Electronegativity - wikipedia Electronegativity `` Electronegative '' redirects here. For the Nightfall EP, see Electronegative ( EP ). Electrostatic potential map of a water molecule, where the oxygen atom has a more negative charge ( red ) than the positive ( blue ) hydrogen atoms Electronegativity, symbol χ, is a chemical property that describes the tendency of an atom to attract electrons ( or electron density ) towards itself. An atom 's electronegativity is affected by both its atomic number and the distance at which its valence electrons reside from the charged nucleus. The higher the associated electronegativity number, the more an element or compound attracts electrons towards it. The term `` electronegativity '' was introduced by Jöns Jacob Berzelius in 1811, though the concept was known even before that and was studied by many chemists including Avogadro. In spite of its long history, an accurate scale of electronegativity was not developed until 1932, when Linus Pauling proposed an electronegativity scale, which depends on bond energies, as a development of valence bond theory. It has been shown to correlate with a number of other chemical properties. Electronegativity can not be directly measured and must be calculated from other atomic or molecular properties. Several methods of calculation have been proposed, and although there may be small differences in the numerical values of the electronegativity, all methods show the same periodic trends between elements. The most commonly used method of calculation is that originally proposed by Linus Pauling. This gives a dimensionless quantity, commonly referred to as the Pauling scale ( χ ), on a relative scale running from around 0.7 to 3.98 ( hydrogen = 2.20 ). When other methods of calculation are used, it is conventional ( although not obligatory ) to quote the results on a scale that covers the same range of numerical values : this is known as an electronegativity in Pauling units. As it is usually calculated, electronegativity is not a property of an atom alone, but rather a property of an atom in a molecule. Properties of a free atom include ionization energy and electron affinity. It is to be expected that the electronegativity of an element will vary with its chemical environment, but it is usually considered to be a transferable property, that is to say that similar values will be valid in a variety of situations. On the most basic level, electronegativity is determined by factors like the nuclear charge ( the more protons an atom has, the more `` pull '' it will have on electrons ) and the number / location of other electrons present in the atomic shells ( the more electrons an atom has, the farther from the nucleus the valence electrons will be, and as a result the less positive charge they will experience -- both because of their increased distance from the nucleus, and because the other electrons in the lower energy core orbitals will act to shield the valence electrons from the positively charged nucleus ). The opposite of electronegativity is electropositivity : a measure of an element 's ability to donate electrons. Caesium is the least electronegative element in the periodic table ( = 0.79 ), while fluorine is most electronegative ( = 3.98 ). Francium and caesium were originally both assigned 0.7 ; caesium 's value was later refined to 0.79, but no experimental data allows a similar refinement for francium. However, francium 's ionization energy is known to be slightly higher than caesium 's, in accordance with the relativistic stabilization of the 7s orbital, and this in turn implies that francium is in fact more electronegative than caesium. Contents 1 Electronegativities of the elements 2 Methods of calculation 2.1 Pauling electronegativity 2.2 Mulliken electronegativity 2.3 Allred -- Rochow electronegativity 2.4 Sanderson electronegativity equalization 2.5 Allen electronegativity 3 Correlation of electronegativity with other properties 4 Trends in electronegativity 4.1 Periodic trends 4.2 Variation of electronegativity with oxidation number 5 Group electronegativity 6 Electropositivity 