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प्रश्न
Account for the following:
Mn shows the highest oxidation state of +7 with oxygen but with fluorine, it shows oxidation state of +4.
Give reasons:
Mn shows the highest oxidation state of +7 with oxygen but with fluorine, it shows the highest oxidation state of +4.
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उत्तर १
In case of oxygen, Mn shows the highest oxidation state of +7. This is because Mn forms pπ–dπ multiple bonds using 2p orbitals of oxygen and 3d orbitals of Mn. With F, Mn displays an oxidation state of +4 because of the single bond formation caused by the unavailability of 2p orbitals in F for multiple bonding.
उत्तर २
Mn shows the highest oxidation state of +7 with oxygen because it can form ppi−dpi multiple bonds using 2p orbital of oxygen and 3d orbital of Mn. On the other hand, Mn shows the highest oxidation state of +4 with flourine because it can form single bond only.
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संबंधित प्रश्न
What are the transition elements? Write two characteristics of the transition elements.
Out of Mn3+ and Cr3+, which is more paramagnetic and why ?
(Atomic nos. : Mn = 25, Cr = 24)
Which of the 3d series of the transition metals exhibits the largest number of oxidation states and why?
What may be the stable oxidation state of the transition element with the following d electron configurations in the ground state of its atom?
3d3
How is the variability in oxidation states of transition metals different from that of the non-transition metals? Illustrate with examples.
Comment on the statement that elements of the first transition series possess many properties different from those of heavier transition elements.
Complete and balance the following chemical equations
`MnO_4^(-) + H_2O + I^(-) ->`
Which of the following ions show higher spin only magnetic moment value?
(i) \[\ce{Ti^3+}\]
(ii) \[\ce{Mn2+}\]
(iii) \[\ce{Fe2+}\]
(iv) \[\ce{Co3+}\]
Transition elements form binary compounds with halogens. Which of the following elements will form \[\ce{MF3}\] type compounds?
(i) \[\ce{Cr}\]
(ii) \[\ce{Co}\]
(iii) \[\ce{Cu}\]
(iv) \[\ce{Ni}\]
Although \[\ce{Cr^3+}\] and \[\ce{Co^2+}\] ions have same number of unpaired electrons but the magnetic moment of \[\ce{Cr^3+}\] is 3.87 B.M. and that of \[\ce{Co^2+}\] is 4.87 B.M. Why?
