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Electronegativity

Electronegativity in Periodic Table

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Electronegativity

Define electronegativity. Also, describe trends in electronegativity in the periodic table.

 The electronegativity is considered to be a measure of the way strong atoms attract the bonding electrons to themselves.  It is found that the higher the electronegativity is, the greater the atoms are in attraction of the electrons.  In the periodic table, the electronegativity of the elements increases from the bottom of a group on the top. However, it does not apply the transition metals and left on the right across a period.  There are the negative ions and the most electronegative element is the fluorine. It is followed by chlorine, oxygen and nitrogen.  The ionic compounds are formed between the widely differing electronegativities having ionic compounds and ionic bonding.  

Taken for example, there has been ionic compounds such as lithium nitride, potassium fluoride and magnesium oxide.  The covalency is when the atoms with similar electronegativity react, covalent bonds are produced where the electrons are shared between the atoms.  The example can be the C-C bond and the C-H bonds.  The Polar covalency becomes higher when electronegativity is covalently bonded with an atom having lower electronegativity.  The bigger share of the bonding of electrons will be taken by higher electronegativity atoms.  The result is that this uneven sharing of the electrons will have smaller charge on the electronegative atoms along with a small positive charge on the atom. It is followed by chlorine, oxygen and nitrogen.  

The ionic compounds are formed between the widely differing electronegativities having ionic compounds and ionic bonding.  Taken for example, there has been ionic compounds such as lithium nitride, potassium fluoride and magnesium oxide.  The covalency is when the atoms with similar electronegativity react, covalent bonds are produced where the electrons are shared between the atoms.  It is found that the higher the electronegativity is, the greater the atoms are in attraction of the electrons.  In the periodic table, the electronegativity of the elements increases from the bottom of a group on the top. However, it does not apply the transition metals and left on the right across a period. The bigger share of the bonding of electrons will be taken by higher electronegativity atoms.  The result is that this uneven sharing of the electrons will have smaller charge on the electronegative atoms along with a small positive charge on the atom. It is followed by chlorine, oxygen and nitrogen.The example can be the C-C bond and the C-H bonds.  The Polar covalency becomes higher when electronegativity is covalently bonded with an atom having lower electronegativity. The bigger share of the bonding of electrons will be taken by higher electronegativity atoms. The result is that this uneven sharing of the electrons will have smaller charge on the electronegative atoms along with a small positive charge on the atom. .  The Polar covalency becomes higher when electronegativity is covalently bonded with an atom having lower electronegativity.The bigger share of the bonding of electrons will be taken by higher electronegativity atoms.  

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