7 See also 8 References 9 Bibliography 10 External links Electronegativities of the elements Periodic table of electronegativity by Pauling scale → Atomic radius decreases → Ionization energy increases → Electronegativity increases → 5 6 7 8 9 10 11 12 13 14 15 16 17 18 Group → ↓ Period 2.20 He Li 0.98 Be 1.57 2.04 2.55 3.04 O 3.44 3.98 Ne Na 0.93 Mg 1.31 Al 1.61 Si 1.90 2.19 2.58 Cl 3.16 Ar 0.82 Ca 1.00 Sc 1.36 Ti 1.54 V 1.63 Cr 1.66 Mn 1.55 Fe 1.83 Co 1.88 Ni 1.91 Cu 1.90 Zn 1.65 Ga 1.81 Ge 2.01 As 2.18 Se 2.55 Br 2.96 Kr 3.00 5 Rb 0.82 Sr 0.95 Y 1.22 Zr 1.33 Nb 1.6 Mo 2.16 Tc 1.9 Ru 2.2 Rh 2.28 Pd 2.20 Ag 1.93 Cd 1.69 In 1.78 Sn 1.96 Sb 2.05 Te 2.1 2.66 Xe 2.60 6 Cs 0.79 Ba 0.89 La 1.1 Hf 1.3 Ta 1.5 2.36 Re 1.9 Os 2.2 Ir 2.20 Pt 2.28 Au 2.54 Hg 2.00 Tl 1.62 Pb 1.87 Bi 2.02 Po 2.0 At 2.2 Rn 2.2 7 Fr 0.7 Ra 0.9 Ac 1.1 Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og Ce 1.12 Pr 1.13 Nd 1.14 Pm 1.13 Sm 1.17 Eu 1.2 Gd 1.2 Tb 1.1 Dy 1.22 Ho 1.23 Er 1.24 Tm 1.25 Yb 1.1 Lu 1.27 Th 1.3 Pa 1.5 U 1.38 Np 1.36 Pu 1.28 Am 1.13 Cm 1.28 Bk 1.3 Cf 1.3 Es 1.3 Fm 1.3 Md 1.3 No 1.3 Lr 1.3 Values are given for the elements in their most common and stable oxidation states. See also : Electronegativities of the elements ( data page ) Jump up ^ Electronegativity of francium was chosen by Pauling as 0.7, close to that of caesium ( also assessed 0.7 at that point ). The base value of hydrogen was later increased by 0.10 and caesium 's electronegativity was later refined to 0.79 ; however, no refinements have been made for francium as no experiment has been conducted and the old value was kept. However, francium is expected and, to a small extent, observed to be more electronegative than caesium. See francium for details. Jump up ^ See Brown, Geoffrey ( 2012 ). The Inaccessible Earth : An integrated view to its structure and composition. Springer Science & Business Media. p. 88. ISBN 9789401115162. Methods of calculation Pauling electronegativity Pauling first proposed the concept of electronegativity in 1932 as an explanation of the fact that the covalent bond between two different atoms ( A -- B ) is stronger than would be expected by taking the average of the strengths of the A -- A and B -- B bonds. According to valence bond theory, of which Pauling was a notable proponent, this `` additional stabilization '' of the heteronuclear bond is due to the contribution of ionic canonical forms to the bonding. The difference in electronegativity between atoms A and B is given by : χ A − χ B = ( e V ) − 1 / 2 E d ( A B ) − ( E d ( A A ) + E d ( B B ) ) / 2 ( displaystyle chi _ ( \rm ( A ) ) - chi _ ( \rm ( B ) ) = ( ( \rm ( eV ) ) ) ^ ( - 1 / 2 ) ( sqrt ( E_ ( \rm ( d ) ) ( ( \rm ( AB ) ) ) - ( E_ ( \rm ( d ) ) ( ( \rm ( AA ) ) ) + E_ ( \rm ( d ) ) ( ( \rm ( BB ) ) ) ) / 2 ) ) ) where the dissociation energies, E, of the A -- B, A -- A and B -- B bonds are expressed in electronvolts, the factor ( eV ) being included to ensure a dimensionless result. Hence, the difference in Pauling electronegativity between hydrogen and bromine is 0.73 ( dissociation energies : H -- Br, 3.79 eV ; H -- H, 4.52 eV ; Br -- Br 2.00 eV ) As only differences in electronegativity are defined, it is necessary to choose an arbitrary reference point in order to construct a scale. Hydrogen was chosen as the reference, as it forms covalent bonds with a large variety of elements : its electronegativity was fixed first at 2.1, later revised to 2.20. It is also necessary to decide which of the two elements is the more electronegative ( equivalent to choosing one of the two possible signs for the square root ). This is usually done using `` chemical intuition '' : in the above example, hydrogen bromide dissolves in water to form H and Br ions, so it may be assumed that bromine is more electronegative than hydrogen. However, in principle, since the same electronegativities should be obtained for any two bonding compounds, the data are in fact overdetermined, and the signs are unique once a reference point is fixed ( usually, for H or F ). To calculate Pauling electronegativity for an element, it is necessary to