Question

The correct order of the first ionization enthalpies is:

• A. Mn < Ti < Zn < Ni
• B. Ti < Mn < Ni < Zn
• C. Zn < Ni < Mn < Ti
• D. Ti < Mn < Zn < Ni

Answer 1

The Correct Option is B

The order of the first ionization enthalpies of the elements can be determined by considering the electronic configuration and the stability of the elements. Let's analyze each element:

1. Titanium (Ti): The electronic configuration of Titanium is [Ar] 3d² 4s². It has a relatively low first ionization enthalpy because it can lose an electron from the 4s orbital with relative ease.
2. Manganese (Mn): The electronic configuration is [Ar] 3d⁵ 4s². The half-filled 3d subshell provides a degree of stability, making the first ionization enthalpy of Mn higher than that of Ti.
3. Nickel (Ni): The electronic configuration is [Ar] 3d⁸ 4s². It has a higher ionization enthalpy compared to Mn because removing an electron disrupts a more stable electron configuration.
4. Zinc (Zn): The electronic configuration is [Ar] 3d¹⁰ 4s². Zinc has a completely filled d-subshell, giving it even higher stability and thus the highest first ionization enthalpy in this group.

Based on this analysis, the correct order of first ionization enthalpies is:

Ti < Mn < Ni < Zn

Therefore, the correct answer is Ti < Mn < Ni < Zn.