Chemistry
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
bartleby

Concept explainers

bartleby

Videos

Textbook Question
Book Icon
Chapter 9, Problem 34E

For each of the following molecules or ions that contain sulfur, write the Lewis structure(s), predict the molecular structure (including bond angles), and give the expected hybrid orbitals for sulfur.

a. SO2

b. SO3

c. Chapter 9, Problem 34E, For each of the following molecules or ions that contain sulfur, write the Lewis structure(s), , example  1

d. Chapter 9, Problem 34E, For each of the following molecules or ions that contain sulfur, write the Lewis structure(s), , example  2

e. SO32−

f. SO42−

g. SF2

h. SF4

i. SF6

j. F3S—SF

k. SF5+

(a)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The Lewis dot structure, molecular geometry, bond angles of the given molecules and expected hybrid orbitals for sulfur is to be stated.

Concept introduction: When the atomic orbitals overlap with each other in the region where density of electrons is high, then molecular orbitals are formed. Overlap of the atomic orbitals determines the efficiency of the interaction between the atomic orbitals.

Energy of bonding molecular orbitals is less than the nonbonding molecular orbitals.

To determine: The Lewis dot structure, molecular geometry, bond angles and expected hybrid orbitals for sulfur in SO2 .

Explanation of Solution

Explanation

There are six valence electrons on each sulfur and oxygen atom. Two oxygen atoms are bonded to sulfur atom. Therefore, the total valence electrons are 6+6×2=18 . Between each sulfur and oxygen, there is a sigma and pi bond. There is a lone pair of electron on sulfur which pushes the oxygen atom down.

Therefore the geometry is bent. The bond angle is less than 120ο . The sulfur utilizes one s and two p orbitals to give hybridization sp2 .

The Lewis structure of SO2 is,

Chemistry, Chapter 9, Problem 34E , additional homework tip  1

Figure 1

(b)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The Lewis dot structure, molecular geometry, bond angles of the given molecules and expected hybrid orbitals for sulfur is to be stated.

Concept introduction: When the atomic orbitals overlap with each other in the region where density of electrons is high, then molecular orbitals are formed. Overlap of the atomic orbitals determines the efficiency of the interaction between the atomic orbitals.

Energy of bonding molecular orbitals is less than the nonbonding molecular orbitals.

To determine: The Lewis dot structure, molecular geometry, bond angles and expected hybrid orbitals for sulfur in SO3 .

Explanation of Solution

Explanation

There are six valence electrons on sulfur and each oxygen atom. Two oxygen atoms are attached to sulfur, therefore, the total number of valence electrons is 6+6×3=24 . There are three bond pairs of electrons surrounding the sulfur atom. The oxygen that is double bonded with sulfur has two lone pair and the other two oxygen atoms have three lone pairs of electrons.

The molecule has trigonal planar geometry with bond angle 120ο . The sulfur atom is doubly bonded to each oxygen, which means one s and two p orbitals are hybridized hence the hybridization of sulfur is sp2 . The Lewis structure of SO3 is,

Chemistry, Chapter 9, Problem 34E , additional homework tip  2

Figure 2

(c)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The Lewis dot structure, molecular geometry, bond angles of the given molecules and expected hybrid orbitals for sulfur is to be stated.

Concept introduction: When the atomic orbitals overlap with each other in the region where density of electrons is high, then molecular orbitals are formed. Overlap of the atomic orbitals determines the efficiency of the interaction between the atomic orbitals.

Energy of bonding molecular orbitals is less than the nonbonding molecular orbitals.

To determine: The Lewis dot structure, molecular geometry, bond angles and expected hybrid orbitals for sulfur in S2O32 .

Explanation of Solution

Explanation

There are six valence electrons on sulfur and each oxygen atom. Three oxygen atoms and one sulfur atom is attached to central sulfur atom and charge on the molecule is 2 , therefore, the total number of valence electrons is 2×6+6×3+2=32 . The sulfur is bonded to one sulfur atom and one of the oxygen atoms by pi bond and other two oxygen atoms are bonded by sigma bond.

By bonding in this way, they complete their octet. The molecular structure is tetrahedral with bond angle approximately equal to 109.5ο . The hybridization of central sulfur atom is sp3 . The Lewis structure of S2O32 is,

Chemistry, Chapter 9, Problem 34E , additional homework tip  3

Figure 3

(d)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The Lewis dot structure, molecular geometry, bond angles of the given molecules and expected hybrid orbitals for sulfur is to be stated.

