is dispersion force the strongest IM for Cl2

Yes, I think so.

Yes, no hydrogen bonding because there aren't any hydrogens. No dipole-dipole because it is nonpolar.

Pure acetic acid (HC2H3O2) is a liquid and is known as glacial acetic acid. Calculate the

ient
M
1) Explain why the lattice energy of MgS is approximately 4 times as large as that of NaCl.
2) Draw the Lewis structure for the acetate ion, CH3CO2—, including any important resonance
3) Why do successive ionization energies increase? (Use only the space below)
4) Why is the first ionization energy of sulfur smaller than the first ionization energy of
molarity of a solution prepared by dissolving 10.00 mL of glacial acetic acid at 25°C in suffic
water to give 500.0 mL of solution. The density of glacial acetic acid at 25°C is 1.05 g/mL

To determine if dispersion forces are the strongest intermolecular force (IMF) for chlorine gas (Cl2), we need to compare it to other potential IMF options.

Dispersion forces, also known as London forces, are temporary attractive forces between molecules that arise due to the temporary fluctuations in electron distribution. These forces exist in all molecules, regardless of their polarity. While dispersion forces can be significant in larger molecules, they are generally the weakest intermolecular force.

In the case of chlorine gas (Cl2), we have two identical chlorine molecules bonded together. The dominant IMF for Cl2 molecules is not dispersion forces, but rather dipole-dipole forces. Each chlorine molecule has a non-zero dipole moment, as the chlorine atom has a higher electronegativity compared to hydrogen or other elements. The dipole-dipole forces between the chlorine molecules result from the attraction between the partial positive charge on one chlorine atom and the partial negative charge on the other chlorine atom.

Dipole-dipole forces are generally stronger than dispersion forces, especially in polar molecules like Cl2 where the dipole moments do not cancel each other out.

In summary, while dispersion forces exist in chlorine gas, the dominant intermolecular force is dipole-dipole forces, making them stronger than dispersion forces.