Which of the following statements is incorrect?
Correct answer: A. An element which has high electronegativity always has high electron gain enthalpy.
- A. An element which has high electronegativity always has high electron gain enthalpy.
- B. Electron gain enthalpy is the property of an isolated atom.
- C. Electronegativity is the property of bonded atoms.
- D. Both electronegativity and electron gain enthalpy are usually directly related to nuclear charge and inversely related to atomic size.
Explanation
Option A is the correct answer because it incorrectly states that high electronegativity always corresponds to high electron gain enthalpy. While high electronegativity often indicates a strong attraction for electrons, exceptions exist, such as nitrogen, which has zero electron gain enthalpy despite high electronegativity. Option B is correct because electron gain enthalpy is a property of isolated atoms, though its value can vary due to electron repulsion and stability factors. Option C correctly describes electronegativity as a property of bonded atoms, influencing the nature of chemical bonds. Option D accurately links both electronegativity and electron gain enthalpy to nuclear charge and atomic size, highlighting their general trends across the periodic table.
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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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