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Electronegativity coefficients

Chemically, it is clear that Zn and Cd are rather similar and that Hg is somewhat distinct. The lighter pair are more electropositive, as indicated both by their electronegativity coefficients and electrode potentials (Table 29.1), while Hg has a... [Pg.1206]

The variations of electronegativity coefficients across periods and down groups... [Pg.2]

This section summarizes the variation, across the periods and down the groups of the Periodic Table, of (i) the ionization energies, (ii) the electron attachment energies (electron affinities), (iii) the atomic sizes and (iv) the electronegativity coefficients of the elements. [Pg.9]

Figure 1.7 The Allred-Rochow electronegativity coefficients of the main group elements of the 2nd, 3rd, 4th and 5th periods... Figure 1.7 The Allred-Rochow electronegativity coefficients of the main group elements of the 2nd, 3rd, 4th and 5th periods...
The trends in first ionization energies, first electron attachment energies, atomic sizes and electronegativity coefficients of the elements across the groups and down the periods of the periodic classification. [Pg.14]

In this case the electropositive sodium atom loses its 3s electron, which is then transferred to the 2p orbital of the electronegative fluorine atom to produce the Na+F ion-pair. Ionic bonding is the subject of Chapter 7. When there is little or no difference in the electronegativity coefficients of the combining atoms, covalent bonds are possible in which two or more electrons are shared between the two atoms. Covalency is the main subject of this chapter. [Pg.35]

Some heteronuclear diatomic molecules were described in detail. Differences in electronegativity coefficients between the combining atoms were shown to be important. [Pg.81]

The HC1 molecule has a dipole moment of 1.03 D and a bond length of 128 pm. Calculate the percentage ionic character, and compare your answer with that for HF. Comment on the differences in electronegativity coefficients in the two molecules. [Pg.82]

The dipole moments of CO and NO are 0.1 D and 0.166 D. respectively. The oxygen atom is the positive end of the CO dipole, despite the difference in electronegativity coefficients of the two atoms which would imply the opposite conclusion. Consider the electronic configurations of the two molecules, and explain the anomalous properties of the CO molecule. [Pg.82]

Table 5.6 Bond length and bond angle data for some compounds with the formula EL,. The differences between the electronegativity coefficients (Allred-Rochow) of the elements are also given... Table 5.6 Bond length and bond angle data for some compounds with the formula EL,. The differences between the electronegativity coefficients (Allred-Rochow) of the elements are also given...
Table 6.4 Bond length, bond angle and electronegativity coefficient (A/) data for some El 3 compounds, where E = N, P or As, and L = H, F or Cl... Table 6.4 Bond length, bond angle and electronegativity coefficient (A/) data for some El 3 compounds, where E = N, P or As, and L = H, F or Cl...
This indicates that the charge separation is equivalent to a partial charge of -0.66c on the oxygen atom and a partial charge of + 0.33c on both hydrogen atoms. This is to be expected from the difference in electronegativity coefficients of the two atoms in each bond. [Pg.5]

The first element, hydrogen, has an Allred Rochow electronegativity coefficient of 2.1, and an electronic configuration Is1. The atom may lose the single electron to become a proton, which exists in aqueous solutions as the hydroxonium ion, H30+(aq), in which the proton is covalently bonded to the oxygen atom of a water molecule. The ion is hydrated, as is discussed extensively in Chapter 2. The reduction of the hydrated proton by an electron forms the reference standard half-reaction for the scale of reduction potentials ... [Pg.104]

The very negative Ln t + /Ln potentials are consistent with the electropositive nature of the lanthanide elements their Allred-Rochow electronegativity coefficients are all 1.1 except for europium, which has a value of 1.0. The lighter elements of Group 3, Sc and Y, both have electronegativity coefficients of 1.3. The nearest p-block element to the lanthanides in these properties is magnesium (Mg2+/Mg) = -2.37 V, and its electronegativity coefficient is 1.2. [Pg.162]

The ease with which a molecule forms an ion, either by accepting or donating one electron, is given by the Mulliken electronegativity coefficient %. Numerically, this is the average of its molecular electron affinity Ea and its ionization potential /p. [Pg.183]

The bonds formed by S with a particular element have less ionic character than those between 0 and the same element. Pauling assigns the following electronegativity coefficients ... [Pg.415]

The energy difference between valence shell. y and p electrons in an atom is of secondary importance for our description of a molecule if the atom uses both s and p electrons for bond formation, or if we describe the molecule using molecular orbitals formed from sp hybridized atomic orbitals. The mean valence electron ionization energies may therefore be used to define a set of electronegativity coefficients. The magnitudes of these electronegativity coefficients are found to increase across a period, and - with a few exceptions - to decrease down a group. [Pg.41]

Allen has suggested that the electronegativity coefficient x should be defined in terms of the mean valence shell ionization energy [3] ... [Pg.53]


See other pages where Electronegativity coefficients is mentioned: [Pg.2]    [Pg.13]    [Pg.13]    [Pg.14]    [Pg.59]    [Pg.74]    [Pg.114]    [Pg.135]    [Pg.146]    [Pg.147]    [Pg.151]    [Pg.4]    [Pg.145]    [Pg.676]    [Pg.676]    [Pg.236]    [Pg.236]    [Pg.236]    [Pg.237]    [Pg.1322]    [Pg.1322]    [Pg.4]    [Pg.145]    [Pg.53]    [Pg.53]    [Pg.53]    [Pg.53]    [Pg.54]   
See also in sourсe #XX -- [ Pg.13 ]

See also in sourсe #XX -- [ Pg.3 , Pg.12 ]

See also in sourсe #XX -- [ Pg.20 ]




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