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प्रश्न
Account for the following:
Mn2+ is more stable than Fe2+ towards oxidation to +3 state.
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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.
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संबंधित प्रश्न
Write down the electronic configuration of Pm3+.
Write down the electronic configuration of Th4+.
Write the different oxidation states of manganese.
Name the elements of 3d transition series that show maximum number of oxidation states. Why does this happen?
The electronic configuration of \[\ce{Cu(II)}\] is 3d9 whereas that of \[\ce{Cu(I)}\] is 3d10. Which of the following is correct?
Explain the observation, at the end of each period, there is a slight increase in the atomic radius of d-block elements.
Define transition metals.
Assertion (A) : Copper is a non-transition element.
Reason (R) : Copper has completely filled d-orbitals in its ground state.
Match the properties with the elements of 3d series:
| (i) | lowest enthalpy of atomisation | (p) | Sc |
| (ii) | shows maximum number of oxidation states | (q) | Mn |
| (iii) | transition metal that does not form coloured compounds |
(r) | Zn |
| (s) | Ti |
Write down the electronic configuration of:
\[\ce{CO^2+}\]
