To evaluate the intermolecular forces of diatomic chlorine ([tex]\(Cl_2\)[/tex]) and diatomic bromine ([tex]\(Br_2\)[/tex]), you can compare their boiling points. Intermolecular forces are related to the boiling point; the higher the boiling point, the stronger the intermolecular forces.
Given the boiling points from the table:
[tex]\[
\begin{aligned}
&\text{Boiling Point of } F_2 = -188^{\circ}C \\
&\text{Boiling Point of } Cl_2 = -34^{\circ}C \\
&\text{Boiling Point of } Br_2 = 59^{\circ}C \\
&\text{Boiling Point of } I_2 = 184^{\circ}C \\
\end{aligned}
\][/tex]
To determine if diatomic chlorine ([tex]\(Cl_2\)[/tex]) has weaker intermolecular forces than diatomic bromine ([tex]\(Br_2\)[/tex]), compare their boiling points directly:
- The boiling point of [tex]\(Cl_2\)[/tex] is [tex]\(-34^{\circ}C\)[/tex].
- The boiling point of [tex]\(Br_2\)[/tex] is [tex]\(59^{\circ}C\)[/tex].
Since [tex]\(-34^{\circ}C\)[/tex] (the boiling point of [tex]\(Cl_2\)[/tex]) is less than [tex]\(59^{\circ}C\)[/tex] (the boiling point of [tex]\(Br_2\)[/tex]), it indicates that diatomic chlorine ([tex]\(Cl_2\)[/tex]) has weaker intermolecular forces compared to diatomic bromine ([tex]\(Br_2\)[/tex]).
Based on this comparison:
- [tex]\(Cl_2\)[/tex] has weaker intermolecular forces than [tex]\(Br_2\)[/tex].
Thus, the statement "Diatomic chlorine has weaker intermolecular forces than diatomic bromine" is True.
