(a) Interpretation: The orbital picture of methane indicating the important overlap of AOs is to be drawn. Concept introduction: According to Valence Bond Theory , the hybridized atom is the one which is bonded to two or more other atoms. The mixing of atomic orbitals is knows as hybridization. The valence atomic orbitals of an atom, on mixing, form a new set of hybrid orbitals of equivalent energy. The mixing of two atomic orbitals, one from each adjacent atom, forms new orbitals. The hybridization of an atom can be determined based on the electron geometry around it. The VSEPR chart depicts the electron and molecular geometry on the basis of numbers of electron groups. The electron geometry of an atom describes the orientation of electron groups around it.

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Answer 1

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Definition Definition Theory that explains how individual atomic orbitals with an unpaired electron each, come close to each other and overlap to form a molecular orbital giving a covalent bond. VBT gives a quantum mechanical approach to the formation of covalent bonds with the help of wave functions using attractive and repulsive energies when two atoms are brought from infinity to their internuclear distance.

Chapter 3, Problem 3.12P

Interpretation Introduction

(a)

Interpretation:

The orbital picture of methane indicating the important overlap of AOs is to be drawn.

Concept introduction:

According to Valence Bond Theory, the hybridized atom is the one which is bonded to two or more other atoms. The mixing of atomic orbitals is knows as hybridization. The valence atomic orbitals of an atom, on mixing, form a new set of hybrid orbitals of equivalent energy. The mixing of two atomic orbitals, one from each adjacent atom, forms new orbitals. The hybridization of an atom can be determined based on the electron geometry around it. The VSEPR chart depicts the electron and molecular geometry on the basis of numbers of electron groups. The electron geometry of an atom describes the orientation of electron groups around it.

Interpretation Introduction

(b)

Interpretation:

The energy diagram of methane indicating the formation of molecular orbitals (MOs) is to be drawn.

Concept introduction:

The molecular orbitals are formed by overlapping of atomic orbitals of adjacent atoms. The number of molecular orbitals formed and the number of atomic orbitals that overlap is equal. The two atomic orbitals, on mixing along bonding axes, form two molecular orbitals: one is σ and other is σ. The σ is the bonding MO, and σ is the antibonding MO. The σ MOs has lower energy and thus a greater stability than the corresponding σ* MOs. Thus, electrons are filled in lower energy first in σ MOs and are considered as LUMO (Lowest Unoccupied Molecular Orbitals), and σ* MOs are considered as HOMO (Highest Occupied Molecular Orbitals). Each single bond in the Lewis structure corresponds to a filled σ MO, and hence each single bond is referred as σ bond.

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1. Answer the questions about the following reaction: (a) Draw in the arrows that can be used make this reaction occur and draw in the product of substitution in this reaction. Be sure to include any relevant stereochemistry in the product structure. + SK F Br + (b) In which solvent would this reaction proceed the fastest (Circle one) Methanol Acetone (c) Imagine that you are working for a chemical company and it was your job to perform a similar reaction to the one above, with the exception of the S atom in this reaction being replaced by an O atom. During the reaction, you observe the formation of three separate molecules instead of the single molecule obtained above. What is the likeliest other products that are formed? Draw them in the box provided.

3. For the reactions below, draw the arrows corresponding to the transformations and draw in the boxes the reactants or products as indicated. Note: Part A should have arrows drawn going from the reactants to the middle structure and the arrows on the middle structure that would yield the final structure. For part B, you will need to draw in the reactant before being able to draw the arrows corresponding to product formation. A. B. Rearrangement ΘΗ

2. Draw the arrows required to make the following reactions occur. Please ensure your arrows point from exactly where you want to exactly where you want. If it is unclear from where arrows start or where they end, only partial credit will be given. Note: You may need to draw in lone pairs before drawing the arrows. A. B. H-Br 人 C Θ CI H Cl Θ + Br O

Answer 2

Question

Definition Definition Theory that explains how individual atomic orbitals with an unpaired electron each, come close to each other and overlap to form a molecular orbital giving a covalent bond. VBT gives a quantum mechanical approach to the formation of covalent bonds with the help of wave functions using attractive and repulsive energies when two atoms are brought from infinity to their internuclear distance.

Chapter 3, Problem 3.12P

Interpretation Introduction

(a)

Interpretation:

The orbital picture of methane indicating the important overlap of AOs is to be drawn.

Concept introduction:

According to Valence Bond Theory, the hybridized atom is the one which is bonded to two or more other atoms. The mixing of atomic orbitals is knows as hybridization. The valence atomic orbitals of an atom, on mixing, form a new set of hybrid orbitals of equivalent energy. The mixing of two atomic orbitals, one from each adjacent atom, forms new orbitals. The hybridization of an atom can be determined based on the electron geometry around it. The VSEPR chart depicts the electron and molecular geometry on the basis of numbers of electron groups. The electron geometry of an atom describes the orientation of electron groups around it.

Interpretation Introduction

(b)

Interpretation:

The energy diagram of methane indicating the formation of molecular orbitals (MOs) is to be drawn.

