The result of this uneven sharing of electrons is a small negative charge on the more electronegative atom and a small positive charge on the atom it is bonded to. When a higher electronegativity atom is covalently bonded to an atom of lower electronegativity, the greater share of the bonding electrons is taken by the higher electronegativity atom. This results in a polar covalent bond, with hydrogen slightly positively charged and chlorine slightly negatively charged. If you know the electronegativity of each atom in a diatomic molecule, you can predict how the bond will polarize.įor example, on the Pauling Scale, hydrogen's electronegativity is 2.18 and chlorine's is 3.16. When atoms of similar electronegativity react, they tend to produce covalent bonds in which electrons are shared between atoms. Highly electropositive elements have a strong tendency to form positive ions.Ĭompounds formed between elements with widely differing electronegativities tend to be ionic compounds, with ionic bonding.Įxamples of ionic compounds are potassium fluoride, lithium nitride, and magnesium oxide. The least electronegative (most electropositive) element is cesium, followed by rubidium, potassium and barium. The most electronegative element is fluorine, followed by oxygen, chlorine and nitrogen.Ītoms with high electronegativity tend to form negative ions. the bottom of a group to the top (although this does not apply to the transition metals) and.Looking at the elements in the periodic table, in general, electronegativity of elements increases from:
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