Hydrogen bond: Difference between revisions
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Hydrogen bonding takes place when a single hydrogen atom binds to either a nitrogen, flourine or oxygen atom (which are very electronegative). Since hydrogen has a single lone electron, and nitrogen, flourine and oxygen atoms require extra electrons to have a full outer shell, this electron is drawn away to the electronegative atom, leaving hydrogen with only a proton in its nucleus. The hydrogen atom now has a positive charge (due to the absence of the electron and the presence of a proton) and it is this proton that is attracted to a pair of non-bonding electrons from the electronegative atom (nitrogen, oxygen or flourine). This bond is stronger than Van der Waals' forces and basic dipole:dipole forces. | Hydrogen bonding takes place when a single [[hydrogen|hydrogen]] [[atom|atom]] binds to either a [[nitrogen|nitrogen]], [[flourine|flourine]] or [[oxygen|oxygen]] atom (which are very [[electronegative|electronegative]]). Since hydrogen has a single lone [[electron|electron]], and nitrogen, flourine and oxygen atoms require extra electrons to have a full outer shell, this electron is drawn away to the electronegative atom, leaving hydrogen with only a [[proton|proton]] in its [[nucleus|nucleus]]. The hydrogen atom now has a positive charge (due to the absence of the electron and the presence of a proton) and it is this proton that is attracted to a pair of non-bonding electrons from the electronegative atom (nitrogen, oxygen or flourine). This bond is stronger than [[Van_der_waals_forces|Van der Waals' forces]] and basic [[dipole:dipole force|dipole:dipole forces]]. | ||
Revision as of 18:49, 25 October 2012
Hydrogen bonding takes place when a single hydrogen atom binds to either a nitrogen, flourine or oxygen atom (which are very electronegative). Since hydrogen has a single lone electron, and nitrogen, flourine and oxygen atoms require extra electrons to have a full outer shell, this electron is drawn away to the electronegative atom, leaving hydrogen with only a proton in its nucleus. The hydrogen atom now has a positive charge (due to the absence of the electron and the presence of a proton) and it is this proton that is attracted to a pair of non-bonding electrons from the electronegative atom (nitrogen, oxygen or flourine). This bond is stronger than Van der Waals' forces and basic dipole:dipole forces.