Concept introduction: When the atomic orbitals overlap with each other in the region where density of electrons is high, then molecular orbitals are formed. Overlap of the atomic orbitals determines the efficiency of the interaction between the atomic orbitals.

Energy of bonding molecular orbitals is less than the nonbonding molecular orbitals.

To determine: The Lewis dot structure, molecular geometry, bond angles and expected hybrid orbitals for sulfur in S2O82 .

Explanation of Solution

Explanation

There are six valence electrons on sulfur and each oxygen atom. There are eight oxygen atoms and two sulfur atoms are present in the molecule and charge on the molecule is 2 , therefore, the total number of valence electrons is 2×6+6×8+2=62 . Each sulfur is bonded to four oxygen atoms, two oxygen atoms are double bonded while two are single bonded.

The two oxygen atoms in the centre are bonded by single bond. By bonding in this way, they complete their octet. The molecular structure is tetrahedral with bond angle approximately equal to 109.5ο . The hybridization of both sulfur atom is sp3 . The Lewis structure of S2O82 is,

Chemistry, Chapter 9, Problem 34E , additional homework tip  4

Figure 4

(e)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The Lewis dot structure, molecular geometry, bond angles of the given molecules and expected hybrid orbitals for sulfur is to be stated.

Concept introduction: When the atomic orbitals overlap with each other in the region where density of electrons is high, then molecular orbitals are formed. Overlap of the atomic orbitals determines the efficiency of the interaction between the atomic orbitals.

Energy of bonding molecular orbitals is less than the nonbonding molecular orbitals.

To determine: The Lewis dot structure, molecular geometry, bond angles and expected hybrid orbitals for sulfur in SO32 .

Explanation of Solution

Explanation

There are six valence electrons on sulfur and each oxygen atom. Three oxygen atoms and one sulfur atom present in the molecule and charge on the molecule is 2 , therefore, the total number of valence electrons is 6+6×3+2=26 . The sulfur is bonded to three oxygen atoms.

One oxygen atom is single bonded with sulfur and one is joined by pi bond. By bonding in this way, they complete their octet. The molecular structure is trigonal pyramidal with bond angle approximately equal to 109.5ο . The hybridization of sulfur atom is sp3 . The Lewis structure of SO32 is,

Chemistry, Chapter 9, Problem 34E , additional homework tip  5

Figure 5

(f)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The Lewis dot structure, molecular geometry, bond angles of the given molecules and expected hybrid orbitals for sulfur is to be stated.

Concept introduction: When the atomic orbitals overlap with each other in the region where density of electrons is high, then molecular orbitals are formed. Overlap of the atomic orbitals determines the efficiency of the interaction between the atomic orbitals.

Energy of bonding molecular orbitals is less than the nonbonding molecular orbitals.

To determine: The Lewis dot structure, molecular geometry, bond angles and expected hybrid orbitals for sulfur in SO42 .

Explanation of Solution

Explanation

There are six valence electrons on sulfur and each oxygen atom. Four oxygen atoms and one sulfur atom is present in the molecule and charge on the molecule is 2 , therefore, the total number of valence electrons is 6+6×4+2=32 . The sulfur is bonded to four oxygen atoms.

Two oxygen atoms are single bonded with sulfur and two joined by pi bond. By bonding in this way, they complete their octet. The molecular structure is tetrahedral with bond angle approximately equal to 109.5ο . The sulfur has no lone pairs of electrons and is attached four oxygen atoms, thus the hybridization of sulfur atom is sp3 . The Lewis structure of SO42 is,

Chemistry, Chapter 9, Problem 34E , additional homework tip  6

Figure 6

(g)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The Lewis dot structure, molecular geometry, bond angles of the given molecules and expected hybrid orbitals for sulfur is to be stated.

Concept introduction: When the atomic orbitals overlap with each other in the region where density of electrons is high, then molecular orbitals are formed. Overlap of the atomic orbitals determines the efficiency of the interaction between the atomic orbitals.

Energy of bonding molecular orbitals is less than the nonbonding molecular orbitals.

To determine: The Lewis dot structure, molecular geometry, bond angles and expected hybrid orbitals for sulfur in SF2 .

Explanation of Solution

Explanation

There are six valence electrons on sulfur and seven valence electrons on each fluorine atom. Two fluorine atoms and one sulfur atom is present in the molecule, therefore, the total number of valence electrons is 6+7×2=20 .

