Pauling, Linus electronegativity scale

TABLE 1.1 1.3 MOLECULAR INTERACTIONS Linus Pauling s Electronegativity Scale for Biochemistry Students 3... 

Electronegativity does not have a unit. The most widely used electronegativity scale today was derived by Linus Pauling. He used bond energy values in the preparation of this scale. 

Around 1935, the American chemist Linus Pauling developed a scale of electronegativity to describe the attraction an element has for electrons in a chemical bond. The values in Figure 5-13 are higher for elements that more strongly attract electrons, which increase the likelihood of a negative partial charge on that atom. 

There are other types of electronegativity scales as well, the most widely utilized of which is the one from the developer of the electronegativity concept, Linus Pauling ... 

Electronegativity is a relative quantity and it does not have a unit. Today, the most commonly used electronegativity scale today is Linus Pauling s scale, which is based on the values of bond energies. 

The most commonly used electronegativity scale was devised by Linus Pauling. Table 1.3 keys Pauling s electronegativity values to the periodic table. 

Numerical estimates of electronegativity can be based on a variety of properties, not just ionization energy and electron affinity. The first and most widely used electronegativity scale was developed by the American chemist Linus Pauling (1901-1994), who based his scale on thermochemical data. Figure 8.6 T shows... 

FIGURE 10.2 Electronegativity of the elements Linus Pauling introduced the scale shown here. He arbitrarily set the electronegativity of fluorine at 4.0 and computed all other values relative to fluorine. 

It was through bond enthalpy terms that Linus Pauling arrived at the famous Pauling electronegativity scale. In the previous Section, you saw that S(H—Cl) = 432 kJ moFk The homonuclear molecules, H2 and CI2, formed by these two atoms have bond enthalpy terms of 436 and 243 kJ moF, respectively. The average is 340kJ moF, yet fi(H—Cl) exceeds this by 92 kJ moF. This shows that the bond in the HCl molecule is unusually strong. 

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