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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3. Propose a synthesis for the following transformation. Do not draw an arrow-pushing mechanism below, but make sure to draw the product of each proposed step (3 points). CN + En CN

3) Propagation of uncertainty. Every measurement has uncertainty. In this problem, we'll evaluate the uncertainty in every step of a titration of potassium hydrogen phthalate (a common acid used in titrations, abbreviated KHP, formula CsH5KO4) with NaOH of an unknown concentration. The calculation that ultimately needs to be carried out is: concentration NaOH 1000 x mass KHP × purity KHP molar mass KHP x volume NaOH Measurements: a) You use a balance to weigh 0.3992 g of KHP. The uncertainty is ±0.15 mg (0.00015 g). b) You use a buret to slowly add NaOH to the KHP until it reaches the endpoint. It takes 18.73 mL of NaOH. The uncertainty of the burst is 0.03 mL.. c) The manufacturer states the purity of KHP is 100%±0.05%. d) Even though we don't think much about them, molar masses have uncertainty as well. The uncertainty comes from the distribution of isotopes, rather than random measurement error. The uncertainty in the elements composing KHP are: a. Carbon: b. Hydrogen: ±0.0008…

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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.

Expert Solution & Answer

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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.

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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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