The principal reason is the hydrogen bonding between HF molecules. The second reason is that London dispersion forces will be higher in HF because it has more electrons than H2
The only intermolecular forces in this long hydrocarbon will be dispersion forces.
London dispersion forces
Dipole-Dipole and covalent sigma bond forces.
Hydrogen fluoride, with the chemical formula HF, is a colorless gas that is the principal source of fluorine. The type of intermolecular forces that exist in HF are London forces, dipole-dipole.
The principal reason is the hydrogen bonding between HF molecules. The second reason is that London dispersion forces will be higher in HF because it has more electrons than H2
The only intermolecular forces in this long hydrocarbon will be dispersion forces.
London dispersion forces
Hydrogen fluoride has higher boiling point than hydrogen bromide ( HF 19.5 C HBr -66 C) because in hydrogen fluoride has two kinds of forces, one is hydrogen bonding and other is London dispersion forces. In Hydrogen bromide there are only london dispersion forces. These are weaker than hydrogen bonds therefore HF has the higher boiling pint.
Dipole-Dipole and covalent sigma bond forces.
Dispersion forces
Hydrogen bonding and London Dispersion forces (the latter of which are in all molecules).
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.
Hydrogen fluoride, with the chemical formula HF, is a colorless gas that is the principal source of fluorine. The type of intermolecular forces that exist in HF are London forces, dipole-dipole.
Dipole-dipole interactions, and London dispersion interactions
C6H14 - dispersion forces H2O - hydrogen bonding, dipole, dispersion HCHO - dipole, dispersion C6H5OH - hydrogen bonding, dipole, dispersion
London dispersion forces (instantaneous induced dipole-dipole interactions.)