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Home  / GENERAL CHEMISTRY Textbook / Chapter 6. Molecule structure / Van der Waals Bond (VWB)

Van der Waals Bond (VWB)

The third type of bond is the Van der Waals bond (VWB). It has been experimentally defined that molecules in which the outermost shells of all the atoms are filled, say, molecules of nitrogen (N2), chlorine (Cl2), ammonia (NH3), and the atoms of inert gases - He, Ne, etc. - also bond among themselves. Such bonds have been named after the Dutch physicist Van der Waals. These are weak bonds.

It has been found experimentally, that, indeed, bonds between inert gas atoms do exist, but their length (the distance between the nuclei) is about two times greater than in the case of a covalent bond and a DAB; and the bonding energy differs by more than 10 times.

As indicated above, the approach of the hydrogen atoms' nuclei in the course of the formation of molecule H2, as seen from the calculation of the hydrogen molecule, leads to the increase of the effective charge (the charge of the nuclei acting upon the bonding electrons in the molecule) by 1.5 times. A ten times greater decrease in the bonding energy when increasing the distance by 2 times, is due not only to the decrease of the Coulomb interaction, but also to the decrease of the effective charge of the nuclei to be bonded, with the increase of the distance between them.

Chapter 6. Molecule structure >> 
Conclusions >>   
**Molecules formed of multi-electron atoms >>  
**Ionization energy of multi-electron atoms >>       
**Chemical Energy. FIEs of element and bonding energy >>
**Chemical Bonding Energy >>
***Bond Lengths >>
Conclusions >>
Valence >>
Conclusions >>     
**Donor - acceptor Bond (DAB) >>  
Van der Waals Bond (VWB)  
Dynamic Bonds >>
Conclusions >> 
Chapter 6 Textbook Questions