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.
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The atomic number of an element is $22$. The highest oxidation state exhibited by it in its compounds is
Medium
View SolutionName the periodic element,which does not show variable oxidation states.
Match the elements in List-$I$ with their electronic configurations in List-$II$.
List-$I$ List-$II$ $(1)$ $Ti^+$ $(A)$ $(n-1)d^4ns^2$ $(2)$ $_{30}Zn$ $(B)$ $(n-1)d^{10}ns^1$ $(3)$ $_{24}Cr$ $(C)$ $(n-1)d^2ns^0$ $(4)$ $_{29}Cu$ $(D)$ $(n-1)d^5ns^1$ $(E)$ $(n-1)d^0ns^2$ $(F)$ $(n-1)d^{10}ns^2$
| List-$I$ | List-$II$ |
| $(1)$ $Ti^+$ | $(A)$ $(n-1)d^4ns^2$ |
| $(2)$ $_{30}Zn$ | $(B)$ $(n-1)d^{10}ns^1$ |
| $(3)$ $_{24}Cr$ | $(C)$ $(n-1)d^2ns^0$ |
| $(4)$ $_{29}Cu$ | $(D)$ $(n-1)d^5ns^1$ |
| $(E)$ $(n-1)d^0ns^2$ | |
| $(F)$ $(n-1)d^{10}ns^2$ |
Easy
View SolutionExplain on what factors the ionization enthalpies of elements having $d^{n}$ configuration depend upon? Explain the variation in ionization enthalpies of transition elements in the $3d$ series.
The highest magnetic moment is shown by the transition metal ion with the outer electronic configuration
Easy
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