Which statement is incorrect about ionization energy?
Correct answer: D. Ionization energy does not depend upon the penetration effect of the inner orbital
- A. Ionization energy depends upon the magnitude of nuclear charge
- B. Ionization energy depends upon the atomic radius
- C. Ionization energy depends upon the shielding effect
- D. Ionization energy does not depend upon the penetration effect of the inner orbital
Explanation
Option D is the correct answer because it incorrectly states that ionization energy does not depend on the penetration effect. In reality, the penetration effect allows inner orbital electrons to be closer to the nucleus, increasing the effective nuclear charge experienced by the outer electrons, and thus increasing ionization energy.Options A, B, and C correctly state the factors affecting ionization energy: nuclear charge, atomic radius, and shielding effect, respectively. Increased nuclear charge strengthens the attraction between electrons and the nucleus, raising ionization energy. A larger atomic radius weakens this attraction, lowering ionization energy. The shielding effect decreases the effective nuclear charge felt by outer electrons, also reducing ionization energy.
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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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