To determine whether diatomic bromine (Br_2) has weaker intermolecular forces than diatomic fluorine (F_2), we need to understand how boiling points are related to intermolecular forces.
Boiling Points and Intermolecular Forces:
- The boiling point of a substance is the temperature at which it changes from a liquid to a gas.
- Higher boiling points indicate stronger intermolecular forces because more energy (in the form of heat) is required to separate the molecules and turn the substance into gas.
- Conversely, lower boiling points indicate weaker intermolecular forces since less energy is needed for the phase change.
Comparison of Boiling Points:
- [tex]\(F_2\)[/tex] (Fluorine): [tex]\(-188^{\circ}C\)[/tex]
- [tex]\(Br_2\)[/tex] (Bromine): [tex]\(59^{\circ}C\)[/tex]
By examining the data:
1. The boiling point of [tex]\(F_2\)[/tex] is [tex]\(-188^{\circ}C\)[/tex], which is much lower than the boiling point of [tex]\(Br_2\)[/tex], which is [tex]\(59^{\circ}C\)[/tex].
2. Since [tex]\(F_2\)[/tex] has a lower boiling point, it implies that it has weaker intermolecular forces compared to [tex]\(Br_2\)[/tex].
Given this reasoning, it is clear that diatomic bromine ([tex]\(Br_2\)[/tex]) does not have weaker intermolecular forces than diatomic fluorine ([tex]\(F_2\)[/tex]). Therefore, the answer is:
False.
