(a) Interpretation: Bonds formed between H and Br should be classified as polarcovalent or ionic based on the electronegativity of atoms. Concept Introduction: The electronegativity of atoms defines the bond characteristics, as the electron distribution of the bond can be predicted by electronegativity. Electronegativity is tendency to pull bond electrons towards an atom. Electronegativity difference between bonded atoms defines the nature of bond as stated in the following table. Electronegativity difference Type of bond Electron distribution in bond. 0.5 > Nonpolar Electrons are equally distributed. 0.5 -1.9 Polar covalent Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom). 1.9 ≤ Ionic Electron has been donated to the more electronegative atom from less electronegative atom.

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Answer 1

Question

Chapter 4, Problem 4.73P

Interpretation Introduction

(a)

Interpretation:

Bonds formed between H and Br should be classified as polarcovalent or ionic based on the electronegativity of atoms.

Concept Introduction:

The electronegativity of atoms defines the bond characteristics, as the electron distribution of the bond can be predicted by electronegativity. Electronegativity is tendency to pull bond electrons towards an atom. Electronegativity difference between bonded atoms defines the nature of bond as stated in the following table.

Electronegativity difference Type of bond Electron distribution in bond.
0.5 > Nonpolar Electrons are equally distributed.
0.5 -1.9 Polar covalent Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤ Ionic Electron has been donated to the more electronegative atom from less electronegative atom.

Expert Solution

Answer to Problem 4.73P

The bond between H and Br atom is polar covalent.

Explanation of Solution

The electronegativity of H and Br atom is 2.1 and 2.8 respectively. The electronegativity difference will be 0.7.

Since,

Electronegativity difference	Type of bond	Electron distribution in bond.
0.5 >	Nonpolar	Electrons are equally distributed.
0.5 -1.9	Polar covalent	Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤	Ionic	Electron has been donated to the more electronegative atom from less electronegative atom.

Thus, the bond will be polar covalent in nature.

Interpretation Introduction

(b)

Interpretation:

Bonds formed between Na and S should be classified as polar covalent or ionic based on the electronegativity of atoms.

Concept Introduction:

The electronegativity of atoms defines the bond characteristics, as the electron distribution of the bond can be predicted by electronegativity. Electronegativity is tendency to pull bond electrons towards an atom. Electronegativity difference between bonded atoms defines the nature of bond as stated in the following table.

Electronegativity difference Type of bond Electron distribution in bond.
0.5 > Nonpolar Electrons are equally distributed.
0.5 -1.9 Polar covalent Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤ Ionic Electron has been donated to the more electronegative atom from less electronegative atom.

Expert Solution

Answer to Problem 4.73P

The bond between Na and S atom is polar covalent.

Explanation of Solution

The electronegativity of Na and S atom is 0.9 and 2.5 respectively. The electronegativity difference will be 1.6.

Since,

Electronegativity difference	Type of bond	Electron distribution in bond.
0.5 >	Nonpolar	Electrons are equally distributed.
0.5 -1.9	Polar covalent	Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤	Ionic	Electron has been donated to the more electronegative atom from less electronegative atom.

Thus, the bond will be polar covalent in nature.

Interpretation Introduction

(c)

Interpretation:

Bonds formed between N and C should be classified as polar covalent or ionic based on the electronegativity of atoms.

Concept Introduction:

The electronegativity of atoms defines the bond characteristics, as the electron distribution of the bond can be predicted by electronegativity. Electronegativity is tendency to pull bond electrons towards an atom. Electronegativity difference between bonded atoms defines the nature of bond as stated in the following table.

Electronegativity difference Type of bond Electron distribution in bond.
0.5 > Nonpolar Electrons are equally distributed.
0.5 -1.9 Polar covalent Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤ Ionic Electron has been donated to the more electronegative atom from less electronegative atom.

Expert Solution

Answer to Problem 4.73P

The bond between N and C atom is polar covalent.

Explanation of Solution

The electronegativity of N and C atom is 3.0 and 2.7 respectively. The electronegativity difference will be 0.5.

Since,

Electronegativity difference	Type of bond	Electron distribution in bond.
0.5 >	Nonpolar	Electrons are equally distributed.
0.5 -1.9	Polar covalent	Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤	Ionic	Electron has been donated to the more electronegative atom from less electronegative atom.

Thus, the bond will be polar covalent in nature.

Interpretation Introduction

(d)

Interpretation:

Bonds formed between Li and O should be classified as polar covalent or ionic based on the electronegativity of atoms.

