Which one would you class it as more metallic in character?
Correct answer: B. Bi
- A. As
- B. Bi
- C. C
- D. Sb
Explanation
Metallic character refers to an element's ability to lose electrons. It increases as you move down a group in the periodic table because the atomic radius becomes larger, allowing for easier electron loss due to increased shielding and decreased ionization energy. Conversely, metallic character decreases across a period from left to right as the effective nuclear charge increases, holding electrons more tightly. In this question, bismuth (Bi) is the most metallic because it is further down the group compared to arsenic (As) and antimony (Sb), and it is also more metallic than carbon (C), which is a non-metal. This makes Bi the element with the highest tendency to lose electrons among the given options.
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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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