Hydrogen bonding in NH3 and H2O, London dispersion forces in CH4
yes . since it is polar
Hydrogen bonding and London dispersion forces.
dispersion forces, dipole-dipole forces and hydrogen bonding
No, covalency does not have its own intermolecular force
Ammonia interact by hydrogen bonds.
Hydrogen bonding is the strongest intermolecular force
Hydrogen bonds. Hydrogen bonds occur whenever hydrogen is bonded with Carbon, Nitrogen, Oxygen, Florine or Sulfur
intramolecular force not intermolecular force (I got it right on a test)
Solid state matter has maximum intermolecular force.
Both NH3 and HCl exhibit hydrogen bonding as intermolecular forces, whereas CH4 does not. This makes CH4 have a lower boiling point. Since there are 3 hydrogen atoms in NH3 and only 1 in HCl(g), the intermolecular forces would be expected to be greater in NH3 than in HCl.
Correct answers from Mastering Chemistry: NH3 - hydrogen bonding CH4 - Dispersion forces NF3 - dipole-dipole
NH3 exhibits hydrogen bonding in addition to dispersion forces. This significantly increases the intermolecular force, and raises the boiling point. PH3 does not exhibit hydrogen bonding and the dominant intermolecular force holding these molecules together is dispersion forces. (Dispersion forces also known as Van Der Waal Force)
Hydrogen bonding is the main intermolecular force in HF.
dispersion, dipole-dipole, and hydrogen bonding forces
In an ammonia molecule, three hydrogen atoms are bonded to nitrogen via covalent bonds.These bonds are polar in nature due to high electronegativity of nitrogen.