With this molecule, CH2CCl2, if it came across another CH2CCl2, there would be a dipole-dipole attraction and london dispersion forces.
Dipole-Dipole- An electrostatic attraction between the poitive end of a dipole and the negative end of another dipole. This could occur with the Cl (negative) of one molecule and the H (positive) of the other molecule.
London Dispersion Forces- A weak force of attraction between two molecules created by temporary dipoles caused by elections moving around two atoms. This happens among all molecules that come across each other because the electrons are constantly moving.
If CH2CCl2 were to come across another molecule such as HF, there would be hydrogen bonding.
Hydrogen Bonding- A special case of dipole-dipole where a temporary covalent bond occurs between a hydrogen of one molecule and a Oxygen, Nitrogen or Fluorine of another molecule. One Hydrogen from CH2CCl2 would be attracted to the Fluorine of the HF. The F would switch constantly between the H of CH2CCl2 and the H of HF.
You correctly identified the forces of attraction. Dispersion is in the bonding of this molecule as it is in any bonding of molecules and since the molecule is polar you are correct to say that dipole-dipole is present in the bonding. It is also correct that not in this molecule but when bonding with another molecule such as HF or H20 that in that circumstance hydrogen bonding would be included as well.
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The forces of attraction are correct here. There is Dipole and London Dispersion Forces. I also like how you put how your atom can have Hydrogen Bonding just not with another atoms of itself. I also like how oyu defined them.
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