Advertisements
Advertisements
प्रश्न
Account for the following:
Mn2+ is more stable than Fe2+ towards oxidation to +3 state.
Advertisements
उत्तर
Electronic configuration of Mn2+ is [Ar]18 3d5 .
Electronic configuration of Fe2+ is [Ar]18 3d6 .
It is known that half-filled and fully-filled orbitals are more stable. Therefore, Mn in the +2 state has a stable d5 configuration. Therefore, Mn2+ shows resistance to oxidation to Mn3+. Also, Fe2+ has a 3d6 configuration and by losing one electron, its configuration changes to a more stable 3d5 configuration. Therefore, Fe2+ gets oxidised to Fe3+ easily.
APPEARS IN
संबंधित प्रश्न
Silver atom has completely filled d orbitals (4d10) in its ground state. How can you say that it is a transition element?
Explain giving reason:
Transition metals and many of their compounds show paramagnetic behaviour.
Write down the electronic configuration of Cu+.
Write down the electronic configuration of Ce4+.
Name the elements of 3d transition series that show maximum number of oxidation states. Why does this happen?
Which among the following elements does not belong to the first transition series?
Which among the following is not considered as a part of transition elements?
The element with electronic configuration [xe]544f145d16S2 belongs to
Define transition metals.
Assertion (A) : Copper is a non-transition element.
Reason (R) : Copper has completely filled d-orbitals in its ground state.
