Transition elements exhibit higher enthalpies of atomization due to

large number of unpaired electrons

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having stronger interatomic interaction

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strong bonding between atoms

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All of the above.

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Solution

The correct option is D
All of the above.

Property of d block metals

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Similar questions

Q. Assertion :The transition metals exhibit higher enthalpies of atomization Reason: Due to strong metallic bond strength

Q. Why do the transition elements have higher enthalpies of atomization? In

3 d

series (

S c

Z n

), which element has the lowest enthalpy of atomization and why?

Choose incorrect option:-
1. Transition elements exhibit higher enthalpies of atomization.
2. Zinc is a transition element
3. Melting and boiling points increases steadily from Sc to Cu.

Q. Statement I : Hydrogen bonding is stronger between noble gases than small electronegative atoms such as fluorine.
Statement II : Noble gases having large dipole moment.

Q. Assertion :Catenation is the ability of an atom to form bonds with other atoms of the same element. It is exhibited by both carbon and silicon. Reason: Carbon exhibits catenation much more than silicon or any other element due to its smaller size which makes the

C - C

bonds strong while the

S i - S i

bonds are comparatively weaker due to its large size and therefore,

S i

does not have enough bond strength to hold together large molecules.

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Transition elements exhibit higher enthalpies of atomization due to

The correct option is D All of the above. Property of d block metals

The correct option is D
All of the above.

Property of d block metals