Let's determine the missing values in the table for the electronegativities of the elements provided. Based on the given answer, we have the following values for Chlorine, Magnesium, and Sodium:
- Chlorine's electronegativity (A) is 3.16.
- Magnesium's electronegativity (B) is 1.31.
- Sodium's electronegativity (C) is 0.93.
Therefore, the completed table with the electronegativities filled in is:
[tex]\[
\begin{tabular}{|l|r|}
\hline Element & Electronegativity \\
\hline Bromine & 2.96 \\
\hline Chlorine & 3.16 \\
\hline Magnesium & 1.31 \\
\hline Sodium & 0.93 \\
\hline Phosphorus & 2.19 \\
\hline
\end{tabular}
\][/tex]
Let's compare the electronegativity values in each column:
1. Group 17 Elements (Halogens):
- Chlorine: 3.16
- Bromine: 2.96
Chlorine has a higher electronegativity (3.16) compared to Bromine (2.96). This trend is consistent with what we expect in the periodic table – electronegativity decreases as we move down a group.
2. Period 3 Elements:
- Sodium (Na): 0.93
- Magnesium (Mg): 1.31
- Phosphorus (P): 2.19
- Chlorine (Cl): 3.16
As we move across Period 3 from left to right, electronegativity increases. Sodium, being the farthest left, has the lowest electronegativity (0.93). Magnesium has a slightly higher electronegativity (1.31). Phosphorus, being further to the right, shows a significant increase (2.19), and Chlorine, being the farthest right in this group, has the highest electronegativity (3.16).
The completed table with comparisons validates the trends observed within both the period and the group of the periodic table.
