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Iodine is the fourth halogen, being a member of group 17 in the periodic table, below fluorine, chlorine, and bromine; since astatine and tennessine are radioactive, iodine is the heaviest stable halogen. Iodine has an electron configuration of [Kr]5s 2 4d 10 5p 5, with the seven electrons in the fifth and outermost shell being its valence ...
Electronegativity is not a uniquely defined property and may depend on the definition. The suggested values are all taken from WebElements as a consistent set. Many of the highly radioactive elements have values that must be predictions or extrapolations, but are unfortunately not marked as such.
Iodine is an insulator in the direction perpendicular to its planes. It has a high ionisation energy (1008.4 kJ/mol), high electron affinity (295 kJ/mol), and high electronegativity (2.66). Iodine is a moderately strong oxidising agent (I 2 + 2e → 2I − = 0.53 V at pH 0). Metal iodides are predominantly ionic in nature.
Electronegativity, symbolized as χ, is the tendency for an atom of a given chemical element to attract shared electrons (or electron density) when forming a chemical bond. [1] An atom's electronegativity is affected by both its atomic number and the distance at which its valence electrons reside from the charged nucleus. The higher the ...
Generally, the higher these values are (including electronegativity) the more nonmetallic the element tends to be. [68] For example, the chemically very active nonmetals fluorine, chlorine, bromine, and iodine have an average electronegativity of 3.19—a figure [i] higher than that of any metallic element.
In iodane chemistry, carbon is considered more electronegative than iodine, despite the Pauling electronegativities of those respective atoms. [2] Thus iodobenzene (C 6 H 5 I) is an iodine(I) compound, (dichloroiodo)benzene (C 6 H 5 ICl 2) and iodosobenzene (C 6 H 5 IO) iodine(III) compounds, and iodoxybenzene (C 6 H 5 IO 2) an iodine(V) compound.
Electron affinity can be defined in two equivalent ways. First, as the energy that is released by adding an electron to an isolated gaseous atom. The second (reverse) definition is that electron affinity is the energy required to remove an electron from a singly charged gaseous negative ion.
These tables list values of molar ionization energies, measured in kJ⋅mol −1.This is the energy per mole necessary to remove electrons from gaseous atoms or atomic ions.