The first ionization energy of an atom depends on:
Correct answer: D. All of the above
- A. Charge on nucleus
- B. Screening effect
- C. Electronic configuration
- D. All of the above
Explanation
Ionization energy, also called ionization potential is the amount of energy required to remove an electron from an isolated atom or molecule. This energy is usually expressed in kJ/mol. It depends on the charge of the nucleus, shielding effect, and electronic configuration.The greater the charge on the nucleus, the more tightly the outer electrons are held, thus more heat energy is required to remove an electron from the atom.The greater the shielding/screening effect on the outer electrons, the less tightly they are held by the nucleus, thus less energy is required to remove an electron.The greater the distance from the nucleus (the electronic configuration), the lesser the force of nuclear attraction and the higher the 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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