Whether the proposed statement by the student about the bond shown below as triple bond should be explained with appropriate argument. Concept introduction: Two or more of orbitals undergo redistributions of their different energies so as to form mathematically averaged orbitals in terms of energy. This phenomenon is referred as hybridization. A single bond has one σ bond, double bond has one σ bond along with one π bond while triple bond has two π bonds in addition to one σ bond.

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Answer 1

Question

Chapter 3, Problem 3CTQ

(a)

Interpretation Introduction

Interpretation: Whether the proposed statement by the student about the bond shown below as triple bond should be explained with appropriate argument.

Concept introduction: Two or more of orbitals undergo redistributions of their different energies so as to form mathematically averaged orbitals in terms of energy. This phenomenon is referred as hybridization.

A single bond has one σ bond, double bond has one σ bond along with one π bond while triple bond has two π bonds in addition to one σ bond.

(b)

Interpretation Introduction

Interpretation: The number of electrons present in a triple bond and in one representation shown below should be indicated.

Concept introduction: Two or more of orbitals undergo redistributions of their different energies so as to form mathematically averaged orbitals in terms of energy. This phenomenon is referred as hybridization.

A single bond has one σ bond, double bond has one σ bond along with one π bond while triple bond has two π bonds in addition to one σ bond.

(c)

Interpretation Introduction

Interpretation: Misconception that might have led to bond identified as triple bond by the student should be known.

Concept introduction: The 2 types of overlapping are as follows:

1. Head-on overlapping (sigma bond)

2. Sideway overlapping (pi bond)

A single bond has one σ bond, double bond has one σ bond along with one π bond while triple bond has two π bonds in addition to one σ bond.

(d)

Interpretation Introduction

Interpretation: The space that could be used to add another p bond so as to generate a triple bond should be determined.

Concept introduction: Two or more of orbitals undergo redistributions of their different energies so as to form mathematically averaged orbitals in terms of energy although they may differ in shape and orientation. This phenomenon is referred as hybridization.

The energy and orientation of the new hybrid orbital depend upon by the kind and number of orbitals used in the hybridization. The new hybrid orbitals are always equal in number to number of atomic orbitals that combine.

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I am slightly confused on how to do this. I think I figured it out but I just want to compare data and take notes on what I have done incorrectly.

1. Consider the 1st and 2nd ionization energies of the element Potassium. a. Which of the two ionization energies will be larger? The 1st or 2nd? b. Discuss the number of valence electrons that Potassium has, as well as provide a definition of ionization energy. 2. Consider the carbon dioxide molecule, which is composed of carbon and oxygen. a. Is this molecule polar or non-polar? b. Explain your answer to Part A in terms of molecular geometry of the molecule (draw the Lewis Structure). c. Explain your answer to Part A in terms of electronegativity and the dipole moments found within the carbon dioxide molecule.

1) For each condensed or skeletal structure below: A. Draw a complete Lewis structure. Note: show all non-bonding electron pairs. B. Indicate the hybridization of all C, O, and N atoms in each of the molecules. C. Label each of the indicated bonds (marked by an arrow) as either a sigma or pi bond. (Note: Remember, e.g. that a double bond is made up of both a o and a π bond). Also indicate which orbitals overlap to form the bond (e.g., Ols-2sp3). D. For atoms having lone pairs in the molecules below, indicate in which orbitals the lone pairs are located. E. Which of the bonds indicated by arrows is shorter? a) c) H CH3 C=CHC=C-CH g) (CH3)3CCN CH3 CH₂CH=CHCECH b) d) CH3 Lo LOH f) CH₂CH(CH3)SH h) (CH3)2CH(CH₂)3Br

Answer 2

Question

Chapter 3, Problem 3CTQ

(a)

Interpretation Introduction

Interpretation: Whether the proposed statement by the student about the bond shown below as triple bond should be explained with appropriate argument.

Concept introduction: Two or more of orbitals undergo redistributions of their different energies so as to form mathematically averaged orbitals in terms of energy. This phenomenon is referred as hybridization.

A single bond has one σ bond, double bond has one σ bond along with one π bond while triple bond has two π bonds in addition to one σ bond.

(b)

Interpretation Introduction

Interpretation: The number of electrons present in a triple bond and in one representation shown below should be indicated.

Concept introduction: Two or more of orbitals undergo redistributions of their different energies so as to form mathematically averaged orbitals in terms of energy. This phenomenon is referred as hybridization.

A single bond has one σ bond, double bond has one σ bond along with one π bond while triple bond has two π bonds in addition to one σ bond.

(c)

Interpretation Introduction

Interpretation: Misconception that might have led to bond identified as triple bond by the student should be known.

Concept introduction: The 2 types of overlapping are as follows:

1. Head-on overlapping (sigma bond)

2. Sideway overlapping (pi bond)

A single bond has one σ bond, double bond has one σ bond along with one π bond while triple bond has two π bonds in addition to one σ bond.

(d)

Interpretation Introduction

Interpretation: The space that could be used to add another p bond so as to generate a triple bond should be determined.

