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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.

Sagot :

GinnyAnsweridn
To determine the correct prediction about the properties of antimony (Sb) and iodine (I), let's analyze the given information step-by-step.

1. Ionization Energy: Ionization energy is the energy required to remove an electron from an atom in the gaseous phase.
- For iodine (I), the first ionization energy is provided as 1008 kJ/mol.
- For antimony (Sb), the ionization energy is not directly given.

2. Electron Affinity: Electron affinity is the energy change when an electron is added to an atom in the gaseous phase.
- The electron affinity of iodine (I) is -295 kJ/mol.
- The electron affinity of antimony (Sb) is -103 kJ/mol.

3. Electronegativity: Electronegativity is a measure of the tendency of an atom to attract a bonding pair of electrons.
- The electronegativity of antimony (Sb) is 2.05.
- The electronegativity of iodine (I) is not given.

Comparing Trends:

- Typically, ionization energy and electronegativity increase across a period and decrease down a group in the periodic table.
- Iodine (I) is in Group 17 (Halogens) and Period 5.
- Antimony (Sb) is in Group 15 and Period 5, indicating that Sb is to the left of I in the same period.

Given these general trends, we can infer:

- Ionization Energy: Iodine (I) is expected to have a higher ionization energy than antimony (Sb) because ionization energy typically increases across a period. This means Sb has a lower ionization energy compared to I.

- Electronegativity: Iodine (I) is expected to have a higher electronegativity than antimony (Sb) as electronegativity also increases across a period. Therefore, Sb has a lower electronegativity compared to I.

Based on these interpretations:
- Sb has a lower ionization energy than I.
- Sb has a lower electronegativity than I.

These observations align with the following prediction:
"Sb has a lower ionization energy and a lower electronegativity than I."

Therefore, the correct answer is:
Sb has a lower ionization energy and a lower electronegativity than I.

This corresponds to:
Sb has a lower ionization energy and a lower electronegativity than I.