For apolar molecule, a dipole moment vector is drawn using δ + and δ − signs for the appropriate atoms. Concept introduction: A polar bond is the result of the electronegativity difference between the atoms due to which electrons are unsymmetrically distributed between the atoms, which leads to the development of charges on the atoms. The atom with a higher electronegative value develops a partially negative charge and the atom with a lower electronegative value develops a partially positive charge. The dipole moment vector would be from a least electronegative atom to most electronegative atom.

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Chapter 2, Problem 2PP

Interpretation Introduction

Interpretation:

For apolar molecule, a dipole moment vector is drawn using δ+ and δ− signs for the appropriate atoms.

Concept introduction:

A polar bond is the result of the electronegativity difference between the atoms due to which electrons are unsymmetrically distributed between the atoms, which leads to the development of charges on the atoms.

The atom with a higher electronegative value develops a partially negative charge and the atom with a lower electronegative value develops a partially positive charge.

The dipole moment vector would be from a least electronegative atom to most electronegative atom.

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Answer 2

Question

Chapter 2, Problem 2PP

Interpretation Introduction

Interpretation:

For apolar molecule, a dipole moment vector is drawn using δ+ and δ− signs for the appropriate atoms.

Concept introduction:

A polar bond is the result of the electronegativity difference between the atoms due to which electrons are unsymmetrically distributed between the atoms, which leads to the development of charges on the atoms.

The atom with a higher electronegative value develops a partially negative charge and the atom with a lower electronegative value develops a partially positive charge.

The dipole moment vector would be from a least electronegative atom to most electronegative atom.

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Answer 3

Question

Chapter 2, Problem 2PP

Interpretation Introduction

Interpretation:

For apolar molecule, a dipole moment vector is drawn using δ+ and δ− signs for the appropriate atoms.

Concept introduction:

A polar bond is the result of the electronegativity difference between the atoms due to which electrons are unsymmetrically distributed between the atoms, which leads to the development of charges on the atoms.

The atom with a higher electronegative value develops a partially negative charge and the atom with a lower electronegative value develops a partially positive charge.

The dipole moment vector would be from a least electronegative atom to most electronegative atom.

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Answer 4

Question

Chapter 2, Problem 2PP

Interpretation Introduction

Interpretation:

For apolar molecule, a dipole moment vector is drawn using δ+ and δ− signs for the appropriate atoms.

Concept introduction:

A polar bond is the result of the electronegativity difference between the atoms due to which electrons are unsymmetrically distributed between the atoms, which leads to the development of charges on the atoms.

The atom with a higher electronegative value develops a partially negative charge and the atom with a lower electronegative value develops a partially positive charge.

The dipole moment vector would be from a least electronegative atom to most electronegative atom.

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Answer 5

Chapter 2, Problem 2PP

Interpretation Introduction

Interpretation:

For apolar molecule, a dipole moment vector is drawn using δ+ and δ− signs for the appropriate atoms.

Concept introduction:

A polar bond is the result of the electronegativity difference between the atoms due to which electrons are unsymmetrically distributed between the atoms, which leads to the development of charges on the atoms.

The atom with a higher electronegative value develops a partially negative charge and the atom with a lower electronegative value develops a partially positive charge.

The dipole moment vector would be from a least electronegative atom to most electronegative atom.

Answer 6

Chapter 2, Problem 2PP

Interpretation Introduction

Interpretation:

For apolar molecule, a dipole moment vector is drawn using δ+ and δ− signs for the appropriate atoms.

Concept introduction:

A polar bond is the result of the electronegativity difference between the atoms due to which electrons are unsymmetrically distributed between the atoms, which leads to the development of charges on the atoms.

The atom with a higher electronegative value develops a partially negative charge and the atom with a lower electronegative value develops a partially positive charge.

The dipole moment vector would be from a least electronegative atom to most electronegative atom.

Answer 7

Chapter 2, Problem 2PP

Interpretation Introduction

Interpretation:

For apolar molecule, a dipole moment vector is drawn using δ+ and δ− signs for the appropriate atoms.

Concept introduction:

A polar bond is the result of the electronegativity difference between the atoms due to which electrons are unsymmetrically distributed between the atoms, which leads to the development of charges on the atoms.

The atom with a higher electronegative value develops a partially negative charge and the atom with a lower electronegative value develops a partially positive charge.

The dipole moment vector would be from a least electronegative atom to most electronegative atom.

Answer 8

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Answer 9

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Answer 10

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Answer 11

Ch. 2 - Practice Problem 2.1 Propose structures for two...Ch. 2 - Prob. 2PP Ch. 2 - Prob. 3PP Ch. 2 - Prob. 4PP Ch. 2 - Prob. 5PP Ch. 2 - Practice Problem 2.6 Using a three-dimensional...Ch. 2 - Practice Problem 2.7 Trichloromethane (, also...Ch. 2 - Prob. 8PP Ch. 2 - Prob. 9PP Ch. 2 - Practice Problem 2.10 Write bond-line structural...

Solution Summary: The author explains that a polar bond is the result of the electronegativity difference between the atoms due to which electrons are unsymmetrically distributed.

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