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Hydrogen ion

February 16, 2024

A hydrogen ion is created when a hydrogen atom loses an electron. A positively charged hydrogen ion (or proton) can readily combine with other particles and therefore is only seen isolated when it is in a gaseous state or a nearly particle-free space.[1] Due to its extremely high charge density of approximately 2×1010 times that of a sodium ion, the bare hydrogen ion cannot exist freely in solution as it readily hydrates, i.e., bonds quickly.[2] The hydrogen ion is recommended by IUPAC as a general term for all ions of hydrogen and its isotopes.[3] Depending on the charge of the ion, two different classes can be distinguished: positively charged ions and negatively charged ions.

Cation (positively charged) edit

Main article: Hydron (chemistry)
 
Zundel cation

A hydrogen atom is made up of a nucleus with charge +1, and a single electron. Therefore, the only positively charged ion possible has charge +1. It is noted H+.

Depending on the isotope in question, the hydrogen cation has different names:

In addition, the ions produced by the reaction of these cations with water as well as their hydrates are called hydrogen ions:

Zundel cations and Eigen cations play an important role in proton diffusion according to the Grotthuss mechanism.

In connection with acids, "hydrogen ions" typically refers to hydrons.

 

In the image at left the hydrogen atom (center) contains a single proton and a single electron. Removal of the electron gives a cation (left), whereas addition of an electron gives an anion (right). The hydrogen anion, with its loosely held two-electron cloud, has a larger radius than the neutral atom, which in turn is much larger than the bare proton of the cation. Hydrogen forms the only cation that has no electrons, but even cations that (unlike hydrogen) still retain one or more electrons are still smaller than the neutral atoms or molecules from which they are derived.

Anion (negatively charged) edit

Main article: Hydrogen anion

Hydrogen anions are formed when additional electrons are acquired:

  • Hydride: general name referring to the negative ion of any hydrogen isotope (H−)
  • Protide: 1H−
  • Deuteride: 2H−, D −
  • Tritide: 3H−, T −

Uses edit

Hydrogen ions drive ATP synthase in photosynthesis. This happens when hydrogen ions get pushed across the membrane creating a high concentration inside the thylakoid membrane and a low concentration in the cytoplasm. However, because of osmosis, the H+ will force itself out of the membrane through ATP synthase. Using their kinetic energy to escape, the protons will spin the ATP synthase which in turn will create ATP. This happens in cellular respiration as well though the concentrated membrane will instead be the inner membrane of the mitochondria.

Hydrogen ions concentration, measured as pH, is also responsible for the acidic or basic nature of a compound. Water molecules split to form H+ and hydroxide anions. This process is referred to as the self-ionization of water.

Ocean acidification edit

The concentration of hydrogen ions and pH are inversely proportional; in an aqueous solution, an increased concentration of hydrogen ions yields a low pH, and subsequently, an acidic product. By definition, an acid is an ion or molecule that can donate a proton, and when introduced to a solution it will react with water molecules (H2O) to form a hydronium ion (H3O+), a conjugate acid of water.[4] For simplistic reasoning, the hydrogen ion (H+) is often used to abbreviate the hydronium ion.

Ocean acidification is the direct consequence of elevated concentrations of hydrogen ions and carbonate saturation from significant absorption of carbon dioxide (CO2) by the world's oceans.[5] The pre-industrial state of the ocean's carbonate chemistry has been notably stable, including the balance of its pH.[6] Following the industrial revolution, anthropogenic emissions of burning fossil fuels, cement production, and changes in land use, have increased the oceans uptake of carbon dioxide from the atmosphere by 30%.[7] In the ocean, the absorption capacity of this greenhouse gas is 59 times higher than in the atmosphere;[8] the ocean acts as the largest carbon sink on the planet, playing a significant role in climate regulation.[9] In addition to carbon fluxes, the natural process of carbon sequestration from the atmosphere into the deep ocean is facilitated by two systems, the biological pump and the solubility pump. The solubility pump is a physico-chemical process that transfers CO2 at the air-sea interface.[10] Based on Henry's Law, the amount of dissolved CO2 in an aqueous solution is directly proportional to the partial pressure of CO2 in the atmosphere.[11] To maintain equilibrium, a state of high atmospheric partial pressure of CO2 leads to an increased oceanic exchange of this gas by molecular diffusion.

