All of the following statements about lst ionization energy of elements are correct EXCEPT:
Correct answer: D. Ne > He
- A. O > N
- B. Be > B
- C. Al > Mg
- D. Ne > He
Explanation
The correct answer is Option D: Ne > He. This statement is incorrect because helium has a higher first ionization energy than neon. The ionization energy generally increases across a period, but helium, being a noble gas with a smaller atomic radius, holds its electrons more tightly than neon. The other options describe correct trends: Option A is incorrect because nitrogen has a higher ionization energy than oxygen due to half-filled p orbital stability, Option B is correct because beryllium's filled 2s orbital gives it higher ionization energy than boron, and Option C is incorrect because magnesium has a higher ionization energy than aluminum due to its filled 3s orbital.
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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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