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In chemistry, polyvalency (or polyvalence, multivalency) is the property of molecules and larger species, such as antibodies, medical drugs, and even nanoparticles surface-functionalized with ligands, like spherical nucleic acids, that exhibit more than one supramolecular interaction.
The large charge pulls on the electron cloud of the iodine. Now, if we consider the iodine atom, we see that it is relatively large and thus the outer shell electrons are relatively well shielded from the nuclear charge. In this case, the aluminum ion's charge will "tug" on the electron cloud of iodine, drawing it closer to itself.
Molecular binding is an attractive interaction between two molecules that results in a stable association in which the molecules are in close proximity to each other. It is formed when atoms or molecules bind together by sharing of electrons.
The MO diagram for dihydrogen. In the classic example of the H 2 MO, the two separate H atoms have identical atomic orbitals. When creating the molecule dihydrogen, the individual valence orbitals, 1s, either: merge in phase to get bonding orbitals, where the electron density is in between the nuclei of the atoms; or, merge out of phase to get antibonding orbitals, where the electron density ...
Electron binding energy; Ionization energy Electron binding energy, more commonly known as ionization energy, [3] is a measure of the energy required to free an electron from its atomic orbital or from a solid. The electron binding energy derives from the electromagnetic interaction of the electron with the nucleus and the other electrons of ...
Hydrogen has only one valence electron, but it can form bonds with more than one atom. In the bifluoride ion ([HF 2] −), for example, it forms a three-center four-electron bond with two fluoride atoms: [F−H F − ↔ F − H−F] Another example is the three-center two-electron bond in diborane (B 2 H 6).
The Wannier functions for different lattice sites in a crystal are orthogonal, allowing a convenient basis for the expansion of electron states in certain regimes. Wannier functions have found widespread use, for example, in the analysis of binding forces acting on electrons.
The following table shows a series of Gibbs free energy of binding between benzene and several cations in the gas phase. [ 2 ] [ 6 ] For a singly charged species, the gas-phase interaction energy correlates with the ionic radius , r i o n {\displaystyle r_{\mathrm {ion} }} (non-spherical ionic radii are approximate).