Jove
Visualize
Contact Us
JoVE
x logofacebook logolinkedin logoyoutube logo
ABOUT JoVE
OverviewLeadershipBlogJoVE Help Center
AUTHORS
Publishing ProcessEditorial BoardScope & PoliciesPeer ReviewFAQSubmit
LIBRARIANS
TestimonialsSubscriptionsAccessResourcesLibrary Advisory BoardFAQ
RESEARCH
JoVE JournalMethods CollectionsJoVE Encyclopedia of ExperimentsArchive
EDUCATION
JoVE CoreJoVE BusinessJoVE Science EducationJoVE Lab ManualFaculty Resource CenterFaculty Site
Terms & Conditions of Use
Privacy Policy
Policies

Related Concept Videos

Ladder Diagrams: Redox Equilibria01:30

Ladder Diagrams: Redox Equilibria

Ladder diagrams are useful tools for understanding redox equilibrium reactions, especially the effects of concentration changes on the electrochemical potential of the reaction. The vertical axis in the redox ladder diagrams represents the electrochemical potential, E. The area of predominance is demarcated using the Nernst equation.
Consider the Fe3+/Fe2+ half-reaction, which has a standard-state potential of +0.771 V. At potentials more positive than +0.771 V, Fe3+ predominates, whereas Fe2+...
Standard Electrode Potentials03:02

Standard Electrode Potentials

On comparing the reactivity of silver and lead, it is observed that the two ionic species, Ag+ (aq) and Pb2+ (aq), show a difference in their redox reactivity towards copper: the silver ion undergoes spontaneous reduction, while the lead ion does not. This relative redox activity can be easily quantified in electrochemical cells by a property called cell potential. This property is commonly known as cell voltage in electrochemistry, and it is a measure of the energy which accompanies the charge...
Redox Reactions01:24

Redox Reactions

Oxidation-reduction or redox reactions involve the transfer of electrons from one molecule or atom to another. When an atom gains an electron, another atom must lose an electron, meaning oxidation and reduction must occur together. Since the redox occurs in pairs, the atom that gets oxidized is also called the reducing agent or reductant, and the atom that is reduced is also called the oxidizing agent or oxidant. A straightforward way to remember the definitions of oxidation and reduction is...
Redox Reactions01:27

Redox Reactions

Redox reactions are vital biochemical processes that underpin energy metabolism in cells. These reactions involve the transfer of electrons between molecules, occurring in tandem as oxidation and reduction. Oxidation refers to the loss of electrons, while reduction denotes their gain. This coupling ensures the seamless flow of electrons through metabolic pathways. For example, in bacterial metabolism, glucose undergoes oxidation to carbon dioxide, while oxygen is simultaneously reduced to...
Redox Equilibria: Overview01:23

Redox Equilibria: Overview

A reduction-oxidation reaction is commonly called a redox reaction. In a redox reaction, electrons are transferred from one species to another rather than being shared between or among atoms. The reducing agent or reductant is the species that loses electrons and gets oxidized in the process. The species that gains electrons and gets reduced in the process is the oxidizing agent or oxidant. Redox reactions are represented as two separate equations called half-reactions, where one equation...
The Nernst Equation02:59

The Nernst Equation

Nonstandard Reaction Conditions
The interconnection between standard cell potentials and various thermodynamic parameters such as the standard free energy change ΔG° and equilibrium constant K has been previously explored. For example, a redox reaction involving zinc(II) and tin(II) ions at 1 M concentration with Eºcell = +0.291 V and ΔG° = −56.2 kJ is spontaneous.

You might also read

Related Articles

Articles linked to this work by shared authors, journal, and citation graph.

Sort by
Same author

Synthesis and preclinical evaluation of BOLD-100 radiolabeled with ruthenium-97 and ruthenium-103.

Dalton transactions (Cambridge, England : 2003)·2024
Same author

Uranium retention in a Callovo-Oxfordian clay rock formation: From laboratory-based models to in natura conditions.

Chemosphere·2022
Same author

The impact of routine pulse oximetry use on outcomes in COVID-19-infected patients at increased risk of severe disease: A retrospective cohort analysis.

South African medical journal = Suid-Afrikaanse tydskrif vir geneeskunde·2021
Same author

New insights into the accessibility of native cellulose to environmental contaminants toward tritium behavior prediction.

Journal of hazardous materials·2021
Same author

Anti-tumor efficacy of a combination therapy with PD-L1 targeted alpha therapy and adoptive cell transfer of PD-1 deficient melanoma-specific human T-lymphocytes.

