Why manganese (Mn) has lower melting point than that of its neighborhood elements? Manganese has 5 free electrons in its d orbital so it take place more in metallic bonding as compared to other elements in its neighborhood (left and right in periodic table) who have 4 free electrons in their d orbital. More metallic bonding means more energy requires in breaking bond and more melting point but it is not so can you please tell me why?

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SAGAR SINGH - IIT DELHI · Answer

Dear student,
Manganese has 5 free electrons in its d orbital so it take place more in metallic bonding as compared to other elements in its neighborhood (left and right in periodic table) who have 4 free electrons in their d orbital. More metallic bonding means more energy requires in breaking bond and more melting point.
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Sumanth · Answer

Manganese has 5 electrons in its d-orbital . This is a half filled stable configuration. Hence these electrons are not free to participate in metallic bonding. That is why Mn has unusually low M.P. Was this answer helpful??

rajesh kumar sahu · Answer

if the configuration is half filled, the it should pair up with another half filled orbital to give very strong metallic bonding and thus provide high melting point. i think the reason is something else.

shreya · Answer

Actually the reason is that there is however more gap btwn mn atoms than other elements of 3d series thus there is already gap n it needs less energy..Helpful??

abirami menath · Answer

Mn has 3d 5 which make it extra stable due to its half filled configeration. so it doesn’t require to take part in metallic bonding further. hence Mn has low melting point

Yadu krishnan · Answer

Actually,melting point depends not only on number of unpaired electrons but also on the heat of atomization.,that is .enthalpy change when it breaks into its constituent atoms.Manganese has less heat of atomization and hence its melting point is also low.

Taha Umrethwala · Answer

Fe, Ni and Co exhibit ferromagnetism which results in a very high net magnetic moment, thus even though no of unpaired electrons decrease the effect is very well made up due to its magnetism. All in all, metallic bonding is much stronger. the metals that follow techtenium however don't exhibit ferromagnetism, thus the regular trend of lowered melting point is observed Oh, and incase u were wondering, Fe,Ni,Co exhibit ferromagnetism due to their specific domain structure.

Rishi Sharma · Answer

Dear Student,
Please find below the solution to your problem.

Manganese has 5 free electrons in its d orbital so it take place more in metallic bonding as compared to other elements in its neighborhood (left and right in periodic table) who have 4 free electrons in their d orbital.
More metallic bonding means more energy requires in breaking bond and more melting point.

Thanks and Regards

John Paul Hilson · Answer

Generally, transition elements have high melting and boiling point due to high enthalpy of atomization but for Manganese the melting point is low because it has low enthalpy of atomization. Low enthalpy of atomization is due to 3d 5 electrons which is held tight by the nucleus and hence weakening metallic bond, since the bond is weak the energy needed to became individual atom(low enthalpy of atomization) is less and hence the melting and also the boiling bond is less.

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