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

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Answer 1

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 3.13P

Interpretation Introduction

(a)

Interpretation:

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

Concept introduction:

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

Interpretation Introduction

(b)

Interpretation:

The energy diagram of ammonium ion 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 numbers of molecular orbitals formed are equal to the number of atomic orbitals that overlap. The two atomic orbitals, on mixing along bonding axes, form two molecular orbitals; one is σ, and other is σ. The σ is a bonding MO, and σ is an antibonding MO. The σ MOs have lower energy and greater stability than the corresponding σ* MOs. Thus electrons are filled in lower energy 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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(a 4 shows scanning electron microscope (SEM) images of extruded actions of packing bed for two capillary columns of different diameters, al 750 (bottom image) and b) 30-μm-i.d. Both columns are packed with the same stationary phase, spherical particles with 1-um diameter. A) When the columns were prepared, the figure shows that the column with the larger diameter has more packing irregularities. Explain this observation. B) Predict what affect this should have on band broadening and discuss your prediction using the van Deemter terms. C) Does this figure support your explanations in application question 33? Explain why or why not and make any changes in your answers in light of this figure. Figure 4 SEM images of sections of packed columns for a) 750 and b) 30-um-i.d. capillary columns.³

fcrip = ↓ bandwidth Il temp 32. What impact (increase, decrease, or no change) does each of the following conditions have on the individual components of the van Deemter equation and consequently, band broadening? Increase temperature Longer column Using a gas mobile phase instead of liquid Smaller particle stationary phase Multiple Paths Diffusion Mass Transfer

34. Figure 3 shows Van Deemter plots for a solute molecule using different column inner diameters (i.d.). A) Predict whether decreasing the column inner diameters increase or decrease bandwidth. B) Predict which van Deemter equation coefficient (A, B, or C) has the greatest effect on increasing or decreasing bandwidth as a function of i.d. and justify your answer. Figure 3 Van Deemter plots for hydroquinone using different column inner diameters (i.d. in μm). The data was obtained from liquid chromatography experiments using fused-silica capillary columns packed with 1.0-μm particles. 35 20 H(um) 큰 20 15 90 0+ 1500 100 75 550 01 02 594 05 μ(cm/sec) 30 15 10

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 3.13P

Interpretation Introduction

(a)

Interpretation:

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

Concept introduction:

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

Interpretation Introduction

(b)

Interpretation:

The energy diagram of ammonium ion 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 numbers of molecular orbitals formed are equal to the number of atomic orbitals that overlap. The two atomic orbitals, on mixing along bonding axes, form two molecular orbitals; one is σ, and other is σ. The σ is a bonding MO, and σ is an antibonding MO. The σ MOs have lower energy and greater stability than the corresponding σ* MOs. Thus electrons are filled in lower energy 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 3.13P

Interpretation Introduction

(a)

Interpretation:

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

Concept introduction:

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

Interpretation Introduction

(b)

Interpretation:

The energy diagram of ammonium ion 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 numbers of molecular orbitals formed are equal to the number of atomic orbitals that overlap. The two atomic orbitals, on mixing along bonding axes, form two molecular orbitals; one is σ, and other is σ. The σ is a bonding MO, and σ is an antibonding MO. The σ MOs have lower energy and greater stability than the corresponding σ* MOs. Thus electrons are filled in lower energy 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 3.13P

Interpretation Introduction

(a)

Interpretation:

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

Concept introduction:

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

Interpretation Introduction

(b)

Interpretation:

The energy diagram of ammonium ion 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 numbers of molecular orbitals formed are equal to the number of atomic orbitals that overlap. The two atomic orbitals, on mixing along bonding axes, form two molecular orbitals; one is σ, and other is σ. The σ is a bonding MO, and σ is an antibonding MO. The σ MOs have lower energy and greater stability than the corresponding σ* MOs. Thus electrons are filled in lower energy 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 3.13P

Interpretation Introduction

(a)

Interpretation:

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

Concept introduction:

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

Interpretation Introduction

(b)

Interpretation:

The energy diagram of ammonium ion 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 numbers of molecular orbitals formed are equal to the number of atomic orbitals that overlap. The two atomic orbitals, on mixing along bonding axes, form two molecular orbitals; one is σ, and other is σ. The σ is a bonding MO, and σ is an antibonding MO. The σ MOs have lower energy and greater stability than the corresponding σ* MOs. Thus electrons are filled in lower energy 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 3.13P

Interpretation Introduction

(a)

Interpretation:

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

Concept introduction:

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

Answer 7

Chapter 3, Problem 3.13P

Interpretation Introduction

(a)

Interpretation:

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

Concept introduction:

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

Answer 8

Interpretation Introduction

(b)

Interpretation:

The energy diagram of ammonium ion 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 numbers of molecular orbitals formed are equal to the number of atomic orbitals that overlap. The two atomic orbitals, on mixing along bonding axes, form two molecular orbitals; one is σ, and other is σ. The σ is a bonding MO, and σ is an antibonding MO. The σ MOs have lower energy and greater stability than the corresponding σ* MOs. Thus electrons are filled in lower energy 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 ammonium ion 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 numbers of molecular orbitals formed are equal to the number of atomic orbitals that overlap. The two atomic orbitals, on mixing along bonding axes, form two molecular orbitals; one is σ, and other is σ. The σ is a bonding MO, and σ is an antibonding MO. The σ MOs have lower energy and greater stability than the corresponding σ* MOs. Thus electrons are filled in lower energy 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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