Concept introduction: Two or more of orbitals undergo redistributions of their different energies so as to form mathematically averaged orbitals in terms of energy although they may differ in shape and orientation. This phenomenon is referred as hybridization.

The energy and orientation of the new hybrid orbital depend upon by the kind and number of orbitals used in the hybridization. The new hybrid orbitals are always equal in number to number of atomic orbitals that combine.

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Answer 3

Question

Chapter 3, Problem 3CTQ

(a)

Interpretation Introduction

Interpretation: Whether the proposed statement by the student about the bond shown below as triple bond should be explained with appropriate argument.

Concept introduction: Two or more of orbitals undergo redistributions of their different energies so as to form mathematically averaged orbitals in terms of energy. This phenomenon is referred as hybridization.

A single bond has one σ bond, double bond has one σ bond along with one π bond while triple bond has two π bonds in addition to one σ bond.

(b)

Interpretation Introduction

Interpretation: The number of electrons present in a triple bond and in one representation shown below should be indicated.

Concept introduction: Two or more of orbitals undergo redistributions of their different energies so as to form mathematically averaged orbitals in terms of energy. This phenomenon is referred as hybridization.

A single bond has one σ bond, double bond has one σ bond along with one π bond while triple bond has two π bonds in addition to one σ bond.

(c)

Interpretation Introduction

Interpretation: Misconception that might have led to bond identified as triple bond by the student should be known.

Concept introduction: The 2 types of overlapping are as follows:

1. Head-on overlapping (sigma bond)

2. Sideway overlapping (pi bond)

A single bond has one σ bond, double bond has one σ bond along with one π bond while triple bond has two π bonds in addition to one σ bond.

(d)

Interpretation Introduction

Interpretation: The space that could be used to add another p bond so as to generate a triple bond should be determined.

Concept introduction: Two or more of orbitals undergo redistributions of their different energies so as to form mathematically averaged orbitals in terms of energy although they may differ in shape and orientation. This phenomenon is referred as hybridization.

The energy and orientation of the new hybrid orbital depend upon by the kind and number of orbitals used in the hybridization. The new hybrid orbitals are always equal in number to number of atomic orbitals that combine.

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Answer 4

Question

Chapter 3, Problem 3CTQ

(a)

Interpretation Introduction

Interpretation: Whether the proposed statement by the student about the bond shown below as triple bond should be explained with appropriate argument.

Concept introduction: Two or more of orbitals undergo redistributions of their different energies so as to form mathematically averaged orbitals in terms of energy. This phenomenon is referred as hybridization.

A single bond has one σ bond, double bond has one σ bond along with one π bond while triple bond has two π bonds in addition to one σ bond.

(b)

Interpretation Introduction

Interpretation: The number of electrons present in a triple bond and in one representation shown below should be indicated.

Concept introduction: Two or more of orbitals undergo redistributions of their different energies so as to form mathematically averaged orbitals in terms of energy. This phenomenon is referred as hybridization.

A single bond has one σ bond, double bond has one σ bond along with one π bond while triple bond has two π bonds in addition to one σ bond.

(c)

Interpretation Introduction

Interpretation: Misconception that might have led to bond identified as triple bond by the student should be known.

Concept introduction: The 2 types of overlapping are as follows:

1. Head-on overlapping (sigma bond)

2. Sideway overlapping (pi bond)

A single bond has one σ bond, double bond has one σ bond along with one π bond while triple bond has two π bonds in addition to one σ bond.

(d)

Interpretation Introduction

Interpretation: The space that could be used to add another p bond so as to generate a triple bond should be determined.

Concept introduction: Two or more of orbitals undergo redistributions of their different energies so as to form mathematically averaged orbitals in terms of energy although they may differ in shape and orientation. This phenomenon is referred as hybridization.

The energy and orientation of the new hybrid orbital depend upon by the kind and number of orbitals used in the hybridization. The new hybrid orbitals are always equal in number to number of atomic orbitals that combine.

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Answer 5

Chapter 3, Problem 3CTQ

(a)

Interpretation Introduction

Interpretation: Whether the proposed statement by the student about the bond shown below as triple bond should be explained with appropriate argument.

Concept introduction: Two or more of orbitals undergo redistributions of their different energies so as to form mathematically averaged orbitals in terms of energy. This phenomenon is referred as hybridization.

A single bond has one σ bond, double bond has one σ bond along with one π bond while triple bond has two π bonds in addition to one σ bond.

(b)

Interpretation Introduction

Interpretation: The number of electrons present in a triple bond and in one representation shown below should be indicated.

Concept introduction: Two or more of orbitals undergo redistributions of their different energies so as to form mathematically averaged orbitals in terms of energy. This phenomenon is referred as hybridization.

A single bond has one σ bond, double bond has one σ bond along with one π bond while triple bond has two π bonds in addition to one σ bond.

(c)

Interpretation Introduction

Interpretation: Misconception that might have led to bond identified as triple bond by the student should be known.

