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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.
It is to be expected that the electronegativity of an element will vary with its chemical environment, [7] but it is usually considered to be a transferable property, that is to say that similar values will be valid in a variety of situations. Caesium is the least electronegative element (0.79); fluorine is the most (3.98).
Linus Pauling originally suggested 64 pm, but that value was eventually replaced by 72 pm, which is half of the fluorine–fluorine bond length. However, 72 pm is too long to be representative of the lengths of the bonds between fluorine and other elements, so values between 54 pm and 60 pm have been suggested by other authors. [5] [6] [7] [8]
Fluorine's first ionization energy is third-highest among all elements, behind helium and neon, [16] which complicates the removal of electrons from neutral fluorine atoms. It also has a high electron affinity , second only to chlorine , [ 17 ] and tends to capture an electron to become isoelectronic with the noble gas neon; [ 3 ] it has 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.
The image shows a periodic table extract with the electronegativity values of metals. [12] Wulfsberg [13] distinguishes: very electropositive metals with electronegativity values below 1.4 electropositive metals with values between 1.4 and 1.9; and electronegative metals with values between 1.9 and 2.54.
Besides, almost all bonds to fluorine are highly polar because of its large electronegativity, so the use of a covalent radius to predict the length of such a bond is inadequate and the bond lengths calculated from these radii are almost always longer than the experimental values. Bonds to fluorine have considerable ionic character, a result of ...
Fluorine forms compounds with all elements except neon and helium. In particular, it forms binary compounds , named fluorides , with all said elements except argon . All of the elements up to einsteinium , element 99, have been checked except for astatine and francium , [ 24 ] and fluorine is also known to form compounds with mendelevium ...