have data on the dissociation energies of at least two types of covalent bond formed by that element. A.L. Allred updated Pauling 's original values in 1961 to take account of the greater availability of thermodynamic data, and it is these `` revised Pauling '' values of the electronegativity that are most often used. The essential point of Pauling electronegativity is that there is an underlying, quite accurate, semi-empirical formula for dissociation energies, namely : E d ( A B ) = ( E d ( A A ) + E d ( B B ) ) / 2 + ( χ A − χ B ) 2 e V ( displaystyle E_ ( \rm ( d ) ) ( ( \rm ( AB ) ) ) = ( E_ ( \rm ( d ) ) ( ( \rm ( AA ) ) ) + E_ ( \rm ( d ) ) ( ( \rm ( BB ) ) ) ) / 2 + ( chi _ ( \rm ( A ) ) - chi _ ( \rm ( B ) ) ) ^ ( 2 ) eV ) or sometimes, a more accurate fit E d ( A B ) = E d ( A A ) E d ( B B ) + 1.3 ( χ A − χ B ) 2 e V ( displaystyle E_ ( \rm ( d ) ) ( ( \rm ( AB ) ) ) = ( sqrt ( E_ ( \rm ( d ) ) ( ( \rm ( AA ) ) ) E_ ( \rm ( d ) ) ( ( \rm ( BB ) ) ) ) ) + 1.3 ( chi _ ( \rm ( A ) ) - chi _ ( \rm ( B ) ) ) ^ ( 2 ) eV ) This is an approximate equation, but holds with good accuracy. Pauling obtained it by noting that a bond can be approximately represented as a quantum mechanical superposition of a covalent bond and two ionic bond - states. The covalent energy of a bond is approximately, by quantum mechanical calculations, the geometric mean of the two energies of covalent bonds of the same molecules, and there is an additional energy that comes from ionic factors, i.e. polar character of the bond. The geometric mean is approximately equal to the arithmetic mean - which is applied in the first formula above - when the energies are of the similar value, e.g., except for the highly electropositive elements, where there is a larger difference of two dissociation energies ; the geometric mean is more accurate and almost always gives a positive excess energy, due to ionic bonding. The square root of this excess energy, Pauling notes, is approximately additive, and hence one can introduce the electronegativity. Thus, it is this semi-empirical formula for bond energy that underlies Pauling electronegativity concept. The formulas are approximate, but this rough approximation is in fact relatively good and gives the right intuition, with the notion of polarity of the bond and some theoretical grounding in quantum mechanics. The electronegativities are then determined to best fit the data. In more complex compounds, there is additional error since electronegativity depends on the molecular environment of an atom. Also, the energy estimate can be only used for single, not for multiple bonds. The energy of formation of a molecule containing only single bonds then can be approximated from an electronegativity table, and depends on the constituents and sum of squares of differences of electronegativities of all pairs of bonded atoms. Such a formula for estimating energy typically has relative error of order of 10 %, but can be used to get a rough qualitative idea and understanding of a molecule. Mulliken electronegativity The correlation between Mulliken electronegativities ( x-axis, in kJ / mol ) and Pauling electronegativities ( y - axis ). Robert S. Mulliken proposed that the arithmetic mean of the first ionization energy ( E ) and the electron affinity ( E ) should be a measure of the tendency of an atom to attract electrons. As this definition is not dependent on an arbitrary relative scale, it has also been termed absolute electronegativity, with the units of kilojoules per mole or electronvolts. χ = ( E i + E e a ) / 2 ( displaystyle chi = ( E_ ( \rm ( i ) ) + E_ ( \rm ( ea ) ) ) / 2 , ) However, it is more usual to use a linear transformation to transform these absolute values into values that resemble the more familiar Pauling values. For ionization energies and electron affinities in electronvolts, χ = 0.187 ( E i + E e a ) + 0.17 ( displaystyle chi = 0.187 ( E_ ( \rm ( i ) ) + E_ ( \rm ( ea ) ) ) + 0.17 , ) and for energies in kilojoules per mole, χ = ( 1.97 × 10 − 3 ) ( E i + E e a ) + 0.19. ( displaystyle chi = ( 1.97 \times 10 ^ ( - 3 ) ) ( E_ ( \rm ( i ) ) + E_ ( \rm ( ea ) ) ) + 0.19. ) The Mulliken electronegativity can only be calculated for an element for which the electron affinity is known, fifty - seven elements as of 2006. The Mulliken electronegativity of an atom is sometimes said to be the negative of the chemical potential. By inserting the energetic definitions of the ionization potential and electron affinity into the Mulliken electronegativity, it is possible to show that the Mulliken chemical potential is a finite difference approximation of the electronic energy with respect to the number of electrons., i.e., μ ( M u l l i k e n ) = − χ ( M u l l i k e n ) = − ( E i + E e a ) / 2 ( displaystyle mu ( ( \rm ( Mulliken ) = - chi ( ( \rm ( Mulliken ) = - ( E_ ( \rm ( i ) ) + E_ ( \rm ( ea ) ) ) / 2 , ) ) ) ) ) Allred -- Rochow electronegativity The correlation between Allred -- Rochow electronegativities ( x-axis, in Å ) and Pauling electronegativities ( y - axis ). A. Louis Allred and Eugene G. Rochow considered that electronegativity should be related to the charge experienced by an electron on the `` surface '' of an atom : The higher the charge per unit area of atomic surface the greater the tendency of that atom to attract electrons. The effective nuclear charge, Z, experienced by valence electrons can be estimated using Slater 's rules, while the surface area of an atom in a molecule can be taken to be proportional to the square of the covalent radius, r. When r is expressed in picometres, χ = 3590 Z e f f r c o v 2 + 0.744 ( displaystyle chi = 3590 ( ( Z_ ( \rm ( eff ) ) ) over ( r_ ( \rm ( cov ) ) ^ ( 2 ) ) ) + 0.744 ) Sanderson electronegativity equalization The correlation between Sanderson electronegativities ( x-axis, arbitrary units ) and Pauling electronegativities ( y - axis ). R.T. Sanderson has also noted the relationship between Mulliken electronegativity and atomic size, and has proposed a method of calculation based on the reciprocal of the atomic volume. With a knowledge of bond lengths, Sanderson 's model allows the estimation of bond energies in a wide range of compounds. Sanderson 's model has also been used to calculate molecular geometry, s - electrons energy, NMR spin - spin constants and other parameters for organic compounds. This work underlies the concept of electronegativity equalization, which suggests that electrons distribute themselves around a molecule to minimize or to equalize the Mulliken electronegativity. This behavior is analogous to the equalization of chemical potential in macroscopic thermodynamics. Allen electronegativity The correlation between Allen electronegativities ( x-axis, in kJ / mol ) and Pauling electronegativities ( y - axis ). Perhaps the simplest definition of electronegativity is that of Leland C. Allen, who has proposed that it is related to the average energy of the valence electrons in a free atom,,, χ = n s ε s + n p ε p n s + n p ( displaystyle chi = ( n_ ( \rm ( s ) ) \varepsilon _ ( \rm ( s ) ) + n_ ( \rm ( p ) ) \varepsilon _ ( \rm ( p ) ) over n_ ( \rm ( s ) ) + n_ ( \rm ( p ) ) ) ) where ε are the one - electron energies of s - and p - electrons in the free atom and n are the number of s - and p - electrons in the valence shell. It is usual to apply a scaling factor, 1.75 × 10 for energies expressed in kilojoules per mole or 0.169 for energies measured in electronvolts, to give values that are numerically similar to Pauling electronegativities. The one - electron energies can be determined directly from spectroscopic data, and so electronegativities calculated by this method are sometimes referred to as spectroscopic electronegativities. The necessary data are available for almost all elements, and this method allows the estimation of electronegativities for elements that can not be treated by the other methods, e.g. francium, which has an Allen electronegativity of 0.67. However, it is not clear what should be considered to be valence electrons for the d - and f - block elements, which leads to an ambiguity for their electronegativities calculated by the Allen method. In this scale neon has the highest electronegativity of all