The sulfur is bonded to two fluorine atoms by sigma bond. By bonding in this way, they complete their octet. The molecular structure is bent due to presence of lone pairs of electrons on sulfur. The bond angle is less than 109.5ο and there are four hybrid orbitals present, thus the hybridization of sulfur atom is sp3 . The Lewis structure of SF2 is,

Chemistry, Chapter 9, Problem 34E , additional homework tip  7

Figure 7

(h)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The Lewis dot structure, molecular geometry, bond angles of the given molecules and expected hybrid orbitals for sulfur is to be stated.

Concept introduction: When the atomic orbitals overlap with each other in the region where density of electrons is high, then molecular orbitals are formed. Overlap of the atomic orbitals determines the efficiency of the interaction between the atomic orbitals.

Energy of bonding molecular orbitals is less than the nonbonding molecular orbitals.

To determine: The Lewis dot structure, molecular geometry, bond angles and expected hybrid orbitals for sulfur in SF4 .

Explanation of Solution

Explanation

There are six valence electrons on sulfur and seven valence electrons on each fluorine atom. Four fluorine atoms and one sulfur atom is present in the molecule, therefore, the total number of valence electrons is 6+7×4=34 . The sulfur is bonded to four fluorine atoms by sigma bond. By bonding in this way, they complete their octet. One lone pair of electron is present on sulfur.

The molecular structure is see-saw due to presence of lone pair of electrons on sulfur. The equatorial bond angles are 120ο and the axial bond angle is 90ο and four hybrid orbitals are required for the accommodation of four bonding electron and one lone pair on sulfur, thus the hybridization of sulfur atom is sp3d . The Lewis structure of SF4 is,

Chemistry, Chapter 9, Problem 34E , additional homework tip  8

Figure 8

(i)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The Lewis dot structure, molecular geometry, bond angles of the given molecules and expected hybrid orbitals for sulfur is to be stated.

Concept introduction: When the atomic orbitals overlap with each other in the region where density of electrons is high, then molecular orbitals are formed. Overlap of the atomic orbitals determines the efficiency of the interaction between the atomic orbitals.

Energy of bonding molecular orbitals is less than the nonbonding molecular orbitals.

To determine: The Lewis dot structure, molecular geometry, bond angles and expected hybrid orbitals for sulfur in SF6 .

Explanation of Solution

Explanation

There are six valence electrons on sulfur and seven valence electrons on each fluorine atom. Six fluorine atoms and one sulfur atom is present in the molecule, therefore, the total number of valence electrons is 6+7×6=48 . The sulfur is bonded to six fluorine atoms by sigma bond. By bonding in this way, they complete their octet. No lone pair of electron is present on sulfur.

The molecular structure is octahedral with bond angle 90ο and each electron from 3s and 3p orbitals are promoted to 3d orbitals for the formation of six sigma bonds with fluorine atoms, thus the hybridization of sulfur atom is sp3d2 . The Lewis structure of SF6 is,

Chemistry, Chapter 9, Problem 34E , additional homework tip  9

Figure 9

(j)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The Lewis dot structure, molecular geometry, bond angles of the given molecules and expected hybrid orbitals for sulfur is to be stated.

Concept introduction: When the atomic orbitals overlap with each other in the region where density of electrons is high, then molecular orbitals are formed. Overlap of the atomic orbitals determines the efficiency of the interaction between the atomic orbitals.

Energy of bonding molecular orbitals is less than the nonbonding molecular orbitals.

To determine: The Lewis dot structure, molecular geometry, bond angles and expected hybrid orbitals for sulfur in F3SSF .

Explanation of Solution

Explanation

There are six valence electrons on sulfur and seven valence electrons on each fluorine atom. Four fluorine atoms and two sulfur atoms are present in the molecule, therefore, the total number of valence electrons is 2×6+7×4=40 . Two sulfur atoms are joined by single bond. Three fluorine atoms are attached to one sulfur and one fluorine atom is attached to another sulfur atom. By bonding in this way, they complete their octet. One lone pair of electron is present on one sulfur and two lone pair of electrons are present on another sulfur.

The molecular structure is see-saw due to presence of lone pair of electrons on sulfur. The equatorial bond angles are 120ο and the axial bond angle is 90ο . Four hybrid orbitals are required for the accommodation of four bonding electron and one lone pair on sulfur, thus the hybridization of sulfur atom bonded to three fluorine atoms is sp3d . The hybridization of sulfur bonded with only one fluorine is sp3 .

The Lewis structure of F3SSF is,

Chemistry, Chapter 9, Problem 34E , additional homework tip  10

Figure 10

(k)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The Lewis dot structure, molecular geometry, bond angles of the given molecules and expected hybrid orbitals for sulfur is to be stated.

Concept introduction: When the atomic orbitals overlap with each other in the region where density of electrons is high, then molecular orbitals are formed. Overlap of the atomic orbitals determines the efficiency of the interaction between the atomic orbitals.

