Dispersion
In CH3Cl, the C-Cl bond is polar. So, there are permanent dipole- permanent dipole forces between molecules of CH3Cl. Also, let's not forget that like all other molecules, there are also Van der Waal's forces(London forces).
There are London dispersion forces and dipole-dipole forces.
dipole-dipole
London forces are present in chlorine molecules.
Cl2 has a stronger intermolecular forces, London dispersion forces, as there are more electrons in Cl2 than in F2 It is the electrons that cause the instantaneous dipole-induced dipole interactions, more electrons = more dipoles and more easily induced dipoles = more london forces.
Intermolecular because intermolecular forces occur between molecules, not within the same molecule. Specifically the forces are London dispersion forces, due to the interaction of instantaneous dipoles.
Because NH3 has a much larger difference in its electronegativity values than of Cl2. Cl2 have a 0 difference which causes it to have weaker forces of attraction.
NaCl is ionically bonded with stong electrostatic attractions whereas Cl2 only has weak Van Der Waals' forces acting between the molecules More strength is needed to break NaCl's bonds than CL2's bonds. Therefore, NaCl is solid and Cl2 is a gas Hope this helps :)
London forces are present in chlorine molecules.
Cl2 has a stronger intermolecular forces, London dispersion forces, as there are more electrons in Cl2 than in F2 It is the electrons that cause the instantaneous dipole-induced dipole interactions, more electrons = more dipoles and more easily induced dipoles = more london forces.
Intermolecular because intermolecular forces occur between molecules, not within the same molecule. Specifically the forces are London dispersion forces, due to the interaction of instantaneous dipoles.
Because NH3 has a much larger difference in its electronegativity values than of Cl2. Cl2 have a 0 difference which causes it to have weaker forces of attraction.
The intermolecular force in CCl4 is dispersion forces. This occurs when slight variations in electron distribution effect the electron distribution of other molecules. Because CCl4 is non polar, it does not have other intermolecular forces holding the molecules together.
NaCl is ionically bonded with stong electrostatic attractions whereas Cl2 only has weak Van Der Waals' forces acting between the molecules More strength is needed to break NaCl's bonds than CL2's bonds. Therefore, NaCl is solid and Cl2 is a gas Hope this helps :)
These are polar forces, intermolecular forces of attraction between molecules.
Dipole forces and London forces are present as intermolecular forces in these molecules.
These are intermolecular forces.
Intramolecular forces are not intermolecular forces !
hydrogen bonding
The intermolecular forces in acetone are weaker.