The Lewis structure of SeF 6 has to be determined. Also, whether SeF 6 is an odd-electron molecule, an electron-deficient molecule, or an expanded valence shell molecule has to be determined. Concept Introduction: A covalent bond is a bond that is formed from the mutual sharing of electrons between atoms. Lewis structures are representations of the covalent bond. In this, Lewis symbols show how the valence electrons are present in the molecule. Steps to write Lewis structures are as follows: 1. The skeleton structure with single bonds between all bonded atoms has to be written 2. Sum the valence electrons of the atoms in the molecule. (a) For cations, one electron is subtracted for each positive charge. (b) For anions, one electron is added for each negative charge. 3. Subtract two electrons from total number of valence electrons for each bond in the skeleton structure. 4. Count the number of electrons required to satisfy the octet rule for each atom in the structure. If the number of electrons needed is less than the number remaining, add one bond for every two electrons needed between atoms to attain an octet. 5. The remaining electrons are placed as lone pairs on atoms that need them to satisfy the octet rule. Some compounds exceed an octet around the central atom and are called as expanded valence shell molecule. The central atom belongs to third and fourth periods. In this, the molecule has electrons more than eight electrons in Lewis structure. The electron-deficient molecule is a molecule in which there are less electrons than electrons available that join atoms in the molecule through covalent bonds. In electron-deficient molecules, atoms have more stable orbitals in the valence shell than the electrons. Odd-electron molecules are atoms with unpaired electrons. They are also called as radicals. Radicals do not obey the octet rule because they do not have completely filled s and p subshell.

Question

Which of the following molecules or ions contain polar bonds?(a) O3(b) S8(c) O22−(d) NO3−(e) CO2(f) H2S(g) BH4−

Answer 1

Question

Chapter 9, Problem 9.75QE

(a)

Interpretation Introduction

Interpretation:

The Lewis structure of SeF6 has to be determined. Also, whether SeF6 is an odd-electron molecule, an electron-deficient molecule, or an expanded valence shell molecule has to be determined.

Concept Introduction:

A covalent bond is a bond that is formed from the mutual sharing of electrons between atoms. Lewis structures are representations of the covalent bond. In this, Lewis symbols show how the valence electrons are present in the molecule.

Steps to write Lewis structures are as follows:

1. The skeleton structure with single bonds between all bonded atoms has to be written

2. Sum the valence electrons of the atoms in the molecule.

(a) For cations, one electron is subtracted for each positive charge.

(b) For anions, one electron is added for each negative charge.

3. Subtract two electrons from total number of valence electrons for each bond in the skeleton structure.

4. Count the number of electrons required to satisfy the octet rule for each atom in the structure. If the number of electrons needed is less than the number remaining, add one bond for every two electrons needed between atoms to attain an octet.

5. The remaining electrons are placed as lone pairs on atoms that need them to satisfy the octet rule.

Some compounds exceed an octet around the central atom and are called as expanded valence shell molecule. The central atom belongs to third and fourth periods. In this, the molecule has electrons more than eight electrons in Lewis structure.

The electron-deficient molecule is a molecule in which there are less electrons than electrons available that join atoms in the molecule through covalent bonds. In electron-deficient molecules, atoms have more stable orbitals in the valence shell than the electrons.

Odd-electron molecules are atoms with unpaired electrons. They are also called as radicals. Radicals do not obey the octet rule because they do not have completely filled s and p subshell.

(b)

Interpretation Introduction

Interpretation:

The Lewis structure of BBr3 has to be determined. Also, whether BBr3 is an odd-electron molecule, an electron-deficient molecule, or an expanded valence shell molecule has to be determined.

Concept Introduction:

Refer to part (a)

(c)

Interpretation Introduction

Interpretation:

The Lewis structure made from NO2 has to be determined. Also, whether NO2 is an odd-electron molecule, an electron-deficient molecule, or an expanded valence shell molecule has to be determined.

