I think it is the German-American physicist Fritz London :)
The only intermolecular forces in this long hydrocarbon will be dispersion forces.
London dispersion forces
Dipole-Dipole and covalent sigma bond forces.
London forces
London dispersion forces (instantaneous induced dipole-dipole interactions.)
The only intermolecular forces in this long hydrocarbon will be dispersion forces.
London dispersion forces
Dipole-Dipole and covalent sigma bond forces.
London forces
Yes, CH3CH2CH3 (propane) can experience London dispersion forces. London dispersion forces are weak intermolecular attractive forces that all molecules exhibit due to temporary shifts in electron distribution, resulting in temporary dipoles.
London dispersion vander walls force
London dispersion forces (instantaneous induced dipole-dipole interactions.)
Hydrogen bonding and London Dispersion forces (the latter of which are in all molecules).
Yes, CH4 (methane) does exhibit London dispersion forces due to temporary fluctuations in electron distribution around the molecule. These dispersion forces are the weakest intermolecular forces and are responsible for the non-polar nature of methane.
In C6H14 (hexane) and H2O (water), there are London dispersion forces, dipole-dipole interactions, and hydrogen bonding. In HCHO (formaldehyde), there are dipole-dipole interactions and London dispersion forces. In C6H5OH (phenol), there are hydrogen bonding, dipole-dipole interactions, and London dispersion forces.
Van der Waals forces are a broader term that includes London dispersion forces as a subset. London dispersion forces are the weakest type of van der Waals forces and are caused by temporary fluctuations in electron distribution. Van der Waals forces also include dipole-dipole interactions and hydrogen bonding, which are stronger than London dispersion forces.
The dominant intermolecular forces in octane are London dispersion forces. These are relatively weak forces that result from temporary fluctuations in electron distribution within atoms and molecules.