/*! 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 4 Classify each bond as nonpolar c... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 1: Problem 4

Classify each bond as nonpolar covalent or polar covalent or state that ions are formed. (a) \(\mathrm{S}-\mathrm{H}\) (b) \(\mathrm{P}-\mathrm{H}\) (c) \(\mathrm{C}-\mathrm{F}\) (d) \(\mathrm{C}-\mathrm{Cl}\)

Short Answer

Expert verified
Question: Classify the following bonds as nonpolar covalent, polar covalent, or ionic: (a) S-H, (b) P-H, (c) C-F, and (d) C-Cl. Answer: (a) S-H is a nonpolar covalent bond. (b) P-H is a nonpolar covalent bond. (c) C-F is a polar covalent bond. (d) C-Cl is a polar covalent bond.

Step by step solution

01

(a) Determine electronegativity difference for S-H bond

The electronegativity value for sulfur (S) is 2.58, and for hydrogen (H) it is 2.20. Thus, the electronegativity difference between the two in the S-H bond is: \(|2.58 - 2.20| = 0.38\).
02

(a) Classify the S-H bond

Since the electronegativity difference is 0.38, which is less than 0.5, the S-H bond is considered a nonpolar covalent bond.
03

(b) Determine electronegativity difference for P-H bond

The electronegativity value for phosphorus (P) is 2.19, and for hydrogen (H) it is 2.20. Thus, the electronegativity difference between the two in the P-H bond is: \(|2.19 - 2.20| = 0.01\).
04

(b) Classify the P-H bond

Since the electronegativity difference is 0.01, which is less than 0.5, the P-H bond is considered a nonpolar covalent bond.
05

(c) Determine electronegativity difference for C-F bond

The electronegativity value for carbon (C) is 2.55, and for fluorine (F) it is 3.98. Thus, the electronegativity difference between the two in the C-F bond is: \(|2.55 - 3.98| = 1.43\).
06

(c) Classify the C-F bond

Since the electronegativity difference is 1.43, which is between 0.5 and 2.0, the C-F bond is considered a polar covalent bond.
07

(d) Determine electronegativity difference for C-Cl bond

The electronegativity value for carbon (C) is 2.55, and for chlorine (Cl) it is 3.16. Thus, the electronegativity difference between the two in the C-Cl bond is: \(|2.55 - 3.16| = 0.61\).
08

(d) Classify the C-Cl bond

Since the electronegativity difference is 0.61, which is between 0.5 and 2.0, the C-Cl bond is considered a polar covalent bond.

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!

Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Nonpolar Covalent Bonds
Nonpolar covalent bonds occur when electrons are shared equally between two atoms. In these bonds, the difference in electronegativity between the atoms is less than 0.5.
This minimal difference means that neither atom has a strong pull on the shared electrons. As a result, the electron cloud remains balanced around both nuclei.
  • For a bond like S-H, with an electronegativity difference of 0.38, the bond is classified as nonpolar covalent.
  • Similarly, the P-H bond has an electronegativity difference of 0.01, confirming it as nonpolar covalent.
This equal sharing is often found in diatomic molecules consisting of the same element, such as O2. It's a simple yet essential concept in understanding molecular behavior and stability.
Polar Covalent Bonds
Polar covalent bonds form when electrons are shared unequally between atoms. This usually occurs when the electronegativity difference is between 0.5 and 2.0.
The atom with higher electronegativity attracts the shared electrons more, creating a partial negative charge. The less electronegative atom takes on a partial positive charge.
  • In a C-F bond, the electronegativity difference is 1.43, making it polar covalent, with fluorine pulling the shared electrons closer.
  • The C-Cl bond has a difference of 0.61, causing chlorine to slightly dominate the shared electrons, resulting in a polar bond.
This unequal sharing leads to dipole moments, where the molecule has a slight electrical polarity. Understanding these bonds helps in predicting a molecule's physical properties, such as solubility and boiling point.
Ionic Bonds
Ionic bonds arise when one atom completely transfers one or more electrons to another, creating ions. These bonds usually form when the electronegativity difference is greater than 2.0.
One atom becomes a positively charged cation, while the other becomes a negatively charged anion. The strong electrostatic attraction between these opposite charges holds the compound together.
  • Common in compounds like NaCl, where sodium donates an electron to chlorine.
  • These bonds result in crystalline structures with distinct physical properties like high melting points.
Ionic bonds are key in forming many salts and minerals. Unlike covalent bonds, they do not share electrons but rather transfer them, resulting in a distinctly different type of chemical interaction.

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

Predict all bond angles for these molecules. (a) \(\mathrm{CH}_{3} \mathrm{OH}\) (b) \(\mathrm{PF}_{3}\) (c) \(\mathrm{H}_{2} \mathrm{CO}_{3}\)

Draw condensed structural formulas for all compounds with the molecular formula \(\mathrm{C}_{4} \mathrm{H}_{8} \mathrm{O}\) that contain (a) A carbonyl group (there are two aldehydes and one ketone). (b) A carbon-carbon double bond and a hydroxyl group (there are eight).

Which statements are true about resonance contributing structures? (a) All contributing structures must have the same number of valence electrons. (b) All contributing structures must have the same arrangement of atoms. (c) All atoms in a contributing structure must have complete valence shells. (d) All bond angles in sets of contributing structures must be the same.

Why does fluorine, the element in the upper right corner of the Periodic Table, have the largest electronegativity of any element?

Cyanic acid, HOCN, and isocyanic acid, HNCO, dissolve in water to yield the same anion on loss of \(\mathrm{H}^{+}\). (a) Write a Lewis structure for cyanic acid. (b) Write a Lewis structure for isocyanic acid. (c) Account for the fact that each acid gives the same anion on loss of \(\mathrm{H}^{+}\). 1.71 In Chapter 6, we study a group of organic cations called carbocations. Following is the structure of one such carbocation, the tert-butyl cation. (a) How many electrons are in the valence shell of the carbon bearing the positive charge? (b) Using VSEPR, predict the bond angles about this carbon. (c) Given the bond angle you predicted in (b), what hybridization do you predict for this carbon?
See all solutions

Recommended explanations on Chemistry Textbooks

The Earths Atmosphere

Read Explanation

Kinetics

Read Explanation

Chemical Reactions

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Chemical Analysis

Read Explanation

Physical 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.