Concept Introduction:

The electronegativity of atoms defines the bond characteristics, as the electron distribution of the bond can be predicted by electronegativity. Electronegativity is tendency to pull bond electrons towards an atom. Electronegativity difference between bonded atoms defines the nature of bond as stated in the following table.

Electronegativity difference Type of bond Electron distribution in bond.
0.5 > Nonpolar Electrons are equally distributed.
0.5 -1.9 Polar covalent Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤ Ionic Electron has been donated to the more electronegative atom from less electronegative atom.

Expert Solution

Answer to Problem 4.73P

The bond between Li and O is ionic.

Explanation of Solution

The electronegativity of Li and O atom is 1.0 and 3.5 respectively. The electronegativity difference will be 2.5.

Since,

Electronegativity difference	Type of bond	Electron distribution in bond.
0.5 >	Nonpolar	Electrons are equally distributed.
0.5 -1.9	Polar covalent	Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤	Ionic	Electron has been donated to the more electronegative atom from less electronegative atom.

Thus, the bond will be ionic in nature.

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Answer 2

Question

Chapter 4, Problem 4.73P

Interpretation Introduction

(a)

Interpretation:

Bonds formed between H and Br should be classified as polarcovalent or ionic based on the electronegativity of atoms.

Concept Introduction:

The electronegativity of atoms defines the bond characteristics, as the electron distribution of the bond can be predicted by electronegativity. Electronegativity is tendency to pull bond electrons towards an atom. Electronegativity difference between bonded atoms defines the nature of bond as stated in the following table.

Electronegativity difference Type of bond Electron distribution in bond.
0.5 > Nonpolar Electrons are equally distributed.
0.5 -1.9 Polar covalent Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤ Ionic Electron has been donated to the more electronegative atom from less electronegative atom.

Expert Solution

Answer to Problem 4.73P

The bond between H and Br atom is polar covalent.

Explanation of Solution

The electronegativity of H and Br atom is 2.1 and 2.8 respectively. The electronegativity difference will be 0.7.

Since,

Electronegativity difference	Type of bond	Electron distribution in bond.
0.5 >	Nonpolar	Electrons are equally distributed.
0.5 -1.9	Polar covalent	Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤	Ionic	Electron has been donated to the more electronegative atom from less electronegative atom.

Thus, the bond will be polar covalent in nature.

Interpretation Introduction

(b)

Interpretation:

Bonds formed between Na and S should be classified as polar covalent or ionic based on the electronegativity of atoms.

Concept Introduction:

The electronegativity of atoms defines the bond characteristics, as the electron distribution of the bond can be predicted by electronegativity. Electronegativity is tendency to pull bond electrons towards an atom. Electronegativity difference between bonded atoms defines the nature of bond as stated in the following table.

Electronegativity difference Type of bond Electron distribution in bond.
0.5 > Nonpolar Electrons are equally distributed.
0.5 -1.9 Polar covalent Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤ Ionic Electron has been donated to the more electronegative atom from less electronegative atom.

Expert Solution

Answer to Problem 4.73P

The bond between Na and S atom is polar covalent.

Explanation of Solution

The electronegativity of Na and S atom is 0.9 and 2.5 respectively. The electronegativity difference will be 1.6.

Since,

Electronegativity difference	Type of bond	Electron distribution in bond.
0.5 >	Nonpolar	Electrons are equally distributed.
0.5 -1.9	Polar covalent	Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤	Ionic	Electron has been donated to the more electronegative atom from less electronegative atom.

Thus, the bond will be polar covalent in nature.

Interpretation Introduction

(c)

Interpretation:

Bonds formed between N and C should be classified as polar covalent or ionic based on the electronegativity of atoms.

Concept Introduction:

The electronegativity of atoms defines the bond characteristics, as the electron distribution of the bond can be predicted by electronegativity. Electronegativity is tendency to pull bond electrons towards an atom. Electronegativity difference between bonded atoms defines the nature of bond as stated in the following table.

Electronegativity difference Type of bond Electron distribution in bond.
0.5 > Nonpolar Electrons are equally distributed.
0.5 -1.9 Polar covalent Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤ Ionic Electron has been donated to the more electronegative atom from less electronegative atom.

Expert Solution

Answer to Problem 4.73P

The bond between N and C atom is polar covalent.

Explanation of Solution

The electronegativity of N and C atom is 3.0 and 2.7 respectively. The electronegativity difference will be 0.5.

