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.

Question

Want to see the full answer?

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)

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Students have asked these similar questions

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.

Write the Lewis structures for the following, and include resonance structures where appropriate. Indicate which has the strongest carbon-oxygen bond.(a) CO2(b) CO

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)

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

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)

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

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)

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

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

Expert Solution & Answer

Answer 13

Expert Solution & Answer

Answer 14

Want to see the full answer?

Check out a sample textbook solution

See solution

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)

Want to see the full answer?

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)

Want to see the full answer?

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)