Why do the transition elements exhibit higher enthalpies of atomisation?
(N/A) Transition elements have a large number of unpaired electrons in their $(n-1)d$ orbitals.
These unpaired electrons lead to stronger interatomic interactions and metallic bonding between the atoms.
Due to this strong metallic bonding,a large amount of energy is required to break these bonds,resulting in higher enthalpies of atomisation.
These unpaired electrons lead to stronger interatomic interactions and metallic bonding between the atoms.
Due to this strong metallic bonding,a large amount of energy is required to break these bonds,resulting in higher enthalpies of atomisation.
Explore More
Similar Questions
Which among the following is colored?
The set of elements which obey the general electronic configuration $(n-1)d^{1-10}ns^2$ is
The number of electrons in the outermost shell of the $3d-$ transition elements generally remains:
Easy
View SolutionWhich of the following represents the correct order of the given properties?
Medium
View SolutionIn which of the following pairs,the outermost electronic configuration will be the same?
Vedclass Products
For Students
Vedclass Test Series
Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.
Start Free TrialFor Teachers
Exam Paper Generator
Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.
Try FreeFor Institutes
Online Exam Module
Live online exams with unlimited students, 360° analytics & white-label branding.
See Demo