To fill in the missing values for the atomic radii of the elements in the provided table, we use known approximations from atomic radius data:
Given:
- Chlorine (Cl) has an atomic radius of 0.97 Å.
- Phosphorus (P) has an atomic radius of 1.28 Å.
- Bromine (Br) has an atomic radius of 1.14 Å.
- Magnesium (Mg) has an atomic radius of 1.60 Å.
- Sodium (Na) has an atomic radius of 1.86 Å.
Let's fill the missing values into the table accordingly:
Completed Table:
\begin{tabular}{|l|r|}
\hline
Element & \begin{tabular}{r}
Atomic Radius \\
([tex]$\tilde{A}$[/tex])
\end{tabular} \\
\hline
Bromine & 1.14 \\
\hline
Chlorine & 0.97 \\
\hline
Magnesium & 1.60 \\
\hline
Sodium & 1.86 \\
\hline
Phosphorus & 1.28 \\
\hline
\end{tabular}
Now, let’s compare the values in each column:
- Group 17 Elements (Chlorine, Bromine):
- Chlorine: 0.97 Å
- Bromine: 1.14 Å
We observe that the atomic radius of Bromine (Br) is larger than that of Chlorine (Cl).
- Period 3 Elements (Sodium, Magnesium, Phosphorus):
- Sodium: 1.86 Å
- Magnesium: 1.60 Å
- Phosphorus: 1.28 Å
As we move across Period 3 from left to right (from Sodium to Phosphorus), the atomic radius generally decreases. This trend is in line with the periodic trend where the effective nuclear charge increases, pulling the electron cloud closer to the nucleus.
In summary:
- Bromine has a larger atomic radius than Chlorine.
- In Period 3, the atomic radii decreases from Sodium to Phosphorus.
