The relative strength of the four intermolecular forces is: ionic> hydrogen bond> dipole dipole> van der Waals dispersion forces. SO2 has a curved structure and a net dipole moment. It is therefore a polar molecule with dipolar forces.
Since CO2 is a linear molecule, it is not polar and therefore the only force acting between the CO2 molecules is the London Dispersion Force, the weakest intermolecular attraction. Although SO2 is an angular and therefore polar molecule, the dipole-dipole interactions between its molecules interact with the London dispersion forces.
SO2 cannot form hydrogen bonds because it is not hydrogen. The bonds are polar because S is slightly positive and O is slightly negative, so there are intermolecular bonds in them, but without hydrogen they are not classified as hydrogen bonds.
SO2 is a polar molecule. In general, dipole forces are stronger than LDF forces.
SO2 has a bond angle of 120 degrees. A single sulfur atom is covalently bonded to two oxygen atoms. It causes the electron pairs to repel each other to form an angle of 120 degrees.Is
H2S, H2Se and H2Te show dipolar intermolecular forces, while H2O has hydrogen bonds. C4H10 is a non-polar hydrocarbon molecule, so it has a dispersive power (42 electrons) and a stronger attraction than CO2 (Kp -0.5 ° C).
The strongest intermolecular attractions are the dipole-dipole interactions.
The relative forces of the four intermolecular forces are: Ionic> hydrogen bond> dipole dipole> van der Waals dispersion forces. SO2 has a curved structure and a net dipole moment. It is therefore a polar molecule with dipole dipole forces.
The SO2 molecule has a dipole moment. This molecule does not have a permanent dipole moment (i.e. the dipole moment of CO2 is zero). This requires the molecule to be linear since oxygen is more electronegative than carbon and therefore C = O. The bond becomes polarized.
(Electrons on oxygen are not shown, but each has two pairs, as above, sulfur has no electrons). SO3 is non-polar and SO2 is polar due to the differences in substituents, but mainly due to geometry.
So for CHCl3 the molecule is tetrahedral, but the atoms around C are not all the same. Such polar molecules create dipole-dipole forces between them (the negative side of one molecule attracts the positive side of the other).
(c) NH3: Hydrogen bond dominates (although there are also dispersion and dipole forces). (b) NO has a higher boiling point because it has dipole forces, while N2 has only dispersion forces. (c) H2Te has a higher boiling point than H2S. Both have dispersion and dipole-dipole forces.
Of all the substances used, water has the strongest intermolecular forces (hydrogen bonds). Glycerin and alcohol also have hydrogen bonds, but these intermolecular forces are somewhat weaker than in water.
Hydrogen bonds are attractions between a hydrogen + hydrogen on one molecule and a single pair on a strongly electronegative atom (N, O or F) on another molecule. c) In HF each molecule has one + hydrogen and three single active pairs. Therefore, ammonia and HF can only form an average of two hydrogen bonds per molecule.
The chemical element with the lowest boiling point is helium and the element with the highest boiling point is tungsten.
Molecules capable of hydrogen bonds have hydrogen atoms covalently bonded to strongly electronegative elements (O, N, F). CO2 can form hydrogen bonds with water, but its linear shape makes it a non-polar molecule. This means that carbon dioxide is less soluble in water than polar molecules.
For example, HCl molecules have a dipolar moment because the hydrogen atom has a small positive charge and the chlorine atom has a small negative charge. Due to the attraction between oppositely charged particles, there is a small dipole-dipole attraction between neighboring HCl molecules.
Carbon dioxide is linear while sulfur dioxide is curved (V shape). In addition to the two double bonds, there is also a solitary pair on the sulfur in sulfur dioxide. To minimize repulsion, the double bonds and single pairs separate as much as possible, then the molecule is folded.