Since,

Electronegativity difference	Type of bond	Electron distribution in bond.
0.5 >	Nonpolar	Electrons are equally distributed.
0.5 -1.9	Polar covalent	Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤	Ionic	Electron has been donated to the more electronegative atom from less electronegative atom.

Thus, the bond will be polar covalent in nature.

Interpretation Introduction

(d)

Interpretation:

Bonds formed between Li and O should be classified as polar covalent or ionic based on the electronegativity of atoms.

Concept Introduction:

The electronegativity of atoms defines the bond characteristics, as the electron distribution of the bond can be predicted by electronegativity. Electronegativity is tendency to pull bond electrons towards an atom. Electronegativity difference between bonded atoms defines the nature of bond as stated in the following table.

Electronegativity difference Type of bond Electron distribution in bond.
0.5 > Nonpolar Electrons are equally distributed.
0.5 -1.9 Polar covalent Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤ Ionic Electron has been donated to the more electronegative atom from less electronegative atom.

Expert Solution

Answer to Problem 4.73P

The bond between Li and O is ionic.

Explanation of Solution

The electronegativity of Li and O atom is 1.0 and 3.5 respectively. The electronegativity difference will be 2.5.

Since,

Electronegativity difference	Type of bond	Electron distribution in bond.
0.5 >	Nonpolar	Electrons are equally distributed.
0.5 -1.9	Polar covalent	Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤	Ionic	Electron has been donated to the more electronegative atom from less electronegative atom.

Thus, the bond will be ionic in nature.

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Answer 3

Question

Chapter 4, Problem 4.73P

Interpretation Introduction

(a)

Interpretation:

Bonds formed between H and Br should be classified as polarcovalent or ionic based on the electronegativity of atoms.

Concept Introduction:

The electronegativity of atoms defines the bond characteristics, as the electron distribution of the bond can be predicted by electronegativity. Electronegativity is tendency to pull bond electrons towards an atom. Electronegativity difference between bonded atoms defines the nature of bond as stated in the following table.

Electronegativity difference Type of bond Electron distribution in bond.
0.5 > Nonpolar Electrons are equally distributed.
0.5 -1.9 Polar covalent Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤ Ionic Electron has been donated to the more electronegative atom from less electronegative atom.

Expert Solution

Answer to Problem 4.73P

The bond between H and Br atom is polar covalent.

Explanation of Solution

The electronegativity of H and Br atom is 2.1 and 2.8 respectively. The electronegativity difference will be 0.7.

Since,

Electronegativity difference	Type of bond	Electron distribution in bond.
0.5 >	Nonpolar	Electrons are equally distributed.
0.5 -1.9	Polar covalent	Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤	Ionic	Electron has been donated to the more electronegative atom from less electronegative atom.

Thus, the bond will be polar covalent in nature.

Interpretation Introduction

(b)

Interpretation:

Bonds formed between Na and S should be classified as polar covalent or ionic based on the electronegativity of atoms.

Concept Introduction:

The electronegativity of atoms defines the bond characteristics, as the electron distribution of the bond can be predicted by electronegativity. Electronegativity is tendency to pull bond electrons towards an atom. Electronegativity difference between bonded atoms defines the nature of bond as stated in the following table.

Electronegativity difference Type of bond Electron distribution in bond.
0.5 > Nonpolar Electrons are equally distributed.
0.5 -1.9 Polar covalent Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤ Ionic Electron has been donated to the more electronegative atom from less electronegative atom.

Expert Solution

Answer to Problem 4.73P

The bond between Na and S atom is polar covalent.

Explanation of Solution

The electronegativity of Na and S atom is 0.9 and 2.5 respectively. The electronegativity difference will be 1.6.

Since,

Electronegativity difference	Type of bond	Electron distribution in bond.
0.5 >	Nonpolar	Electrons are equally distributed.
0.5 -1.9	Polar covalent	Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤	Ionic	Electron has been donated to the more electronegative atom from less electronegative atom.

Thus, the bond will be polar covalent in nature.

Interpretation Introduction

(c)

Interpretation:

Bonds formed between N and C should be classified as polar covalent or ionic based on the electronegativity of atoms.

Concept Introduction:

The electronegativity of atoms defines the bond characteristics, as the electron distribution of the bond can be predicted by electronegativity. Electronegativity is tendency to pull bond electrons towards an atom. Electronegativity difference between bonded atoms defines the nature of bond as stated in the following table.

