9.3. Polarity and Intermolecular Forces http://www.ck12.org
i. SF 6- Which substance in each of the following pairs would be expected to have the higher boiling point? Explain.
a. ICl or Br 2
b. HCl or HF
c. Kr or Ar
d. CF 4 or CH 4
e. NH 3 or PH 3 - Ethanol and dimethyl ether both have the same molecular formula, C 2 H 6 O. However, the boiling point of
ethanol is much higher (78°C) than that of dimethyl ether (−25°C). What could be the explanation for this
difference?
Further Reading / Supplemental Links
- Electronegativity (http://www.chemguide.co.uk/atoms/bonding/electroneg.html
- IntermolecularBonding–vanderWaalsForces (http://www.chemguide.co.uk/atoms/bonding/vdw.html
- IntermolecularBonding–HydrogenBonds (http://www.chemguide.co.uk/atoms/bonding/hbond.html
Points to Consider
Lewis electron-dot structures and VSEPR theory explain the bonding patterns and molecular geometries of molecules,
but not the specific way in which electrons in atomic orbitals interact with one another as a covalent bond forms.
- How can atomic orbitals be modified to explain how electrons are arranged in a molecule?
- How are single bonds different from double or triple bonds?