elements, followed by fluorine, helium, and oxygen. Electronegativity using the Allen scale Group → 5 6 7 8 9 10 11 12 13 14 15 16 17 18 ↓ Period 2.300 He 4.160 Li 0.912 Be 1.576 2.051 2.544 3.066 O 3.610 4.193 Ne 4.787 Na 0.869 Mg 1.293 Al 1.613 Si 1.916 2.253 2.589 Cl 2.869 Ar 3.242 0.734 Ca 1.034 Sc 1.19 Ti 1.38 V 1.53 Cr 1.65 Mn 1.75 Fe 1.80 Co 1.84 Ni 1.88 Cu 1.85 Zn 1.59 Ga 1.756 Ge 1.994 As 2.211 Se 2.424 Br 2.685 Kr 2.966 5 Rb 0.706 Sr 0.963 Y 1.12 Zr 1.32 Nb 1.41 Mo 1.47 Tc 1.51 Ru 1.54 Rh 1.56 Pd 1.58 Ag 1.87 Cd 1.52 In 1.656 Sn 1.824 Sb 1.984 Te 2.158 2.359 Xe 2.582 6 Cs 0.659 Ba 0.881 Lu 1.09 Hf 1.16 Ta 1.34 1.47 Re 1.60 Os 1.65 Ir 1.68 Pt 1.72 Au 1.92 Hg 1.76 Tl 1.789 Pb 1.854 Bi 2.01 Po 2.19 At 2.39 Rn 2.60 7 Fr 0.67 Ra 0.89 See also : Electronegativities of the elements ( data page ) Correlation of electronegativity with other properties The variation of the isomer shift ( y - axis, in mm / s ) of ( SnX ) anions, as measured by Sn Mössbauer spectroscopy, against the sum of the Pauling electronegativities of the halide substituents ( x-axis ). The wide variety of methods of calculation of electronegativities, which all give results that correlate well with one another, is one indication of the number of chemical properties which might be affected by electronegativity. The most obvious application of electronegativities is in the discussion of bond polarity, for which the concept was introduced by Pauling. In general, the greater the difference in electronegativity between two atoms the more polar the bond that will be formed between them, with the atom having the higher electronegativity being at the negative end of the dipole. Pauling proposed an equation to relate `` ionic character '' of a bond to the difference in electronegativity of the two atoms, although this has fallen somewhat into disuse. Several correlations have been shown between infrared stretching frequencies of certain bonds and the electronegativities of the atoms involved : however, this is not surprising as such stretching frequencies depend in part on bond strength, which enters into the calculation of Pauling electronegativities. More convincing are the correlations between electronegativity and chemical shifts in NMR spectroscopy or isomer shifts in Mössbauer spectroscopy ( see figure ). Both these measurements depend on the s - electron density at the nucleus, and so are a good indication that the different measures of electronegativity really are describing `` the ability of an atom in a molecule to attract electrons to itself ''. Trends in electronegativity Periodic trends The variation of Pauling electronegativity ( y - axis ) as one descends the main groups of the periodic table from the second period to the sixth period In general, electronegativity increases on passing from left to right along a period, and decreases on descending a group. Hence, fluorine is the most electronegative of the elements ( not counting noble gases ), whereas caesium is the least electronegative, at least of those elements for which substantial data is available. This would lead one to believe that caesium fluoride is the compound whose bonding features the most ionic character. There are some exceptions to this general rule. Gallium and germanium have higher electronegativities than aluminium and silicon, respectively, because of the d - block contraction. Elements of the fourth period immediately after the first row of the transition metals have unusually small atomic radii because the 3d - electrons are not effective at shielding the increased nuclear charge, and smaller atomic size correlates with higher electronegativity ( see Allred - Rochow electronegativity, Sanderson electronegativity above ). The anomalously high electronegativity of lead, in particular when compared to thallium and bismuth, appears to be an artifact of data selection ( and data availability ) -- methods of calculation other than the Pauling method show the normal periodic trends for these elements. Variation of electronegativity with oxidation number In inorganic chemistry it is common to consider a single value of the