which one of the following substances will have both dispersion forces and dipole - dipole forces?
a) bf₃
b) co₂
c) br₂
d) hcl

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# Brief Explanations:
- **Dispersion forces**: These are present in all molecules as they result from temporary fluctuations in electron distribution. So, all the given substances ($BF_3$, $CO_2$, $Br_2$, $HCl$) have dispersion forces.
- **Dipole - dipole forces**: These occur in polar molecules. A polar molecule has a permanent dipole moment.
    - For $BF_3$: The central $B$ atom has $sp^2$ hybridization and a trigonal planar geometry. The bond dipoles cancel out ($\mu = 0$), so it is non - polar.
    - For $CO_2$: The central $C$ atom has $sp$ hybridization and a linear geometry. The bond dipoles ($C = O$ bonds are polar) cancel out ($\mu=0$), so it is non - polar.
    - For $Br_2$: It is a non - polar molecule as it consists of two identical $Br$ atoms ($\mu = 0$).
    - For $HCl$: The $H - Cl$ bond is polar ($Cl$ is more electronegative than $H$). The molecule has a permanent dipole moment ($\mu
eq0$), so it is polar and has dipole - dipole forces in addition to dispersion forces.

# Answer:
d) $HCl$

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