More the ionization energy of an element:
Correct answer: C. Less the metallic character
- A. More the electropositivity
- B. More the reducing power
- C. Less the metallic character
- D. Bigger the atomic radius
Explanation
Ionization energy is the energy required to remove an electron from a neutral gaseous atom, and it is a measure of the tendency of an element to form a cation. Elements with high ionization energies tend to have low electropositivity and reducing power because they are less likely to give up electrons.On the other hand, metallic character refers to the ability of an element to lose electrons and form positive ions. Elements with low ionization energies tend to have high metallic character, while those with high ionization energies tend to have low metallic character. Therefore, as the ionization energy of an element increases, its metallic character decreases.
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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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