The Lewis structure of CN − has to be determined. Concept Introduction: 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. A polar bond is a type of chemical bond where pair of electrons are unequally shared between two atoms. Polar molecules must contain polar bonds that form due to difference in electronegativity between the bonded atoms. The larger difference in electronegativity accounts for the more polar bond.

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Answer 1

Question

Chapter 9, Problem 9.40QE

(a)

Interpretation Introduction

Interpretation:

The Lewis structure of CN− has to be determined.

Concept Introduction:

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.

A polar bond is a type of chemical bond where pair of electrons are unequally shared between two atoms. Polar molecules must contain polar bonds that form due to difference in electronegativity between the bonded atoms. The larger difference in electronegativity accounts for the more polar bond.

(b)

Interpretation Introduction

Interpretation:

The Lewis structure of C2F4 has to be determined.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The Lewis structure of CH2CHCN has to be determined.

Concept Introduction:

Refer to part (a)

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Students have asked these similar questions

Na+ forms an “ionic bond” (i.e. an electrostatic attraction) with the OCN− ion. (a) Draw the full Lewis structure of the ionic compound. Be sure to show how you have derived this. (b) Which atom in the OCN− anion is the sodium cation most likely to attract? Explain.

A certain element, M, is a main-group metal that reacts with chlorine to give a compound with the chemical formula MCl2 and with oxygen to give the compound MO.(a) To which group in the periodic table does element M belong?(b) The chloride contains 44.7% chlorine by mass. Name the element M

2. Draw the Lewis structures for each of the following ions or molecules. Give the number of electrons in each species. Remember to enclose ions in square brackets with the charge as a superscript outside the right bracket. (a) Br 20 (c) BrF 3 (e) PCI 4* (b) IOF 3 (I is the central atom) (d) ASF 3

Answer 2

Question

Chapter 9, Problem 9.40QE

(a)

Interpretation Introduction

Interpretation:

The Lewis structure of CN− has to be determined.

Concept Introduction:

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.

A polar bond is a type of chemical bond where pair of electrons are unequally shared between two atoms. Polar molecules must contain polar bonds that form due to difference in electronegativity between the bonded atoms. The larger difference in electronegativity accounts for the more polar bond.

(b)

Interpretation Introduction

Interpretation:

The Lewis structure of C2F4 has to be determined.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The Lewis structure of CH2CHCN has to be determined.

Concept Introduction:

Refer to part (a)

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Answer 3

Question

Chapter 9, Problem 9.40QE

(a)

Interpretation Introduction

Interpretation:

The Lewis structure of CN− has to be determined.

Concept Introduction:

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.

A polar bond is a type of chemical bond where pair of electrons are unequally shared between two atoms. Polar molecules must contain polar bonds that form due to difference in electronegativity between the bonded atoms. The larger difference in electronegativity accounts for the more polar bond.

(b)

Interpretation Introduction

Interpretation:

The Lewis structure of C2F4 has to be determined.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The Lewis structure of CH2CHCN has to be determined.

Concept Introduction:

Refer to part (a)

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Answer 4

Question

Chapter 9, Problem 9.40QE

(a)

Interpretation Introduction

Interpretation:

The Lewis structure of CN− has to be determined.

Concept Introduction:

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.

A polar bond is a type of chemical bond where pair of electrons are unequally shared between two atoms. Polar molecules must contain polar bonds that form due to difference in electronegativity between the bonded atoms. The larger difference in electronegativity accounts for the more polar bond.

(b)

Interpretation Introduction

Interpretation:

The Lewis structure of C2F4 has to be determined.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The Lewis structure of CH2CHCN has to be determined.

Concept Introduction:

Refer to part (a)

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Answer 5

Chapter 9, Problem 9.40QE

(a)

Interpretation Introduction

Interpretation:

The Lewis structure of CN− has to be determined.

Concept Introduction:

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.

A polar bond is a type of chemical bond where pair of electrons are unequally shared between two atoms. Polar molecules must contain polar bonds that form due to difference in electronegativity between the bonded atoms. The larger difference in electronegativity accounts for the more polar bond.

(b)

Interpretation Introduction

Interpretation:

The Lewis structure of C2F4 has to be determined.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The Lewis structure of CH2CHCN has to be determined.

Concept Introduction:

Refer to part (a)

Answer 6

Chapter 9, Problem 9.40QE

(a)

Interpretation Introduction

Interpretation:

The Lewis structure of CN− has to be determined.

Concept Introduction:

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.

A polar bond is a type of chemical bond where pair of electrons are unequally shared between two atoms. Polar molecules must contain polar bonds that form due to difference in electronegativity between the bonded atoms. The larger difference in electronegativity accounts for the more polar bond.

Answer 7

Chapter 9, Problem 9.40QE

(a)

Interpretation Introduction

Interpretation:

The Lewis structure of CN− has to be determined.

Concept Introduction:

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.

A polar bond is a type of chemical bond where pair of electrons are unequally shared between two atoms. Polar molecules must contain polar bonds that form due to difference in electronegativity between the bonded atoms. The larger difference in electronegativity accounts for the more polar bond.

Answer 8

(b)

Interpretation Introduction

Interpretation:

The Lewis structure of C2F4 has to be determined.

Concept Introduction:

Refer to part (a).

Answer 9

(b)

Interpretation Introduction

Interpretation:

The Lewis structure of C2F4 has to be determined.

Concept Introduction:

Refer to part (a).

Answer 10

(c)

Interpretation Introduction

Interpretation:

The Lewis structure of CH2CHCN has to be determined.

Concept Introduction:

Refer to part (a)

Answer 11

(c)

Interpretation Introduction

Interpretation:

The Lewis structure of CH2CHCN 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 Lewis symbols show how the valence electrons are present in a molecule.

Concept explainers

Videos

Interpretation:

The Lewis structure of C2F4 has to be determined.

Concept Introduction:

Refer to part (a).

Interpretation:

The Lewis structure of CH2CHCN has to be determined.

Concept Introduction:

Refer to part (a)

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Chapter 9 Solutions

Solution Summary: The author explains how Lewis symbols show how the valence electrons are present in a molecule.

Concept explainers

Videos

Interpretation: The Lewis structure of C2F4 has to be determined. Concept Introduction: Refer to part (a).

Interpretation: The Lewis structure of CH2CHCN has to be determined. Concept Introduction: Refer to part (a)

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Chapter 9 Solutions

Interpretation:

The Lewis structure of C2F4 has to be determined.

Concept Introduction:

Refer to part (a).

Interpretation:

The Lewis structure of CH2CHCN has to be determined.

Concept Introduction:

Refer to part (a)