In the surface waters, dissolved atmospheric carbon dioxide (CO2(aq)) reacts with water molecules to form carbonic acid (H2CO3), a weak diprotic acid. Diprotic acids consist of two ionizable hydrogen atoms in each molecule.[12] In an aqueous solution, partial dissociation of carbonic acid releases a hydrogen proton (H+) and a bicarbonate ion (HCO3−), and subsequently, the bicarbonate ion dissociates into an additional hydrogen proton and a carbonate ion (CO32-).[13] The dissolving and dissociating of these inorganic carbon species generate an increase in the concentration of hydrogen ions and inversely lowers ambient surface ocean pH. The carbonate buffering system governs the acidity of seawater by maintaining dissolved inorganic carbon species in chemical equilibrium.

The chemical equation consists of reactants and products that may react in either direction. More reactants added to a system yield more product production (the chemical reaction shifts to the right) and if more product is added, additional reactants will form, shifting the chemical reaction to the left. Therefore, in this model, a high concentration of the beginning reactant, carbon dioxide, produces an increased amount of end-product (H+ and CO32-), thus lowering pH and creating a more acidic solution. The natural buffering system of the ocean resist the change in pH by producing more bicarbonate ions generated by free acid protons reacting with carbonate ions to form an alkaline character.[14] However, increasing atmospheric CO2 concentrations may exceed the buffering capacity threshold, consequently resulting in higher rates of ocean acidification. Shifts in the ocean's carbonate chemistry has the potential to manipulate ocean biogeochemical cycles for many elements and compounds causing profound impacts on marine ecosystems. Furthermore, the solubility of CO2 is temperature dependent; elevated surface water temperatures reduce CO2 solubility. A continual rise in atmospheric partial pressure of CO2 could potentially convert the ocean from acting as sink (the vertical transport of carbon to the depths of the ocean) to becoming a source (CO2 degassing from the ocean), further increasing global temperatures.[15]

See also edit

References edit

  1. ^ "Hydrogen ion - chemistry". britannica.com. Retrieved 18 March 2018.
  2. ^ due to its extremely high charge density of approximately 2×1010 times that of a sodium ion
  3. ^ Compendium of Chemical Terminology, 2nd edition McNaught, A.D. and Wilkinson, A. Blackwell Science, 1997 ISBN 0-86542-684-8, also online 2005-12-12 at the Wayback Machine
  4. ^ OpenStax, Chemistry. OpenStax CNX. Jun 20, 2016 http://cnx.org/contents/85abf193-2bd2-4908-8563-90b8a7ac8df6@9.311.
  5. ^ W.S. Broecker, T. Takahashi (1997) Neutralization of fossil fuel CO2 by marine calcium carbonate
  6. ^ P.N. Pearson, M.R. Palmer (2000) Atmospheric carbon dioxide concentrations over the past 60 million years Nature, 406, pp. 695-699
  7. ^ C.L. Sabine, et al. (2004). The oceanic sink for anthropogenic CO2 Science, 305 (5682), pp. 367-371
  8. ^ Lal R. (2008). Carbon sequestration. Philosophical transactions of the Royal Society of London. Series B, Biological sciences, 363(1492), 815–830. https://doi.org/10.1098/rstb.2007.2185
  9. ^ Ben I. Mcneil & Richard J. Matear (2007). Climate change feedbacks on future oceanic acidification, Tellus B: Chemical and Physical Meteorology, 59:2, 191-198
  10. ^ Hessen, D., Ågren, G., Anderson, T., Elser, J., & De Ruiter, P. (2004). Carbon Sequestration in Ecosystems: The Role of Stoichiometry. Ecology, 85(5), 1179-1192. Retrieved November 22, 2020, from http://www.jstor.org/stable/3450161
  11. ^ Avishay DM, Tenny KM. Henry's Law. [Updated 2020 Sep 7]. In: StatPearls [Internet]. Treasure Island (FL): StatPearls Publishing; 2020 Jan-. Available from: https://www.ncbi.nlm.nih.gov/books/NBK544301/
  12. ^ OpenStax, Chemistry. OpenStax CNX. Jun 20, 2016 http://cnx.org/contents/85abf193-2bd2-4908-8563-90b8a7ac8df6@9.311.
  13. ^ OpenStax, Chemistry. OpenStax CNX. Jun 20, 2016 http://cnx.org/contents/85abf193-2bd2-4908-8563-90b8a7ac8df6@9.311.
  14. ^ Middelburg, J. J., Soetaert, K., & Hagens, M. (2020). Ocean Alkalinity, Buffering and Biogeochemical Processes. Reviews of geophysics (Washington, D.C. : 1985), 58(3), e2019RG000681. https://doi.org/10.1029/2019RG000681
  15. ^ Matsumoto, K. (2007). Biology-mediated temperature control on atmosphericpCO2and ocean biogeochemistry. Geophysical Research Letters, 34(20). doi:10.1029/2007gl031301

