H2s Polar Or Nonpolar
Why is everyone saying that H2S is polar when it is not non-polar? 3
My teacher taught me that when we look at the polarity of a molecule, we first look at the types of bonds that exist. In this case, the ES in the HS bond is 0.38, which is less than 0.4, so regardless of the polar (curve) geometry, the bond is still a non-polar molecule. However, water with the same geometry will be polar, because the EN difference between oxygen and hydrogen is> 0.4, i.e. the bond is polar.
So I don't understand why everyone says H2S is polar because it's square. If it is polar, why is its boiling point less than CO2, a non-polar gas molecule?
updateThanks for the reply, but do you think O3 is polar? !! (The shape is also curved) But it's a little funny, isn't it? Ozone is almost soluble in polar solvents, but very well soluble in non-polar solvents.
There are several things to consider when determining whether a molecule is polar.
1) Connection type Non-polar coordinate vs. Polar coordinate vs. Ionic coolant (as it happens)
2) Molecular electrical geometry
If a molecule has electrically compatible geometry, regardless of the type of bond, it is non-polar.
If a molecule has disproportionate electrical geometry, it is polar, regardless of the bonds.
The molecule is polar. You are right that hydrogen sulfur bond is not polar due to differences in electronegativity. You are wrong when you say:
Regardless of polar geometry (curve), it is always a non-polar molecule.
The geometry of H2S is curved in sulfur due to isolated joints. This means that the end of a single pair of molecules has a higher electron density than two hydrogen atoms, so a molecule with a dopole moment of 0.97 D is usually polar.
The boiling points of two molecules can be explained by the interneuclear forces acting between the molecules. CO2 is non-polar with a dopole moment of 0 and is therefore an interneuclear bond due to the parasitic force of London. H2S is polar, so it binds internally through dipole-dipole interactions. The former is stronger than the latter, which gives CO2 a higher melting point and boiling point.