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Noncovalent Bonding

Noncovalent bonding

There are three principle kinds of noncovalent forces.

1. Ionic Interactions

At any given pH, proteins have charged groups that may participate in binding them to each other or to other types of molecules. For example, as the figure shows, negatively-charged carboxyl groups on aspartic acid (Asp) and glutamic acid (Glu) residues may be attracted by the positively-charged free amino groups on lysine (Lys) and arginine (Arg) residues.

Ionic interactions are highly sensitive to

  • changes in pH.

    As the pH drops,

    • H+ bind to the carboxyl groups (COO-) of aspartic acid (Asp) and glutamic acid (Glu), neutralizing their negative charge, and
    • H+ bind to the unoccupied pair of electrons on the N atom of the amino (NH2) groups of lysine (Lys) and arginine (Arg) giving them a positive charge.

    The result: Not only does the net charge on the molecule change (it becomes more positive) but many of the opportunities that its R groups have for ionic (electrostatic) interactions with other molecules and ions are altered.

    As the pH rises,
    • H+ are removed from the COOH groups of Asp and Glu, giving them a negative charge (COO), and
    • H+ are removed from the NH3+ groups of Lys and Arg removing their positive charge.

    The result: Again the net charge on the molecule changes (it becomes more negative) and, again, many of the opportunities its R groups have for electrostatic interactions with other molecules or ions are altered.

    Link to example showing how all serum proteins become negatively-charged at a pH of 8.6.
  • salt concentration. Increasing salt concentration reduces the strength of ionic binding by providing competing ions for the charged residues.

2. Hydrophobic Interactions

The side chains (R groups) of such amino acids as phenylalanine and leucine are nonpolar and hence interact poorly with polar molecules like water. For this reason, most of the nonpolar residues in globular proteins are directed toward the interior of the molecule whereas such polar groups as aspartic acid and lysine are on the surface exposed to the solvent. When nonpolar residues are exposed at the surface of two different molecules, it is energetically more favorable for their two "oily" nonpolar surfaces to approach each other closely displacing the polar water molecules from between them.

The strength of hydrophobic interactions is not appreciably affected by changes in pH or in salt concentration.

3. Hydrogen Bonds

Hydrogen bonds can form whenever

  • a strongly electronegative atom (e.g., oxygen, nitrogen) approaches
  • a hydrogen atom which is covalently attached to a second strongly-electronegative atom.

Some common examples:

  • between the −C=O group and the H-N− group of nearby peptide bonds in proteins (giving rise to the alpha helix [View] and beta configuration)
  • Between −C=O groups and hydroxyl (H-O−) groups in
Link to a separate page on hydrogen bonds.

Noncovalent interactions are individually weak but collectively strong.

All three forms of noncovalent interactions are individually weak (on the order of 5 kcal/mole) as compared with a covalent bond (with its 90–100 kcal/mole of bond energy). And what strength these interactions do have requires that the interacting groups can approach each other closely (an angstrom or less). So we can conclude that all the examples given at the top of the page require:

  • a substantial number of noncovalent interactions working together to hold the structures together;
  • a surface topography that enables substantial areas of two interacting surfaces to approach each other closely; that is, they must fit each other. [View an example.]

24 February 2011