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Question:
The correct order of the first ionization enthalpies is:
The correct order of the first ionization enthalpies is:
Updated On: Sep 30, 2024
- Mn < Ti < Zn < Ni
- Ti < Mn < Ni < Zn
- Zn < Ni < Mn < Ti
- Ti < Mn < Zn < Ni
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The Correct Option is B
Solution and Explanation
${Ti \to |Ar| \; 3d^2 \; 4s^2}$
${Mn \to |Ar| \; 3d^5 \; 4s^2}$
${Ni \to |Ar \; | 3d^8 \; 4s^2}$
${Zn \to |Ar| \; 3d^{10} \; 4s^2}$
Correct order of I.P. is
[Ti < Mn < Ni < Zn]
${Mn \to |Ar| \; 3d^5 \; 4s^2}$
${Ni \to |Ar \; | 3d^8 \; 4s^2}$
${Zn \to |Ar| \; 3d^{10} \; 4s^2}$
Correct order of I.P. is
[Ti < Mn < Ni < Zn]
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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
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