Difference between revisions of "Electronegativity"

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'''Electronegativity''' is a measure of how strongly an [[atom]] in a [[molecule]] rejects extra [[electron]]s away from itself. This occurs because an atom has a positively charged centre (made up of [[proton]]s and [[neutron]]s) which is continuously orbited by electrons. Outside electrons are rejected because the charge distribution of an atom can be thought of as a positive centre surrounded by negativity. This negativity rejects any outside electrons (which also have a negative charge). Electronegativity increases as the number of electrons and orbital shells around the [[nucleus]] increases; they shield the outside electrons from the postive nucleus, which attacts them, making their rejection easier.<ref>Salters-Nuffield Salter's Advanced Chemistry: Chemical Ideas' - 2003</ref>  Generally, electronegativity increases across a horizontal row of the [[Periodic table of the elements|periodic table]], as well as up a vertical column.<ref>Solomon's Organic Chemistry, Fifth Edition, 1992</ref>  [[Fluorine]] is the most electronegative known element.
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'''Electronegativity''' is a measure of how strongly an [[atom]] in a [[molecule]] attracts extra [[electron]]s to itself.  
  
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==References==
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The difference in electronegativity can cause different bonds to form. An example is that as chlorine is much more electronegative than hydrogen, hydrogen chloride has a permanent dipole, as the chlorine attracts the electrons being shared to a greater extent.
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Instantaneous dipole bonds are formed when bonded atoms are of similar electronegativity, meaning that the electrons are more or less shared evenly between atoms, and example being chlorine (Cl<sub>2</sub>). --[[User:Badger15|Badger15]] 14:53, 4 March 2009 (EST)
  
 
[[Category:Chemistry]]
 
[[Category:Chemistry]]

Revision as of 19:53, March 4, 2009

Electronegativity is a measure of how strongly an atom in a molecule attracts extra electrons to itself.

The difference in electronegativity can cause different bonds to form. An example is that as chlorine is much more electronegative than hydrogen, hydrogen chloride has a permanent dipole, as the chlorine attracts the electrons being shared to a greater extent.

Instantaneous dipole bonds are formed when bonded atoms are of similar electronegativity, meaning that the electrons are more or less shared evenly between atoms, and example being chlorine (Cl2). --Badger15 14:53, 4 March 2009 (EST)

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