Electronegativities of atoms

You need not memorize these values, but you should know the trends, the extremes, and that the electronegativity of hydrogen is about the same as boron, H (2.1), B (2.0). 

Electronegativities increase across a period and decrease down a group. 

These problems have both answers and solutions given. 

What is measured by the electronegativity of an element Which element is the most electronegative  

Answer The electronegativity of an element is a measure of the ability of that element to attract a shared pair of electrons to itself. The most electronegative element is fluorine with a value of 4.0. 

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An extended set of physicochemical descriptors was used in this study, including, for example, partial atomic charge and effective polari2 ability of the protons, average of electronegativities of atoms two bonds away, or maximum, T-atomic charge of atoms two bonds away. 

Increased shielding of methyl protons Decreasing electronegativity of atom attached to CH3... 

Pauling s electronegativity difference, where represents the electronegativity of atom X. 

Bond Energies and the Relative Electronegativity of Atoms.—In Table II there are collected the energies of single bonds obtained in the preceding sections. One additional value, obtained by a method to be described later, is also included 1.44 v. e. for N N. Under each bond energy is given the value for a normal covalent bond, calculated from additivity, and below that the difference A. It is seen that A is positive in twenty of the twenty-one cases. The exception, C I, may be due to experimental error, and be not real. 

The Nature of the Chemical Bond Fifty Years Later The Relative Electronegativity of Atoms Seen in Perspective... 

One of the most pervasive ideas to emerge from the series of papers entitled The Nature of the Chemical Bond is the concept of the relative electronegativity of atoms. The sections that follow examine some of the consequences of this concept. 

Sen KD, Bohm MC, Schmidt PC (1987) Electronegativity of Atoms and Molecular Fragments. 66 99-123... 

As another example, the functional expression for the energy in terms of p(r) is known only approximately. However exact formulas have been developed that relate the energies of atoms and molecules to the electrostatic potentials at their nuclei [49-52], This has been done as well for the chemical potentials (electronegativities) of atoms [53]. Thus, both the intrinsic significance and the practical applications of the electrostatic potential continue to be active areas of investigation. 

Linus Pauling, "The Nature of the Chemical Bond. IV. The Energy of Single Bonds and the Relative Electronegativity of Atoms," JACS 54 (1932) 35703582 and Pauling, The Nature of the Chemical Bond. 

Pauling L. (1932). Nature of the chemical bond. IV. The energy of single bonds and the relative electronegativity of atoms. Jour. Amer. Chem. Soc., 54 3570-3582. 

Table 2.3 Electronegativities of Atoms According to the Scale Devised by Pauling...

Some atoms are more electronegative than others that is, they more strongly attract electrons. The relative electronegativities of atoms encountered in this text are F > O > N > 0 S > P 11. For example, the two electron pairs making up a 0=0 (carbonyl) bond are not shared equally the carbon is relatively electron-deficient as the oxygen draws away the electrons. Many reactions involve an electron-rich atom (a nucleophile) reacting with an electron-deficient atom (an electrophile). Some common nucleophiles and electrophiles in biochemistry are shown at right. 

The Partial Ionic Character of Covalent Bonds and the Relative Electronegativity of Atoms... 

The differences in electronegativity of atoms for the bonds in Table 3-6 are given in the columns headed Za. — %b. If the extra ionic energy A (A— B) were given accurately by the equation... 

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