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Pauling invoked the principle of electroneutrality in a 1952 paper to suggest that pi bonding is present, for example, in molecules with 4 Si-O bonds. [8] The oxygen atoms in such molecules would form polar covalent bonds with the silicon atom because their electronegativity (electron withdrawing power) was higher than that of silicon.
One of Pauling's examples is olivine, M 2 SiO 4, where M is a mixture of Mg 2+ at some sites and Fe 2+ at others. The structure contains distinct SiO 4 tetrahedra which do not share any oxygens (at corners, edges or faces) with each other. The lower-valence Mg 2+ and Fe 2+ cations are surrounded by polyhedra which do share oxygens.
Pauling's rules; Pauling–Corey–Branson alpha helix; Pauling's principle of electroneutrality; Quantum chemistry; Quantum graph; Residual entropy; Resonance (chemistry) Slater–Pauling rule; Space-filling model; Valence bond theory; Vitamin C megadosage; Xenic acid; Advocating nuclear disarmament
Periodic variation of Pauling electronegativities. The tendency of an atom in a molecule to attract the shared pair of electrons towards itself is known as electronegativity. It is a dimensionless quantity because it is only a tendency. [17] The most commonly used scale to measure electronegativity was designed by Linus Pauling.
Pauling's principle of electroneutrality; Photovoltaic effect; Photovoltaics; Pi electron donor-acceptor; Pople diagram; Post–Hartree–Fock; Potential energy surface; Primogenic Effect; Principal interacting orbital; Principal quantum number
Pauli exclusion principle; Pauling's principle of electroneutrality; Peptide bond; Perpendicular paramagnetic bond; Phi bond; Pi backbonding; Pi bond; Pi-stacking; Pnictogen bond; Polar bond; Polyhedral skeletal electron pair theory; Polyvalency (chemistry) Primogenic Effect; Pseudorotation; Pyramidal alkene
The basic rule given above makes several approximations. One simplification is rounding to the nearest integer. Because we are describing the number of electrons in a band using an average value, the s and d shells can be filled to non-integer numbers of electrons, allowing the Slater–Pauling rule to give more accurate predictions.
The polar substituent constants are similar in principle to σ values from the Hammett equation, as an increasing value corresponds to a greater electron-withdrawing ability. Bent's rule suggests that as the electronegativity of the groups increase, more p character is diverted towards those groups, which leaves more s character in the bond ...