/*! 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 6 Explain what an ionic bond is.... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 9: Problem 6

Explain what an ionic bond is.

Short Answer

Expert verified
An ionic bond is a type of chemical bond that involves a complete transfer of valence electrons between atoms and produces oppositely charged ions. An example is NaCl (Sodium Chloride), where Sodium gives up an electron to Chlorine, forming an ionic bond.

Step by step solution

01

Define Ionic Bond

An ionic bond is a type of chemical bond formed through an electrostatic attraction between two oppositely charged ions. Ionic bonding is the complete transfer of valence electron(s) between atoms. It is a type of chemical bond that generates two oppositely charged ions.
02

Understand the Formation of Ions

During Ionic Bonding, atoms that lose electrons during this process become positively charged ions known as cations, while atoms that gain electrons become negatively charged ions known as anions.
03

Explain Examples of Ionic Bonds

A common example of an ionic bond is NaCl (Sodium Chloride), where Sodium (Na) gives up an electron to Chlorine (Cl), and they bond to form NaCl.

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.

Cation
A cation is an ion with a positive charge. This happens when an atom loses one or more of its valence electrons.
  • This loss leads to more protons than electrons in the atom, which gives it a positive charge.
  • Common cations include sodium (\( ext{Na}^+ \)), potassium (\( ext{K}^+ \)), and calcium (\( ext{Ca}^{2+} \)).
Cations are typically metals because metals tend to lose electrons to achieve a stable electron configuration. A stable electron configuration often means having full outer energy levels, similar to noble gases. When an atom becomes a cation, it might participate in forming ionic bonds by attracting anions with their complementary negative charge.
Anion
Anions are ions that carry a negative charge. This results from an atom gaining extra electrons.
  • When an atom picks up extra electrons, the number of electrons surpasses the number of protons, resulting in a negative charge.
  • This is common with nonmetals that need to gain electrons to fill their outer energy levels, achieving stability.
>
Some well-known anions include chloride (\( ext{Cl}^- \)), oxide (\( ext{O}^{2-} \)), and sulfide (\( ext{S}^{2-} \)). These negatively charged ions often pair with cations to form ionic bonds. Anions are key players in ionic compounds as they balance the positive charge from cations, resulting in a neutral compound.
Electrostatic Attraction
Electrostatic attraction is the force that holds oppositely charged particles together in an ionic bond. This powerful force arises because opposite charges attract each other.
  • In ionic bonding, this force pulls the positive cations and negative anions together.
  • The strength of the attraction depends on the size of the charges and the distance between them.
This interaction forms a stable structure known as a crystal lattice, a three-dimensional arrangement that maximizes attractive forces and minimizes repulsive forces between ions. Electrostatic attraction is fundamental to the stability and properties of ionic compounds, contributing to characteristics like high melting and boiling points seen in substances like sodium chloride (NaCl).
Valence Electron Transfer
Valence electron transfer is essential in forming ionic bonds. It involves the movement of electrons from one atom to another.
  • During this process, an atom (usually a metal) loses one or more electrons, becoming a cation.
  • Another atom (usually a nonmetal) gains these electrons, becoming an anion.
This transfer is driven by the atoms' desire to achieve a full outer shell of electrons, akin to the electron configuration of noble gases. The complete transfer of valence electrons leads to the formation of stable ions with full valence shells. This stability is the driving force behind the formation of ionic bonds, creating compounds like NaCl where sodium loses an electron and chlorine gains one.

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 are ionic compounds? Which are covalent compounds? \(\mathrm{RbCl}, \mathrm{PF}_{5}, \mathrm{BrF}_{3},\) \(\mathrm{KO}_{2}, \mathrm{CI}_{4}\)

From the lattice energy of \(\mathrm{KCl}\) in Table 9.1 and the ionization energy of \(\mathrm{K}\) and electron affinity of \(\mathrm{Cl}\) in Tables 8.2 and 8.3 , calculate the \(\Delta H^{\circ}\) for the reaction $$ \mathrm{K}(g)+\mathrm{Cl}(g) \longrightarrow \mathrm{KCl}(s) $$ (a) Draw three resonance structures to represent the ion. (b) Given the following information $$ 2 \mathrm{H}+\mathrm{H}^{+} \longrightarrow \mathrm{H}_{3}^{+} \quad \Delta H^{\circ}=-849 \mathrm{~kJ} / \mathrm{mol} $$ and $$ \mathrm{H}_{2} \longrightarrow 2 \mathrm{H} \quad \Delta H^{\circ}=436.4 \mathrm{~kJ} / \mathrm{mol} $$ calculate \(\Delta H^{\circ}\) for the reaction $$ \mathrm{H}^{+}+\mathrm{H}_{2} \longrightarrow \mathrm{H}_{3}^{+} $$

Write Lewis structures for the following ions: (a) \(\mathrm{NO}_{2}^{+},\) (b) \(\mathrm{S}_{2}^{2-},\) (c) \(\mathrm{BrF}_{2}^{+}\), (d) \(\mathrm{SCN}^{-}\). Show formal charges.

The following species have been detected in interstellar space: (a) \(\mathrm{CH},(\mathrm{b}) \mathrm{OH},(\mathrm{c}) \mathrm{C}_{2},(\mathrm{~d}) \mathrm{HNC},(\mathrm{e}) \mathrm{HCO} .\) Draw Lewis structures for these species and indicate whether they are diamagnetic or paramagnetic.

Although nitrogen dioxide \(\left(\mathrm{NO}_{2}\right)\) is a stable compound, there is a tendency for two such molecules to combine to form dinitrogen tetroxide \(\left(\mathrm{N}_{2} \mathrm{O}_{4}\right) .\) Why? Draw four resonance structures of \(\mathrm{N}_{2} \mathrm{O}_{4},\) showing formal charges.
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Analysis

Read Explanation

The Earths Atmosphere

Read Explanation

Chemical Reactions

Read Explanation

Making Measurements

Read Explanation

Inorganic Chemistry

Read Explanation

Nuclear 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.