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The only intermolecular forces in this long hydrocarbon will be dispersion forces.
London dispersion forces
Dipole-Dipole and covalent sigma bond forces.
London dispersion forces (instantaneous induced dipole-dipole interactions.)
London Dispersion Forces
yes, CH4 has London dispersion forces because it is a non-polar molecule and non-polar molecules have London dispersion forces present in them. there are no other forces present in CH4.
no
Methane is non polar.So dispersion forces are formed.
Volatile means that a substance evaporate easily.Methane is volatile because:- molecules of methane are bonded by dispersion forces- dispersion forces are the weakest form of intermolecular bonding, meaning that there is only a small amount of energy (or heat) required to break the weak dispersion forces between the methane molecules
The only intermolecular forces in this long hydrocarbon will be dispersion forces.
London dispersion forces
Dipole-Dipole and covalent sigma bond forces.
CHF3 is a polar molecule. The fluorine atoms are electronegative and draw electrons towards their end of the molecule, leaving the hydrogen with a slight positive charge on it. So dipole-dipole forces will act between the molecules. The molecules will also exert dispersion forces on each other, but these are much weaker than the dipole-dipole forces.
In a single molecule of CH4 you would have intramolecular forces that are covalent bonds. The intermolecular forces that exist between molecules of CH4 are called dispersion forces. These forces are the only intermolecular forces that occur between non-polar molecules.
Covalent bonds are the intramolecular forces that hold the hydrogens to the carbon in methane, CH4. The intermolecular forces holding several methane molecules together are London dispersion forces (van der Waals forces).
Dispersion forces
Hydrogen bonding and London Dispersion forces (the latter of which are in all molecules).