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
Write down the electronic configuration of Co2+.
Write down the electronic configuration of Th4+.
Write the different oxidation states of manganese.
Which transition metal of 3d series has positive E° (M2+/M) value and why?
Electronic configuration of Cu3+ is ____________.
The electronic configuration of \[\ce{Cu(II)}\] is 3d9 whereas that of \[\ce{Cu(I)}\] is 3d10. Which of the following is correct?
Zn2+ ion is iso – electronic with
Name the element of 3d series which exhibits the largest number of oxidation states. Give reason.
Assertion (A) : Copper is a non-transition element.
Reason (R) : Copper has completely filled d-orbitals in its ground state.
Write down the electronic configuration of:
\[\ce{CO^2+}\]
