prob. 1.40PCh. 1 - Prob. 1.41PCh. 1 - Prob. 1.42PCh. 1 - Prob. 1.43PCh. 1 - Prob. 1.44PCh. 1 - Prob. 1.45PCh. 1 - Prob. 1.46PCh. 1 - Prob. 1.47PCh. 1 - Prob. 1.48PCh. 1 - Prob. 1.49PCh. 1 - Prob. 1.50PCh. 1 - Prob. 1.51PCh. 1 - Prob. 1.52PCh. 1 - Prob. 1.53PCh. 1 - Prob. 1.54PCh. 1 - Prob. 1.55PCh. 1 - Prob. 1.56PCh. 1 - Prob. 1.57PCh. 1 - Prob. 1.58PCh. 1 - Prob. 1.59PCh. 1 - Prob. 1.60PCh. 1 - Prob. 1.61PCh. 1 - Prob. 1.62PCh. 1 - Prob. 1.63PCh. 1 - Prob. 1.64PCh. 1 - Prob. 1.65PCh. 1 - Prob. 1.66PCh. 1 - Prob. 1.67PCh. 1 - Prob. 1.68PCh. 1 - Prob. 1.69PCh. 1 - Prob. 1.70PCh. 1 - Prob. 1.71PCh. 1 - Prob. 1.72PCh. 1 - Prob. 1.73PCh. 1 - Prob. 1.74PCh. 1 - Prob. 1.75PCh. 1 - Prob. 1.76PCh. 1 - Prob. 1.77PCh. 1 - Prob. 1.78PCh. 1 - Prob. 1.79PCh. 1 - Prob. 1.80PCh. 1 - Prob. 1.81PCh. 1 - Prob. 1.82PCh. 1 - Prob. 1.1YTCh. 1 - Prob. 1.2YTCh. 1 - Prob. 1.3YTCh. 1 - Prob. 1.4YTCh. 1 - Prob. 1.5YTCh. 1 - Prob. 1.6YTCh. 1 - Prob. 1.7YTCh. 1 - Prob. 1.8YTCh. 1 - Prob. 1.9YTCh. 1 - Prob. 1.10YTCh. 1 - Prob. 1.11YTCh. 1 - Prob. 1.12YTCh. 1 - Prob. 1.13YTCh. 1 - Prob. 1.14YTCh. 1 - Prob. 1.15YTCh. 1 - Prob. 1.16YTCh. 1 - Prob. 1.17YT
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
Introduction to General, Organic and Biochemistry
Chemistry
ISBN:9781285869759
Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher:Cengage Learning
Text book image
Organic Chemistry: A Guided Inquiry
Chemistry
ISBN:9780618974122
Author:Andrei Straumanis
Publisher:Cengage Learning
SEE MORE TEXTBOOKS
Types of bonds; Author: Edspira;https://www.youtube.com/watch?v=Jj0V01Arebk;License: Standard YouTube License, CC-BY