February 16, 2024
hydrogen, this, article, needs, additional, citations, verification, please, help, improve, this, article, adding, citations, reliable, sources, unsourced, material, challenged, removed, find, sources, news, newspapers, books, scholar, jstor, october, 2014, le. This article needs additional citations for verification Please help improve this article by adding citations to reliable sources Unsourced material may be challenged and removed Find sources Hydrogen ion news newspapers books scholar JSTOR October 2014 Learn how and when to remove this template message A hydrogen ion is created when a hydrogen atom loses an electron A positively charged hydrogen ion or proton can readily combine with other particles and therefore is only seen isolated when it is in a gaseous state or a nearly particle free space 1 Due to its extremely high charge density of approximately 2 1010 times that of a sodium ion the bare hydrogen ion cannot exist freely in solution as it readily hydrates i e bonds quickly 2 The hydrogen ion is recommended by IUPAC as a general term for all ions of hydrogen and its isotopes 3 Depending on the charge of the ion two different classes can be distinguished positively charged ions and negatively charged ions Contents 1 Cation positively charged 2 Anion negatively charged 3 Uses 4 Ocean acidification 5 See also 6 ReferencesCation positively charged editMain article Hydron chemistry nbsp Zundel cationA hydrogen atom is made up of a nucleus with charge 1 and a single electron Therefore the only positively charged ion possible has charge 1 It is noted H Depending on the isotope in question the hydrogen cation has different names Hydron general name referring to the positive ion of any hydrogen isotope H Proton 1H i e the cation of protium Deuteron 2H D Triton 3H T In addition the ions produced by the reaction of these cations with water as well as their hydrates are called hydrogen ions Hydronium ion H3O Zundel cation H5O2 named for Georg Zundel Eigen cation H9O4 or H3O 3H2O named for Manfred Eigen Zundel cations and Eigen cations play an important role in proton diffusion according to the Grotthuss mechanism In connection with acids hydrogen ions typically refers to hydrons nbsp In the image at left the hydrogen atom center contains a single proton and a single electron Removal of the electron gives a cation left whereas addition of an electron gives an anion right The hydrogen anion with its loosely held two electron cloud has a larger radius than the neutral atom which in turn is much larger than the bare proton of the cation Hydrogen forms the only cation that has no electrons but even cations that unlike hydrogen still retain one or more electrons are still smaller than the neutral atoms or molecules from which they are derived Anion negatively charged editMain article Hydrogen anion Hydrogen anions are formed when additional electrons are acquired Hydride general name referring to the negative ion of any hydrogen isotope H Protide 1H Deuteride 2H D Tritide 3H T Uses editHydrogen ions drive ATP synthase in photosynthesis This happens when hydrogen ions get pushed across the membrane creating a high concentration inside the thylakoid membrane and a low concentration in the cytoplasm However because of osmosis the H will force itself out of the membrane through ATP synthase Using their kinetic energy to escape the protons will spin the ATP synthase which in turn will create ATP This happens in cellular respiration as well though the concentrated membrane will instead be the inner membrane of the mitochondria Hydrogen ions concentration measured as pH is also responsible for the acidic or basic nature of a compound Water molecules split to form H and hydroxide anions This process is referred to as the self ionization of water Ocean acidification editThe concentration of hydrogen ions and pH are inversely proportional in an aqueous solution an increased concentration of hydrogen ions yields a low pH and subsequently an acidic product By definition an acid is an ion or molecule that can donate a proton and when introduced to a solution it will react with water molecules H2O to form a hydronium ion H3O a conjugate acid of water 4 For simplistic reasoning the hydrogen ion H is often used to abbreviate the hydronium ion Ocean acidification is the direct consequence of elevated concentrations of hydrogen ions and carbonate saturation from significant absorption of carbon dioxide CO2 by the world s oceans 5 The pre industrial state of the ocean s carbonate chemistry has been notably stable including the balance of its pH 6 Following the industrial revolution anthropogenic emissions of burning fossil fuels cement production and changes in land use have increased the oceans uptake of carbon dioxide from the atmosphere by 30 7 In the ocean the absorption capacity of this greenhouse gas is 59 times higher than in the atmosphere 8 the ocean acts as the largest carbon sink on the planet playing a significant role in climate regulation 9 In addition to carbon fluxes the natural process of carbon sequestration from the atmosphere into the