Molecular Formula: H2SO4
This Molecule is a polar molecule. The reason for this is the distribution of the electrons. They are unevenly distributed
through the molecule, with more pull in the oxygen bonded to the Hydrogen.
The forces acting on this molecule, should it pass another of the same molecule, would be:
London Forces- The weak attraction made by all molecules due to temporary polarity
Dipole-Dipole- Electrostatic bonds from the attraction of one molecule's negative end to another's positive
Hydrogen Bonds- Strong bonds made from a molecule's Hydrogen to another's Oxygen, Nitrogen, or Fluorine
Nice appearance. The giant picture of the molecule was easy to see especially for an elderly person with poor eyesight!
ReplyDeleteSpot on Lewis structure, my good chap!
ReplyDeleteI had no idea sulfuric acid had polar bonds. Good job. :)
ReplyDeleteYes, I agree. Sulfuric acid has dipoles and can hydrogen bond and like all molecules dispersion. You have all the forces!
ReplyDeletePretty effective - Love the "Duct tape of Acids" analogy.
ReplyDeleteYes, it is a polar molecule. Correct.
ReplyDelete