Electronegativity difference Type of bond Electron distribution in bond.
0.5 > Nonpolar Electrons are equally distributed.
0.5 -1.9 Polar covalent Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤ Ionic Electron has been donated to the more electronegative atom from less electronegative atom.

Expert Solution

Answer to Problem 4.73P

The bond between N and C atom is polar covalent.

Explanation of Solution

The electronegativity of N and C atom is 3.0 and 2.7 respectively. The electronegativity difference will be 0.5.

Since,

Electronegativity difference	Type of bond	Electron distribution in bond.
0.5 >	Nonpolar	Electrons are equally distributed.
0.5 -1.9	Polar covalent	Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤	Ionic	Electron has been donated to the more electronegative atom from less electronegative atom.

Thus, the bond will be polar covalent in nature.

Interpretation Introduction

(d)

Interpretation:

Bonds formed between Li and O should be classified as polar covalent or ionic based on the electronegativity of atoms.

Concept Introduction:

The electronegativity of atoms defines the bond characteristics, as the electron distribution of the bond can be predicted by electronegativity. Electronegativity is tendency to pull bond electrons towards an atom. Electronegativity difference between bonded atoms defines the nature of bond as stated in the following table.

Electronegativity difference Type of bond Electron distribution in bond.
0.5 > Nonpolar Electrons are equally distributed.
0.5 -1.9 Polar covalent Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤ Ionic Electron has been donated to the more electronegative atom from less electronegative atom.

Expert Solution

Answer to Problem 4.73P

The bond between Li and O is ionic.

Explanation of Solution

The electronegativity of Li and O atom is 1.0 and 3.5 respectively. The electronegativity difference will be 2.5.

Since,

Electronegativity difference	Type of bond	Electron distribution in bond.
0.5 >	Nonpolar	Electrons are equally distributed.
0.5 -1.9	Polar covalent	Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤	Ionic	Electron has been donated to the more electronegative atom from less electronegative atom.

Thus, the bond will be ionic in nature.

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Answer 4

Question

Chapter 4, Problem 4.73P

Interpretation Introduction

(a)

Interpretation:

Bonds formed between H and Br should be classified as polarcovalent or ionic based on the electronegativity of atoms.

Concept Introduction:

The electronegativity of atoms defines the bond characteristics, as the electron distribution of the bond can be predicted by electronegativity. Electronegativity is tendency to pull bond electrons towards an atom. Electronegativity difference between bonded atoms defines the nature of bond as stated in the following table.

Electronegativity difference Type of bond Electron distribution in bond.
0.5 > Nonpolar Electrons are equally distributed.
0.5 -1.9 Polar covalent Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤ Ionic Electron has been donated to the more electronegative atom from less electronegative atom.

Expert Solution

Answer to Problem 4.73P

The bond between H and Br atom is polar covalent.

Explanation of Solution

The electronegativity of H and Br atom is 2.1 and 2.8 respectively. The electronegativity difference will be 0.7.

Since,

Electronegativity difference	Type of bond	Electron distribution in bond.
0.5 >	Nonpolar	Electrons are equally distributed.
0.5 -1.9	Polar covalent	Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤	Ionic	Electron has been donated to the more electronegative atom from less electronegative atom.

Thus, the bond will be polar covalent in nature.

Interpretation Introduction

(b)

Interpretation:

Bonds formed between Na and S should be classified as polar covalent or ionic based on the electronegativity of atoms.

Concept Introduction:

The electronegativity of atoms defines the bond characteristics, as the electron distribution of the bond can be predicted by electronegativity. Electronegativity is tendency to pull bond electrons towards an atom. Electronegativity difference between bonded atoms defines the nature of bond as stated in the following table.

Electronegativity difference Type of bond Electron distribution in bond.
0.5 > Nonpolar Electrons are equally distributed.
0.5 -1.9 Polar covalent Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤ Ionic Electron has been donated to the more electronegative atom from less electronegative atom.

Expert Solution

Answer to Problem 4.73P

The bond between Na and S atom is polar covalent.

Explanation of Solution

The electronegativity of Na and S atom is 0.9 and 2.5 respectively. The electronegativity difference will be 1.6.

Since,

Electronegativity difference	Type of bond	Electron distribution in bond.
0.5 >	Nonpolar	Electrons are equally distributed.
0.5 -1.9	Polar covalent	Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤	Ionic	Electron has been donated to the more electronegative atom from less electronegative atom.

