To draw: The Lewis structures of the given compounds. Interpretation: The Lewis structures of the given compounds are to be drawn. Concept introduction: The Lewis structure shows the connectivity between atoms by identifying the lone pairs of electrons in a compound. Lewis structures are also called Lewis dot structures. The valence electrons around an atom are shown by dots. Bonds between atoms are shown by lines and the lone pair of electrons is shown by a pair of dots. The rules to draw Lewis structure are given as, Determine the electronegativity and the number of valence electrons contributed by each atom. Generally lowest electronegativity atom is the central atom. Write the skeleton structure of the molecule. Use two valence electrons to form each bond in skeleton structure between the central and outer atoms. Satisfy the octets of atoms by distributing remaining valence electrons as nonbonding electrons. It is usually best start with the outer atoms.

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Answer 1

Question

Chapter 1, Problem 1.52SP

1.

Interpretation Introduction

To draw: The Lewis structures of the given compounds.

Interpretation: The Lewis structures of the given compounds are to be drawn.

Concept introduction: The Lewis structure shows the connectivity between atoms by identifying the lone pairs of electrons in a compound. Lewis structures are also called Lewis dot structures. The valence electrons around an atom are shown by dots. Bonds between atoms are shown by lines and the lone pair of electrons is shown by a pair of dots.

The rules to draw Lewis structure are given as,

Determine the electronegativity and the number of valence electrons contributed by each atom.

Generally lowest electronegativity atom is the central atom.

Write the skeleton structure of the molecule.

Use two valence electrons to form each bond in skeleton structure between the central and outer atoms.

Satisfy the octets of atoms by distributing remaining valence electrons as nonbonding electrons. It is usually best start with the outer atoms.

2.

Interpretation Introduction

To show: The kinds of orbitals that overlap to form each bond in the given compounds.

Interpretation: The kinds of orbitals that overlap to form each bond in the given compounds are to be shown.

Concept introduction: In the sigma bond formation hybridized orbitals overlap with other hybridized or unhybridized orbitals. In the formation of pi bonds only unhybridized orbitals are involved.

3.

Interpretation Introduction

To determine: The approximate bond angles in the given compounds.

Interpretation: The approximate bond angles in the given compounds are to be stated.

Concept introduction: All the carbon atoms with single bond formation always arranged in tetrahedral manner. In tetrahedral arrangement the bond angles between the atoms is always 109° 28'. This angle is thermodynamically more stable angle for tetrahedrally arranged atoms.

The actual bond angles in “sp”, “sp2” and “sp3” hybridization are 180°, 120° and 109.5° respectively.

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Deducing the reactants of a Diels-Alder reaction n the molecule on the right-hand side of this organic reaction be made in good yield from no more than two reactants, in one step, by moderately heating the reactants? ? Δ • If your answer is yes, then draw the reactant or reactants in the drawing area below. You can draw the reactants in any arrangement you like. • If your answer is no, check the box under the drawing area instead. Explanation Check Click and drag to start drawing a structure. >

Predict the major products of the following organic reaction: + Some important notes: A ? • Draw the major product, or products, of the reaction in the drawing area below. • If there aren't any products, because no reaction will take place, check the box below the drawing area instead. • Be sure to use wedge and dash bonds when necessary, for example to distinguish between major products that are enantiomers. Explanation Check Click and drag to start drawing a structure.

Answer 2

Question

Chapter 1, Problem 1.52SP

1.

Interpretation Introduction

To draw: The Lewis structures of the given compounds.

Interpretation: The Lewis structures of the given compounds are to be drawn.

Concept introduction: The Lewis structure shows the connectivity between atoms by identifying the lone pairs of electrons in a compound. Lewis structures are also called Lewis dot structures. The valence electrons around an atom are shown by dots. Bonds between atoms are shown by lines and the lone pair of electrons is shown by a pair of dots.

The rules to draw Lewis structure are given as,

Determine the electronegativity and the number of valence electrons contributed by each atom.

Generally lowest electronegativity atom is the central atom.

Write the skeleton structure of the molecule.

Use two valence electrons to form each bond in skeleton structure between the central and outer atoms.

Satisfy the octets of atoms by distributing remaining valence electrons as nonbonding electrons. It is usually best start with the outer atoms.

2.

Interpretation Introduction

To show: The kinds of orbitals that overlap to form each bond in the given compounds.

Interpretation: The kinds of orbitals that overlap to form each bond in the given compounds are to be shown.

Concept introduction: In the sigma bond formation hybridized orbitals overlap with other hybridized or unhybridized orbitals. In the formation of pi bonds only unhybridized orbitals are involved.

3.

Interpretation Introduction

To determine: The approximate bond angles in the given compounds.

Interpretation: The approximate bond angles in the given compounds are to be stated.

Concept introduction: All the carbon atoms with single bond formation always arranged in tetrahedral manner. In tetrahedral arrangement the bond angles between the atoms is always 109° 28'. This angle is thermodynamically more stable angle for tetrahedrally arranged atoms.

