The electronegativity of the [1]A element first decreases and then increases. This behavior is due to poor shielding of:
Correct answer: C. d- electron
- A. S electron
- B. p - electron
- C. d- electron
- D. f - electron
Explanation
Electronegativity is the tendency of an atom to attract electrons. In group 1 elements, as we go down the group, the atomic size increases due to the addition of electron shells, which generally decreases electronegativity. However, the presence of d electrons, which are less effective at shielding the nuclear charge, can cause variations. These d electrons have a higher energy level and are more dispersed, leading to poor shielding and causing a temporary increase in electronegativity. The other options are incorrect because s and p electrons provide more effective shielding, and f electrons typically affect elements outside the context of group 1.
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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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