Answered

Selected properties of antimony (Sb) and iodine (I) are listed in the table below.

\begin{tabular}{|c|c|c|c|c|}
\hline Element & \begin{tabular}{c}
Atomic radius \\
[tex]$( pm )$[/tex]
\end{tabular} & \begin{tabular}{c}
First ionization \\
energy \\
[tex]$( kJ / mol )$[/tex]
\end{tabular} & \begin{tabular}{c}
Electron affinity \\
[tex]$( kJ / mol )$[/tex]
\end{tabular} & Electronegativity \\
\hline Sb & 145 & [tex]$?$[/tex] & -103 & 2.05 \\
\hline I & 140 & 1008 & -295 & [tex]$?$[/tex] \\
\hline \hline
\end{tabular}

Which predictions can most likely be made?

A. Sb has a lower ionization energy but a higher electronegativity than I.
B. Sb has a higher ionization energy but a lower electronegativity than I.
C. Sb has a lower ionization energy and a lower electronegativity than I.
D. Sb has a higher ionization energy and a higher electronegativity than I.



Answer :

GinnyAnswer
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.