Energy of bonding molecular orbitals is less than the nonbonding molecular orbitals.

To determine: The Lewis dot structure, molecular geometry, bond angles and expected hybrid orbitals for sulfur in SF5+ .

Explanation of Solution

Explanation

There are six valence electrons on sulfur and seven valence electrons on each fluorine atom. Five fluorine atoms and one sulfur atom is present in the molecule and charge on the molecule is +1 , therefore, the total number of valence electrons is 6+7×51=40 . The sulfur is bonded to five fluorine atoms by sigma bond. By bonding in this way, they complete their octet.

The molecular structure is trigonal bipyramidal with equatorial bond angles 120ο and the axial bond angle 90ο . The sulfur has no lone pairs of electrons and is attached to five fluorine atoms, thus the hybridization of sulfur atom is sp3d .

The Lewis structure of SF5+ is,

Chemistry, Chapter 9, Problem 34E , additional homework tip  11

Figure 11

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!
Students have asked these similar questions
E and F
XeOF2 is a compound that can be made at low temperatures. Xenon is the only inner (central) atom, i.e., Xe is bonded to the two F atoms and to the O atom. What is the electron group geometry and the molecular shape of XeOF2? electron group geometry molecular shape a. trigonal planar b. tetrahedral C. trigonal bipyramidal d. e. trigonal bipyramidal octahedral trigonal planar trigonal pyramidal see-saw T-shaped square planar Which of the following three molecules is(are) polar: TeF2, TeF4, TeF6 a. Only TeF2 is polar b. TeF2 and TeF4 are polar c. TeF2 and TeF6 are polar d. TeF4 and TeF6 are polar e. All of TeF2, TeF4, and TeF6 are polar
Lewis structure rules don't always work. In some cases, an atom can be stable with fewer or more than 8 electrons in the valence shell. In some cases, the sum of all valence electrons in the molecule adds up to an odd number and you will have an unpaired electron. a. Explain why nitrogen cannot have an expanded octet but phosphorus can. b. Draw the Lewis structure for the following molecules. i. BeF2 ii. SF4 ii. ICI

