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Lone pair
In chemistry, a lone pair refers to a pair of valence electrons that are not shared with another atom〔IUPAC ''Gold Book'' definition: (''lone (electron) pair'' )〕 and is sometimes called a non-bonding pair. Lone pairs are found in the outermost electron shell of atoms. They can be identified by using a Lewis structure. Electron pairs are therefore considered lone pairs if two electrons are paired but are not used in chemical bonding. Thus, the number of lone pair electrons plus the number of bonding electrons equals the total number of valence electrons around an atom.
Lone pairs are a concept used in VSEPR theory which explains the shapes of molecules. They are also referred to in the chemistry of Lewis acids and bases. However not all non-bonding pairs of electrons are considered by chemists to be lone pairs. Examples are the transition metals where the non-bonding pairs do not influence molecular geometry and are said to be stereochemically inactive.
== Examples ==
A ''single'' lone pair can be found with atoms in the nitrogen group such as nitrogen in ammonia, ''two'' lone pairs can be found with atoms in the chalcogen group such as oxygen in water and the halogens can carry ''three'' lone pairs such as in hydrogen chloride.
In VSEPR theory the electron pairs on the oxygen atom in water form the vertices of a tetrahedron with the lone pairs on two of the four vertices. The H–O–H bond angle is with 104.5°, less than the 109° predicted for a tetrahedral angle, and this can be explained by a repulsive interaction between the lone pairs.〔''Organic Chemistry'' Marye Anne Fox , James K. Whitesell 2nd Edition 2001〕〔''Organic chemistry'' John McMurry 5th edition 2000〕〔''Concise Inorganic Chemistry'' J.D. Lee 4th Edition 1991〕
抄文引用元・出典: フリー百科事典『 ウィキペディア（Wikipedia）』
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