Sure! Let's fill in the missing values for the atomic radii in the table.
According to the information provided:
- Bromine (Group 17 element) has an atomic radius of approximately 1.2 Å.
- Magnesium (Period 3 element) has an atomic radius of approximately 1.60 Å.
- Sodium (Period 3 element) has an atomic radius of approximately 1.80 Å.
So we can substitute these values into the table:
[tex]$A = 1.2$[/tex]
[tex]$B = 1.6$[/tex]
[tex]$C = 1.8$[/tex]
The completed table will look like this:
\begin{tabular}{|l|r|}
\hline Element & \begin{tabular}{r}
Atomic Radius \\
[tex]$(\AA)$[/tex]
\end{tabular} \\
\hline Bromine & 1.2 \\
\hline Chlorine & 0.97 \\
\hline Magnesium & 1.60 \\
\hline Sodium & 1.80 \\
\hline Phosphorus & 1.28 \\
\hline
\end{tabular}
Now, let's compare the values:
- Bromine and Chlorine (Group 17 elements): Bromine has a larger atomic radius (1.2 Å) compared to Chlorine (0.97 Å). This trend is typical in the periodic table, where atomic radius increases as we move down a group.
- Magnesium and Sodium (Period 3 elements): Sodium has a larger atomic radius (1.80 Å) compared to Magnesium (1.60 Å). In Period 3, the atomic radius generally decreases as we move from left to right across the period.
- Phosphorus (Period 3 element): Phosphorus has an atomic radius of 1.28 Å, which follows the trend of decrease in atomic radius across Period 3. From Sodium (1.80 Å), Magnesium (1.60 Å), to Phosphorus (1.28 Å), the atomic radii decrease as we move from left to right.
Thus, the filled-in table allows us to observe the trends in atomic radii within a group and across a period in the periodic table.
