For each polar molecule in the molecule and indicate the

Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo Tro

Problem 88P Chapter 10

Introductory Chemistry | 5th Edition

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Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo Tro

Introductory Chemistry | 5th Edition

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Problem 88P

PROBLEM 88P

For each polar molecule in Problem draw the molecule and indicate the positive and negative ends of the dipole moment.

Problem

Classify each diatomic molecule as polar or nonpolar.

(a) I2

(b) NO

(c) HCl

(d) N2

Step-by-Step Solution:

Solution 88P

Here, we are going to classify the molecules as polar or nonpolar. Polarity of a molecule can be determined as follows.

Determining the geometry of the molecule.A molecule is said to be polar when the two bonding atoms have sufficiently different electronegativities. Determination of the dipole moment of the molecule.

(a) I2

Step 1: The Lewis structure of the molecule is as follows

The molecule contains one bonding electron pair and 6 lone pair of electrons. Therefore, I2 is a linear molecule.

Step2: Determination of the polarity of the bond.

The electronegativity difference between I-I is zero. Therefore I-I is non polar

Step 3: The molecule has no dipole moment.

Thus, I2 is a non polar molecule.

(b) NO

Step 1: The Lewis structure of the molecule is as follows

The molecule contains two bonding electron pair and 7 nonbonding of electrons. Therefore, NO is a linear molecule.

Step 2: Determination of the polarity of the bond.

The electronegativity of N and O is 3.0 and 3.44 respectively

The electronegativity difference between N-O is 0.44. Therefore N-O is polar.

Step 3: Calculation of dipole moment.

Thus, NO has a net dipole moment.

Thus, NO is a polar molecule.Thus the structure for NO by depicting the positive and negative ends of the dipole moment.

(c) HCl

Step 1: The Lewis structure of the molecule is as follows

The molecule contains one bonding electron pair and 3 lone pair of electrons. Therefore, HCl is a linear molecule.

Step 2: Determination of the polarity of the bond.

The electronegativity of H and Cl is 2.2 and 3.16 respectively

The electronegativity difference between H-Cl is 0.96. Therefore H-Cl is polar.

Step 3: Calculation of dipole moment.

Thus, HCl has a net dipole moment.

Thus, HCl is a polar molecule.Thus the structure for NO by depicting the positive and negative ends of the dipole moment.

(d) N2

Step 1: The Lewis structure of the molecule is as follows

The molecule contains three bonding electron pair and 0  lone pair of electrons. Therefore, N2 is a linear molecule.

Step 2: Determination of the polarity of the bond.

The electronegativity of N is 3.0

The electronegativity difference between N-N is 0.0. Therefore N-N is non polar.

Step 3 of 3

Chapter 10, Problem 88P is Solved
Textbook: Introductory Chemistry
Edition: 5
Author: Nivaldo Tro
ISBN: 9780321910295

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