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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.
'''Electronegativity''' is a measure of how strongly an [[atom]] in a [[molecule]] attracts extra [[electron]]s 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.
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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]]