Ionization energy decreases down the group because:
Correct answer: D. Atomic radius increase
- A. Shielding remains constant
- B. Atomic radius remains constant
- C. Proton number increases
- D. Atomic radius increase
Explanation
Ionization energy is the energy needed to remove an electron from its atom. Down the group, Atomic radius as well as shielding increases, as a result, the attraction forces between electrons and nucleus reduces. Hence, less energy is required for electrons surrounding the nucleus to be removed from the atom i.e. 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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