The actual bond angles in “sp”, “sp2” and “sp3” hybridization are 180°, 120° and 109.5° respectively.

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Answer 3

Question

Chapter 1, Problem 1.52SP

1.

Interpretation Introduction

To draw: The Lewis structures of the given compounds.

Interpretation: The Lewis structures of the given compounds are to be drawn.

Concept introduction: The Lewis structure shows the connectivity between atoms by identifying the lone pairs of electrons in a compound. Lewis structures are also called Lewis dot structures. The valence electrons around an atom are shown by dots. Bonds between atoms are shown by lines and the lone pair of electrons is shown by a pair of dots.

The rules to draw Lewis structure are given as,

Determine the electronegativity and the number of valence electrons contributed by each atom.

Generally lowest electronegativity atom is the central atom.

Write the skeleton structure of the molecule.

Use two valence electrons to form each bond in skeleton structure between the central and outer atoms.

Satisfy the octets of atoms by distributing remaining valence electrons as nonbonding electrons. It is usually best start with the outer atoms.

2.

Interpretation Introduction

To show: The kinds of orbitals that overlap to form each bond in the given compounds.

Interpretation: The kinds of orbitals that overlap to form each bond in the given compounds are to be shown.

Concept introduction: In the sigma bond formation hybridized orbitals overlap with other hybridized or unhybridized orbitals. In the formation of pi bonds only unhybridized orbitals are involved.

3.

Interpretation Introduction

To determine: The approximate bond angles in the given compounds.

Interpretation: The approximate bond angles in the given compounds are to be stated.

Concept introduction: All the carbon atoms with single bond formation always arranged in tetrahedral manner. In tetrahedral arrangement the bond angles between the atoms is always 109° 28'. This angle is thermodynamically more stable angle for tetrahedrally arranged atoms.

The actual bond angles in “sp”, “sp2” and “sp3” hybridization are 180°, 120° and 109.5° respectively.

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Check out a sample textbook solution

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Answer 4

Question

Chapter 1, Problem 1.52SP

1.

Interpretation Introduction

To draw: The Lewis structures of the given compounds.

Interpretation: The Lewis structures of the given compounds are to be drawn.

Concept introduction: The Lewis structure shows the connectivity between atoms by identifying the lone pairs of electrons in a compound. Lewis structures are also called Lewis dot structures. The valence electrons around an atom are shown by dots. Bonds between atoms are shown by lines and the lone pair of electrons is shown by a pair of dots.

The rules to draw Lewis structure are given as,

Determine the electronegativity and the number of valence electrons contributed by each atom.

Generally lowest electronegativity atom is the central atom.

Write the skeleton structure of the molecule.

Use two valence electrons to form each bond in skeleton structure between the central and outer atoms.

Satisfy the octets of atoms by distributing remaining valence electrons as nonbonding electrons. It is usually best start with the outer atoms.

2.

Interpretation Introduction

To show: The kinds of orbitals that overlap to form each bond in the given compounds.

Interpretation: The kinds of orbitals that overlap to form each bond in the given compounds are to be shown.

Concept introduction: In the sigma bond formation hybridized orbitals overlap with other hybridized or unhybridized orbitals. In the formation of pi bonds only unhybridized orbitals are involved.

3.

Interpretation Introduction

To determine: The approximate bond angles in the given compounds.

Interpretation: The approximate bond angles in the given compounds are to be stated.

Concept introduction: All the carbon atoms with single bond formation always arranged in tetrahedral manner. In tetrahedral arrangement the bond angles between the atoms is always 109° 28'. This angle is thermodynamically more stable angle for tetrahedrally arranged atoms.

The actual bond angles in “sp”, “sp2” and “sp3” hybridization are 180°, 120° and 109.5° respectively.

Expert Solution & Answer

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Check out a sample textbook solution

See solution

Answer 5

Chapter 1, Problem 1.52SP

1.

Interpretation Introduction

To draw: The Lewis structures of the given compounds.

Interpretation: The Lewis structures of the given compounds are to be drawn.

Concept introduction: The Lewis structure shows the connectivity between atoms by identifying the lone pairs of electrons in a compound. Lewis structures are also called Lewis dot structures. The valence electrons around an atom are shown by dots. Bonds between atoms are shown by lines and the lone pair of electrons is shown by a pair of dots.

The rules to draw Lewis structure are given as,

Determine the electronegativity and the number of valence electrons contributed by each atom.

Generally lowest electronegativity atom is the central atom.

Write the skeleton structure of the molecule.

Use two valence electrons to form each bond in skeleton structure between the central and outer atoms.

Satisfy the octets of atoms by distributing remaining valence electrons as nonbonding electrons. It is usually best start with the outer atoms.

2.

Interpretation Introduction

To show: The kinds of orbitals that overlap to form each bond in the given compounds.

Interpretation: The kinds of orbitals that overlap to form each bond in the given compounds are to be shown.