Concept Introduction:

Refer to part (a)

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Which of the following molecules or ions contain polar bonds?(a) O3(b) S8(c) O22−(d) NO3−(e) CO2(f) H2S(g) BH4−

Identify the electron pair geometry and the molecular structure of each of the following molecules or ions:(a) IF6+(b) CF4(c) BF3(d) SiF5−(e) BeCl2

Three main group elements, X, Y and Z, from three different groups inthe Periodic Table, each form a neutral trifluoride, i.e. XF3, YF3 andZF3. (a) To which three groups of the Periodic Table could the elementsX, Y and Z belong? Are any of these atoms X, Y or Zhypervalent in the trifluorides formed? (b) Use VSEPR theory to deduce the shapes of the molecules XF3,YF3 and ZF3, showing full working, and sketch these shapes (c) Only two of the three trifluorides have a non-zero dipole moment.For these molecules to which groups of the Periodic Table do thecentral atoms belong?

Answer 2

Question

Chapter 9, Problem 9.75QE

(a)

Interpretation Introduction

Interpretation:

The Lewis structure of SeF6 has to be determined. Also, whether SeF6 is an odd-electron molecule, an electron-deficient molecule, or an expanded valence shell molecule has to be determined.

Concept Introduction:

A covalent bond is a bond that is formed from the mutual sharing of electrons between atoms. Lewis structures are representations of the covalent bond. In this, Lewis symbols show how the valence electrons are present in the molecule.

Steps to write Lewis structures are as follows:

1. The skeleton structure with single bonds between all bonded atoms has to be written

2. Sum the valence electrons of the atoms in the molecule.

(a) For cations, one electron is subtracted for each positive charge.

(b) For anions, one electron is added for each negative charge.

3. Subtract two electrons from total number of valence electrons for each bond in the skeleton structure.

4. Count the number of electrons required to satisfy the octet rule for each atom in the structure. If the number of electrons needed is less than the number remaining, add one bond for every two electrons needed between atoms to attain an octet.

5. The remaining electrons are placed as lone pairs on atoms that need them to satisfy the octet rule.

Some compounds exceed an octet around the central atom and are called as expanded valence shell molecule. The central atom belongs to third and fourth periods. In this, the molecule has electrons more than eight electrons in Lewis structure.

The electron-deficient molecule is a molecule in which there are less electrons than electrons available that join atoms in the molecule through covalent bonds. In electron-deficient molecules, atoms have more stable orbitals in the valence shell than the electrons.

Odd-electron molecules are atoms with unpaired electrons. They are also called as radicals. Radicals do not obey the octet rule because they do not have completely filled s and p subshell.

(b)

Interpretation Introduction

Interpretation:

The Lewis structure of BBr3 has to be determined. Also, whether BBr3 is an odd-electron molecule, an electron-deficient molecule, or an expanded valence shell molecule has to be determined.

Concept Introduction:

Refer to part (a)

(c)

Interpretation Introduction

Interpretation:

The Lewis structure made from NO2 has to be determined. Also, whether NO2 is an odd-electron molecule, an electron-deficient molecule, or an expanded valence shell molecule has to be determined.

Concept Introduction:

Refer to part (a)

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Answer 3

Question

Chapter 9, Problem 9.75QE

(a)

Interpretation Introduction

Interpretation:

The Lewis structure of SeF6 has to be determined. Also, whether SeF6 is an odd-electron molecule, an electron-deficient molecule, or an expanded valence shell molecule has to be determined.

Concept Introduction:

A covalent bond is a bond that is formed from the mutual sharing of electrons between atoms. Lewis structures are representations of the covalent bond. In this, Lewis symbols show how the valence electrons are present in the molecule.

Steps to write Lewis structures are as follows:

1. The skeleton structure with single bonds between all bonded atoms has to be written

2. Sum the valence electrons of the atoms in the molecule.

(a) For cations, one electron is subtracted for each positive charge.

(b) For anions, one electron is added for each negative charge.

3. Subtract two electrons from total number of valence electrons for each bond in the skeleton structure.

4. Count the number of electrons required to satisfy the octet rule for each atom in the structure. If the number of electrons needed is less than the number remaining, add one bond for every two electrons needed between atoms to attain an octet.

