Water volumes move volumes of water
capable of either donating
a proton
Called a hydrogen cation, H+,
known as a Brønsted–Lowry acid,
or
forming
a covalent bond with an electron pair,
known as a Lewis acid.[1]
Photodisintegration of deuterium
A photon carrying 2.22 MeV or more energy can photodisintegrate an atom of deuterium:
The first category of acids are the proton donors, or Brønsted–Lowry acids.
In the special case of aqueous solutions, proton donors form the hydronium ion H3O+ and are known as Arrhenius acids. Brønsted and Lowry generalized the Arrhenius theory to include non-aqueous solvents.
A Brønsted–Lowry or Arrhenius acid usually contains a hydrogen atom bonded to a chemical structure that is still energetically favorable after loss of H+.
Aqueous Arrhenius acids have characteristic properties that provide a practical description of an acid.[2] Acids form aqueous solutions with a sour taste and react with bases and certain metals such as calcium to form salts.
The word acid is derived from the Latin acidus, meaning 'sour'.[3] An aqueous solution of an acid has a pH less than 7 and is colloquially also referred to as "acid" (as in "dissolved in acid"), while the strict definition refers only to the solute.[1]
A lower pH means a higher acidity, and thus a higher concentration of hydrogen cations
which are otherwise called Protons and otherways called positive charges in the solution.
Chemicals or substances having the property of an acid are said to be acidic.
AC id IC then would mean Proton Charged Cat ion~s collecting at the Cat thode
The Brønsted–Lowry theory (also called proton theory of acids and bases[1]) is an acid–base reaction theory which was developed independently in 1923 by physical chemists Johannes Nicolaus Brønsted (in Denmark) and Thomas Martin Lowry (in the United Kingdom).[2][3]
The basic concept of this theory is that when an acid and a base react with each other, the acid forms its conjugate base, and the base forms its conjugate acid by exchange of a proton (the hydrogen cation, or H+). This theory generalises the Arrhenius theory.
Non-aqueous solutions
The hydrogen ion, or hydronium ion, is a Brønsted–Lowry acid when dissolved in H2O and the hydroxide ion is a base because of the autoionization of water reaction
An analogous reaction occurs in liquid ammonia
Thus, the ammonium ion, NH+4, in liquid ammonia corresponds to the hydronium ion in water and the amide ion, NH−2 in ammonia, to the hydroxide ion in water. Ammonium salts behave as acids, and metal amides behave as bases.[10]
Some non-aqueous solvents can behave as bases, i.e. accept protons, in relation to Brønsted–Lowry acids.
where S stands for a solvent molecule. The most important of such solvents are dimethylsulfoxide, DMSO, and acetonitrile, CH3CN, as these solvents have been widely used to measure the acid dissociation constants of carbon-containing molecules. Because DMSO accepts protons more strongly than H2O the acid becomes stronger in this solvent than in water.[11] Indeed, many molecules behave as acids in non-aqueous solutions but not in aqueous solutions. An extreme case occurs with carbon acids, where a proton is extracted from a C−H bond.[12]
Some non-aqueous solvents can behave as acids. An acidic solvent will make dissolved substances more basic. For example, the compound CH3COOH is known as acetic acid since it behaves as an acid in water. However, it behaves as a base in liquid hydrogen fluoride, a much more acidic solvent.[13]
A Lewis acid (named for the American physical chemist Gilbert N. Lewis) is a chemical species that contains an empty orbital which is capable of accepting an electron pair from a Lewis base to form a Lewis adduct.- A Lewis base, then, is any species that has a filled orbital containing an electron pair which is not involved in bonding but may form a dative bond with a Lewis acid to form a Lewis adduct. For example, NH3 is a Lewis base, because it can donate its lone pair of electrons. Trimethylborane [(CH3)3B] is a Lewis acid as it is capable of accepting a lone pair. In a Lewis adduct, the Lewis acid and base share an electron pair furnished by the Lewis base, forming a dative bond.[1]
- H2O + H2O ⇌ H3O+ + OH−
Chemically pure water has an electrical conductivity of 0.055 μS/cm. According to the theories of Svante Arrhenius, this must be due to the presence of ions. The ions are produced by the water self-ionization reaction, which applies to pure water and any aqueous solution:
In chemistry, pH (/piːˈeɪtʃ/ pee-AYCH) is a logarithmic scale used to specify the acidity or basicity of aqueous solutions.
