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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.
The electronegativity of aluminium is 1.61 (Pauling scale). ... The real price for aluminium declined from $14,000 per metric ton in 1900 to $2,340 in 1948 ...
See also: Electronegativities of the elements (data page) There are no reliable sources for Pm, Eu and Yb other than the range of 1.1–1.2; see Pauling, Linus (1960).
The anomalously high electronegativity of lead, in particular when compared to thallium and bismuth, is an artifact of electronegativity varying with oxidation state: its electronegativity conforms better to trends if it is quoted for the +2 state with a Pauling value of 1.87 instead of the +4 state.
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.
This is a list of chemical elements and their atomic properties, ordered by atomic number (Z).. Since valence electrons are not clearly defined for the d-block and f-block elements, there not being a clear point at which further ionisation becomes unprofitable, a purely formal definition as number of electrons in the outermost shell has been used.
(room temperature) (alpha, polycrystalline) calculated from single crystal values 56.2 LNG (10 −8 Ωm) 56.2 WEL (10 −8 Ωm) (293 K–298 K) 55 22 Ti titanium; use 0.39 μΩm 0.420 μΩm CRC (10 −8 Ωm) 39 LNG (10 −8 Ωm) 42.0 WEL (10 −8 Ωm) (293 K–298 K) 40 23 V vanadium; use 24.1 nΩm 181 nΩm 197 nΩm 201 nΩm 202 nΩm 348 nΩm
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.