Question:
Four successive members of the first row transition elements are listed below with their atomic numbers. Which one of them is expected to have the highest third ionization enthalpy?
Four successive members of the first row transition elements are listed below with their atomic numbers. Which one of them is expected to have the highest third ionization enthalpy?
Updated On: Jul 27, 2022
- Vanadium (Z = 23)
- Chromium (Z = 24)
- Iron (Z = 26)
- Manganese (Z = 25)
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The Correct Option is D
Solution and Explanation
${ }_{23} V =1 s^{2}\, 2 s^{2}\, 2 p^{6},\, 3 s^{2} \,3 p^{6}\, 3 d^{3}, \,4 s^{2}$
${ }_{24} Cr =1 s^{2}\, 2 s^{2}\, 2 p^{6},\, 3 s^{2}\, 3 p^{6} \,3 d^{5},\, 4 s^{1}$
${ }_{26} Fe =1 s^{2}\, 2 s^{2}\, 2 p^{6},\, 3 s^{2}\, 3 p^{6}\, 3 d^{6},\, 4 s^{2}$
${ }_{25} Mn =1 s^{2}\, 2 s^{2} \,2 p^{6}, \,3 s^{2}\, 3 p^{6}\, 3 d^{5},\, 4 s^{2}$
Third electron which is removed in third ionisation enthalpy belongs to $3 d$ -subshells. It means in all elements, shell and subshells are same therefore, required amount of energy is pased upon stability of $d$-subshell. Hence, $Mn$ hows highest third ionisation energy.
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Concepts Used:
Properties of D Block Elements
- Multiple oxidation states- The oxidation states of d block elements show very few energy gaps; therefore, they exhibit many oxidation states. Also, the energy difference between s and d orbital is very less. Therefore both the electrons are involved in ionic and covalent bond formation, which ultimately leads to multiple oxidation states.
- Formation of complex compounds- Ligands show a binding behavior and can form so many stable complexes with the help of transition metals. This property is mainly due to:
- Availability of vacant d orbitals.
- Comparatively small sizes of metals.
- Hardness- Transition elements are tough and have high densities because of the presence of unpaired electrons.
- Melting and boiling points- Melting and boiling points of transition are very high because of the presence of unpaired electrons and partially filled d orbitals. They form strong bonds and have high melting and boiling points.
- Atomic radii- The atomic and ionic radius of the transition elements decreases as we move from Group 3 to group 6. However, it remains the same between group 7 and group 10, and from group 11 to group 12 increases.
- Ionization enthalpy- The ionization enthalpies of the transition elements are generally on the greater side as compared to the S block elements