electronegativity to be valid for most `` normal '' situations. While this approach has the advantage of simplicity, it is clear that the electronegativity of an element is not an invariable atomic property and, in particular, increases with the oxidation state of the element. Allred used the Pauling method to calculate separate electronegativities for different oxidation states of the handful of elements ( including tin and lead ) for which sufficient data was available. However, for most elements, there are not enough different covalent compounds for which bond dissociation energies are known to make this approach feasible. This is particularly true of the transition elements, where quoted electronegativity values are usually, of necessity, averages over several different oxidation states and where trends in electronegativity are harder to see as a result. Acid Formula Chlorine oxidation state pK Hypochlorous acid HClO + 1 + 7.5 Chlorous acid HClO + 3 + 2.0 Chloric acid HClO + 5 -- 1.0 Perchloric acid HClO + 7 -- 10 The chemical effects of this increase in electronegativity can be seen both in the structures of oxides and halides and in the acidity of oxides and oxoacids. Hence CrO and Mn O are acidic oxides with low melting points, while Cr O is amphoteric and Mn O is a completely basic oxide. The effect can also be clearly seen in the dissociation constants of the oxoacids of chlorine. The effect is much larger than could be explained by the negative charge being shared among a larger number of oxygen atoms, which would lead to a difference in pK of log ( ⁄ ) = -- 0.6 between hypochlorous acid and perchloric acid. As the oxidation state of the central chlorine atom increases, more electron density is drawn from the oxygen atoms onto the chlorine, reducing the partial negative charge on the oxygen atoms and increasing the acidity. Group electronegativity In organic chemistry, electronegativity is associated more with different functional groups than with individual atoms. The terms group electronegativity and substituent electronegativity are used synonymously. However, it is common to distinguish between the inductive effect and the resonance effect, which might be described as σ - and π - electronegativities, respectively. There are a number of linear free - energy relationships that have been used to quantify these effects, of which the Hammett equation is the best known. Kabachnik parameters are group electronegativities for use in organophosphorus chemistry. Electropositivity Electropositivity is a measure of an element 's ability to donate electrons, and therefore form positive ions ; thus, it is opposed to electronegativity. Mainly, this is an attribute of metals, meaning that, in general, the greater the metallic character of an element the greater the electropositivity. Therefore, the alkali metals are most electropositive of all. This is because they have a single electron in their outer shell and, as this is relatively far from the nucleus of the atom, it is easily lost ; in other words, these metals have low ionization energies. While electronegativity increases along periods in the periodic table, and decreases down groups, electropositivity decreases along periods ( from left to right ) and increases down groups. See also Electronegativities of the elements ( data page ) Chemical polarity References ^ Jump up to : IUPAC, Compendium of Chemical Terminology, 2nd ed. ( the `` Gold Book '' ) ( 1997 ). Online corrected version : ( 2006 -- ) `` Electronegativity ''. ^ Jump up to : Jensen, W.B. ( 1996 ). `` Electronegativity from Avogadro to Pauling : Part 1 : Origins of the Electronegativity Concept ''. Journal of Chemical Education. 73 ( 1 ) : 11 -- 20. Bibcode : 1996JChEd... 73... 11J. doi : 10.1021 / ed073p11. ^ Jump up to : Pauling, L. ( 1932 ). `` The Nature of the Chemical Bond. IV. The Energy of Single Bonds and the Relative Electronegativity of Atoms ''. Journal of the American Chemical Society. 54 ( 9 ) : 3570 -- 3582. Bibcode : 1932JAChS... 