Among the following elements (whose electronic configuration are given below),the one having the highest ionization energy is:
Correct answer: B. [Ne] 3s2 3p3
- A. [Ne] 3s2 3p1
- B. [Ne] 3s2 3p3
- C. [Ne] 3s2 3p2
- D. [Ar] 3d10 4s2 4p³
Explanation
The configuration [Ne] 3s²3p³ represents an element with a half-filled p-subshell. Half-filled and completely filled subshells have extra stability, making it more difficult to remove an electron and thus resulting in a higher ionization energy compared to other configurations in the same period.
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About Periodic Properties and Trends
Periodic properties arise from electron configuration and effective nuclear charge, producing trends in atomic and ionic radius, ionization energy, electron affinity, electronegativity, metallic character and reactivity. Comparisons run across periods and down groups, with attention to common exceptions. The topic also relates these trends to the behavior of s-block and p-block elements.
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