Concept introduction:

The molecular orbitals are formed by overlapping of atomic orbitals of adjacent atoms. The number of molecular orbitals formed and the number of atomic orbitals that overlap is equal. The two atomic orbitals, on mixing along bonding axes, form two molecular orbitals: one is σ and other is σ. The σ is the bonding MO, and σ is the antibonding MO. The σ MOs has lower energy and thus a greater stability than the corresponding σ* MOs. Thus, electrons are filled in lower energy first in σ MOs and are considered as LUMO (Lowest Unoccupied Molecular Orbitals), and σ* MOs are considered as HOMO (Highest Occupied Molecular Orbitals). Each single bond in the Lewis structure corresponds to a filled σ MO, and hence each single bond is referred as σ bond.

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Answer 3

Question

Definition Definition Theory that explains how individual atomic orbitals with an unpaired electron each, come close to each other and overlap to form a molecular orbital giving a covalent bond. VBT gives a quantum mechanical approach to the formation of covalent bonds with the help of wave functions using attractive and repulsive energies when two atoms are brought from infinity to their internuclear distance.

Chapter 3, Problem 3.12P

Interpretation Introduction

(a)

Interpretation:

The orbital picture of methane indicating the important overlap of AOs is to be drawn.

Concept introduction:

According to Valence Bond Theory, the hybridized atom is the one which is bonded to two or more other atoms. The mixing of atomic orbitals is knows as hybridization. The valence atomic orbitals of an atom, on mixing, form a new set of hybrid orbitals of equivalent energy. The mixing of two atomic orbitals, one from each adjacent atom, forms new orbitals. The hybridization of an atom can be determined based on the electron geometry around it. The VSEPR chart depicts the electron and molecular geometry on the basis of numbers of electron groups. The electron geometry of an atom describes the orientation of electron groups around it.

Interpretation Introduction

(b)

Interpretation:

The energy diagram of methane indicating the formation of molecular orbitals (MOs) is to be drawn.

Concept introduction:

The molecular orbitals are formed by overlapping of atomic orbitals of adjacent atoms. The number of molecular orbitals formed and the number of atomic orbitals that overlap is equal. The two atomic orbitals, on mixing along bonding axes, form two molecular orbitals: one is σ and other is σ. The σ is the bonding MO, and σ is the antibonding MO. The σ MOs has lower energy and thus a greater stability than the corresponding σ* MOs. Thus, electrons are filled in lower energy first in σ MOs and are considered as LUMO (Lowest Unoccupied Molecular Orbitals), and σ* MOs are considered as HOMO (Highest Occupied Molecular Orbitals). Each single bond in the Lewis structure corresponds to a filled σ MO, and hence each single bond is referred as σ bond.

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Answer 4

Question

Definition Definition Theory that explains how individual atomic orbitals with an unpaired electron each, come close to each other and overlap to form a molecular orbital giving a covalent bond. VBT gives a quantum mechanical approach to the formation of covalent bonds with the help of wave functions using attractive and repulsive energies when two atoms are brought from infinity to their internuclear distance.

Chapter 3, Problem 3.12P

Interpretation Introduction

(a)

Interpretation:

The orbital picture of methane indicating the important overlap of AOs is to be drawn.

Concept introduction:

According to Valence Bond Theory, the hybridized atom is the one which is bonded to two or more other atoms. The mixing of atomic orbitals is knows as hybridization. The valence atomic orbitals of an atom, on mixing, form a new set of hybrid orbitals of equivalent energy. The mixing of two atomic orbitals, one from each adjacent atom, forms new orbitals. The hybridization of an atom can be determined based on the electron geometry around it. The VSEPR chart depicts the electron and molecular geometry on the basis of numbers of electron groups. The electron geometry of an atom describes the orientation of electron groups around it.

Interpretation Introduction

(b)

Interpretation:

The energy diagram of methane indicating the formation of molecular orbitals (MOs) is to be drawn.

Concept introduction:

The molecular orbitals are formed by overlapping of atomic orbitals of adjacent atoms. The number of molecular orbitals formed and the number of atomic orbitals that overlap is equal. The two atomic orbitals, on mixing along bonding axes, form two molecular orbitals: one is σ and other is σ. The σ is the bonding MO, and σ is the antibonding MO. The σ MOs has lower energy and thus a greater stability than the corresponding σ* MOs. Thus, electrons are filled in lower energy first in σ MOs and are considered as LUMO (Lowest Unoccupied Molecular Orbitals), and σ* MOs are considered as HOMO (Highest Occupied Molecular Orbitals). Each single bond in the Lewis structure corresponds to a filled σ MO, and hence each single bond is referred as σ bond.

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Answer 5

Chapter 3, Problem 3.12P

Interpretation Introduction

(a)

Interpretation:

The orbital picture of methane indicating the important overlap of AOs is to be drawn.