deep ocean is facilitated by two systems the biological pump and the solubility pump The solubility pump is a physico chemical process that transfers CO2 at the air sea interface 10 Based on Henry s Law the amount of dissolved CO2 in an aqueous solution is directly proportional to the partial pressure of CO2 in the atmosphere 11 To maintain equilibrium a state of high atmospheric partial pressure of CO2 leads to an increased oceanic exchange of this gas by molecular diffusion In the surface waters dissolved atmospheric carbon dioxide CO2 aq reacts with water molecules to form carbonic acid H2CO3 a weak diprotic acid Diprotic acids consist of two ionizable hydrogen atoms in each molecule 12 In an aqueous solution partial dissociation of carbonic acid releases a hydrogen proton H and a bicarbonate ion HCO3 and subsequently the bicarbonate ion dissociates into an additional hydrogen proton and a carbonate ion CO32 13 The dissolving and dissociating of these inorganic carbon species generate an increase in the concentration of hydrogen ions and inversely lowers ambient surface ocean pH The carbonate buffering system governs the acidity of seawater by maintaining dissolved inorganic carbon species in chemical equilibrium The chemical equation consists of reactants and products that may react in either direction More reactants added to a system yield more product production the chemical reaction shifts to the right and if more product is added additional reactants will form shifting the chemical reaction to the left Therefore in this model a high concentration of the beginning reactant carbon dioxide produces an increased amount of end product H and CO32 thus lowering pH and creating a more acidic solution The natural buffering system of the ocean resist the change in pH by producing more bicarbonate ions generated by free acid protons reacting with carbonate ions to form an alkaline character 14 However increasing atmospheric CO2 concentrations may exceed the buffering capacity threshold consequently resulting in higher rates of ocean acidification Shifts in the ocean s carbonate chemistry has the potential to manipulate ocean biogeochemical cycles for many elements and compounds causing profound impacts on marine ecosystems Furthermore the solubility of CO2 is temperature dependent elevated surface water temperatures reduce CO2 solubility A continual rise in atmospheric partial pressure of CO2 could potentially convert the ocean from acting as sink the vertical transport of carbon to the depths of the ocean to becoming a source CO2 degassing from the ocean further increasing global temperatures 15 See also editAcid Protonation Dihydrogen cation Trihydrogen cationReferences edit Hydrogen ion chemistry britannica com Retrieved 18 March 2018 due to its extremely high charge density of approximately 2 1010 times that of a sodium ion Compendium of Chemical Terminology 2nd edition McNaught A D and Wilkinson A Blackwell Science 1997 ISBN 0 86542 684 8 also online Archived 2005 12 12 at the Wayback Machine OpenStax Chemistry OpenStax CNX Jun 20 2016 http cnx org contents 85abf193 2bd2 4908 8563 90b8a7ac8df6 9 311 W S Broecker T Takahashi 1997 Neutralization of fossil fuel CO2 by marine calcium carbonate P N Pearson M R Palmer 2000 Atmospheric carbon dioxide concentrations over the past 60 million years Nature 406 pp 695 699 C L Sabine et al 2004 The oceanic sink for anthropogenic CO2 Science 305 5682 pp 367 371 Lal R 2008 Carbon sequestration Philosophical transactions of the Royal Society of London Series B Biological sciences 363 1492 815 830 https doi org 10 1098 rstb 2007 2185 Ben I Mcneil amp Richard J Matear 2007 Climate change feedbacks on future oceanic acidification Tellus B Chemical and Physical Meteorology 59 2 191 198 Hessen D Agren G Anderson T Elser J amp De Ruiter P 2004 Carbon Sequestration in Ecosystems The Role of Stoichiometry Ecology 85 5 1179 1192 Retrieved November 22 2020 from http www jstor org stable 3450161 Avishay DM Tenny KM Henry s Law Updated 2020 Sep 7 In StatPearls Internet Treasure Island FL StatPearls Publishing 2020 Jan Available from https www ncbi nlm nih gov books NBK544301 OpenStax Chemistry OpenStax CNX Jun 20 2016 http cnx org contents 85abf193 2bd2 4908 8563 90b8a7ac8df6 9 311 OpenStax Chemistry OpenStax CNX Jun 20 2016 http cnx org contents 85abf193 2bd2 4908 8563 90b8a7ac8df6 9 311 Middelburg J J Soetaert K amp Hagens M 2020 Ocean Alkalinity Buffering and Biogeochemical Processes Reviews of geophysics Washington D C 1985 58 3 e2019RG000681 https doi org 10 1029 2019RG000681 Matsumoto K 2007 Biology mediated temperature control on atmosphericpCO2and ocean biogeochemistry Geophysical Research Letters 34 20 doi 10 1029 2007gl031301 nbsp This article includes a list of related items that share the same name or similar names If an internal link incorrectly led you here you may wish to change the link to point directly to the intended article Retrieved from https en wikipedia org w index php title Hydrogen ion amp oldid 1175924185, wikipedia, wiki, book, books, library,

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