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Page "Actinium" ¶ 7
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oxidation and state
As with most lanthanides and actinides, actinium assumes oxidation state + 3 in nearly all its chemical compounds.
As with most lanthanides and actinides, actinium exists in the oxidation state + 3, and the Ac < sup > 3 +</ sup > ions are colorless in solutions.
The oxidation state + 3 originates from the 6d < sup > 1 </ sup > 7s < sup > 2 </ sup > electronic configuration of actinium, that is it easily donates 3 electrons assuming a stable closed-shell structure of the noble gas radon.
Except for AcPO < sub > 4 </ sub >, they are all similar to the corresponding lanthanum compounds and contain actinium in the oxidation state + 3.
In chemical compounds, they usually assume the oxidation state + 3, especially in solutions.
It always exhibits the oxidation state of + 2.
To separate berkelium from the unreacted americium, this solution was added to a mixture of ammonium and ammonium sulfate and heated to convert all the dissolved americium into the oxidation state + 6.
This trivalent oxidation state (+ 3 ) is the most stable, especially in aqueous solutions, but tetravalent (+ 4 ) and possibly divalent (+ 2 ) berkelium compounds are also known.
Chemical experiments have confirmed bohrium's predicted position as a heavier homologue to rhenium with the formation of a stable + 7 oxidation state.
The atom is also the smallest entity that can be envisaged to retain the chemical properties of the element, such as electronegativity, ionization potential, preferred oxidation state ( s ), coordination number, and preferred types of bonds to form ( e. g., metallic, ionic, covalent ).
The most common oxidation state of carbon in inorganic compounds is + 4, while + 2 is found in carbon monoxide and other transition metal carbonyl complexes.
This conversion to the right is called disproportionation, because the ingredient chlorine both increases and decreases in formal oxidation state.
Chlorine exists in all odd numbered oxidation states from − 1 to + 7, as well as the elemental state of zero and four in chlorine dioxide ( see table below, and also structures in chlorite ).
A few calcium compounds in the oxidation state + 1 have also been investigated recently.
Like zinc, it prefers oxidation state + 2 in most of its compounds and like mercury it shows a low melting point compared to transition metals.
Although cadmium usually has an oxidation state of + 2, it also exists in the + 1 state.
The oxidation state + 1 can be reached by dissolving cadmium in a mixture of cadmium chloride and aluminium chloride, forming the Cd < sub > 2 </ sub >< sup > 2 +</ sup > cation, which is similar to the Hg < sub > 2 </ sub >< sup > 2 +</ sup > cation in mercury ( I ) chloride.
Complexation reactions also include ligand exchange, in which one or more ligands are replaced by another, and redox processes which change the oxidation state of the central metal atom.
Isovalent substitution is where the ion that is substituting the original ion is of the same oxidation state as the ion it is replacing.
Aliovalent substitution is where the ion that is substituting the original ion is of a different oxidation state as the ion it is replacing.
All the members of the group readily portray their oxidation state of + 5 and the state becomes more stable as the group is descended.
Being a typical member of the lanthanide series, europium usually assumes the oxidation state + 3, but the oxidation state + 2 is also common: all europium compounds with oxidation state + 2 are slightly reducing.

oxidation and +
Several other oxidation states are known, which range from + 2 to + 7 and can be identified by their characteristic optical absorption spectra.
Dysprosium combines with various non-metals at high temperatures to form binary compounds with varying composition and oxidation states + 3 and sometimes + 2, such as DyN, DyP, DyH < sub > 2 </ sub > and DyH < sub > 3 </ sub >; DyS, DyS < sub > 2 </ sub >, Dy < sub > 2 </ sub > S < sub > 3 </ sub > and Dy < sub > 5 </ sub > S < sub > 7 </ sub >; DyB < sub > 2 </ sub >, DyB < sub > 4 </ sub >, DyB < sub > 6 </ sub > and DyB < sub > 12 </ sub >, as well as Dy < sub > 3 </ sub > C and Dy < sub > 2 </ sub > C < sub > 3 </ sub >.
For this group, + 4 and + 3 states are also known for the heavier members and dubnium may also form these reducing oxidation states.

oxidation and 2
The method initiates by converting mercury into Hg < sup > 2 +</ sup > by oxidation from nitric and sulfuric acids, followed by a reduction of Hg < sup > 2 +</ sup > with tin ( II ) chloride.
The role of the bacteria is the further oxidation of the ore, but also the regeneration of the chemical oxidant Fe < sup > 3 +</ sup > from Fe < sup > 2 +</ sup >.
2 cups / day ) significantly reduced lipid oxidation and increased plasma antioxidant capacity in women with metabolic syndrome.

oxidation and is
Once the grains are ground, vitamin E begins to deteriorate immediately and half of it is lost by oxidation and exposure to the air within one week.
The oxidation pathway starts with the removal of the amino group by a transaminase, the amino group is then fed into the urea cycle.
Following months to years of photo-degradation and oxidation in the ocean, this precursor gradually hardens, developing a dark gray or black color, a crusty and waxy texture, and a peculiar odor that is at once sweet, earthy, marine, and animalic.
In electrochemistry, the anode is where oxidation occurs and is the positive polarity contact in an electrolytic cell.
If, conversely, tin is used to coat steel, when a breach of the coating occurs it actually accelerates oxidation of the iron.
An antioxidant is a molecule that inhibits the oxidation of other molecules.
Early research on the role of antioxidants in biology focused on their use in preventing the oxidation of unsaturated fats, which is the cause of rancidity.
Peroxide is also produced from the oxidation of reduced flavoproteins, such as complex I.
They showed by oxidizing boron with air that boric acid is an oxidation product of boron.
The critical reaction is the oxidation of sulfide by ferric iron.
It is believed that early in the Earth's history, the evolution of photosynthetic plants altered the global atmosphere of the earth, changing the ancient atmosphere by oxidation.
Respiration is the oxidation of carbon whereby it is broken down into simpler structures ; essentially the opposite of photosynthesis.
Vitamin C is especially prone to oxidation during cooking and may be completely destroyed by protracted cooking.
Combustion is not necessarily favorable to the maximum degree of oxidation and it can be temperature-dependent.

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