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प्रश्न
Why +2 oxidation state of manganese is more stable?
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उत्तर
- Manganese, having five unpaired electrons, exhibits six different oxidation states. The small energy difference between the 3d and 4s orbitals allows manganese to lose electrons from both, resulting in oxidation states ranging from +2 to +7.
- Electronic configuration of Mn2+ = [Ar]3d54s0
- Half-filled (d5) d-orbitals provide the Mn2+ ion additional stability, making Mn in the +2 oxidation state more stable.
संबंधित प्रश्न
Why do interstitial compounds have higher melting points than corresponding pure metals?
Account for the following:
Cr2+ is a strong reducing agent.
Account for the following:
Cu+ ion is unstable in aqueous solution.
Explain briefly how +2 state becomes more and more stable in the first half of the first row transition elements with increasing atomic number?
To what extent do the electronic configurations decide the stability of oxidation states in the first series of the transition elements? Illustrate your answer with examples.
What are the characteristics of the transition elements and why are they called transition elements?
How would you account for the following:
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Which among the following transition metal has the lowest melting point?
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The magnetic nature of elements depends on the presence of unpaired electrons. Identify the configuration of transition element, which shows highest magnetic moment.
Which of the following ions show higher spin only magnetic moment value?
(i) \[\ce{Ti^3+}\]
(ii) \[\ce{Mn2+}\]
(iii) \[\ce{Fe2+}\]
(iv) \[\ce{Co3+}\]
Why EΘ values for Mn, Ni and Zn are more negative than expected?
A solution of \[\ce{KMnO4}\] on reduction yields either a colourless solution or a brown precipitate or a green solution depending on pH of the solution. What different stages of the reduction do these represent and how are they carried out?
EΘ of Cu is + 0.34V while that of Zn is – 0.76V. Explain.
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Which of the following ions has the maximum magnetic moment?
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\[\ce{MnO^{-4}_{ (aq)} + 8H^+ + 5e^- -> Mn^{2+}_{ (aq)} + 4H2O_{(l)}}\], E0 = +1.51 V
What is the cell potential for the redox reaction?
What is the oxidation state of chromium in chromate ion and dichromate ion?
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Describe the oxidising action of potassium dichromate and write the ionic equation for its reaction with H2S.
Compare the general characteristics of the first series of the transition metals with those of the second and third series metals in the respective vertical columns. Give special emphasis on the following point:
Oxidation states
