The element with highest first ionization energy is:
Correct answer: D. N
- A. B
- B. C
- C. O
- D. N
Explanation
Generally, smaller the atom, with greater nuclear charge, more strongly the electrons are bound to the nucleus, and hence higher the ionization energy of the atom. By moving from left to right in a period, the outer shell remains the same, while the nuclear charge increases effectively, making the removal of an electron difficult, and hence the value of ionization energy increases. Although the number of electrons also increases in this case, the shielding is not very effective within the same shell. The trend of ionization energies of short periods is shown in Fig. 1.4. The figure also reveals that inert gases have the highest values of ionization energy because, due to complete outermost shell in them, the removal of an electron is extreme.
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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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