Which of the following statements is incorrect in relation to ionization enthalpy?
Correct answer: D. Removing an electron from an orbital with a lower principal quantum number (n) is easier than from a higher n orbital.
- A. Ionization enthalpy increases for each successive electron removed.
- B. The greatest increase in ionization enthalpy occurs when removing an electron from a noble gas core.
- C. A significant jump in ionization enthalpy occurs after removing the last valence electron.
- D. Removing an electron from an orbital with a lower principal quantum number (n) is easier than from a higher n orbital.
Explanation
Option D is the correct answer because it incorrectly states that removing an electron from a lower n value orbital is easier than from a higher n value orbital. In reality, electrons in orbitals with lower n values are closer to the nucleus and more strongly attracted, making them harder to remove. Options A, B, and C correctly describe trends in ionization enthalpy: successive electron removal increases ionization enthalpy (Option A), removing an electron from a noble gas configuration requires significant energy (Option B), and a jump in ionization enthalpy occurs after the last valence electron is removed (Option C).
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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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