Why do the transition elements exhibit variable oxidation states?

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(N/A) Transition elements exhibit variable oxidation states because their $(n-1)d$ and $ns$ orbitals have comparable energies.
The general electronic configuration of transition elements is $(n-1)d^{1-10}ns^{1-2}$.
Since the energy difference between the $(n-1)d$ and $ns$ orbitals is very small,electrons from both shells can participate in chemical bond formation.
For the first transition series,the $4s$ electrons are primarily responsible for lower oxidation states,while both $3d$ and $4s$ electrons contribute to higher oxidation states.
The table below illustrates the oxidation states of the first transition series:
$Sc$$Ti$$V$$Cr$$Mn$$Fe$$Co$$Ni$$Cu$$Zn$
$+2$$+2$$+2$$+2$$+2$$+2$$+2$$+1$$+2$
$+3$$+3$$+3$$+3$$+3$$+3$$+3$$+3$$+2$
$+4$$+4$$+4$$+4$$+4$$+4$$+4$
$+5$$+5$$+5$
$+6$$+6$$+6$
$+7$

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