Methane or CH4 is not a dipole. It is because the molecule of this element has no polarity. The polarity if CH4 is neutral.
Since CH4 is not polar it has no dipole forces, and the London dispersion forces associated with CH4 are very weak.
No. Methane is nonpolar so intermolecular interactions are limited to London dispersion forces.
No, it is not.
no
CH3OH has an H bond with an oxygen molecule, causing H bonding to be a force. It also has dipole-dipole interaction because it's a polar molecule. Thus, it has all three of the forces (including London dispersion).
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.
no
nh3-nh3 because they are both polar molecules
No it doesn't; as there is practically no difference in electronegativity between carbon and hydrogen to create a dipole.
CH3OH has an H bond with an oxygen molecule, causing H bonding to be a force. It also has dipole-dipole interaction because it's a polar molecule. Thus, it has all three of the forces (including London dispersion).
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.
no
Correct answers from Mastering Chemistry: NH3 - hydrogen bonding CH4 - Dispersion forces NF3 - dipole-dipole
nh3-nh3 because they are both polar molecules
No it doesn't; as there is practically no difference in electronegativity between carbon and hydrogen to create a dipole.
Ion-ion forces
it is polar. therefore, dipole-dipole and dispersion forces (always present)
Dipole-Dipole forces and London Forces
Dipole-Dipole forces
I suppose that these are dipole-dipole forces.
These are intermolecular forces.