To determine which predictions can most likely be made about the ionization energy and electronegativity of antimony (Sb) and iodine (I), we will reason through some periodic trends.
Given Data:
- Atomic Radius: Iodine (I) = 140 pm, Antimony (Sb) = 145 pm
- First Ionization Energy: Iodine (I) = 1008 kJ/mol, Antimony (Sb) = not provided
- Electron Affinity: Iodine (I) = -295 kJ/mol, Antimony (Sb) = -103 kJ/mol
- Electronegativity: Iodine (I) = not provided, Antimony (Sb) = 2.05
Periodic Trends:
1. Ionization Energy:
- Trend: Ionization energy increases across a period and decreases down a group.
- Reasoning for I and Sb:
- Iodine is in Group 17 and Period 5.
- Antimony is in Group 15 and Period 5.
- Since both elements are in the same period but different groups, iodine should have a higher ionization energy compared to antimony because it is further to the right in the periodic table.
2. Electronegativity:
- Trend: Electronegativity increases across a period and decreases down a group.
- Reasoning for I and Sb:
- For elements in the same period, those further to the right generally have higher electronegativity.
- Thus, iodine is expected to have a higher electronegativity compared to antimony.
Reasoning Based on Data and Trends:
- Iodine, being in Group 17 and thus to the right of antimony in Group 15, should have a higher ionization energy.
- Iodine should also be more electronegative because it is further to the right in its period compared to antimony.
Given the observations:
- Iodine (I) should have a higher ionization energy than antimony (Sb).
- Iodine (I) should have a higher electronegativity than antimony (Sb).
Correct Prediction:
The correct prediction gathered from the periodic trends and given data is:
- Sb has a lower ionization energy and a lower electronegativity than I.
Thus, among the provided options:
- "Sb has a lower ionization energy and a lower electronegativity than I." is the most accurate prediction based on the given properties and periodic trends.
So, the answer is:
Sb has a lower ionization energy and a lower electronegativity than I.
