Ionic Bond

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Ionic Bond

This lesson aligns with NGSS PS1.A

Introduction

A chemical bond is formed when two atoms transfer one or more electrons in order to achieve the nearest inert gas configuration. The process of two atoms coming together to release energy and attain stability encompasses three main methods. One of these involves the donation or acceptance of electrons to achieve an octet configuration. The resulting bond is termed an ionic bond or electrovalent bond. This type of bond is established when one atom gains electrons, while the other atom loses electrons from its outermost level or orbit. In this article, we will learn about ionic bond, properties of ionic bond as well as how ionic bond is formed.

What is an Ionic bond?

An ionic bond, also referred to as an electrovalent bond, represents a form of chemical bonding that arises due to the electrostatic attraction between oppositely charged ions within a compound or molecule.

The formation of an ionic bond occurs when the valence (outermost) electrons of one atom are permanently transferred to another atom following the octet rule.

The atom losing electrons transforms into a positively charged ion, termed a cation, while the atom gaining electrons assumes a negative charge and is referred to as an anion. The combination of these ions through an ionic bond results in the creation of ionic compounds.

It is noteworthy that the elements involved in the formation of ionic bonds typically include metals and nonmetals.

In this interaction, Lithium, classified as a metal, undergoes electron loss, while Fluorine, characterized as a non-metal, undergoes electron acceptance. This exchange leads to the establishment of an ionic bond, giving rise to a compound known as Lithium fluoride, with its chemical formula denoted as LiF.

How Ionic Bonds are Formed?

Electronegativity is a property of an atom, indicating its capacity to attract or retain electrons. The formation of ionic bonds depends upon a significant difference in electronegativity between the involved atoms. This notable difference in electronegativities gives rise to an electrostatic attraction, where electrons from one atom are drawn towards the nuclei of the other atom. Through the transfer of electrons, atoms attain a stable electronic configuration resembling that of inert gases. Consequently, the outermost (valence) shells of the atoms achieve completeness.

Sodium (Na) has a valency of one, possessing a single electron in its outermost (valence) shell. Conversely, chlorine holds seven electrons in its outermost shell and requires one additional electron for shell completion. Consequently, sodium willingly donates its sole electron, transforming into a sodium ion (Na+), adopting the nearest inert gas ‘s electronic configuration, neon.

In contrast, chlorine, characterized by higher electronegativity than sodium, accepts the electron, forming a chloride (Cl–) ion and achieving its nearest inert gas configuration resembling argon. The two ions result in the formation of an ionic bond, yielding NaCl, commonly recognized as table salt.

Properties of Ionic Bonds

Involving the transfer of electrons from one atom to another.
Ionic bonds are established between a metal and a nonmetal, characterized by a marked electronegativity difference that enables the nonmetal to attract electrons from the metal.
The attractive force between the nuclei and electrons is electrostatic, leading to charge separation. Ionic bonds are recognized for their high reactivity in appropriate mediums.
The strength of these bonds is directly related to the quantity of charges and inversely proportional to the distance between charged ions.
Ionic compounds exhibit high melting and boiling points, attributed to the energy required to break the lattice structure holding atoms together.
These compounds typically maintain a lattice structure and crystalline form at room temperature. However, they are brittle and prone to breaking along planes where pressure is applied.
In aqueous environments, ionic compounds dissolve smoothly, breaking into ions that serve as carriers of electricity. Additionally, they conduct electricity in a molten state.
On the contrary, ionic compounds are insoluble in nonpolar solvents.
The high reactivity of ionic compounds is evident.
Their bonds are non-directional, that’s why they do not exhibit isomerism.

Summary

The ionic bond is defined by the electrostatic force of attraction that binds together two ions carrying opposite charges.
The formation of an ionic bond occurs when the valence (outermost) electrons of one atom are permanently transferred to another atom following the octet rule.
The atom losing electrons transforms into a positively charged ion, termed a cation.
The atom gaining electrons assumes a negative charge and is referred to as an anion.
The strength of these bonds is directly related to the quantity of charges and inversely proportional to the distance between charged ions.

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