Ionization energy depends upon:
Correct answer: D. All of the above and nature of orbital
- A. Nuclear charge only
- B. Atomic size only
- C. Shielding effect only
- D. All of the above and nature of orbital
Explanation
Correct: Ionization energy, the energy required to remove an electron from an atom, is influenced by multiple factors:Nuclear charge: Higher nuclear charge exerts a stronger pull on electrons, making them harder to remove,thus increasing ionization energy.Atomic size: Larger atoms have greater electron-nucleus distance, resulting in weaker attraction and lower ionization energy.Shielding effect: Inner electrons shield outer electrons from the full brunt of the nuclear charge, making them easier to remove, hence lowering ionization energy.Nature of orbital: Electrons in higher energy orbitals are further away from the nucleus and experience less attraction, leading to lower ionization energy compared to electrons in lower energy orbitals.Therefore, all these factors, along with the specific orbital involved, contribute to determining the ionization energy of an element.
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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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