Concept introduction:

According to Valence Bond Theory, the hybridized atom is the one which is bonded to two or more other atoms. The mixing of atomic orbitals is knows as hybridization. The valence atomic orbitals of an atom, on mixing, form a new set of hybrid orbitals of equivalent energy. The mixing of two atomic orbitals, one from each adjacent atom, forms new orbitals. The hybridization of an atom can be determined based on the electron geometry around it. The VSEPR chart depicts the electron and molecular geometry on the basis of numbers of electron groups. The electron geometry of an atom describes the orientation of electron groups around it.

Interpretation Introduction

(b)

Interpretation:

The energy diagram of methane indicating the formation of molecular orbitals (MOs) is to be drawn.

Concept introduction:

The molecular orbitals are formed by overlapping of atomic orbitals of adjacent atoms. The number of molecular orbitals formed and the number of atomic orbitals that overlap is equal. The two atomic orbitals, on mixing along bonding axes, form two molecular orbitals: one is σ and other is σ. The σ is the bonding MO, and σ is the antibonding MO. The σ MOs has lower energy and thus a greater stability than the corresponding σ* MOs. Thus, electrons are filled in lower energy first in σ MOs and are considered as LUMO (Lowest Unoccupied Molecular Orbitals), and σ* MOs are considered as HOMO (Highest Occupied Molecular Orbitals). Each single bond in the Lewis structure corresponds to a filled σ MO, and hence each single bond is referred as σ bond.

Answer 6

Chapter 3, Problem 3.12P

Interpretation Introduction

(a)

Interpretation:

The orbital picture of methane indicating the important overlap of AOs is to be drawn.

Concept introduction:

According to Valence Bond Theory, the hybridized atom is the one which is bonded to two or more other atoms. The mixing of atomic orbitals is knows as hybridization. The valence atomic orbitals of an atom, on mixing, form a new set of hybrid orbitals of equivalent energy. The mixing of two atomic orbitals, one from each adjacent atom, forms new orbitals. The hybridization of an atom can be determined based on the electron geometry around it. The VSEPR chart depicts the electron and molecular geometry on the basis of numbers of electron groups. The electron geometry of an atom describes the orientation of electron groups around it.

Answer 7

Chapter 3, Problem 3.12P

Interpretation Introduction

(a)

Interpretation:

The orbital picture of methane indicating the important overlap of AOs is to be drawn.

Concept introduction:

According to Valence Bond Theory, the hybridized atom is the one which is bonded to two or more other atoms. The mixing of atomic orbitals is knows as hybridization. The valence atomic orbitals of an atom, on mixing, form a new set of hybrid orbitals of equivalent energy. The mixing of two atomic orbitals, one from each adjacent atom, forms new orbitals. The hybridization of an atom can be determined based on the electron geometry around it. The VSEPR chart depicts the electron and molecular geometry on the basis of numbers of electron groups. The electron geometry of an atom describes the orientation of electron groups around it.

Answer 8

Interpretation Introduction

(b)

Interpretation:

The energy diagram of methane indicating the formation of molecular orbitals (MOs) is to be drawn.

Concept introduction:

The molecular orbitals are formed by overlapping of atomic orbitals of adjacent atoms. The number of molecular orbitals formed and the number of atomic orbitals that overlap is equal. The two atomic orbitals, on mixing along bonding axes, form two molecular orbitals: one is σ and other is σ. The σ is the bonding MO, and σ is the antibonding MO. The σ MOs has lower energy and thus a greater stability than the corresponding σ* MOs. Thus, electrons are filled in lower energy first in σ MOs and are considered as LUMO (Lowest Unoccupied Molecular Orbitals), and σ* MOs are considered as HOMO (Highest Occupied Molecular Orbitals). Each single bond in the Lewis structure corresponds to a filled σ MO, and hence each single bond is referred as σ bond.

Answer 9

Interpretation Introduction

(b)

Interpretation:

The energy diagram of methane indicating the formation of molecular orbitals (MOs) is to be drawn.

Concept introduction:

The molecular orbitals are formed by overlapping of atomic orbitals of adjacent atoms. The number of molecular orbitals formed and the number of atomic orbitals that overlap is equal. The two atomic orbitals, on mixing along bonding axes, form two molecular orbitals: one is σ and other is σ. The σ is the bonding MO, and σ is the antibonding MO. The σ MOs has lower energy and thus a greater stability than the corresponding σ* MOs. Thus, electrons are filled in lower energy first in σ MOs and are considered as LUMO (Lowest Unoccupied Molecular Orbitals), and σ* MOs are considered as HOMO (Highest Occupied Molecular Orbitals). Each single bond in the Lewis structure corresponds to a filled σ MO, and hence each single bond is referred as σ bond.

Answer 10

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Answer 13

Ch. 3 - Prob. 3.1P Ch. 3 - Prob. 3.2P Ch. 3 - Prob. 3.3P Ch. 3 - Prob. 3.4P Ch. 3 - Prob. 3.5P Ch. 3 - Prob. 3.6P Ch. 3 - Prob. 3.7P Ch. 3 - Prob. 3.8P Ch. 3 - Prob. 3.9P Ch. 3 - Prob. 3.10P

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