Question

why oxidation number of certain element have a long range??​

Answer 1

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Answer 2

Following is the reason for a long range of oxidation number:

Explanation:

• The largest part of transition metals has numerous oxidation states, since it is comparatively easy to lose electron(s) for transition metals paralleled to the alkali metals and alkaline earth metals.  

• Alkali metals have only 1 electron in their valence s-orbital and hence their oxidation state is nearly always +1 (from losing it) and alkaline earth metals have 2 electrons in their valences-orbital, causing an oxidation state of +2 (from losing both).  

• This is not the case for transition metals as they have 5 d-orbitals. The d-orbital has a range of oxidation states. The s-orbital also donates to governing the oxidation states.

• For remembering the stability of higher oxidation states for transition metals it is vital to know the trend: the stability of the higher oxidation states gradually increases down a group.  

• For example, in group 6, (chromium) Cr is most stable at +3 oxidation state, giving that we would not find many stable forms of Cr in the +4 and +5 oxidation states.

• By conflict, there are several stable forms of Tungsten (W) and Molybdenum (Mo) at +5 and +4 oxidation states.