Question

which imfs are present in the following molecules?br₂cl₂london dispersionlondon dispersiondipole - dipoledipole - dipole

Explanation:

• For \(Br_2\):
• \(Br_2\) is a non - polar molecule. Non - polar molecules only have London dispersion forces. London dispersion forces are the weakest intermolecular forces and are present in all molecules (but are the only forces in non - polar molecules). Since \(Br_2\) has a symmetrical structure (two identical \(Br\) atoms), there is no permanent dipole moment, so dipole - dipole forces are absent.
• For \(Cl_2\):
• \(Cl_2\) is also a non - polar molecule. Similar to \(Br_2\), it consists of two identical \(Cl\) atoms. The electron distribution is symmetrical around the bond axis. So, it lacks a permanent dipole moment. London dispersion forces arise from temporary fluctuations in electron density, and since there is no polarity (no separation of positive and negative charges within the molecule), dipole - dipole forces do not exist in \(Cl_2\).

Answer:

• For \(Br_2\): London dispersion.
• For \(Cl_2\): London dispersion.