5. The remaining electrons are placed as lone pairs on atoms that need them to satisfy the octet rule.

Some compounds exceed an octet around the central atom and are called as expanded valence shell molecule. The central atom belongs to third and fourth periods. In this, the molecule has electrons more than eight electrons in Lewis structure.

The electron-deficient molecule is a molecule in which there are less electrons than electrons available that join atoms in the molecule through covalent bonds. In electron-deficient molecules, atoms have more stable orbitals in the valence shell than the electrons.

Odd-electron molecules are atoms with unpaired electrons. They are also called as radicals. Radicals do not obey the octet rule because they do not have completely filled s and p subshell.

(b)

Interpretation Introduction

Interpretation:

The Lewis structure of BBr3 has to be determined. Also, whether BBr3 is an odd-electron molecule, an electron-deficient molecule, or an expanded valence shell molecule has to be determined.

Concept Introduction:

Refer to part (a)

(c)

Interpretation Introduction

Interpretation:

The Lewis structure made from NO2 has to be determined. Also, whether NO2 is an odd-electron molecule, an electron-deficient molecule, or an expanded valence shell molecule has to be determined.

Concept Introduction:

Refer to part (a)

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Answer 4

Question

Chapter 9, Problem 9.75QE

(a)

Interpretation Introduction

Interpretation:

The Lewis structure of SeF6 has to be determined. Also, whether SeF6 is an odd-electron molecule, an electron-deficient molecule, or an expanded valence shell molecule has to be determined.

Concept Introduction:

A covalent bond is a bond that is formed from the mutual sharing of electrons between atoms. Lewis structures are representations of the covalent bond. In this, Lewis symbols show how the valence electrons are present in the molecule.

Steps to write Lewis structures are as follows:

1. The skeleton structure with single bonds between all bonded atoms has to be written

2. Sum the valence electrons of the atoms in the molecule.

(a) For cations, one electron is subtracted for each positive charge.

(b) For anions, one electron is added for each negative charge.

3. Subtract two electrons from total number of valence electrons for each bond in the skeleton structure.

4. Count the number of electrons required to satisfy the octet rule for each atom in the structure. If the number of electrons needed is less than the number remaining, add one bond for every two electrons needed between atoms to attain an octet.

5. The remaining electrons are placed as lone pairs on atoms that need them to satisfy the octet rule.

Some compounds exceed an octet around the central atom and are called as expanded valence shell molecule. The central atom belongs to third and fourth periods. In this, the molecule has electrons more than eight electrons in Lewis structure.

The electron-deficient molecule is a molecule in which there are less electrons than electrons available that join atoms in the molecule through covalent bonds. In electron-deficient molecules, atoms have more stable orbitals in the valence shell than the electrons.

Odd-electron molecules are atoms with unpaired electrons. They are also called as radicals. Radicals do not obey the octet rule because they do not have completely filled s and p subshell.

(b)

Interpretation Introduction

Interpretation:

The Lewis structure of BBr3 has to be determined. Also, whether BBr3 is an odd-electron molecule, an electron-deficient molecule, or an expanded valence shell molecule has to be determined.

Concept Introduction:

Refer to part (a)

(c)

Interpretation Introduction

Interpretation:

The Lewis structure made from NO2 has to be determined. Also, whether NO2 is an odd-electron molecule, an electron-deficient molecule, or an expanded valence shell molecule has to be determined.

Concept Introduction:

Refer to part (a)

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Answer 5

Chapter 9, Problem 9.75QE

(a)

Interpretation Introduction

Interpretation:

The Lewis structure of SeF6 has to be determined. Also, whether SeF6 is an odd-electron molecule, an electron-deficient molecule, or an expanded valence shell molecule has to be determined.

Concept Introduction:

A covalent bond is a bond that is formed from the mutual sharing of electrons between atoms. Lewis structures are representations of the covalent bond. In this, Lewis symbols show how the valence electrons are present in the molecule.

Steps to write Lewis structures are as follows:

1. The skeleton structure with single bonds between all bonded atoms has to be written

2. Sum the valence electrons of the atoms in the molecule.

(a) For cations, one electron is subtracted for each positive charge.

