Question

decide which intermolecular forces act between the molecules of each compound in the table below.

compound	intermolecular forces (check all that apply)
$cl_2$<br>chlorine	√
carbon tetrabromide	√	√
$ch_2cl_2$<br>dichloromethane	√	√
ammonia	√	√	√

Explanation:

Step1: Analyze $Cl_2$

$Cl_2$ is a non - polar molecule. Non - polar molecules only have dispersion forces between them.

Step2: Analyze carbon tetrabromide ($CBr_4$)

$CBr_4$ is non - polar. It has dispersion forces. Also, due to its symmetrical structure being broken by the large bromine atoms to some extent, it has weak dipole - induced dipole forces (but mainly dispersion).

Step3: Analyze $CH_2Cl_2$

$CH_2Cl_2$ is a polar molecule. Polar molecules have dispersion forces due to electron cloud fluctuations and dipole - dipole forces due to the presence of a permanent dipole.

Step4: Analyze ammonia ($NH_3$)

$NH_3$ has N - H bonds. Nitrogen is highly electronegative. So, it has dispersion forces, dipole - dipole forces and hydrogen - bonding (since H is bonded to N).

Answer:

compound	dispersion	dipole	hydrogen - bonding
carbon tetrabromide	Yes	No	No
$CH_2Cl_2$	Yes	Yes	No
ammonia	Yes	Yes	Yes