54.2610 C. doi : 10.1021 / ja01348a011. ^ Jump up to : Pauling, Linus ( 1960 ). Nature of the Chemical Bond. Cornell University Press. pp. 88 -- 107. ISBN 0 - 8014 - 0333 - 2. Jump up ^ Greenwood, N.N. ; Earnshaw, A. ( 1984 ). Chemistry of the Elements. Pergamon. p. 30. ISBN 0 - 08 - 022057 - 6. Jump up ^ More details and sources for this point can be found in the article on francium. ^ Jump up to : Allred, A.L. ( 1961 ). `` Electronegativity values from thermochemical data ''. Journal of Inorganic and Nuclear Chemistry. 17 ( 3 -- 4 ) : 215 -- 221. doi : 10.1016 / 0022 - 1902 ( 61 ) 80142 - 5. Jump up ^ Mulliken, R.S. ( 1934 ). `` A New Electroaffinity Scale ; Together with Data on Valence States and on Valence Ionization Potentials and Electron Affinities ''. Journal of Chemical Physics. 2 ( 11 ) : 782 -- 793. Bibcode : 1934JChPh... 2... 782M. doi : 10.1063 / 1.1749394. Jump up ^ Mulliken, R.S. ( 1935 ). `` Electronic Structures of Molecules XI. Electroaffinity, Molecular Orbitals and Dipole Moments ''. J. Chem. Phys. 3 ( 9 ) : 573 -- 585. Bibcode : 1935JChPh... 3... 573M. doi : 10.1063 / 1.1749731. Jump up ^ Pearson, R.G. ( 1985 ). `` Absolute electronegativity and absolute hardness of Lewis acids and bases ''. J. Am. Chem. Soc. 107 ( 24 ) : 6801 -- 6806. doi : 10.1021 / ja00310a009. Jump up ^ Huheey, J.E. ( 1978 ). Inorganic Chemistry ( 2nd Edn. ). New York : Harper & Row. p. 167. Jump up ^ This second relation has been recalculated using the best values of the first ionization energies and electron affinities available in 2006. Jump up ^ Allred, A.L. ; Rochow, E.G. ( 1958 ). `` A scale of electronegativity based on electrostatic force ''. Journal of Inorganic and Nuclear Chemistry. 5 ( 4 ) : 264 -- 268. doi : 10.1016 / 0022 - 1902 ( 58 ) 80003 - 2. Jump up ^ Housecroft C.E. and Sharpe A.G. Inorganic Chemistry ( 2nd ed., Pearson Prentice - Hall 2005 ) p. 38 Jump up ^ Sanderson, R.T. ( 1983 ). `` Electronegativity and bond energy ''. Journal of the American Chemical Society. 105 ( 8 ) : 2259 -- 2261. doi : 10.1021 / ja00346a026. Jump up ^ Sanderson, R.T. ( 1983 ). Polar Covalence. New York : Academic Press. ISBN 0 - 12 - 618080 - 6. Jump up ^ Zefirov, N.S. ; M.A. Kirpichenok ; F.F. Izmailov ; M.I. Trofimov ( 1987 ). Doklady Akademii Nauk SSSR. 296 : 883. Missing or empty title = ( help ) Jump up ^ Trofimov, M.I. ; Smolenskii, E.A. ( 2005 ). `` Application of the electronegativity indices of organic molecules to tasks of chemical informatics ''. Russian Chemical Bulletin. 54 ( 9 ) : 2235 -- 2246. doi : 10.1007 / s11172 - 006 - 0105 - 6. Jump up ^ SW Rick ; SJ Stuart ( 2002 ). `` Electronegativity equalization models ''. In Kenny B. Lipkowitz ; Donald B. Boyd. Reviews in computational chemistry. Wiley. p. 106. ISBN 0 - 471 - 21576 - 7. Jump up ^ Robert G. Parr ; Weitao Yang ( 1994 ). Density - functional theory of atoms and molecules. Oxford University Press. p. 91. ISBN 0 - 19 - 509276 - 7. Jump up ^ Allen, Leland C. ( 1989 ). `` Electronegativity is the average one - electron energy of the valence - shell electrons in ground - state free atoms ''. Journal of the American Chemical Society. 111 ( 25 ) : 9003 -- 9014. doi : 10.1021 / ja00207a003. Jump up ^ Mann, Joseph B., Meek, Terry L., Allen, Leland C. ( 2000 ). `` Configuration Energies of the Main Group Elements ''. Journal of the American Chemical Society. 122 ( 12 ) : 2780 -- 2783. doi : 10.1021 / ja992866e. CS1 maint : Multiple names : authors list ( link ) Jump up ^ Mann, Joseph B., Meek, Terry L., Knight, Eugene T., Capitani, Joseph F., Allen, Leland C. ( 2000 ). `` Configuration energies of the d - block elements ''. Journal of the American Chemical Society. 122 ( 21 ) : 5132 -- 5137. doi : 10.1021 / ja9928677. CS1 maint : Multiple names : authors list ( link ) ^ Jump up to : The widely quoted Pauling electronegativity of 0.7 for francium is an extrapolated value of uncertain provenance. The Allen electronegativity of caesium is 0.66. Jump up ^ See, e.g., Bellamy, L.J. ( 1958 ). The Infra - Red Spectra of Complex Molecules. New York : Wiley. p. 392. ISBN 0 - 412 - 13850 - 6. Jump up ^ Spieseke, H. ; Schneider, W.G. ( 1961 ). `` Effect of Electronegativity and Magnetic Anisotropy of Substituents on C13 and H1 Chemical Shifts in CH3X and CH3CH2X Compounds ''. Journal of Chemical Physics. 