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Metallic character of the elements:

Correct answer: B. Increases down the groups

  • A. Decreases down the groups
  • B. Increases down the groups
  • C. Remains the same across the periods
  • D. Increases across the periods

Explanation

The correct answer is that metallic character increases down the groups. This is because as we move down a group in the periodic table, the atomic size increases due to the addition of electron shells. As a result, the valence electrons are further from the nucleus and experience less effective nuclear charge, making them easier to lose and thus increasing metallic character.Option A is incorrect because metallic character increases, not decreases, down a group. Option C is incorrect because metallic character decreases as we move across a period from left to right, due to increased nuclear charge attracting electrons more strongly. Option D is incorrect because metallic character does not increase across a period for the same reason.

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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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