The transition metals exhibit higher enthalpies of atomisation due to
- Atheir ability to show variable oxidation states
- Bthe presence of incompletely filled $d-$ subshell
- Ctheir ability to exist in the solid state with unpaired electrons
- Dstrong interatomic interaction arises because of having large number of unpaired electrons in their atoms
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Similar Questions
Explain the exceptions in the general electronic configuration of $3d$-series elements.
Medium
View SolutionWhich of the following does not represent the correct order of the property indicated?
MediumAIPMT 1997
View SolutionIdentify the order in which the spin-only magnetic moment (in $BM$) increases for the following four ions:
$(I) Fe^{2+}$
$(II) Ti^{2+}$
$(III) Cu^{2+}$
$(IV) V^{2+}$
$(I) Fe^{2+}$
$(II) Ti^{2+}$
$(III) Cu^{2+}$
$(IV) V^{2+}$
Why are the $d$-block elements known as "Transition" elements? Why are zinc,cadmium,and mercury not considered transition elements?
Difficult
View SolutionGiven below are two statements :
Statement $I$ : The higher oxidation states are more stable down the group among transition elements unlike $p-$block elements.
Statement $II$ : Copper can not liberate hydrogen from weak acids.
In the light of the above statements,choose the correct answer from the options given below :
Statement $I$ : The higher oxidation states are more stable down the group among transition elements unlike $p-$block elements.
Statement $II$ : Copper can not liberate hydrogen from weak acids.
In the light of the above statements,choose the correct answer from the options given below :
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