Oncoimmunology·2021
Same author

Production of scandium radionuclides for theranostic applications: towards standardization of quality requirements.

EJNMMI radiopharmacy and chemistry·2021

Related Experiment Video

Updated: Jun 17, 2026

Experimental Column Setup for Studying Anaerobic Biogeochemical Interactions Between Iron (Oxy)Hydroxides, Trace Elements, and Bacteria
06:52

Experimental Column Setup for Studying Anaerobic Biogeochemical Interactions Between Iron (Oxy)Hydroxides, Trace Elements, and Bacteria

Published on: December 19, 2017

Astatine standard redox potentials and speciation in acidic medium.

J Champion1, C Alliot, E Renault

  • 1Laboratoire SUBATECH, IN2P3/CNRS/EMN Nantes/Universite de Nantes, 4 rue A. Kastler, BP 20722, 44307 Nantes Cedex 03, France.

The Journal of Physical Chemistry. A
|December 18, 2009
PubMed
Summary

Astatine (At) does not exist as At(0) in aqueous solutions. Instead, it forms as At(-), At(+), and AtO(+) across different oxidation states, as determined by combined experimental and theoretical methods.

More Related Videos

EPR Monitored Redox Titration of the Cofactors of Saccharomyces cerevisiae Nar1
06:01

EPR Monitored Redox Titration of the Cofactors of Saccharomyces cerevisiae Nar1

Published on: November 26, 2014

Setup of Capillary Electrophoresis-Inductively Coupled Plasma Mass Spectrometry (CE-ICP-MS) for Quantification of Iron Redox Species (Fe(II), Fe(III))
04:48

Setup of Capillary Electrophoresis-Inductively Coupled Plasma Mass Spectrometry (CE-ICP-MS) for Quantification of Iron Redox Species (Fe(II), Fe(III))

Published on: May 4, 2020

Related Experiment Videos

Last Updated: Jun 17, 2026

Experimental Column Setup for Studying Anaerobic Biogeochemical Interactions Between Iron (Oxy)Hydroxides, Trace Elements, and Bacteria
06:52

Experimental Column Setup for Studying Anaerobic Biogeochemical Interactions Between Iron (Oxy)Hydroxides, Trace Elements, and Bacteria

Published on: December 19, 2017

EPR Monitored Redox Titration of the Cofactors of Saccharomyces cerevisiae Nar1
06:01

EPR Monitored Redox Titration of the Cofactors of Saccharomyces cerevisiae Nar1

Published on: November 26, 2014

Setup of Capillary Electrophoresis-Inductively Coupled Plasma Mass Spectrometry (CE-ICP-MS) for Quantification of Iron Redox Species (Fe(II), Fe(III))
04:48

Setup of Capillary Electrophoresis-Inductively Coupled Plasma Mass Spectrometry (CE-ICP-MS) for Quantification of Iron Redox Species (Fe(II), Fe(III))

Published on: May 4, 2020

Area of Science:

  • Inorganic Chemistry
  • Radiochemistry
  • Physical Chemistry

Background:

  • Astatine (At) speciation in acidic aqueous solutions remains poorly understood.
  • Key questions regarding the existence of At(0) and the chemical form of At(+III) persist in scientific literature.

Purpose of the Study:

  • To definitively establish the speciation of astatine in acidic aqueous solutions.
  • To resolve the ambiguity surrounding the existence of At(0) and the speciation of At(+III).

Main Methods:

  • Utilized a combined experimental and theoretical approach.
  • Experimentally determined distribution coefficients (D) in biphasic systems to characterize species.
  • Employed quasi-relativistic quantum chemistry calculations for theoretical insights.

Main Results:

  • Astatine in the oxidation state 0 (At(0)) cannot exist in aqueous solution.
  • The prevalent oxidation states are At(-I), At(+I), and At(+III), existing as At(-), At(+), and AtO(+), respectively, within the 1-2 pH range.
  • Determined standard redox potentials for At(+)/At(-) as 0.36 ± 0.01 V and AtO(+)/At(+) as 0.74 ± 0.01 V vs NHE.

Conclusions:

  • Astatine speciation in acidic aqueous solutions is characterized by At(-), At(+), and AtO(+).
  • The existence of At(0) in aqueous solution is refuted by this study.
  • Established the chemical forms and redox potentials for key astatine species, advancing understanding in radiochemistry.