Due to different reasons phosphorus and vanadium exhibit variable oxidation states.What are the reasons for their variable oxidation states in each of the case?
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The transition elements have outer electrons that occupy a very large shell.
This is a table that shows each element's outermost electron shell configuration.
Why do transition elements exhibit variable oxidation numbers or variable valency?
The transition elements have outer electrons that occupy a very large shell.
This is a table that shows each element's outermost electron shell configuration.
The cyan colored elements are all transition metals (although the lanthanide and actinide series are also technically transition metals). The transition metals are all metals and therefore have a tendency to lose electrons, but because these electrons in the highest energy level are actually on a lower principal energy number than the ones before them (ie the first row of transition metals fills the 3d shell, and the 4s shell had already been filled), this makes it relatively easy to lose some or all of their electrons to land in stable states.
This is a table that shows each element's outermost electron shell configuration.
Why do transition elements exhibit variable oxidation numbers or variable valency?
The transition elements have outer electrons that occupy a very large shell.
This is a table that shows each element's outermost electron shell configuration.
The cyan colored elements are all transition metals (although the lanthanide and actinide series are also technically transition metals). The transition metals are all metals and therefore have a tendency to lose electrons, but because these electrons in the highest energy level are actually on a lower principal energy number than the ones before them (ie the first row of transition metals fills the 3d shell, and the 4s shell had already been filled), this makes it relatively easy to lose some or all of their electrons to land in stable states.
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