Triplets?

Chemistry Level pending

The above are space-filling models for three hydrogen compounds with carbon group elements. The boiling points of these three compounds are as follows: CH 4 ( − 16 2 ∘ C ) < SiH 4 ( − 11 2 ∘ C ) < GeH 4 ( − 8 8 ∘ C ) . \text{CH}_4 (-162^\circ\text{C}) < \text{SiH}_4 (-112^\circ\text{C}) < \text{GeH}_4 (-88^\circ\text{C}). Which of the following is the most relevant explanation for the differences in the boiling points?

covalent bond dipole-dipole force hydrogen bond van der Waals force

Lakshan Dumpa by Lakshan Dumpa , 24, India

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1 solution

Lu Chee Ket
Jan 29, 2016

http://www.masterorganicchemistry.com/2010/10/01/how-intermolecular-forces-affect-boiling-points/

Tetrahedron structures do not leave with the so called hydrogen bonds. Since they are not ionic bonds,

  1. Van Der Waals Dipole-dipole interactions not the general one for this case.

  2. Van der waals Dispersion forces due to temporary dipoles by polarization is the one for this case.

Answer: V a n d e r w a a l s f o r c e \boxed{Van~der~waals~force}

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