5. (03.06 MC) The boiling points of diatomic halogens are compared in the table.
Boiling Points of Diatomic
Halogens
Molecule
Boiling Point
F2
-188 °C
Cl
-34 °C
Br
59 °C
12
184 °C
Which of
e following statements best explains the trends in boiling points? (4 points)
A) the atomic size increases down the group, and this decreases the strength of the intermolecular forces. B)the total number of electrons decreases down the group, and this decreases the strength of the intermolecular forces. C)the total number of electrons increases down the group, and this increases the strength of intermolecular forces d)the chances of forming a permanent dipole increases down the group, and this increases the strength of the intermolecular forces koi

Where's the pictures ?

The correct answer would be b) volume versus temperature, because they are also directly proportional.

Answerthis solution will not form a precipitateexplanationsolubility equilbrium:         pbf₂(s)  ⇄ pb²⁺(aq) + 2 f⁻(aq)the solubility product expression is    (we exclude solids from the equilibrium expression).now suppose we have the trial ion product q, which we can define as    then, we can interpret  q as the product of the concentration of the ions that we have and ksp as the product of the ion concentrations that are needed to form a saturated solution.if q > ksp, then that implies that there will be a surplus of ions that exceed the amount that is required to form a saturated solution. a precipitate will then form (the precipitate continually  forms until the surplus ions are removed and q is decreased to ksp's value).if q = ksp, the saturated solution that forms is barely saturated and the precipitate will be minimal.if q < ksp, then the ion concentration will not be enough to form a saturated solution (so no precipitate).using our information, we calculate the trial ion product:     since q = 2.7  × 10⁻⁸ < ksp =  4  ×  10⁻⁸, a precipitate will not form.