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

Concentration Trial1 Concentration of iodide solution (mA) 255.8 Concentration of thiosulfate solution (mM) 47.0 Concentration of hydrogen peroxide solution (mM) 110.1 Temperature of iodide solution ('C) 25.0 Volume of iodide solution (1) used (mL) 10.0 Volume of thiosulfate solution (5:03) used (mL) Volume of DI water used (mL) Volume of hydrogen peroxide solution (H₂O₂) used (mL) 1.0 2.5 7.5 Time (s) 16.9 Dark blue Observations Initial concentration of iodide in reaction (mA) Initial concentration of thiosulfate in reaction (mA) Initial concentration of hydrogen peroxide in reaction (mA) Initial Rate (mA's)

Draw the condensed or line-angle structure for an alkene with the formula C5H10. Note: Avoid selecting cis-/trans- isomers in this exercise. Draw two additional condensed or line-angle structures for alkenes with the formula C5H10. Record the name of the isomers in Data Table 1. Repeat steps for 2 cyclic isomers of C5H10

Explain why the following names of the structures are incorrect. CH2CH3 CH3-C=CH-CH2-CH3 a. 2-ethyl-2-pentene CH3 | CH3-CH-CH2-CH=CH2 b. 2-methyl-4-pentene

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)