The intermolecular force present in CH₄ is London dispersion forces, H₂0 has all the three types of molecular forces, Co experience dipole-dipole forces and dipole-dipole forces also exist in CH₃Cl
<h2>Further Explanation</h2>
CH₄ is a non polar molecule. Methane gas is made up of a carbon atom that is bound to four hydrogen atoms. All these atoms shared the same electrons and this molecule has no charge. Also, methane cannot produce hydrogen bonding
H₂0 is a polar molecule and contains intermolecular dipole-dipole hydrogen bonds. When water attracts and bonds with each other, they show some properties which include high heat of vaporization and surface tension.
Water contains O-H bonds, the negative atoms (o) attracts and bonds with the positive hydrogen and leads to a strong hydrogen bond which is a strong type of dipole-dipole forces.
Co is a polar molecule because it also experiences dipole-dipole forces and the attraction between the CO molecules are strong.
CH₃Cl (chloromethane) is also a perfect example of dipole-dipole interaction.
There are different types of intermolecular forces that take place between molecules
Dipole-dipole interactions: this interaction takes place when a molecule that is partially positively charged interacts electrostatically with another nearby molecule that is partially negatively charged.
London dispersion forces: These types of intermolecular forces can occur between polar and non-polar molecules; in fact, they can exist between all types of molecules. These forces are also the weakest out of types of intermolecular forces
Hydrogen bonding: is another type of dipole-dipole interaction that exists between N, O or F atom.
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KEYWORDS:
- intermolecular forces
- dipole-dipole interaction
- london dispersion forces
- hydrogen bonding
- force of attraction
