Question

question 15 (1 point)
which of the following diatomic molecules has the highest boiling point?
h₂
n₂
o₂
br₂
cl₂
you can use this periodic table during the quiz.
however, as stated in the course outline, and in the orientation session, this quiz is not open book.
you cannot access course material while you write the quiz. nor can you google your answers, work as a group, use a cheat sheet, etc.

Explanation:

Boiling point of diatomic molecules depends on the strength of London dispersion forces. London dispersion forces increase with the increase in molar mass. Calculate the molar mass of each molecule:

• \(M(H_2)=2\times1 = 2\space g/mol\)
• \(M(N_2)=2\times14 = 28\space g/mol\)
• \(M(O_2)=2\times16 = 32\space g/mol\)
• \(M(Br_2)=2\times80 = 160\space g/mol\)
• \(M(Cl_2)=2\times35.5 = 71\space g/mol\)

Since \(Br_2\) has the highest molar mass among the given diatomic molecules, it has the strongest London dispersion forces and thus the highest boiling point.

Answer:

\(Br_2\)