(b) For anions, one electron is added for each negative charge.

3. Subtract two electrons from total number of valence electrons for each bond in the skeleton structure.

4. Count the number of electrons required to satisfy the octet rule for each atom in the structure. If the number of electrons needed is less than the number remaining, add one bond for every two electrons needed between atoms to attain an octet.

5. The remaining electrons are placed as lone pairs on atoms that need them to satisfy the octet rule.

Some compounds exceed an octet around the central atom and are called as expanded valence shell molecule. The central atom belongs to third and fourth periods. In this, the molecule has electrons more than eight electrons in Lewis structure.

The electron-deficient molecule is a molecule in which there are less electrons than electrons available that join atoms in the molecule through covalent bonds. In electron-deficient molecules, atoms have more stable orbitals in the valence shell than the electrons.

Odd-electron molecules are atoms with unpaired electrons. They are also called as radicals. Radicals do not obey the octet rule because they do not have completely filled s and p subshell.

(b)

Interpretation Introduction

Interpretation:

The Lewis structure of BBr3 has to be determined. Also, whether BBr3 is an odd-electron molecule, an electron-deficient molecule, or an expanded valence shell molecule has to be determined.

Concept Introduction:

Refer to part (a)

(c)

Interpretation Introduction

Interpretation:

The Lewis structure made from NO2 has to be determined. Also, whether NO2 is an odd-electron molecule, an electron-deficient molecule, or an expanded valence shell molecule has to be determined.

Concept Introduction:

Refer to part (a)

Answer 6

Chapter 9, Problem 9.75QE

(a)

Interpretation Introduction

Interpretation:

The Lewis structure of SeF6 has to be determined. Also, whether SeF6 is an odd-electron molecule, an electron-deficient molecule, or an expanded valence shell molecule has to be determined.

Concept Introduction:

A covalent bond is a bond that is formed from the mutual sharing of electrons between atoms. Lewis structures are representations of the covalent bond. In this, Lewis symbols show how the valence electrons are present in the molecule.

Steps to write Lewis structures are as follows:

1. The skeleton structure with single bonds between all bonded atoms has to be written

2. Sum the valence electrons of the atoms in the molecule.

(a) For cations, one electron is subtracted for each positive charge.

(b) For anions, one electron is added for each negative charge.

3. Subtract two electrons from total number of valence electrons for each bond in the skeleton structure.

4. Count the number of electrons required to satisfy the octet rule for each atom in the structure. If the number of electrons needed is less than the number remaining, add one bond for every two electrons needed between atoms to attain an octet.

5. The remaining electrons are placed as lone pairs on atoms that need them to satisfy the octet rule.

Some compounds exceed an octet around the central atom and are called as expanded valence shell molecule. The central atom belongs to third and fourth periods. In this, the molecule has electrons more than eight electrons in Lewis structure.

The electron-deficient molecule is a molecule in which there are less electrons than electrons available that join atoms in the molecule through covalent bonds. In electron-deficient molecules, atoms have more stable orbitals in the valence shell than the electrons.

Odd-electron molecules are atoms with unpaired electrons. They are also called as radicals. Radicals do not obey the octet rule because they do not have completely filled s and p subshell.

Answer 7

Chapter 9, Problem 9.75QE

(a)

Interpretation Introduction

Interpretation:

The Lewis structure of SeF6 has to be determined. Also, whether SeF6 is an odd-electron molecule, an electron-deficient molecule, or an expanded valence shell molecule has to be determined.

Concept Introduction:

A covalent bond is a bond that is formed from the mutual sharing of electrons between atoms. Lewis structures are representations of the covalent bond. In this, Lewis symbols show how the valence electrons are present in the molecule.

Steps to write Lewis structures are as follows:

1. The skeleton structure with single bonds between all bonded atoms has to be written

2. Sum the valence electrons of the atoms in the molecule.

(a) For cations, one electron is subtracted for each positive charge.

(b) For anions, one electron is added for each negative charge.

