Na2S2O3 oxidation number
Oxidation no of sulphur is +2.
This compound is sodium thiosulphate. S represents +6 oxidation number.
The oxidation numbers for elements in Group 1A (alkali metals) are typically +1. For elements in Group 2A (alkaline earth metals), the oxidation number is typically +2.
There is at least one oxidation number shared by all the elements in a periodic table column, but some of the elements may have more than one oxidation number and some of these additional oxidation numbers may not be possible for all the elements in a column.
Elements with oxidation numbers of +1 include elements in Group 1 of the periodic table, like hydrogen and sodium. Elements with oxidation numbers of -1 include elements in Group 17, like fluorine and chlorine.
Oxidation no of sulphur is +2.
The oxidation number of Sulfur (S) in Na2S2O3 is +2. This is because the overall charge of the compound is zero, and since each Sodium (Na) atom has an oxidation state of +1, the oxidation state of Sulfur must be +2 to balance the charges in the compound.
Oxidation numbers in Fe2O3 are respectively: Fe => +3 and O => -2
This compound is sodium thiosulphate. S represents +6 oxidation number.
The oxidation numbers for elements in Group 1A (alkali metals) are typically +1. For elements in Group 2A (alkaline earth metals), the oxidation number is typically +2.
There is at least one oxidation number shared by all the elements in a periodic table column, but some of the elements may have more than one oxidation number and some of these additional oxidation numbers may not be possible for all the elements in a column.
Elements with oxidation numbers of +1 include elements in Group 1 of the periodic table, like hydrogen and sodium. Elements with oxidation numbers of -1 include elements in Group 17, like fluorine and chlorine.
The oxidation numbers of the elements in a compound must add up to zero. This is because in a compound, the overall charge is neutral. The sum of the oxidation numbers helps determine the charge of the compound.
The oxidation numbers in group A elements typically increase by one as you move from left to right across the periodic table. For example, group 1 elements usually have an oxidation state of +1, while group 7 elements typically have an oxidation state of -1.
Elements with fixed oxidation numbers include alkali metals (group 1 elements) which have a +1 oxidation state, alkaline earth metals (group 2 elements) which have a +2 oxidation state, and nonmetals in group 17 (halogens) which have a -1 oxidation state in compounds.
Of course they can have.Many elements have several oxidation numbers.
The oxidation number of an atom is determined by the number of electrons it gains, loses, or shares when forming a chemical bond. The rules for assigning oxidation numbers are based on the electronegativity of the elements and the structure of the compound. Generally, less electronegative elements have more positive oxidation numbers, while more electronegative elements have more negative oxidation numbers.