General Chemistry
General Chemistry
7th Edition
ISBN: 9780073402758
Author: Chang, Raymond/ Goldsby
Publisher: McGraw-Hill College
bartleby

Concept explainers

bartleby

Videos

Question
Book Icon
Chapter 10, Problem 10.36QP

(a)

Interpretation Introduction

Interpretation:

The hybrid orbitals of the carbon atoms in the given molecule have to be found.

Concept Introduction:

Hybridization is the phenomenon of intermixing of the atomic orbitals of different energy that results in the formation of new set of hybrid orbitals which have equivalent energies.  The various types of atomic orbitals are: s, p, and d orbitals. Types of hybridization that involves s, p and d orbitals are sp,sp2,sp3,sp3d,sp3d2,sp3d3.

The valency of carbon atom is four, which means it can make four bonding with the other atoms.

There are two major types of bonding:

σ-bondformsbyhead-to-headoveralpofatomicorbitals.π-bondformsbylateraloveralpofatomicorbitals

  • If the carbon atom is bonded with four σ-bonds, then it is sp3 hybridized carbon atom.
  • If the carbon atom is bonded with three σ-sigmabond and one π-bond, then it is sp2hybridized carbon atom.
  • If the carbon atom is bonded with two σ-bond and two π-bonds, then it is sphybridized carbon atom.

(a)

Expert Solution
Check Mark

Explanation of Solution

In the given molecule, the hybrid orbitals of each carbon atom are shown below:

General Chemistry, Chapter 10, Problem 10.36QP , additional homework tip  1

(b)

Interpretation Introduction

Interpretation:

The hybrid orbitals of the carbon atoms in the given molecule have to be found.

Concept Introduction:

Hybridization is the phenomenon of intermixing of the atomic orbitals of different energy that results in the formation of a new set of hybrid orbitals which have equivalent energies. The various types of atomic orbitals are: s, p, and d orbitals. Types of hybridization that involves s, p and d orbitals are sp,sp2,sp3,sp3d,sp3d2,sp3d3.

The valency of carbon atom is four, which means it can make four bonding with the other atoms.

There are two major types of bonding:

σ-bondformsbyhead-to-headoveralpofatomicorbitals.π-bondformsbylateraloveralpofatomicorbitals

  • If the carbon atom is bonded with four σ-bonds, then it is sp3 hybridized carbon atom. 
  • If the carbon atom is bonded with three σ-sigmabond and one π-bond, then it is sp2hybridized carbon atom.
  • If the carbon atom is bonded with two σ-bond and two π-bonds, then it is sphybridized carbon atom.

(b)

Expert Solution
Check Mark

Explanation of Solution

In the given molecule, the hybrid orbitals of each carbon atom are shown below:

General Chemistry, Chapter 10, Problem 10.36QP , additional homework tip  2

(c)

Interpretation Introduction

Interpretation:

The hybrid orbitals of the carbon atoms in the given molecule have to be found.

Concept Introduction:

Hybridization is the phenomenon of intermixing of the atomic orbitals of different energy that results in the formation of new set of hybrid orbitals which have equivalent energies.  The various types of atomic orbitals are: s, p, and d orbitals.  Types of hybridization that involves s, p and d orbitals are sp,sp2,sp3,sp3d,sp3d2,sp3d3.

The valency of carbon atom is four, which means it can make four bonding with the other atoms.

There are two major types of bonding:

σ-bondformsbyhead-to-headoveralpofatomicorbitals.π-bondformsbylateraloveralpofatomicorbitals

  • If the carbon atom is bonded with four σ-bonds, then it is sp3 hybridized carbon atom. 
  • If the carbon atom is bonded with three σ-sigmabond and one π-bond, then it is sp2hybridized carbon atom.
  • If the carbon atom is bonded with two σ-bond and two π-bonds, then it is sphybridized carbon atom.

(c)

Expert Solution
Check Mark

Explanation of Solution

In the given molecule, the hybrid orbitals of each carbon atom are shown below:

General Chemistry, Chapter 10, Problem 10.36QP , additional homework tip  3

(d)

Interpretation Introduction

Interpretation:

The hybrid orbitals of the carbon atoms in the given molecule have to be found.

