Chapter 4, Problem 63P

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 to Problem 63P

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.

Answer to Problem 63P

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.

Answer to Problem 63P

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.

Answer to Problem 63P

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.