The oxidation number is 0 in elemental form. It can have other oxidation numbers as -2, +4 and +6 in its compounds such as H2S, SO2 and SO3 respectively.
-2, 0, 2, 4 and 6 oxidation states
Oxidation numbers from -2 to +6 are possible. Some examples are given: -2 in sulphides; 0 in the elemental form; +4 in SO2, +6 in SO3
When considered the compound as a whole, it has the oxidation number of zero. When it is considered as ions the hydrogen ions has +I and sulfate ion -II oxidation numbers. When compared with respect to elements, sulfur has +VI, hydrogen has +I and oxygen has -II as their oxidation numbers.
Because they have the same number of valence electrons
The oxidation number in atomic sulfur is 0. With other non metals, it produces many ions where its oxidation number varies from -2 to +6. The oxidation number of sulfide ion (which is produced usually with ions from metals) is -2.
This should be SO4-2 ion. sulfur shows +6 in this ion.
This should be SO4-2 ion. sulfur shows +6 in this ion.
The oxidation number of an atom in a compound depends on what is attached to it.The following are examples of oxidation numbers (ON #)for sulfur :S8 ON # 0H2S ON # -2SO2 ON # +4SO3 ON # +6H2SO4 ON# +6
There are s8 sulfur molecules. It shows 0 oxidation number.
generally sulphur shows many numbers. It has 0 in S8 molecules.
For most elements, their highest attainable oxidation number is equal to the number of valence electrons. Examples are the maximum oxidation numbers for: sulfur is +6, phosphorus is +5 and chlorine is +7. Fluorine is an exception which bears oxidation numbers 0, -1/2 and -1.
The only oxidation number is 2+.
Sulfur can have a wide range of oxidation in its compounds -2 in H2S 0 in elementary sulfur (S8) +4 in SO2 +6 in SO3
The oxidation state of an individual sulfur atom in BaSo4 is +6.