Chapter 9 Solutions

Chemistry

Ch. 9 - Which is the more correct statement: The methane...Ch. 9 - Compare and contrast the MO model with the local...Ch. 9 - What are the relationships among bond order, bond...Ch. 9 - The molecules N2 and CO are isoelectronic but...Ch. 9 - Do lone pairs about a central atom affect the...Ch. 9 - In the hybrid orbital model, compare and contrast ...Ch. 9 - In the molecular orbital mode l, compare and...Ch. 9 - Why are d orbitals sometimes used to form hybrid...Ch. 9 - The atoms in a single bond can rotate about the...Ch. 9 - As compared with CO and O2, CS and S2 are very...Ch. 9 - Compare and contrast bonding molecular orbitals...Ch. 9 - What modification to the molecular orbital model...Ch. 9 - Why does the molecular orbital model do a better...Ch. 9 - The three NO bonds in NO3 are all equivalent in...Ch. 9 - Use the localized electron model to describe the...Ch. 9 - Use the localized electron model to describe the...Ch. 9 - Use the localized electron model to describe the...Ch. 9 - Use the localized electron model to describe the...Ch. 9 - The space-filling models of ethane and ethanol are...Ch. 9 - The space-filling models of hydrogen cyanide and...Ch. 9 - Give the expected hybridization of the central...Ch. 9 - Give the expected hybridization of the central...Ch. 9 - Give the expected hybridization of the central...Ch. 9 - Give the expected hybridization of the central...Ch. 9 - For each of the following molecules, write the...Ch. 9 - For each of the following molecules or ions that...Ch. 9 - Prob. 35ECh. 9 - The allene molecule has the following Lewis...Ch. 9 - Indigo is the dye used in coloring blue jeans. The...Ch. 9 - Urea, a compound formed in the liver, is one of...Ch. 9 - Biacetyl and acetoin are added to margarine to...Ch. 9 - Many important compounds in the chemical industry...Ch. 9 - Two molecules used in the polymer industry are...Ch. 9 - Hot and spicy foods contain molecules that...Ch. 9 - One of the first drugs to be approved for use in...Ch. 9 - Minoxidil (C9H15N15O) is a compound produced by...Ch. 9 - Consider the following molecular orbitals formed...Ch. 9 - Sketch the molecular orbital and label its type (...Ch. 9 - Which of the following are predicted by the...Ch. 9 - Which of the following are predicted by the...Ch. 9 - Using the molecular orbital model, write electron...Ch. 9 - Consider the following electron configuration:...Ch. 9 - Using the molecular orbital model to describe the...Ch. 9 - A Lewis structure obeying the octet rule can be...Ch. 9 - Using the molecular orbital model, write electron...Ch. 9 - Using the molecular orbital model, write electron...Ch. 9 - In which of the following diatomic molecules would...Ch. 9 - In terms of the molecular orbital model, which...Ch. 9 - Show how two 2p atomic orbitals can combine to...Ch. 9 - Show how a hydrogen 1s atomic orbital and a...Ch. 9 - Use Figs. 4-54 and 4-55 to answer the following...Ch. 9 - Acetylene (C2H2) can be produced from the reaction...Ch. 9 - Describe the bonding in NO+, NO, and NO, using...Ch. 9 - Describe the bonding in the O3 molecule and the...Ch. 9 - Describe the bonding in the CO32 ion using the...Ch. 9 - Draw the Lewis structures, predict the molecular...Ch. 9 - The antibiotic thiarubin-A was discovered by...Ch. 9 - Two structures can be drawn for cyanuric acid: a....Ch. 9 - Give the expected hybridization for the molecular...Ch. 9 - Vitamin B6 is an organic compound whose deficiency...Ch. 9 - Aspartame is an artificial sweetener marketed...Ch. 9 - Prob. 73AECh. 9 - The three most stable oxides of carbon are carbon...Ch. 9 - Complete the following resonance structures for...Ch. 9 - Prob. 77AECh. 9 - The transport of O2 in the blood is carried out by...Ch. 9 - Using molecular orbital theory, explain why the...Ch. 9 - Describe the bonding in the first excited state of...Ch. 9 - Using an MO energy-level diagram, would you expect...Ch. 9 - Show how a dxz. atomic orbital and a pz, atomic...Ch. 9 - What type of molecular orbital would result from...Ch. 9 - Consider three molecules: A, B, and C. Molecule A...Ch. 9 - Draw the Lewis structures for TeCl4, ICl5, PCl5,...Ch. 9 - A variety of chlorine oxide fluorides and related...Ch. 9 - Pelargondin is the molecule responsible for the...Ch. 9 - Complete a Lewis structure for the compound shown...Ch. 9 - Which of the following statements concerning SO2...Ch. 9 - Consider the molecular orbital electron...Ch. 9 - Place the species B2+ , B2, and B2 in order of...Ch. 9 - Consider the following computer-generated model of...Ch. 9 - Cholesterol (C27liu;O) has the following...Ch. 9 - Cyanamide (H2NCN), an important industrial...Ch. 9 - A flask containing gaseous N2 is irradiated with...Ch. 9 - Values of measured bond energies may vary greatly...Ch. 9 - Use the MO model to explain the bonding in BeH2....Ch. 9 - Prob. 101CPCh. 9 - Arrange the following from lowest to highest...Ch. 9 - Use the MO model to determine which of the...Ch. 9 - Given that the ionization energy of F2 is 290...Ch. 9 - Carbon monoxide (CO) forms bonds to a variety of...Ch. 9 - Prob. 106CPCh. 9 - As the bead engineer of your starship in charge of...Ch. 9 - Determine the molecular structure and...Ch. 9 - Although nitrogen trifluoride (NF3) is a thermally...
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:9781133611097
    Author:Steven S. Zumdahl
    Publisher:Cengage Learning
    Text book image
    Chemistry
    Chemistry
    ISBN:9781305957404
    Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
    Publisher:Cengage Learning
    Text book image
    Chemistry: An Atoms First Approach
    Chemistry
    ISBN:9781305079243
    Author:Steven S. Zumdahl, Susan A. Zumdahl
    Publisher:Cengage Learning
  • Text book image
    Chemistry & Chemical Reactivity
    Chemistry
    ISBN:9781337399074
    Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
    Publisher:Cengage Learning
    Text book image
    Chemistry & Chemical Reactivity
    Chemistry
    ISBN:9781133949640
    Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
    Publisher:Cengage Learning
    Text book image
    Introductory Chemistry: A Foundation
    Chemistry
    ISBN:9781337399425
    Author:Steven S. Zumdahl, Donald J. DeCoste
    Publisher:Cengage Learning
Text book image
Chemistry
Chemistry
ISBN:9781133611097
Author:Steven S. Zumdahl
Publisher:Cengage Learning
Text book image
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Text book image
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
Text book image
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Text book image
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Text book image
Introductory Chemistry: A Foundation
Chemistry
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
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