Which of the following metalloids exhibits the greatest metallic character?

• A. Silicon (Si)
• B. Boron (B)
• C. Antimony (Sb)
• D. Arsenic (As)

Answer: (C)

Verified step by step guidance

1. Understand that metallic character refers to how readily an element can lose electrons to form positive ions, which is a property more common in metals than nonmetals.
2. Recall that metallic character generally increases as you move down a group (column) in the periodic table because atoms have more electron shells, making it easier to lose electrons.
3. Identify the group and period positions of the given metalloids: Boron (B) and Silicon (Si) are in Period 2 and 3 respectively, while Arsenic (As) and Antimony (Sb) are in Period 4 and 5 respectively, all in Group 13-15 region.
4. Compare their positions: since metallic character increases down a group, Antimony (Sb), being the lowest in the group among the options, will exhibit the greatest metallic character.
5. Conclude that among the given metalloids, Antimony (Sb) has the greatest metallic character due to its position lower in the periodic table, which corresponds to increased metallic properties.