Concept introduction: The 2 types of overlapping are as follows:

1. Head-on overlapping (sigma bond)

2. Sideway overlapping (pi bond)

A single bond has one σ bond, double bond has one σ bond along with one π bond while triple bond has two π bonds in addition to one σ bond.

(d)

Interpretation Introduction

Interpretation: The space that could be used to add another p bond so as to generate a triple bond should be determined.

Concept introduction: Two or more of orbitals undergo redistributions of their different energies so as to form mathematically averaged orbitals in terms of energy although they may differ in shape and orientation. This phenomenon is referred as hybridization.

The energy and orientation of the new hybrid orbital depend upon by the kind and number of orbitals used in the hybridization. The new hybrid orbitals are always equal in number to number of atomic orbitals that combine.

Answer 6

Chapter 3, Problem 3CTQ

(a)

Interpretation Introduction

Interpretation: Whether the proposed statement by the student about the bond shown below as triple bond should be explained with appropriate argument.

Concept introduction: Two or more of orbitals undergo redistributions of their different energies so as to form mathematically averaged orbitals in terms of energy. This phenomenon is referred as hybridization.

A single bond has one σ bond, double bond has one σ bond along with one π bond while triple bond has two π bonds in addition to one σ bond.

Answer 7

Chapter 3, Problem 3CTQ

(a)

Interpretation Introduction

Interpretation: Whether the proposed statement by the student about the bond shown below as triple bond should be explained with appropriate argument.

Concept introduction: Two or more of orbitals undergo redistributions of their different energies so as to form mathematically averaged orbitals in terms of energy. This phenomenon is referred as hybridization.

A single bond has one σ bond, double bond has one σ bond along with one π bond while triple bond has two π bonds in addition to one σ bond.

Answer 8

(b)

Interpretation Introduction

Interpretation: The number of electrons present in a triple bond and in one representation shown below should be indicated.

Concept introduction: Two or more of orbitals undergo redistributions of their different energies so as to form mathematically averaged orbitals in terms of energy. This phenomenon is referred as hybridization.

A single bond has one σ bond, double bond has one σ bond along with one π bond while triple bond has two π bonds in addition to one σ bond.

Answer 9

(b)

Interpretation Introduction

Interpretation: The number of electrons present in a triple bond and in one representation shown below should be indicated.

Concept introduction: Two or more of orbitals undergo redistributions of their different energies so as to form mathematically averaged orbitals in terms of energy. This phenomenon is referred as hybridization.

A single bond has one σ bond, double bond has one σ bond along with one π bond while triple bond has two π bonds in addition to one σ bond.

Answer 10

(c)

Interpretation Introduction

Interpretation: Misconception that might have led to bond identified as triple bond by the student should be known.

Concept introduction: The 2 types of overlapping are as follows:

1. Head-on overlapping (sigma bond)

2. Sideway overlapping (pi bond)

A single bond has one σ bond, double bond has one σ bond along with one π bond while triple bond has two π bonds in addition to one σ bond.

Answer 11

(c)

Interpretation Introduction

Interpretation: Misconception that might have led to bond identified as triple bond by the student should be known.

Concept introduction: The 2 types of overlapping are as follows:

1. Head-on overlapping (sigma bond)

2. Sideway overlapping (pi bond)

A single bond has one σ bond, double bond has one σ bond along with one π bond while triple bond has two π bonds in addition to one σ bond.

Answer 12

(d)

Interpretation Introduction

Interpretation: The space that could be used to add another p bond so as to generate a triple bond should be determined.

Concept introduction: Two or more of orbitals undergo redistributions of their different energies so as to form mathematically averaged orbitals in terms of energy although they may differ in shape and orientation. This phenomenon is referred as hybridization.

The energy and orientation of the new hybrid orbital depend upon by the kind and number of orbitals used in the hybridization. The new hybrid orbitals are always equal in number to number of atomic orbitals that combine.

Answer 13

(d)

Interpretation Introduction

Interpretation: The space that could be used to add another p bond so as to generate a triple bond should be determined.

Concept introduction: Two or more of orbitals undergo redistributions of their different energies so as to form mathematically averaged orbitals in terms of energy although they may differ in shape and orientation. This phenomenon is referred as hybridization.

The energy and orientation of the new hybrid orbital depend upon by the kind and number of orbitals used in the hybridization. The new hybrid orbitals are always equal in number to number of atomic orbitals that combine.

Answer 14

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Answer 15

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Answer 16

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Answer 17

Ch. 3 - Prob. 1CTQ Ch. 3 - What neutral atom is represented by the electron...Ch. 3 - Prob. 3CTQ Ch. 3 - Consider any one of the four identical hybrid...Ch. 3 - Prob. 5CTQ Ch. 3 - Prob. 6CTQ Ch. 3 - Prob. 7CTQ Ch. 3 - Prob. 8CTQ Ch. 3 - Prob. 9CTQ Ch. 3 - Prob. 10CTQ

Solution Summary: The author explains that the proposed statement about the bond shown below as triple bond should be explained with appropriate argument.

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