/*! 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 41 Why do polar covalent compounds ... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 4: Problem 41

Why do polar covalent compounds dissolve in water?

Short Answer

Expert verified
Answer: Polar covalent compounds dissolve in water because their partial charges interact with the partial charges of water molecules through electrostatic interactions. This process, called hydration, forms a hydration shell around the solute molecules, enabling them to dissolve in water.

Step by step solution

01

Define Polar Covalent Compounds

Polar covalent compounds are formed when atoms share electrons unequally, which creates a partial positive charge on one atom and partial negative charge on another. This unequal sharing of electrons results in a polar molecule, with a dipole moment.
02

Define Water's Polarity

Water is a polar molecule due to its bent molecular geometry and the difference in electronegativity between oxygen and hydrogen atoms. Oxygen is more electronegative than hydrogen, which means it attracts electrons more strongly. This results in a partial negative charge on the oxygen atom and partial positive charges on the hydrogen atoms.
03

Explain the Solvation Process

The process of dissolving a solute in a solvent is called solvation. In the case of polar covalent compounds dissolved in water, the process is called hydration. During this process, the polar water molecules interact with the polar solute molecules via electrostatic forces, which causes the formation of a hydration shell around the solute molecules.
04

Describe the Importance of Electrostatic Interactions

Electrostatic interactions, or the attractions between opposite partial charges, play a crucial role in the dissolution process. When polar covalent compounds dissolve in water, the partially negative oxygen atoms of water molecules are attracted to the partially positive ends of the solute molecules, while the partially positive hydrogen atoms of water are attracted to the partially negative ends of the solute. This interaction between the water molecules and the solute molecules causes the polar covalent compound to dissolve in water.
05

Conclusion

Polar covalent compounds dissolve in water because of the polarity of both the compound and water molecules. The electrostatic interactions between the partial positive and negative charges facilitate the dissolution process, allowing the polar covalent compounds to dissolve in water.

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

compounds conduct electricity in fused state or in aqueous solution.

In what type of solvents do the (a) polar compounds and (b) non-polar compounds dissolve?

Define the following terms on the basis of electron transfer. (a) Oxidation (b) Reduction (c) Redox reaction (d) Oxidizing agent (c) Reducing agent

Why do the non-polar covalent compounds not conduct electricity?

Mention the oxidizing agent, reducing agent in the following redox reactions and give reason in support of your answer. (i) \(\mathrm{Mg}+2 \mathrm{HCl} \rightarrow \mathrm{MgCl}_{2}+\mathrm{H}_{2}\) (ii) \(2 \mathrm{ZnS}+3 \mathrm{O}_{2} \rightarrow 2 \mathrm{ZnO}+2 \mathrm{SO}_{2}\) (iii) \(2 \mathrm{KMnO}_{4}+16 \mathrm{HCl} \rightarrow 2 \mathrm{KCl}+2 \mathrm{MnCl}_{2}+8 \mathrm{H}_{2} \mathrm{O}+5 \mathrm{Cl}_{2}\) (iv) \(2 \mathrm{H}_{2} \mathrm{~S}+\mathrm{SO}_{2} \rightarrow 2 \mathrm{H}_{2} \mathrm{O}+3 \mathrm{~S}\) (v) \(4 \mathrm{HCl}+\mathrm{O}_{2} \rightarrow 2 \mathrm{H}_{2} \mathrm{O}+\mathrm{Cl}_{2}\)
See all solutions

Recommended explanations on Chemistry Textbooks

Inorganic Chemistry

Read Explanation

Chemical Reactions

Read Explanation

Organic Chemistry

Read Explanation

Physical Chemistry

Read Explanation

Chemical Analysis

Read Explanation

The Earths Atmosphere

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.