The ionization energy of an element is:
Correct answer: D. The energy required when electron is removed from outermost shell.
- A. The energy released when an electron is added to an atom of the element
- B. The same as the electron affinity of the element
- C. Equal in magnitude but of opposite sign to the electron affinity of the element
- D. The energy required when electron is removed from outermost shell.
Explanation
The ionization energy of an element is the energy needed to remove an electron from an atom's outermost shell. This is absorbed energy as opposed to being released. The other options are incorrect because they either involve adding electrons (not removing) or incorrectly relate ionization energy to electron affinity.
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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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