visual representation for electronegativity

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L.C. Allen suggests that electronegativity is the average one-electron energy of the valence shell electrons in the ground state free atoms. This means that values of the Allen electronegativity can be calculated from spectroscopic data. The values obtained correlate well with Pauling electronegativity and with Allred-Rochow electronegativity. The Allen electronegativity is given the symbol Χ spec .

Pauling scale

The Allen electronegativity is given the symbol Χ spec . For the s - and p -block elements, then:

Χ spec = (mε s + nε p )/(m + n)

• m = number of s -electrons
• n = number of p -electrons
• ε p = p ionization energy
• ε s = s ionization energy
• Electronegativity (Allred-Rochow)
• Electronegativity (Pauling)
• Electronegativity (Mulliken-Jaffe)
• Electronegativity (Mulliken-Jaffe) p-orbital
• Electronegativity (Mulliken-Jaffe - s)
• Electronegativity (Mulliken-Jaffe - sp)
• Electronegativity (Mulliken-Jaffe -sp 2 )
• Electronegativity (Mulliken-Jaffe -sp 3 )
• Electronegativity (Sanderson)

Literature sources

• L.C. Allen, J. Am. Chem. Soc. , 1989, 111 , 9003.
• J.E. Huheey, E.A. Keiter, and R.L. Keiter in Inorganic Chemistry : Principles of Structure and Reactivity , 4th edition, HarperCollins, New York, USA, 1993.

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Electronegativity Definition and Trend

Electronegativity is a measure of how easily an atom attracts a pair of electrons to form a chemical bond. A high electronegativity value means an atom readily attracts electrons to form a chemical bond with another atom. A low electronegativity value means an atom readily donates electrons to form a bond or is electropositive .

While there are charts of electronegativity values for elements of the periodic table, there is no true single electronegativity value for an atom. Rather, it depends on the other atoms in a molecule and also depends on the nuclear charge and number of electrons. The most common method of calculating electronegativity is the Pauling scale , which was proposed by Linus Pauling. The Pauling scale runs from 0.79 to 3.98. The Pauling scale is dimensionless, but sometimes the values are cited in Pauling units .

Most Electronegative and Most Electropositive Elements

The most electronegative element is fluorine , with an electronegativity value of 3.98 on the Pauling scale. The least electronegative or most electropositive element is cesium, which has a value of 0.79. However, francium is probably even more electropositive than cesium because it has a higher ionization energy. Francium’s electronegativity value is estimated to be around 0.79, but it has not been measured empirically.

Electronegativity and Chemical Bonding

Comparing electronegativity values allows prediction of the type of chemical bond two atoms will form. Atoms with the same electronegativity values (e.g., H 2 , N 2 ) form covalent bonds. Atoms with slightly different electronegativity values (e.g., CO, H 2 O) form polar covalent bonds. All hydrogen halides (e.g., HCl, HF) form polar covalent bonds. Atoms with very different electronegativity values (e.g., NaCl) form ionic bonds. Note that electronegativity does not help in predicting whether or not a chemical bond will actually form. Argon has a high electronegativity value, yet it’s a noble gas that forms few chemical bonds.

Electronegativity Periodic Table Trend

Electronegativity follows a trend ( periodicity ) on the periodic table. The trend is shown in the graphic (which is also available as a PDF for printing ).

• Electronegativity increases moving left to right across a period, from the alkali metals to the halogens . The noble gases are an exception to the trend.
• Electronegativity decreases moving down a periodic table group. This is because the distance between the nucleus and the valence electrons increase.
• Electronegativity follows the same general trend as ionization energy . Elements with low electronegativities tend to have low ionization energies. Similarly, an atom with a high electronegativity tends to have a high ionization energy.
• Jensen, William B. (January 1, 1996). “Electronegativity from Avogadro to Pauling: Part 1: Origins of the Electronegativity Concept.” J. Chem. Educ . 73, 1. 11, ACS Publications.
• Mullay, J. (1987). Estimation of atomic and group electronegativities. Structure and Bonding . 66. pp. 1–25. doi:10.1007/BFb0029834. ISBN 978-3-540-17740-1.
• Pauling, Linus (September 1, 1932). “The Nature of the Chemical Bond. IV. The Energy of Single Bonds and the Relative Electronegativity of Atoms.” J. Am. Chem. Soc . 54, 9, 3570-3582. ACS Publications.
• Pauling, Linus (January 31, 1960). The Nature of the Chemical Bond and the Structure of Molecules and Crystals: An Introduction to Mode (3rd ed.). Cornell University Press.

