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Ions and Ionic Charges

Ions and Ionic Charges

In ordinary chemical reactions, the nucleus — which contains the protons and neutrons of each atom and thus identifies the element — remains unchanged. Electrons, however, can be added to atoms by transfer from other atoms, lost by transfer to other atoms, or shared with other atoms. The transfer and sharing of electrons among atoms govern the chemistry of the elements. During the formation of some compounds, atoms gain or lose electrons to form electrically charged particles called...

Ionic Bonds

Ionic Bonds

Overview
When atoms gain or lose electrons to achieve a more stable electron configuration they form ions. Ionic bonds are electrostatic attractions between ions with opposite charges. Ionic compounds are rigid and brittle when solid and may dissociate into their constituent ions in water. Covalent compounds, by contrast, remain intact unless a chemical reaction breaks them.
Opposing Charges Hold Ions Together in Ionic Compounds
Ionic bonds are reversible electrostatic interactions between ions...

Ionic Bonding and Electron Transfer

Ionic Bonding and Electron Transfer

Ions are atoms or molecules bearing an electrical charge. A cation (a positive ion) forms when a neutral atom loses one or more electrons from its valence shell, and an anion (a negative ion) forms when a neutral atom gains one or more electrons in its valence shell. Compounds composed of ions are called ionic compounds (or salts), and their constituent ions are held together by ionic bonds: electrostatic forces of attraction between oppositely charged cations and anions.

Ion Exchange

Ion Exchange

Ion exchange chromatography separates charged molecules from a solution by reversibly exchanging them with mobile, or 'active', ions associated with the oppositely charged stationary phase. This method can be used to separate ions, soften and deionize water, and purify solutions. The polymers comprising the ion-exchange column are high-molecular-weight and chemically stable polymers, crosslinked to be porous and essentially insoluble. They are also functionalized with either acidic or...

Ionic Compounds: Formulas and Nomenclature

Ionic Compounds: Formulas and Nomenclature

An element composed of atoms that readily lose electrons (a metal) can react with an element composed of atoms that readily gain electrons (a nonmetal) to produce ions through complete electron transfer. The compound formed by this transfer is stabilized by the electrostatic attractions (ionic bonds) between the oppositely charged ions.

Ions as Acids and Bases

Ions as Acids and Bases

Salts with Acidic Ions
Salts are ionic compounds composed of cations and anions, either of which may be capable of undergoing an acid or base ionization reaction with water. Aqueous salt solutions, therefore, may be acidic, basic, or neutral, depending on the relative acid-base strengths of the salt’s constituent ions. For example, dissolving the ammonium chloride in water results in its dissociation, as described by the equation:

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Updated: Aug 9, 2025

Merging Ion Concentration Polarization between Juxtaposed Ion Exchange Membranes to Block the Propagation of the Polarization Zone

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Strong ions and charge-balance.

¹Department of Biomedicine, Aarhus University, Århus C, Denmark.

Scandinavian Journal of Clinical and Laboratory Investigation

|February 22, 2023

Summary

This summary is machine-generated.

Predicting fluid pH, buffer capacity, and acid content relies on physical chemistry principles like electroneutrality and mass conservation. Strong ions are crucial for acid-base homeostasis, contrary to some physiological narratives.

Keywords:

Electrochemistry acid-base equilibrium biological buffers chemistry computer simulation ions models physical water-electrolyte balance

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Ion Mobility-Mass Spectrometry Techniques for Determining the Structure and Mechanisms of Metal Ion Recognition and Redox Activity of Metal Binding Oligopeptides

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Published on: September 7, 2019

Area of Science:

Physiology
Physical Chemistry
Biochemistry

Background:

Physiological acid-base balance is often explained using the Henderson-Hasselbalch equation.
A persistent narrative in physiology questions the role of strong ions in acid-base homeostasis.
The importance of strong ions in biological fluids is frequently underestimated or dismissed.

Purpose of the Study:

To refute common arguments against the significance of strong ions in acid-base balance.
To demonstrate that physical chemistry principles (electroneutrality, mass conservation) are sufficient for predicting fluid pH and buffer capacity.
To highlight the limitations of the Henderson-Hasselbalch equation when strong ions are ignored.

Main Methods:

Application of fundamental physical chemistry principles: electroneutrality, conservation of mass, and dissociation rules.
Analysis of common arguments against the role of strong ions in acid-base homeostasis.
Evaluation of simple chemical systems (e.g., sodium bicarbonate solutions) using both traditional and strong ion approaches.

Main Results:

The study refutes common arguments that downplay the importance of strong ions in acid-base homeostasis.
Ignoring strong ions renders even simple chemical systems, like sodium bicarbonate solutions, incomprehensible.
A complete description of acid-base systems requires a charge-balance statement that includes strong ions, buffer concentrations, and water dissociation.

Conclusions:

Predicting fluid pH, buffer capacity, and acid content is achievable using fundamental physical chemistry principles.
Strong ions play a critical and often overlooked role in acid-base homeostasis.
The Henderson-Hasselbalch equation alone is insufficient for a complete understanding of acid-base systems; charge balance including strong ions is essential.