Thus, the bond will be polar covalent in nature.

Interpretation Introduction

(c)

Interpretation:

Bonds formed between N and C should be classified as polar covalent or ionic based on the electronegativity of atoms.

Concept Introduction:

The electronegativity of atoms defines the bond characteristics, as the electron distribution of the bond can be predicted by electronegativity. Electronegativity is tendency to pull bond electrons towards an atom. Electronegativity difference between bonded atoms defines the nature of bond as stated in the following table.

Electronegativity difference Type of bond Electron distribution in bond.
0.5 > Nonpolar Electrons are equally distributed.
0.5 -1.9 Polar covalent Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤ Ionic Electron has been donated to the more electronegative atom from less electronegative atom.

Expert Solution

Answer to Problem 4.73P

The bond between N and C atom is polar covalent.

Explanation of Solution

The electronegativity of N and C atom is 3.0 and 2.7 respectively. The electronegativity difference will be 0.5.

Since,

Electronegativity difference	Type of bond	Electron distribution in bond.
0.5 >	Nonpolar	Electrons are equally distributed.
0.5 -1.9	Polar covalent	Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤	Ionic	Electron has been donated to the more electronegative atom from less electronegative atom.

Thus, the bond will be polar covalent in nature.

Interpretation Introduction

(d)

Interpretation:

Bonds formed between Li and O should be classified as polar covalent or ionic based on the electronegativity of atoms.

Concept Introduction:

The electronegativity of atoms defines the bond characteristics, as the electron distribution of the bond can be predicted by electronegativity. Electronegativity is tendency to pull bond electrons towards an atom. Electronegativity difference between bonded atoms defines the nature of bond as stated in the following table.

Electronegativity difference Type of bond Electron distribution in bond.
0.5 > Nonpolar Electrons are equally distributed.
0.5 -1.9 Polar covalent Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤ Ionic Electron has been donated to the more electronegative atom from less electronegative atom.

Expert Solution

Answer to Problem 4.73P

The bond between Li and O is ionic.

Explanation of Solution

The electronegativity of Li and O atom is 1.0 and 3.5 respectively. The electronegativity difference will be 2.5.

Since,

Electronegativity difference	Type of bond	Electron distribution in bond.
0.5 >	Nonpolar	Electrons are equally distributed.
0.5 -1.9	Polar covalent	Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤	Ionic	Electron has been donated to the more electronegative atom from less electronegative atom.

Thus, the bond will be ionic in nature.

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Answer 5

Chapter 4, Problem 4.73P

Interpretation Introduction

(a)

Interpretation:

Bonds formed between H and Br should be classified as polarcovalent or ionic based on the electronegativity of atoms.

Concept Introduction:

The electronegativity of atoms defines the bond characteristics, as the electron distribution of the bond can be predicted by electronegativity. Electronegativity is tendency to pull bond electrons towards an atom. Electronegativity difference between bonded atoms defines the nature of bond as stated in the following table.

Electronegativity difference Type of bond Electron distribution in bond.
0.5 > Nonpolar Electrons are equally distributed.
0.5 -1.9 Polar covalent Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤ Ionic Electron has been donated to the more electronegative atom from less electronegative atom.

Expert Solution

Answer to Problem 4.73P

The bond between H and Br atom is polar covalent.

Explanation of Solution

The electronegativity of H and Br atom is 2.1 and 2.8 respectively. The electronegativity difference will be 0.7.

Since,

Electronegativity difference	Type of bond	Electron distribution in bond.
0.5 >	Nonpolar	Electrons are equally distributed.
0.5 -1.9	Polar covalent	Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤	Ionic	Electron has been donated to the more electronegative atom from less electronegative atom.

Thus, the bond will be polar covalent in nature.

Interpretation Introduction

(b)

Interpretation:

Bonds formed between Na and S should be classified as polar covalent or ionic based on the electronegativity of atoms.

Concept Introduction:

The electronegativity of atoms defines the bond characteristics, as the electron distribution of the bond can be predicted by electronegativity. Electronegativity is tendency to pull bond electrons towards an atom. Electronegativity difference between bonded atoms defines the nature of bond as stated in the following table.

Electronegativity difference Type of bond Electron distribution in bond.
0.5 > Nonpolar Electrons are equally distributed.
0.5 -1.9 Polar covalent Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤ Ionic Electron has been donated to the more electronegative atom from less electronegative atom.

