Which of the following properties best predicts the metallic character of elements in the periodic table?

• A. Small atomic radius
• B. High electronegativity
• C. Low ionization energy
• D. High electron affinity

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 (cations), which is a key property of metals.
2. Recall that ionization energy is the energy required to remove an electron from an atom in its gaseous state; lower ionization energy means it is easier for the atom to lose an electron.
3. Compare the given properties: small atomic radius, high electronegativity, low ionization energy, and high electron affinity, and consider how each relates to the ease of losing electrons.
4. Recognize that low ionization energy directly indicates an element's tendency to lose electrons easily, which is characteristic of metals and thus predicts metallic character best.
5. Conclude that among the options, low ionization energy is the property that best predicts metallic character because it reflects how easily an element can form positive ions.