The Lewis structure of IF 3 has to be determined. Also, whether IF 3 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.

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Answer 1

Question

Chapter 9, Problem 9.76QE

(a)

Interpretation Introduction

Interpretation:

The Lewis structure of IF3 has to be determined. Also, whether IF3 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 ICl4− has to be determined. Also, whether ICl4− 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 of N2+ has to be determined. Also, whether N2+ 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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Two substances with empirical formula HNO are hyponi-trous acid ( μ=62.04 g /mol) and nitroxyl (μ=31.02 g/mol).(a) What is the molecular formula of each species?(b) For each species, draw the Lewis structure having the lowestformal charges. (Hint:Hyponitrous acid has an N=N bond.)(c) Predict the shape around the N atoms of each species.(d) When hyponitrous acid loses two protons, it forms the hy-ponitrite ion. Draw cisand transforms of this ion.

Cyanogen (CN)2 is known as pseodohalogen because it has some properties like halogens. It is composed of two CN’s joined together.(i) Draw the Lewis structure for all the possible combination for (CN)2.(ii) Calculate the formal charge and determine which one of the structures that you have drawn is most stable.(iii) For the stable structure, determine the geometry around the two central atoms.(iv) For the stable structure, draw the dipole arrows for the bonds.(v) Base on the stable structure, determine the polarity of molecule and state your reason.

Write Lewis structures for the following molecules or ions. (Assign lone pairs, radical electrons, and atomic charges where appropriate.) (a) SbO43− (b) ICl6− (c) SO32- (d) HOBrO

Answer 2

Question

Chapter 9, Problem 9.76QE

(a)

Interpretation Introduction

Interpretation:

The Lewis structure of IF3 has to be determined. Also, whether IF3 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 ICl4− has to be determined. Also, whether ICl4− 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 of N2+ has to be determined. Also, whether N2+ 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 9.76QE

(a)

Interpretation Introduction

Interpretation:

The Lewis structure of IF3 has to be determined. Also, whether IF3 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 ICl4− has to be determined. Also, whether ICl4− 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 of N2+ has to be determined. Also, whether N2+ 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 9.76QE

(a)

Interpretation Introduction

Interpretation:

The Lewis structure of IF3 has to be determined. Also, whether IF3 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 ICl4− has to be determined. Also, whether ICl4− 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 of N2+ has to be determined. Also, whether N2+ 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 9.76QE

(a)

Interpretation Introduction

Interpretation:

The Lewis structure of IF3 has to be determined. Also, whether IF3 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 ICl4− has to be determined. Also, whether ICl4− 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 of N2+ has to be determined. Also, whether N2+ 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 9.76QE

(a)

Interpretation Introduction

Interpretation:

The Lewis structure of IF3 has to be determined. Also, whether IF3 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 9.76QE

(a)

Interpretation Introduction

Interpretation:

The Lewis structure of IF3 has to be determined. Also, whether IF3 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 ICl4− has to be determined. Also, whether ICl4− 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 ICl4− has to be determined. Also, whether ICl4− 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 of N2+ has to be determined. Also, whether N2+ 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 of N2+ has to be determined. Also, whether N2+ 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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Answer 14

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Answer 15

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 IF_3 has to be determined.

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Interpretation:

The Lewis structure of ICl4− has to be determined. Also, whether ICl4− 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 of N2+ has to be determined. Also, whether N2+ 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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Chapter 9 Solutions

Solution Summary: The author explains how the Lewis structure of IF_3 has to be determined.

Concept explainers

Videos

Interpretation: The Lewis structure of ICl4− has to be determined. Also, whether ICl4− 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 of N2+ has to be determined. Also, whether N2+ 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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Chapter 9 Solutions

Interpretation:

The Lewis structure of ICl4− has to be determined. Also, whether ICl4− 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 of N2+ has to be determined. Also, whether N2+ 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)