Concept Introduction:

Hybridization is the phenomenon of intermixing of the atomic orbitals of different energy that results in the formation of a new set of hybrid orbitals which have equivalent energies. The various types of atomic orbitals are: s, p, and d orbitals. Types of hybridization that involves s, p and d orbitals are sp,sp2,sp3,sp3d,sp3d2,sp3d3.

The valency of carbon atom is four, which means it can make four bonding with the other atoms.

There are two major types of bonding:

σ-bondformsbyhead-to-headoveralpofatomicorbitals.π-bondformsbylateraloveralpofatomicorbitals

  • If the carbon atom is bonded with four σ-bonds, then it is sp3 hybridized carbon atom. 
  • If the carbon atom is bonded with three σ-sigmabond and one π-bond, then it is sp2hybridized carbon atom.
  • If the carbon atom is bonded with two σ-bond and two π-bonds, then it is sphybridized carbon atom.

(d)

Expert Solution
Check Mark

Explanation of Solution

In the given molecule, the hybrid orbitals of each carbon atom are shown below:

General Chemistry, Chapter 10, Problem 10.36QP , additional homework tip  4

(e)

Interpretation Introduction

Interpretation:

The hybrid orbitals of the carbon atoms in the given molecule have to be found.

Concept Introduction:

Hybridization is the phenomenon of intermixing of the atomic orbitals of different energy that results in the formation of a new set of hybrid orbitals which have equivalent energies. The various types of atomic orbitals are: s, p, and d orbitals. Types of hybridization that involves s, p and d orbitals are sp,sp2,sp3,sp3d,sp3d2,sp3d3.

The valency of carbon atom is four, which means it can make four bonding with the other atoms.

There are two major types of bonding:

σ-bondformsbyhead-to-headoveralpofatomicorbitals.π-bondformsbylateraloveralpofatomicorbitals

  • If the carbon atom is bonded with four σ-bonds, then it is sp3 hybridized carbon atom. 
  • If the carbon atom is bonded with three σ-sigmabond and one π-bond, then it is sp2hybridized carbon atom.
  • If the carbon atom is bonded with two σ-bond and two π-bonds, then it is sphybridized carbon atom.

(e)

Expert Solution
Check Mark

Explanation of Solution

In the given molecule, the hybrid orbitals of each carbon atom are shown below:

General Chemistry, Chapter 10, Problem 10.36QP , additional homework tip  5

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!