35 ( 2 ) : 722. Bibcode : 1961JChPh... 35... 722S. doi : 10.1063 / 1.1731992. Jump up ^ Clasen, C.A. ; Good, M.L. ( 1970 ). `` Interpretation of the Moessbauer spectra of mixed - hexahalo complexes of tin ( IV ) ''. Inorganic Chemistry. 9 ( 4 ) : 817 -- 820. doi : 10.1021 / ic50086a025. Jump up ^ `` Electropositivity, '' Microsoft Encarta Online Encyclopedia 2009. ( Archived 2009 - 10 - 31 ). Bibliography Jolly, William L. ( 1991 ). Modern Inorganic Chemistry ( 2nd ed. ). New York : McGraw - Hill. pp. 71 -- 76. ISBN 0 - 07 - 112651 - 1. Mullay, J. ( 1987 ). `` Estimation of atomic and group electronegativities ''. Structure and Bonding. Structure and Bonding. 66 : 1 -- 25. ISBN 3 - 540 - 17740 - X. doi : 10.1007 / BFb0029834. External links Wikimedia Commons has media related to Electronegativity. WebElements, lists values of electronegativities by a number of different methods of calculation Video explaining electronegativity Periodic table Periodic table forms Standard 18 - column 18 - column, large cells 32 - column, large cells Alternative Alternatives Chemical Galaxy Janet 's left step table Extended Extension beyond the 7th period Fricke model large cells Pyykkö model Sets of elements By periodic table structure Groups 1 ( Alkali metals ) 2 ( Alkaline earth metals ) 5 6 7 8 9 10 11 12 13 14 15 ( Pnictogens ) 16 ( Chalcogens ) 17 ( Halogens ) 18 ( Noble gases ) Periods 5 6 7 8 + Aufbau Fricke Pyykkö Blocks s - block p - block d - block f - block g - block Aufbau principle By metallicity Metals Alkali metals Alkaline earth metals Lanthanides Actinides Superactinides Eka - superactinides Transition metals Post-transition metals Metalloids Lists of metalloids by source Dividing line Nonmetals Polyatomic nonmetals Diatomic nonmetals Noble gases Other sets Nutritional elements Platinum - group metals ( PGM ) Rare - earth elements Refractory metals Precious metals Coinage metals Noble metal Heavy metals Native metals Transuranium elements Transactinide elements Major actinides Minor actinides Elements Lists By : Abundance ( in humans ) Atomic properties Nuclear stability Production Symbol Properties Atomic weight Crystal structure Electron affinity Electron configuration Electronegativity Allen Pauling Goldschmidt classification Maximum valence Data pages Abundance Atomic radius Boiling point Critical point Density Elasticity Electrical resistivity Electron affinity Electron configuration Electronegativity Hardness Heat capacity Heat of fusion Heat of vaporization Ionization energy Melting point Oxidation state Speed of sound Thermal conductivity Thermal expansion coefficient Vapor pressure History Element discoveries Mendeleev 's predictions Naming Etymology controversies places scientists in East Asia See also IUPAC nomenclature systematic element name Trivial name Dmitri Mendeleev Book Chemistry Portal Retrieved from `` https://en.wikipedia.org/w/index.php?title=Electronegativity&oldid=796630568 '' Categories : Chemical properties Chemical bonding Dimensionless numbers of chemistry Hidden categories : Pages with citations lacking titles CS1 maint : Multiple names : authors list Talk Contents About Wikipedia Wikibooks Wikiquote Afrikaans Aragonés Asturianu বাংলা Беларуская Български Bosanski Català Čeština Cymraeg Dansk Deutsch Dolnoserbski Eesti Ελληνικά Español Esperanto Estremeñu Euskara فارسی Français Gaeilge Galego 한국어 हिन्दी Hrvatski Bahasa Indonesia Italiano עברית ಕನ್ನಡ ქართული Қазақша Kreyòl ayisyen Latviešu Lietuvių Lumbaart Magyar Македонски മലയാളം Bahasa Melayu Монгол Nederlands 日本 語 Norsk Norsk nynorsk Occitan Oʻzbekcha / ўзбекча پنجابی Plattdüütsch Polski Português Română Русский Scots Simple English Slovenčina Slovenščina Српски / srpski Srpskohrvatski / српскохрватски Suomi Svenska தமிழ் ไทย Türkçe Українська اردو Tiếng Việt Winaray 吴语 粵語 中文 Edit links This page was last edited on 22 August 2017, at 04 : 04. 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Question: the ability of an atom to attract electron towards itself is called
Answer: Electronegativity