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Highest electronegative element → F (Fluorine) Lowest electronegative element → Cs (Cesium) Highest electron affinity            →   Cl (Chlorine) Lowest electron affinity            →   Noble gases Most electropositive stable element → Cs(cesium) Least electropositive element →       F(Fluorine) Highest ionization potential →       He(helium) Lowest ionization potential →      Cs(Cesium) Largest atomic radius →             Cs (Cesium)  Smallest atomic radius   →        H (Hydrogen) Largest anionic radius → I- (Iodide ion) Smallest anionic radius → H- (Hydride ion) Largest cationic radius → Smallest cationic radius → H+ (Hydrogen ion) Highest melting point metal → W (Tungsten) Lowest melting point metal → Hg (Mercury) Highest boiling point metal / element → W (Tungsten)  Lowest bo...

  The tendency of an atom in a compound to attract shared electrons towards itself is known as electronegativity of an atom. Pauling gave an arbitrary scale to measure the electronegativity of different elements. This scale is based upon the calculation of bond energies, In this scale fluorine has the maximum value of electronegativity, i. e. 4.0. whereas noble gases have the minimum value, i. e. 0.0. On Mulliken scale, the average of ionization potential and electron affinity is known as electronegativity. In general, the smaller atoms as well  as the atoms with nearly filled shells of electrons, attract electrons more than larger atoms and are, therefore, more electronegative. Determination of Electronegativity   Pauling's scale: Pauling's   scale of electronegativity is based upon the calculation of bond energies. He considered the formation of AB covalent molecule as:  1/2A2+1/2B2 → AB   1/2(A-A) +1/2 (B-B) → A-B  According to Pauling, the bond dis...

    The chemical properties of the elements are also determined by the tendency of their atoms to accept an additional electron. This tendency is measured by the electron affinity, i.e., the energy released when a gaseous atom accepts an electron forming a free gaseous ion. X(g)+e = X-(g) + energy released     The energy released is measured in electron volt per atom (e. v. /atom) or   kilo joule per mole (k. j./mole ). Thus, larger is the energy released, the greater is the electron affinity. in other words, it is a measure of the force with which the added electron is bound by the nucleus of the atom. There may be first, second or higher electron affinity just like ionization potential.           O(g)+e = O-(g) + 1.47 e. v.          O- (g)+e = O2- (g) - 8.75 e. v.     The second and higher electron affinities are always negative because there occurs a repulsion between negatively charged ion and ...

           The minimum energy required to remove most loosely bound electron from the isolated gaseous atom is known as ionization potential or ionization energy.