Expert Solution

Answer to Problem 4.73P

The bond between Na and S atom is polar covalent.

Explanation of Solution

The electronegativity of Na and S atom is 0.9 and 2.5 respectively. The electronegativity difference will be 1.6.

Since,

Electronegativity difference	Type of bond	Electron distribution in bond.
0.5 >	Nonpolar	Electrons are equally distributed.
0.5 -1.9	Polar covalent	Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤	Ionic	Electron has been donated to the more electronegative atom from less electronegative atom.

Thus, the bond will be polar covalent in nature.

Interpretation Introduction

(c)

Interpretation:

Bonds formed between N and C should be classified as polar covalent or ionic based on the electronegativity of atoms.

Concept Introduction:

The electronegativity of atoms defines the bond characteristics, as the electron distribution of the bond can be predicted by electronegativity. Electronegativity is tendency to pull bond electrons towards an atom. Electronegativity difference between bonded atoms defines the nature of bond as stated in the following table.

Electronegativity difference Type of bond Electron distribution in bond.
0.5 > Nonpolar Electrons are equally distributed.
0.5 -1.9 Polar covalent Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤ Ionic Electron has been donated to the more electronegative atom from less electronegative atom.

Expert Solution

Answer to Problem 4.73P

The bond between N and C atom is polar covalent.

Explanation of Solution

The electronegativity of N and C atom is 3.0 and 2.7 respectively. The electronegativity difference will be 0.5.

Since,

Electronegativity difference	Type of bond	Electron distribution in bond.
0.5 >	Nonpolar	Electrons are equally distributed.
0.5 -1.9	Polar covalent	Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤	Ionic	Electron has been donated to the more electronegative atom from less electronegative atom.

Thus, the bond will be polar covalent in nature.

Interpretation Introduction

(d)

Interpretation:

Bonds formed between Li and O should be classified as polar covalent or ionic based on the electronegativity of atoms.

Concept Introduction:

The electronegativity of atoms defines the bond characteristics, as the electron distribution of the bond can be predicted by electronegativity. Electronegativity is tendency to pull bond electrons towards an atom. Electronegativity difference between bonded atoms defines the nature of bond as stated in the following table.

Electronegativity difference Type of bond Electron distribution in bond.
0.5 > Nonpolar Electrons are equally distributed.
0.5 -1.9 Polar covalent Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤ Ionic Electron has been donated to the more electronegative atom from less electronegative atom.

Expert Solution

Answer to Problem 4.73P

The bond between Li and O is ionic.

Explanation of Solution

The electronegativity of Li and O atom is 1.0 and 3.5 respectively. The electronegativity difference will be 2.5.

Since,

Electronegativity difference	Type of bond	Electron distribution in bond.
0.5 >	Nonpolar	Electrons are equally distributed.
0.5 -1.9	Polar covalent	Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤	Ionic	Electron has been donated to the more electronegative atom from less electronegative atom.

Thus, the bond will be ionic in nature.

Answer 6

Chapter 4, Problem 4.73P

Interpretation Introduction

(a)

Interpretation:

Bonds formed between H and Br should be classified as polarcovalent or ionic based on the electronegativity of atoms.

Concept Introduction:

The electronegativity of atoms defines the bond characteristics, as the electron distribution of the bond can be predicted by electronegativity. Electronegativity is tendency to pull bond electrons towards an atom. Electronegativity difference between bonded atoms defines the nature of bond as stated in the following table.

Electronegativity difference Type of bond Electron distribution in bond.
0.5 > Nonpolar Electrons are equally distributed.
0.5 -1.9 Polar covalent Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤ Ionic Electron has been donated to the more electronegative atom from less electronegative atom.

Expert Solution

Answer to Problem 4.73P

The bond between H and Br atom is polar covalent.

Explanation of Solution

The electronegativity of H and Br atom is 2.1 and 2.8 respectively. The electronegativity difference will be 0.7.

Since,

Electronegativity difference	Type of bond	Electron distribution in bond.
0.5 >	Nonpolar	Electrons are equally distributed.
0.5 -1.9	Polar covalent	Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤	Ionic	Electron has been donated to the more electronegative atom from less electronegative atom.

Thus, the bond will be polar covalent in nature.

Answer 7

Chapter 4, Problem 4.73P

Interpretation Introduction

(a)

Interpretation:

Bonds formed between H and Br should be classified as polarcovalent or ionic based on the electronegativity of atoms.

