Salt bridges: Difference between revisions
Jump to navigation
Jump to search
Eric Martz (talk | contribs) adding content |
Eric Martz (talk | contribs) adding content |
||
| Line 1: | Line 1: | ||
In proteins, salt bridges occur between amino acid side-chains with opposite positive or negative full-electron charges, namely, (at neutral pH) Glu- or Asp- vs. Arg+ or Lys+. They | <applet load='1cbr' size='300' frame='true' align='right' caption='Insert caption here' /> | ||
In proteins, salt bridges occur between amino acid side-chains with opposite positive or negative full-electron charges, namely, (at neutral pH) Glu- or Asp- vs. Arg+ or Lys+. They may also occur between ionized organic ligands, such as acetylcholine+, or inorganic ions, such as K+ or Cl-, and amino acid side-chains. | |||
A salt bridge is generally considered to exist when the centers of charge are 4 Å or less apart<ref>Jeffrey, George A., An introduction to hydrogen bonding, Oxford University Press, 1997. Page 192.</ref>. The energetic significance of such complementary charge pairs is a complex function of the local environment. | A salt bridge is generally considered to exist when the centers of charge are 4 Å or less apart<ref>Jeffrey, George A., An introduction to hydrogen bonding, Oxford University Press, 1997. Page 192.</ref>. The energetic significance of such complementary charge pairs is a complex function of the local environment. | ||
Revision as of 21:14, 3 February 2010
|
In proteins, salt bridges occur between amino acid side-chains with opposite positive or negative full-electron charges, namely, (at neutral pH) Glu- or Asp- vs. Arg+ or Lys+. They may also occur between ionized organic ligands, such as acetylcholine+, or inorganic ions, such as K+ or Cl-, and amino acid side-chains.
A salt bridge is generally considered to exist when the centers of charge are 4 Å or less apart[1]. The energetic significance of such complementary charge pairs is a complex function of the local environment.
Putative salt bridges can be displayed by FirstGlance in Jmol.
ReferencesReferences
- ↑ Jeffrey, George A., An introduction to hydrogen bonding, Oxford University Press, 1997. Page 192.