Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 8: Problem 10

What is meant by a chemical bond? Why do atoms form bonds with each other? Why do some elements exist as molecules in nature instead of as free atoms?

Short Answer

Expert verified
A chemical bond is the attractive force that holds atoms together in a molecule or an ionic compound due to the sharing or transfer of electrons. Atoms form bonds to achieve a stable configuration called the octet rule, where their outermost electron shell has 8 electrons. Chemical bonds include covalent, ionic, and metallic bonds. Some elements, like hydrogen, oxygen, and nitrogen, exist as molecules in nature instead of free atoms because forming molecular structures, such as diatomic molecules, provides a more stable configuration and satisfies the octet rule.

Step by step solution

01

Define a chemical bond

A chemical bond is the attractive force that holds atoms together in a molecule or an ionic compound due to the sharing or transfer of electrons. Chemical bonds enable the formation of molecules and compounds, which are essential for various chemical reactions.
02

Reason for the formation of chemical bonds

Atoms form bonds with each other to achieve a stable configuration by obtaining a complete set of electrons in their outermost electron shell. This is known as the octet rule, which states that atoms (with few exceptions) are most stable when they have 8 electrons in their outermost shell. By forming chemical bonds, atoms can gain, lose, or share electrons to achieve the stable configuration. This eventually lowers their potential energy, making the bonded atoms more stable than individual atoms.
03

Types of chemical bonds

There are several types of chemical bonds, including: 1. Covalent Bonds: These bonds involve the sharing of electrons between two atoms. For example, a water molecule (H2O) consists of two hydrogen atoms sharing their electrons with an oxygen atom. 2. Ionic Bonds: These bonds involve the transfer of electrons between two atoms, resulting in the formation of ions. For example, table salt (sodium chloride, NaCl) is formed by an ionic bond between sodium (Na) and chlorine (Cl). 3. Metallic Bonds: These bonds are characteristic of metals in which electrons are delocalized and move freely among the positively charged metal ions, creating a "sea of electrons."
04

Elements existing as molecules in nature

Some elements exist as molecules in nature instead of as free atoms due to their higher stability when forming particular molecular structures. Examples of these elements include hydrogen (H2), oxygen (O2), nitrogen (N2), and the halogens, such as chlorine (Cl2) and fluorine (F2). These elements form diatomic (two-atom) molecules because their electrons are equally shared, leading to a lower energy state and thus a more stable configuration. The formation of these molecules also satisfies the octet rule, contributing to their stability in nature.

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.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

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

Oxidation of the cyanide ion produces the stable cyanate ion, \(\mathrm{OCN}^{-}\) . The fulminate ion, \(\mathrm{CNO}^{-}\), on the other hand, is very unstable. Fulminate salts explode when struck; \(\mathrm{Hg}(\mathrm{CNO})_{2}\) is used in blasting caps. Write the Lewis structures and assign formal charges for the cyanate and fulminate ions. Why is the fulminate ion so unstable? (C is the central atom in \(\mathrm{OCN}^{-}\) and \(\mathrm{N}\) is the central atom in \(\mathrm{CNO}^{-}\) )

Compare the electron affinity of fluorine to the ionization energy of sodium. Is the process of an electron being “pulled” from the sodium atom to the fluorine atom exothermic or endothermic? Why is NaF a stable compound? Is the overall formation of NaF endothermic or exothermic? How can this be?

Predict the molecular structure (including bond angles) for each of the following. (See Exercises 115 and 116.) a. \(\mathrm{XeCl}_{2}\) b. \(\mathrm{ICl}_{3}\) c. \(\mathrm{TeF}_{4}\) d. \(\mathrm{PCl}_{5}\)

Write electron configurations for the most stable ion formed by each of the elements Al, Ba, Se, and I (when in stable ionic compounds).

Use the following data to estimate \(\Delta H_{\mathrm{f}}^{\circ}\) for barium bromide. $$\mathrm{Ba}(s)+\mathrm{Br}_{2}(g) \longrightarrow \mathrm{BaBr}_{2}(s)$$ $\begin{array}{ll}{\text { Lattice energy }} & {-1985 \mathrm{kJ} / \mathrm{mol}} \\ {\text { First ionization energy of Ba }} & \quad {503 \mathrm{kJ} / \mathrm{mol}} \\ {\text { Second ionization energy of } \mathrm{Ba}} & \quad {965 \mathrm{kJ} / \mathrm{mol}} \\ {\text { Electron affinity of } \mathrm{Br}} & {-325 \mathrm{kJ} / \mathrm{mol}}\\\\{\text { Bond energy of } \mathrm{Br}_{2}} & \quad {193 \mathrm{kJ} / \mathrm{mol}} \\\ {\text { Enthalpy of sublimation of } \mathrm{Ba}} & \quad {178 \mathrm{kJ} / \mathrm{mol}}\end{array}$
See all solutions

Recommended explanations on Chemistry Textbooks

Nuclear Chemistry

Read Explanation

Making Measurements

Read Explanation

Chemistry Branches

Read Explanation

Kinetics

Read Explanation

Ionic and Molecular Compounds

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.

Sign-up for free