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> | + | '''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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Revision as of 15:51, January 3, 2009
Electronegativity is a measure of how strongly an atom in a molecule rejects extra electrons away from itself. This occurs because an atom has a positively charged centre (made up of protons and neutrons) 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.[1] Generally, electronegativity increases across a horizontal row of the periodic table, as well as up a vertical column.[2] Fluorine is the most electronegative known element.