Concept introduction: In the sigma bond formation hybridized orbitals overlap with other hybridized or unhybridized orbitals. In the formation of pi bonds only unhybridized orbitals are involved.

3.

Interpretation Introduction

To determine: The approximate bond angles in the given compounds.

Interpretation: The approximate bond angles in the given compounds are to be stated.

Concept introduction: All the carbon atoms with single bond formation always arranged in tetrahedral manner. In tetrahedral arrangement the bond angles between the atoms is always 109° 28'. This angle is thermodynamically more stable angle for tetrahedrally arranged atoms.

The actual bond angles in “sp”, “sp2” and “sp3” hybridization are 180°, 120° and 109.5° respectively.

Answer 6

Chapter 1, Problem 1.52SP

1.

Interpretation Introduction

To draw: The Lewis structures of the given compounds.

Interpretation: The Lewis structures of the given compounds are to be drawn.

Concept introduction: The Lewis structure shows the connectivity between atoms by identifying the lone pairs of electrons in a compound. Lewis structures are also called Lewis dot structures. The valence electrons around an atom are shown by dots. Bonds between atoms are shown by lines and the lone pair of electrons is shown by a pair of dots.

The rules to draw Lewis structure are given as,

Determine the electronegativity and the number of valence electrons contributed by each atom.

Generally lowest electronegativity atom is the central atom.

Write the skeleton structure of the molecule.

Use two valence electrons to form each bond in skeleton structure between the central and outer atoms.

Satisfy the octets of atoms by distributing remaining valence electrons as nonbonding electrons. It is usually best start with the outer atoms.

Answer 7

Chapter 1, Problem 1.52SP

1.

Interpretation Introduction

To draw: The Lewis structures of the given compounds.

Interpretation: The Lewis structures of the given compounds are to be drawn.

Concept introduction: The Lewis structure shows the connectivity between atoms by identifying the lone pairs of electrons in a compound. Lewis structures are also called Lewis dot structures. The valence electrons around an atom are shown by dots. Bonds between atoms are shown by lines and the lone pair of electrons is shown by a pair of dots.

The rules to draw Lewis structure are given as,

Determine the electronegativity and the number of valence electrons contributed by each atom.

Generally lowest electronegativity atom is the central atom.

Write the skeleton structure of the molecule.

Use two valence electrons to form each bond in skeleton structure between the central and outer atoms.

Satisfy the octets of atoms by distributing remaining valence electrons as nonbonding electrons. It is usually best start with the outer atoms.

Answer 8

2.

Interpretation Introduction

To show: The kinds of orbitals that overlap to form each bond in the given compounds.

Interpretation: The kinds of orbitals that overlap to form each bond in the given compounds are to be shown.

Concept introduction: In the sigma bond formation hybridized orbitals overlap with other hybridized or unhybridized orbitals. In the formation of pi bonds only unhybridized orbitals are involved.

Answer 9

2.

Interpretation Introduction

To show: The kinds of orbitals that overlap to form each bond in the given compounds.

Interpretation: The kinds of orbitals that overlap to form each bond in the given compounds are to be shown.

Concept introduction: In the sigma bond formation hybridized orbitals overlap with other hybridized or unhybridized orbitals. In the formation of pi bonds only unhybridized orbitals are involved.

Answer 10

3.

Interpretation Introduction

To determine: The approximate bond angles in the given compounds.

Interpretation: The approximate bond angles in the given compounds are to be stated.

Concept introduction: All the carbon atoms with single bond formation always arranged in tetrahedral manner. In tetrahedral arrangement the bond angles between the atoms is always 109° 28'. This angle is thermodynamically more stable angle for tetrahedrally arranged atoms.

The actual bond angles in “sp”, “sp2” and “sp3” hybridization are 180°, 120° and 109.5° respectively.

Answer 11

3.

Interpretation Introduction

To determine: The approximate bond angles in the given compounds.

Interpretation: The approximate bond angles in the given compounds are to be stated.

Concept introduction: All the carbon atoms with single bond formation always arranged in tetrahedral manner. In tetrahedral arrangement the bond angles between the atoms is always 109° 28'. This angle is thermodynamically more stable angle for tetrahedrally arranged atoms.

The actual bond angles in “sp”, “sp2” and “sp3” hybridization are 180°, 120° and 109.5° respectively.

Answer 12

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Answer 13

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Answer 14

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Answer 15

Ch. 1.2C - a. Nitrogen has relatively stable isotopes...Ch. 1.4 - Draw Lewis structures for the following compounds....Ch. 1.5 - Write Lewis structures for the following molecular...Ch. 1.5 - Circle any lone pairs (pairs of nonbonding...Ch. 1.6 - Use electronegativities to predict the direction...Ch. 1.8 - Prob. 1.6P Ch. 1.9B - Draw the important resonance forms for the...Ch. 1.9B - Prob. 1.8P Ch. 1.9B - Prob. 1.9P Ch. 1.9B - Use resonance structures to identify the areas of...

Solution Summary: The author explains how to draw the Lewis structures of the given compounds.

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