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The D-And-f-Block Elements
Question
In the series Sc (Z = 21) to Zn(Z = 30), the enthalpy of atomisation of zinc is the lowest i.e., 26, kJ mol. Why?
Solution
The extent of metallic bonding an element undergoes deideds the enthalpy of atomization the more extensive the metallic bonding of an element the more will be its enthalpy of atomization.
Sc & Zn belongs to 3rd group of periodic table. In all transition metals (except Zn, electronic configuration: 3d10 4s2), there are some unpaired electrons that account for their stronger metallic bonding. Due to the absence of these unpaired electrons, the inter-atomic electronic bonding is the weakest in Zn and as a result, it has the least enthalpy of atomization.
Sc & Zn belongs to 3rd group of periodic table. In all transition metals (except Zn, electronic configuration: 3d10 4s2), there are some unpaired electrons that account for their stronger metallic bonding. Due to the absence of these unpaired electrons, the inter-atomic electronic bonding is the weakest in Zn and as a result, it has the least enthalpy of atomization.
Some More Questions From The d-And-f-Block Elements Chapter
Why is the highest oxidation state of a metal exhibited in its oxide or fluoride only?
Which is a stronger reducing agent Cr2+ or Fe2+ and why?
Explain why Cu+ ion is not stable in aqueous solutions?
Actinoid contraction is greater from element to element than lanthanoid contraction. Why?
On what ground can you say that scandium (Z = 21) is a transition element but zinc (Z = 30) is not?
The outer electronic configuration of copper is 3d10 4s1, yet it is considered transition element. Why?
Why the melting points of transition elements are high?
Why Zn, Cd and Hg are not regarded as transition elements?
Name the first element of 3rd transition series.
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Mock Test Series
Mock Test Series