Within the NH3 compound, three hydrogen bonds exists, Hydrogen bonds only occurs with Nitrogen, Oxygen and fluorine. Basically Hydrogen bond is an attractive interaction of hydrogen atom with an electronegative element. Hydrogen bond only occurs with oxygen, nitrogen and Florine because these three elements are really high in their electronegtivity (their attraction for electrons) and they actually snatches the electron from the hydrogen nuclei to its own, not forever but it shares most of the electron than hydrogen itself, which makes the compound polar, like soluble in water.
dispersion forces, dipole-dipole forces and hydrogen bonding
Hydrogen bonds. Hydrogen bonds occur whenever hydrogen is bonded with Carbon, Nitrogen, Oxygen, Florine or Sulfur
Hydrogen bonding and London dispersion forces.
All molecules have van der Waals forces, the weakest of all intermolecular attractions due to electron motion in the molecule.
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.
hydrogen bonds
gravity
hydrogen bond
dispersion, dipole-dipole, and hydrogen bonding forces
Ammonia form hydrogen bonds.
Because NH3 has a much larger difference in its electronegativity values than of Cl2. Cl2 have a 0 difference which causes it to have weaker forces of attraction.
Look at intermolecular forces and judge from there
hydrogen bond
dispersion, dipole-dipole, and hydrogen bonding forces
co2
Ammonia form hydrogen bonds.
Because NH3 has a much larger difference in its electronegativity values than of Cl2. Cl2 have a 0 difference which causes it to have weaker forces of attraction.
Correct answers from Mastering Chemistry: NH3 - hydrogen bonding CH4 - Dispersion forces NF3 - dipole-dipole
In vanderwaal's Equation 'a' measures the intermolecular force of attraction and 'b' measures the volume of the molecule. N2 has greater volume (due to it's larger size) and hence 'b' is greater for N2. NH3 has greater dipole moment and hence 'a' is greater for NH3.
Look at intermolecular forces and judge from there
Both are polar substances capable of a strong type of intermolecular attraction called hydrogen bonding. NH3 and H2O molecules therefore attract one another.
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)
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0,522 moles of ammonia contain 3,143.10e23 molecules of NH3.