Acidic solutions are solutions with high concentrations of:
protons called hydrogen or cations using the symbol H+
and are measured to have lower pH values than basic or alkaline solutions. Historically, pH denotes "potential of hydrogen" (or "power of hydrogen").[1]
The pH scale is logarithmic and inversely indicates the activity of hydrogen cations in the solution
![{\displaystyle {\ce {pH}}=-\log _{10}(a_{{\ce {H+}}})\thickapprox -\log _{10}([{\ce {H+}}]/{\text{M}})}](https://wikimedia.org/api/rest_v1/media/math/render/svg/fe31ce01f515ddddc195f7a5b6a13dd32c80a7a8)
where [H+] is the equilibrium molar concentration of H+ (in M = mol/L) in the solution. At 25 °C (77 °F), solutions of which the pH is less than 7 are acidic, and solutions of which the pH is greater than 7 are basic.
Solutions with a pH of 7 at 25 °C are neutral and have the same concentration of
H+ ions as OH− ions, the definition of pure water.
The neutral value of the pH depends on the temperature and is lower than 7 if the temperature increases above 25 °C. The pH range is commonly given as zero to 14, but a pH value can be less than 0 for very concentrated strong acids or greater than 14 for very concentrated strong bases.[2]
- The water molecule is therefore dipolar .
- The water molecule is therefore a battery.
- The net charge of the hyperboloid/triangular water molecule is zero
- The electrical field is not evenly distributed on the water molecule.
- The larger oxygen atom attracts the electrons more strongly than the smaller hydrogen.
- This gives water an asymmetrical distribution of charge to fit its asymmetrical shape
- The side of the water molecule with the hydrogen atoms has a net positive charge.
- The side of the water molecule with the hydrogen atom is the Cathode
- The side of the water molecule with the two electron orbitals is
- The side of the water molecule without protons and
- The side that has a net negative charge.
- The Anode where An ions can be found as electrons
- Molecules that have ends with partial negative and positive charges are known as polar molecules.
- It is this polar property that allows water to separate polar solute molecules and explains why water can dissolve so many substances. Water changes to neutralize itself electron/proton balance wise.
- A water molecule is formed when two atoms of hydrogen
- Two proton/electron +/- pairs Cathode/Anode Cation/Anion inverse pairs
- bond covalently aka magnetically with an atom of oxygen.
- attach in proton/electron nodes as groups of 2 or pairs
- via the organizing attraction/repulsion of polar magnetic+/- arrangement
- In a covalent bond electrons are shared between atoms.
- In a covalent bond protons share electron bonds in pairs of pairs
- In water the sharing is not equal.
- Eight Proton Electron pairs form Oxygen arranged Octagonally
- One Proton Electron pair forms Hydrogen arranged Linearly
- The oxygen atom attracts electrons more than four times as strongly as the hydrogen.
- This gives water an asymmetrical distribution of charge in a ratio of 16:2 or 8:1
- Molecules that have nodes with alternating negative and positive charges
- Are batteries and are known as polar molecules.
- It is this polar property that allows water to
- store via the organization of the Octagon and
- conduct current between separate polar solute nodes
- nodes found on molecule surfaces at geometric intervals
- and explains why water can dissolve so many substances.
- by rearranging the geometric structure of the charges as they
- display themselves when organized into apparent structure
- A covalent bond is a proton/electron
- +/-
- Cathode/Anode
- Cat ion/An ion
- Alternating
- pair
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