What intermolecular forces are present in CH_4?

What intermolecular forces are present in CH_4?

Just London (dispersion forces).Because methane is a non-polar molecule it

is not capable of hydrogen bonding or dipole-dipole intermolecular


The only intermolecular forces in methane are London dispersion

forces.The major intermolecular forces would be dipole-dipole forces and

London dispersion forces.The electronegativities of C and H are so close

that C-H bonds are nonpolar. There are no bond dipoles and no dipole-dipole

interactions.Even if the molecule had polar C-H bonds, the symmetry of

molecule would cause the bond dipoles to cancel. The molecule would still

be nonpolar. It is a blob with no positive or negative

ends.https://www.elmhurst.edu/~chm/vchembook/images/210methane.gifThe only

forces left to consider are London dispersion forces.In a nonpolar

molecule, electrons are always moving. At any instant, they might be at one

end of the molecule. This would instantaneously create a temporary dipole,

making that end negative and the other end


positive charge attracts the electrons in an adjacent molecule. This

temporary attractive force is the London dispersion forceThe

London dispersion forces are so weak that methane does not condense to a

liquid until it cools to −161.5 °C.