3. Subtract two electrons from total number of valence electrons for each bond in the skeleton structure.

4. Count the number of electrons required to satisfy the octet rule for each atom in the structure. If the number of electrons needed is less than the number remaining, add one bond for every two electrons needed between atoms to attain an octet.

5. The remaining electrons are placed as lone pairs on atoms that need them to satisfy the octet rule.

Some compounds exceed an octet around the central atom and are called as expanded valence shell molecule. The central atom belongs to third and fourth periods. In this, the molecule has electrons more than eight electrons in Lewis structure.

The electron-deficient molecule is a molecule in which there are less electrons than electrons available that join atoms in the molecule through covalent bonds. In electron-deficient molecules, atoms have more stable orbitals in the valence shell than the electrons.

Odd-electron molecules are atoms with unpaired electrons. They are also called as radicals. Radicals do not obey the octet rule because they do not have completely filled s and p subshell.

Answer 8

(b)

Interpretation Introduction

Interpretation:

The Lewis structure of BBr3 has to be determined. Also, whether BBr3 is an odd-electron molecule, an electron-deficient molecule, or an expanded valence shell molecule has to be determined.

Concept Introduction:

Refer to part (a)

Answer 9

(b)

Interpretation Introduction

Interpretation:

The Lewis structure of BBr3 has to be determined. Also, whether BBr3 is an odd-electron molecule, an electron-deficient molecule, or an expanded valence shell molecule has to be determined.

Concept Introduction:

Refer to part (a)

Answer 10

(c)

Interpretation Introduction

Interpretation:

The Lewis structure made from NO2 has to be determined. Also, whether NO2 is an odd-electron molecule, an electron-deficient molecule, or an expanded valence shell molecule has to be determined.

Concept Introduction:

Refer to part (a)

Answer 11

(c)

Interpretation Introduction

Interpretation:

The Lewis structure made from NO2 has to be determined. Also, whether NO2 is an odd-electron molecule, an electron-deficient molecule, or an expanded valence shell molecule has to be determined.

Concept Introduction:

Refer to part (a)

Answer 12

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Answer 13

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Ch. 9 - Prob. 9.1QE Ch. 9 - Prob. 9.2QE Ch. 9 - Prob. 9.3QE Ch. 9 - What main factors control the magnitude of lattice...Ch. 9 - Prob. 9.5QE Ch. 9 - Prob. 9.6QE Ch. 9 - Prob. 9.7QE Ch. 9 - Prob. 9.8QE Ch. 9 - Prob. 9.9QE Ch. 9 - Prob. 9.10QE

Solution Summary: The author explains how the Lewis structure of SeF_6 has to be determined.

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Interpretation:

The Lewis structure of BBr3 has to be determined. Also, whether BBr3 is an odd-electron molecule, an electron-deficient molecule, or an expanded valence shell molecule has to be determined.

Concept Introduction:

Refer to part (a)

Interpretation:

The Lewis structure made from NO2 has to be determined. Also, whether NO2 is an odd-electron molecule, an electron-deficient molecule, or an expanded valence shell molecule has to be determined.

Concept Introduction:

Refer to part (a)

Chapter 9 Solutions

Solution Summary: The author explains how the Lewis structure of SeF_6 has to be determined.

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Interpretation: The Lewis structure of BBr3 has to be determined. Also, whether BBr3 is an odd-electron molecule, an electron-deficient molecule, or an expanded valence shell molecule has to be determined. Concept Introduction: Refer to part (a)

Interpretation: The Lewis structure made from NO2 has to be determined. Also, whether NO2 is an odd-electron molecule, an electron-deficient molecule, or an expanded valence shell molecule has to be determined. Concept Introduction: Refer to part (a)

Chapter 9 Solutions

Interpretation:

The Lewis structure of BBr3 has to be determined. Also, whether BBr3 is an odd-electron molecule, an electron-deficient molecule, or an expanded valence shell molecule has to be determined.

Concept Introduction:

Refer to part (a)

Interpretation:

The Lewis structure made from NO2 has to be determined. Also, whether NO2 is an odd-electron molecule, an electron-deficient molecule, or an expanded valence shell molecule has to be determined.

Concept Introduction:

Refer to part (a)