/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 8 What does it mean to say that a ... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 11: Problem 8

What does it mean to say that a bond is polar? Give two examples of molecules with polar bonds. Indicate in your examples the direction of the polarity.

Short Answer

Expert verified
A polar bond is a covalent bond between two atoms where electrons are unequally shared due to differing electronegativity values, creating an electric dipole. Two examples of molecules with polar bonds are HCl and H2O. In HCl, the polarity points from H\((\delta^+)\) to Cl\((\delta^-)\), while in H2O, the polarity points from the H atoms (\(\delta^+\)) to the O atom (\(\delta^-\)).

Step by step solution

01

Definition of Polar Bond

A polar bond is a type of covalent bond between two atoms, where the electrons forming the bond are not equally shared by the two atoms due to differing electronegativity values. This results in a partially positive charge on the atom with lower electronegativity (and hence lesser electron-attracting power) and a partially negative charge on the atom with higher electronegativity. This creates an electric dipole, causing the bond to be polar.
02

Example 1: HCl (Hydrogen Chloride)

In a HCl molecule, the electron pair in the H-Cl bond is more attracted to the Cl atom due to its higher electronegativity value compared to H. As a result, the Cl atom acquires a partial negative charge (\(\delta^-\)), while the H atom acquires a partial positive charge (\(\delta^+\)). This leads to a polar bond, with the direction of polarity pointing from H to Cl, as shown below: H\((\delta^+)\)鈥擟l\((\delta^-)\)
03

Example 2: H2O (Water)

In a water molecule, the two O-H bonds are polar due to the difference in electronegativity values of O and H atoms. Since O is more electronegative than H, it attracts the bonded electron pairs more towards itself, resulting in a partial negative charge (\(\delta^-\)) on the O atom, and partial positive charges (\(\delta^+\)) on both H atoms. The directions of polarity point from H atoms to the O atom, as shown below: H 釐▅ O鈥擧 (\(\delta^+\)) (\(\delta^+\)) (\(\delta^-\))

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91影视!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Which of the following molecules contain polar covalent bonds? a. nitrogen, \(\mathrm{N}_{2}\) b. astatine, \(\mathrm{At}_{2}\) c. carbon monoxide, \(\mathrm{CO}\) d. hydrogen fluoride, HF

Describe in general terms the structure of ionic solids such as NaCl. How are the ions packed in the crystal?

In each of the following diatomic molecules, which end of the molecule is negative relative to the other end? a. hydrogen chloride, HCl b. carbon monoxide, \(\mathrm{CO}\) c. bromine monofluoride, BrF

Why is the presence of a dipole moment in the water molecule so important? What are some properties of water that are determined by its polarity?

Explain briefly how substances with ionic bonding differ in properties from substances with covalent bonding.
See all solutions

Recommended explanations on Chemistry Textbooks

Chemistry Branches

Read Explanation

The Earths Atmosphere

Read Explanation

Making Measurements

Read Explanation

Chemical Analysis

Read Explanation

Nuclear Chemistry

Read Explanation

Inorganic Chemistry

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.