Barium in group 2 has just two oxidation numbers, 0 in the metal, +2 in its compounds.
BA is in the group2. It generally shows +2 oxidation state.
Metallic aluminium has the oxidation number zero. In compounds in the form of ions, it takes the oxidation number +III.Metallic aluminium has the oxidation number zero. In compounds in the form of ions, it takes the oxidation number +III.
In a reaction where one reactant is being oxidised another reactant is necessarily being reduced. Reduction cannot occur without oxidation, and vice versa.
You didn't say what the reactant is? Example 2NaCl → 2Na + Cl2 reactant is on the left so it's NaCl So the state is solid or salt to be specific.
Regarding the oxidation states of the atoms in the tetrathionate ion: The tetrathionate polyatomic ion is made of four sulfur atoms, each with an oxidation number of +1, and six oxygen atoms each with an oxidation number of -1. Note, this is one of the rare exceptions to the 'rule' that oxygen normally has a minus two oxidation number. Other -1 oxygen compounds are the peroxides. An interesting half reaction is the oxidation of two thiosulfate ions to tetrathionate, in which sulfur has an oxidation number of +2 in the reactant and +1 in the product. Oxygen has an oxidation number of -2 in the reactant, and -1 in the product. 2S2O3-2 ----> S4O6-2 + 2 e-
BA is in the group2. It generally shows +2 oxidation state.
Metallic aluminium has the oxidation number zero. In compounds in the form of ions, it takes the oxidation number +III.Metallic aluminium has the oxidation number zero. In compounds in the form of ions, it takes the oxidation number +III.
Minimum oxidation number: -1 Maximum oxidation number: 1 Min. common oxidation no.: 0 Max. common oxidation no.: 1 I got this of a really cool website that has alot of infromation and useful facts about each element and trust me you'll use it a lot in chemistry. www.chemicool.com
In a reaction where one reactant is being oxidised another reactant is necessarily being reduced. Reduction cannot occur without oxidation, and vice versa.
In these reaction, an element simultaneously undergoes oxidation as well as reduction. This is possible only when the element exhibits minimum three different oxidation states and on the reactant side, it is present in an intermediate oxidation state while higher and lower oxidation states are exhibited by it in the form of products.
Barium is +2 valenced ion, so its oxidation state is +2 in ion form (Ba2+) and 0 in elemental (Ba) form
false
You didn't say what the reactant is? Example 2NaCl → 2Na + Cl2 reactant is on the left so it's NaCl So the state is solid or salt to be specific.
The Krebs cycle uses acetyl CoA as a reactant.
Regarding the oxidation states of the atoms in the tetrathionate ion: The tetrathionate polyatomic ion is made of four sulfur atoms, each with an oxidation number of +1, and six oxygen atoms each with an oxidation number of -1. Note, this is one of the rare exceptions to the 'rule' that oxygen normally has a minus two oxidation number. Other -1 oxygen compounds are the peroxides. An interesting half reaction is the oxidation of two thiosulfate ions to tetrathionate, in which sulfur has an oxidation number of +2 in the reactant and +1 in the product. Oxygen has an oxidation number of -2 in the reactant, and -1 in the product. 2S2O3-2 ----> S4O6-2 + 2 e-
-2 oxidation state
K = +1 oxidation state Cl = +3 oxidation state O = -2 oxidation state