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?
Write down the electronic configuration of Cr3+.
Write down the electronic configuration of Pm3+.
Write down the electronic configuration of Cu+.
Write down the electronic configuration of Ce4+.
Write down the electronic configuration of Co2+.
Write down the electronic configuration of Th4+.
What is effective atomic number of Fe (z = 26) in [Fe(CN)6]4-?
(a) 12
(b) 30
(c) 26
(d) 36
The element with electronic configuration [xe]544f145d16S2 belongs to
Explain the observation, at the end of each period, there is a slight increase in the atomic radius of d-block elements.
