Prab: CSV import

2025-02-18T01:55:07Z

CSV import

← Older revision		Revision as of 01:55, 18 February 2025
Line 40:		Line 40:
	[[Category:Physical chemistry]]		[[Category:Physical chemistry]]
	{{Chemistry-stub}}		{{Chemistry-stub}}
			<gallery>
			File:NaF.gif\|Sodium fluoride (NaF) ionic bonding
			File:Ionic_Bonding_LiF.svg\|Lithium fluoride (LiF) ionic bonding
			File:NaCl_bonds.svg\|Sodium chloride (NaCl) ionic bonding
			</gallery>

Prab: CSV import

2024-03-19T06:42:56Z

CSV import

New page

'''Ionic bonding''' is a type of [[chemical bond]] that involves the electrostatic attraction between oppositely charged [[ion]]s. These ions are atoms that have gained or lost [[electron]]s, thus acquiring a charge. Ionic bonds are formed when one atom (typically a [[metal]]) loses one or more electrons, becoming a positively charged ion (cation), and another atom (typically a [[nonmetal]]) gains those electrons, becoming a negatively charged ion (anion). The resulting attraction between the oppositely charged ions leads to the formation of a stable ionic compound.

==Overview==
Ionic bonding is one of the primary types of chemical bonding, alongside [[covalent bond]]ing and [[metallic bonding]]. It is characterized by the transfer of electrons from one atom to another, contrasting with covalent bonding, where electrons are shared between atoms. Ionic bonds typically occur between elements that are significantly different in [[electronegativity]], which is the ability of an atom to attract electrons towards itself. Metals, with low electronegativity, tend to lose electrons, while nonmetals, with high electronegativity, tend to gain electrons.

==Formation==
The formation of an ionic bond can be viewed as a process involving several steps:
# One atom (the metal) loses one or more electrons, forming a cation.
# Another atom (the nonmetal) gains those electrons, forming an anion.
# The resulting oppositely charged ions attract each other, forming an ionic compound.

This process releases energy, making the formation of the ionic bond energetically favorable.

==Properties of Ionic Compounds==
Ionic compounds have distinct properties due to the strong electrostatic forces holding the ions together in a lattice structure. These properties include:
* High melting and boiling points, due to the strong attraction between ions.
* Solid state at room temperature.
* Ability to conduct electricity when melted or dissolved in water, as the ions are free to move.
* Generally soluble in water but insoluble in nonpolar solvents.

==Examples==
Common examples of ionic compounds include table salt ([[sodium chloride]]), which is formed from sodium (Na) and chlorine (Cl) ions, and calcium carbonate ([[CaCO3]]), formed from calcium (Ca) ions and carbonate (CO3) ions.

==Ionic vs. Covalent Bonds==
While ionic bonds involve the transfer of electrons and the formation of ions, covalent bonds involve the sharing of electrons between atoms. The distinction between the two is not always clear-cut, as there is a continuum between purely ionic and purely covalent bonds based on the difference in electronegativity between the bonded atoms.

==Environmental and Biological Significance==
Ionic compounds play crucial roles in the environment and biological systems. For example, the ionic compound sodium chloride is essential for life, serving as an important electrolyte in the body. Ionic compounds are also involved in many geological processes, such as the formation of minerals.

==See Also==
* [[Electronegativity]]
* [[Metal]]
* [[Nonmetal]]
* [[Electron]]
* [[Chemical bond]]
* [[Covalent bond]]
* [[Metallic bonding]]

[[Category:Chemical bonds]]
[[Category:Physical chemistry]]
{{Chemistry-stub}}

Ionic bonding - Revision history

Prab: CSV import

Prab: CSV import