18 Questions
Which transition element has the highest enthalpy of atomization?
W
Which characteristic is responsible for the paramagnetic behavior of transition elements?
Presence of unpaired electrons
Which transition element has the lowest ionization enthalpy?
Sc
In which transition element do we observe a significant increase in metallic/ionic radii going from M to M2+?
Mn
Which transition element exhibits the highest oxidation state?
Ta
Among the transition elements listed, which one shows a positive value for the 3+/2+ redox potential?
Cr
Which property is responsible for the stabilisation of energy states?
Exchange energy
Why does the loss of exchange energy increase stability?
It decreases the number of possible pairs of parallel spins
Which configuration results in no loss of exchange energy?
d6
Why does Mn+ have a lower ionisation enthalpy than Cr+?
Mn+ has a 3d54s1 configuration
Why does Fe2+ have a lower ionisation enthalpy than Mn2+?
Fe2+ has a d6 configuration
Why is the third ionisation enthalpy of Fe lower than that of Mn?
Fe has a more stable electron configuration
Why do transition elements exhibit stronger bonding between atoms compared to non-transition elements?
Transition elements have a higher number of unpaired electrons in their atoms.
In the series Sc (Z = 21) to Zn (Z = 30), why does zinc (Z = 30) have the lowest enthalpy of atomisation?
Zinc has the least number of unpaired electrons.
What accounts for the increase in ionisation enthalpy along each series of transition elements from left to right?
Increase in nuclear charge
How does the variation in ionisation enthalpy along a series of transition elements compare to that along a period of non-transition elements?
It increases at a slower rate
Why does the first ionisation enthalpy of metals in the 3d series show an irregular trend?
Presence of unpaired electrons in 3d orbitals
What effect does the removal of one electron have on the relative energies of 4s and 3d orbitals in transition elements?
It destabilizes the 4s orbital.
Test your knowledge on transition elements enthalpies, including atomisation and ionisation enthalpies. Explore the factors influencing the strength of bonding in transition elements.
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