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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