Concept Introduction:

The electronegativity of atoms defines the bond characteristics, as the electron distribution of the bond can be predicted by electronegativity. Electronegativity is tendency to pull bond electrons towards an atom. Electronegativity difference between bonded atoms defines the nature of bond as stated in the following table.

Electronegativity difference Type of bond Electron distribution in bond.
0.5 > Nonpolar Electrons are equally distributed.
0.5 -1.9 Polar covalent Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤ Ionic Electron has been donated to the more electronegative atom from less electronegative atom.

Answer 8

Expert Solution

Answer to Problem 4.73P

The bond between H and Br atom is polar covalent.

Answer 9

Expert Solution

Answer 10

Expert Solution

Answer 11

Expert Solution

Answer 12

Explanation of Solution

The electronegativity of H and Br atom is 2.1 and 2.8 respectively. The electronegativity difference will be 0.7.

Since,

Electronegativity difference	Type of bond	Electron distribution in bond.
0.5 >	Nonpolar	Electrons are equally distributed.
0.5 -1.9	Polar covalent	Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤	Ionic	Electron has been donated to the more electronegative atom from less electronegative atom.

Thus, the bond will be polar covalent in nature.

Answer 13

Interpretation Introduction

(b)

Interpretation:

Bonds formed between Na and S should be classified as polar covalent or ionic based on the electronegativity of atoms.

Concept Introduction:

The electronegativity of atoms defines the bond characteristics, as the electron distribution of the bond can be predicted by electronegativity. Electronegativity is tendency to pull bond electrons towards an atom. Electronegativity difference between bonded atoms defines the nature of bond as stated in the following table.

Electronegativity difference Type of bond Electron distribution in bond.
0.5 > Nonpolar Electrons are equally distributed.
0.5 -1.9 Polar covalent Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤ Ionic Electron has been donated to the more electronegative atom from less electronegative atom.

Expert Solution

Answer to Problem 4.73P

The bond between Na and S atom is polar covalent.

Explanation of Solution

The electronegativity of Na and S atom is 0.9 and 2.5 respectively. The electronegativity difference will be 1.6.

Since,

Electronegativity difference	Type of bond	Electron distribution in bond.
0.5 >	Nonpolar	Electrons are equally distributed.
0.5 -1.9	Polar covalent	Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤	Ionic	Electron has been donated to the more electronegative atom from less electronegative atom.

Thus, the bond will be polar covalent in nature.

Answer 14

Interpretation Introduction

(b)

Interpretation:

Bonds formed between Na and S should be classified as polar covalent or ionic based on the electronegativity of atoms.

Concept Introduction:

The electronegativity of atoms defines the bond characteristics, as the electron distribution of the bond can be predicted by electronegativity. Electronegativity is tendency to pull bond electrons towards an atom. Electronegativity difference between bonded atoms defines the nature of bond as stated in the following table.

Electronegativity difference Type of bond Electron distribution in bond.
0.5 > Nonpolar Electrons are equally distributed.
0.5 -1.9 Polar covalent Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤ Ionic Electron has been donated to the more electronegative atom from less electronegative atom.

Answer 15

Expert Solution

Answer to Problem 4.73P

The bond between Na and S atom is polar covalent.

Answer 16

Expert Solution

Answer 17

Expert Solution

Answer 18

Expert Solution

Answer 19

Explanation of Solution

The electronegativity of Na and S atom is 0.9 and 2.5 respectively. The electronegativity difference will be 1.6.

Since,

Electronegativity difference	Type of bond	Electron distribution in bond.
0.5 >	Nonpolar	Electrons are equally distributed.
0.5 -1.9	Polar covalent	Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤	Ionic	Electron has been donated to the more electronegative atom from less electronegative atom.

Thus, the bond will be polar covalent in nature.

Answer 20

Interpretation Introduction

(c)

Interpretation:

Bonds formed between N and C should be classified as polar covalent or ionic based on the electronegativity of atoms.

Concept Introduction:

The electronegativity of atoms defines the bond characteristics, as the electron distribution of the bond can be predicted by electronegativity. Electronegativity is tendency to pull bond electrons towards an atom. Electronegativity difference between bonded atoms defines the nature of bond as stated in the following table.

Electronegativity difference Type of bond Electron distribution in bond.
0.5 > Nonpolar Electrons are equally distributed.
0.5 -1.9 Polar covalent Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤ Ionic Electron has been donated to the more electronegative atom from less electronegative atom.