Chapter 10 Solutions

General Chemistry

Ch. 10.6 - Prob. 1RCCh. 10.6 - Prob. 2RCCh. 10.6 - Prob. 1PECh. 10 - Prob. 10.1QPCh. 10 - Prob. 10.2QPCh. 10 - 10.3 How many atoms arc directly bonded to the...Ch. 10 - 10.4 Discuss the basic features of the VSEPR...Ch. 10 - 10.5 In the trigonal bipyramidal arrangement, why...Ch. 10 - 10.6 The geometry of CH4 could be square planar,...Ch. 10 - Prob. 10.7QPCh. 10 - Prob. 10.8QPCh. 10 - Prob. 10.9QPCh. 10 - Prob. 10.10QPCh. 10 - 10.11 Describe the geometry around each of the...Ch. 10 - 10.12 Which of these species are tetrahedral?...Ch. 10 - 10.13 Define dipole moment. What are the units and...Ch. 10 - 10.14 What is the relationship between the dipole...Ch. 10 - 10.15 Explain why an atom cannot have a permanent...Ch. 10 - 10.16 The bonds in beryllium hydride (BeH2)...Ch. 10 - 10.17 Referring to Table 10.3. arrange the...Ch. 10 - 10.18 The dipole moments of the hydrogen halides...Ch. 10 - 10.19 List these molecules in order of increasing...Ch. 10 - 10.20 Docs the molecule OCS have a higher or lower...Ch. 10 - 10.21 Which of these molecules has a higher dipole...Ch. 10 - 10.22 Arrange these compounds in order of...Ch. 10 - 10.23 What is valence bond theory? How does it...Ch. 10 - 10.24 Use valence bond theory to explain the...Ch. 10 - 10.25Draw a potential energy curve for the bond...Ch. 10 - 10.26 What is the hybridization of atomic...Ch. 10 - 10.27 How does a hybrid orbital differ from a pure...Ch. 10 - 10.28 What is the angle between these two hybrid...Ch. 10 - 10.29 How would you distinguish between a sigma...Ch. 10 - 10.30 Which of these pairs of atomic orbitals of...Ch. 10 - 10.31 The following potential energy curve...Ch. 10 - 10.32 What is the hybridization state of Si in...Ch. 10 - 10.33 Describe the change in hybridization (if...Ch. 10 - 10.34 Consider the reaction Describe the changes...Ch. 10 - 10.35 What hybrid orbitals are used by nitrogen...Ch. 10 - Prob. 10.36QPCh. 10 - 10.37 Specify which hybrid orbitals are used by...Ch. 10 - 10.38 What is the hybridization state of the...Ch. 10 - 10.39 The allene molecule H2C=C=CH2 is linear (the...Ch. 10 - 10.40 Describe the hybridization of phosphorus in...Ch. 10 - 10.41 How many sigma bonds and pi bonds are there...Ch. 10 - 10.42 How many pi bonds and sigma bonds are there...Ch. 10 - 10.43 Give the formula of a cation comprised of...Ch. 10 - 10.44 Give the formula of an anion comprised of...Ch. 10 - 10.45 What is molecular orbital theory? How does...Ch. 10 - 10.46 Define these terms: bonding molecular...Ch. 10 - 10.47 Sketch the shapes of these molecular...Ch. 10 - 10.48 Explain the significance of bond order. Can...Ch. 10 - 10.49 Explain in molecular orbital terms the...Ch. 10 - Prob. 10.50QPCh. 10 - Prob. 10.51QPCh. 10 - Prob. 10.52QPCh. 10 - Prob. 10.53QPCh. 10 - Prob. 10.54QPCh. 10 - Prob. 10.55QPCh. 10 - 10.56 Compare the Lewis and molecular orbital...Ch. 10 - Prob. 10.57QPCh. 10 - 10.58 Compare the relative stability of these...Ch. 10 - Prob. 10.59QPCh. 10 - Prob. 10.60QPCh. 10 - Prob. 10.61QPCh. 10 - Prob. 10.62QPCh. 10 - Prob. 10.63QPCh. 10 - Prob. 10.64QPCh. 10 - Prob. 10.65QPCh. 10 - Prob. 10.66QPCh. 10 - Prob. 10.67QPCh. 10 - Prob. 10.68QPCh. 10 - 10.69 Draw Lewis structures and give the other...Ch. 10 - Prob. 10.70QPCh. 10 - Prob. 10.71QPCh. 10 - Prob. 10.72QPCh. 10 - Prob. 10.73QPCh. 10 - Prob. 10.74QPCh. 10 - Prob. 10.75QPCh. 10 - Prob. 10.76QPCh. 10 - Prob. 10.77QPCh. 10 - Prob. 10.78QPCh. 10 - Prob. 10.79QPCh. 10 - Prob. 10.80QPCh. 10 - Prob. 10.81QPCh. 10 - Prob. 10.82QPCh. 10 - Prob. 10.83QPCh. 10 - 10.84 The ionic character of the bond in a...Ch. 10 - Prob. 10.85QPCh. 10 - 10.86 Aluminum trichloride (AlCl3) is an...Ch. 10 - Prob. 10.87QPCh. 10 - Prob. 10.88QPCh. 10 - 10.90 Progesterone is a hormone responsible for...Ch. 10 - Prob. 10.91SPCh. 10 - Prob. 10.92SPCh. 10 - Prob. 10.93SPCh. 10 - 10.94 The molecule benzyne (C6H4) is a very...Ch. 10 - Prob. 10.95SPCh. 10 - 10.96 As mentioned in the chapter, the Lewis...Ch. 10 - Prob. 10.97SPCh. 10 - Prob. 10.98SPCh. 10 - Prob. 10.99SPCh. 10 - Prob. 10.100SPCh. 10 - Prob. 10.101SPCh. 10 - Prob. 10.102SP
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.
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