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What Is Electronegativity and How Does It Work?

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Electronegativity is the property of an atom which increases with its tendency to attract the electrons of a bond. If two bonded atoms have the same electronegativity values as each other, they share electrons equally in a covalent bond. Usually, the electrons in a chemical bond are more attracted to one atom (the more electronegative one) than to the other. This results in a polar covalent bond. If the electronegativity values are very different, the electrons aren't shared at all. One atom essentially takes the bond electrons from the other atom, forming an ionic bond.

Key Takeaways: Electronegativity

• Electronegativity is an atom's tendency to attract electrons to itself in a chemical bond.
• The most electronegative element is fluorine. The least electronegative or most electropositive element is francium.
• The greater the difference between atom electronegativity values, the more polar the chemical bond formed between them.

Avogadro and other chemists studied electronegativity before it was formally named by Jöns Jacob Berzelius in 1811. In 1932, Linus Pauling proposed an electronegativity scale based on bond energies. Electronegativity values on the Pauling scale are dimensionless numbers that run from about 0.7 to 3.98. The Pauling scale values are relative to the electronegativity of hydrogen (2.20). While the Pauling scale is most often used, other scales include the Mulliken scale, Allred-Rochow scale, Allen scale, and Sanderson scale.

Electronegativity is a property of an atom within a molecule, rather than an inherent property of an atom by itself. Thus, electronegativity actually varies depending on an atom's environment. However, most of the time an atom displays similar behavior in different situations. Factors that affect electronegativity include the nuclear charge and the number and location of electrons in an atom.

Electronegativity Example

The chlorine atom has a higher electronegativity than the hydrogen atom, so the bonding electrons will be closer to the Cl than to the H in the HCl molecule.

In the O 2 molecule, both atoms have the same electronegativity. The electrons in the covalent bond are shared equally between the two oxygen atoms.

Most and Least Electronegative Elements

The most electronegative element on the periodic table is fluorine (3.98). The least electronegative element is cesium (0.79). The opposite of electronegativity is electropositivity, so you could simply say cesium is the most electropositive element. Note that older texts list both francium and cesium as least electronegative at 0.7, but the value for cesium was experimentally revised to the 0.79 value. There is no experimental data for francium, but its ionization energy is higher than that of cesium, so it is expected that francium is slightly more electronegative.

Electronegativity as a Periodic Table Trend

Like electron affinity, atomic/ionic radius, and ionization energy, electronegativity shows a definite trend on the periodic table .

• Electronegativity generally increases moving from left to right across a period. The noble gases tend to be exceptions to this trend.
• Electronegativity generally decreases moving down a periodic table group. This correlates with the increased distance between the nucleus and the valence electron.

Electronegativity and ionization energy follow the same periodic table trend. Elements that have low ionization energies tend to have low electronegativities. The nuclei of these atoms don't exert a strong pull on electrons . Similarly, elements that have high ionization energies tend to have high electronegativity values. The atomic nucleus exerts a strong pull on electrons.

Jensen, William B. "Electronegativity from Avogadro to Pauling: Part 1: Origins of the Electronegativity Concept." 1996, 73, 1. 11, J. Chem. Educ., ACS Publications, January 1, 1996.

Greenwood, N. N. "Chemistry of the Elements." A. Earnshaw, (1984). 2nd Edition, Butterworth-Heinemann, December 9, 1997.

Pauling, Linus. "The Nature of the Chemical Bond. IV. The Energy of Single Bonds and the Relative Electronegativity of Atoms". 1932, 54, 9, 3570-3582, J. Am. Chem. Soc., ACS Publications, September 1, 1932.

Pauling, Linus. "The Nature of the Chemical Bond and the Structure of Molecules and Crystals: An Introduction to Mode." 3rd Edition, Cornell University Press, January 31, 1960.

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Question: Electronegativity is a measure of the ability of an atom's nucleus to attract electrons from a different atom within a covalent bond. A higher electronegativity value corresponds to a stronger pull on the electrons by this atom in a bond. This is a strictly theoretical value that cannot be measured in the lab. Select the best visual representation of

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To determine the best visual representation of electronegativity, identify which figure accurately illustrates the ability of an atom's nucleus to attract electrons from another atom in a chemical bond.

1. Figure B is the correct representation of the electronegativity. As, the nucleus of one atom attracts the electrons from another atom in a chemical bond. This is completely depicted in figure B so, its the correct answer. 2. As the number of proto …

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