Explain the effect of intramolecular bonding on strength of acids.

Dear Menka,

hree types of force can operate between covalent molecules:

• Dispersion Forces
  also known as London Forces (named after Fritz London who first described these forces theoretically 1930) or as Weak Intermolecular Forces or as van der Waal's Forces (namd after the person who contributed to our understanding of non-ideal gas behaviour).

   

• Dipole-dipole interactions

   

• Hydrogen bonds

Relative strength of Intermolecular Forces:

• Intermolecular forces (dispersion forces, dipole-dipole interactions and hydrogen bonds) are much weaker than intramolecular forces (covalent bonds, ionic bonds or metallic bonds)

   

• dispersion forces are the weakest intermolecular force (one hundredth-one thousandth the strength of a covalent bond), hydrogen bonds are the strongest intermolecular force (about one-tenth the strength of a covalent bond).

   

• dispersion forces < dipole-dipole interactions < hydrogen bonds

Dispersion Forces (London Forces, Weak Intermolecular Forces, van der Waal's Forces)

• are very weak forces of attraction between molecules resulting from:

1. momentary dipoles occurring due to uneven electron distributions in neighbouring molecules as they approach one another

    

2. the weak residual attraction of the nuclei in one molecule for the electrons in a neighbouring molecule.

• The more electrons that are present in the molecule, the stronger the dispersion forces will be.

   

• Dispersion forces are the only type of intermolecular force operating between non-polarmolecules, for example, dispersion forces operate between hydrogen (H₂) molecules, chlorine (Cl₂) molecules, carbon dioxide (CO₂) molecules, dinitrogen tetroxide (N₂O₄) molecules and methane (CH₄) molecules.

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