Expert Solution

Answer to Problem 4.73P

The bond between N and C atom is polar covalent.

Explanation of Solution

The electronegativity of N and C atom is 3.0 and 2.7 respectively. The electronegativity difference will be 0.5.

Since,

Electronegativity difference	Type of bond	Electron distribution in bond.
0.5 >	Nonpolar	Electrons are equally distributed.
0.5 -1.9	Polar covalent	Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤	Ionic	Electron has been donated to the more electronegative atom from less electronegative atom.

Thus, the bond will be polar covalent in nature.

Answer 21

Interpretation Introduction

(c)

Interpretation:

Bonds formed between N and C should be classified as polar covalent or ionic based on the electronegativity of atoms.

Concept Introduction:

The electronegativity of atoms defines the bond characteristics, as the electron distribution of the bond can be predicted by electronegativity. Electronegativity is tendency to pull bond electrons towards an atom. Electronegativity difference between bonded atoms defines the nature of bond as stated in the following table.

Electronegativity difference Type of bond Electron distribution in bond.
0.5 > Nonpolar Electrons are equally distributed.
0.5 -1.9 Polar covalent Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤ Ionic Electron has been donated to the more electronegative atom from less electronegative atom.

Answer 22

Expert Solution

Answer to Problem 4.73P

The bond between N and C atom is polar covalent.

Answer 23

Expert Solution

Answer 24

Expert Solution

Answer 25

Expert Solution

Answer 26

Explanation of Solution

The electronegativity of N and C atom is 3.0 and 2.7 respectively. The electronegativity difference will be 0.5.

Since,

Electronegativity difference	Type of bond	Electron distribution in bond.
0.5 >	Nonpolar	Electrons are equally distributed.
0.5 -1.9	Polar covalent	Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤	Ionic	Electron has been donated to the more electronegative atom from less electronegative atom.

Thus, the bond will be polar covalent in nature.

Answer 27

Interpretation Introduction

(d)

Interpretation:

Bonds formed between Li and O should be classified as polar covalent or ionic based on the electronegativity of atoms.

Concept Introduction:

The electronegativity of atoms defines the bond characteristics, as the electron distribution of the bond can be predicted by electronegativity. Electronegativity is tendency to pull bond electrons towards an atom. Electronegativity difference between bonded atoms defines the nature of bond as stated in the following table.

Electronegativity difference Type of bond Electron distribution in bond.
0.5 > Nonpolar Electrons are equally distributed.
0.5 -1.9 Polar covalent Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤ Ionic Electron has been donated to the more electronegative atom from less electronegative atom.

Expert Solution

Answer to Problem 4.73P

The bond between Li and O is ionic.

Explanation of Solution

The electronegativity of Li and O atom is 1.0 and 3.5 respectively. The electronegativity difference will be 2.5.

Since,

Electronegativity difference	Type of bond	Electron distribution in bond.
0.5 >	Nonpolar	Electrons are equally distributed.
0.5 -1.9	Polar covalent	Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤	Ionic	Electron has been donated to the more electronegative atom from less electronegative atom.

Thus, the bond will be ionic in nature.

Answer 28

Interpretation Introduction

(d)

Interpretation:

Bonds formed between Li and O should be classified as polar covalent or ionic based on the electronegativity of atoms.

Concept Introduction:

The electronegativity of atoms defines the bond characteristics, as the electron distribution of the bond can be predicted by electronegativity. Electronegativity is tendency to pull bond electrons towards an atom. Electronegativity difference between bonded atoms defines the nature of bond as stated in the following table.

Electronegativity difference Type of bond Electron distribution in bond.
0.5 > Nonpolar Electrons are equally distributed.
0.5 -1.9 Polar covalent Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤ Ionic Electron has been donated to the more electronegative atom from less electronegative atom.

Answer 29

Expert Solution

Answer to Problem 4.73P

The bond between Li and O is ionic.

Answer 30

Expert Solution

Answer 31

Expert Solution

Answer 32

Expert Solution

Answer 33

Explanation of Solution

The electronegativity of Li and O atom is 1.0 and 3.5 respectively. The electronegativity difference will be 2.5.

Since,

Electronegativity difference	Type of bond	Electron distribution in bond.
0.5 >	Nonpolar	Electrons are equally distributed.
0.5 -1.9	Polar covalent	Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom).
1.9 ≤	Ionic	Electron has been donated to the more electronegative atom from less electronegative atom.

Thus, the bond will be ionic in nature.