In the following, the element with the highest ionization energy is:
Correct answer: C. [Ne] 3s2 3p3
- A. [Ne] 3s2 3p1
- B. [Ne] 3s2 3p2
- C. [Ne] 3s2 3p3
- D. [Ne] 3s2 3p4
Explanation
The element with the highest ionization energy is fluorine (F) with the electron configuration [Ne] 3s2 3p3. Fluorine has the highest ionization energy due to its small atomic size and high effective nuclear charge, making it more difficult to remove an electron. This extra stability is attributed to the half-filled p-subshell in group V elements. Therefore, option C is correct. Options A, B, and D correspond to nitrogen, oxygen, and neon, respectively, and do not exhibit the highest ionization energy in this context.
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About s-Block and p-Block Elements
The s and p blocks are studied through their valence-shell configurations, periodic trends and characteristic chemical properties. Work covers the reactions of Group I and Group II elements, the behaviour of Group IV elements, and how atomic size, ionization energy, electronegativity and metallic character change across periods and down groups.
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