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A graph comparing the atomic radius of elements with atomic numbers 1–100. Accuracy of ±5 pm. Electrons in atoms fill electron shells from the lowest available energy level. As a consequence of the Aufbau principle, each new period begins with the first two elements filling the next unoccupied s-orbital. Because an atom's s-orbital electrons ...
The atomic radius is half of the distance between two nuclei of two atoms. The atomic radius is the distance from the atomic nucleus to the outermost electron orbital in an atom . In general, the atomic radius decreases as we move from left-to-right in a period , and it increases when we go down a group .
The radius increases sharply between the noble gas at the end of each period and the alkali metal at the beginning of the next period. These trends of the atomic radii (and of various other chemical and physical properties of the elements) can be explained by the electron shell theory of the atom; they provided important evidence for the ...
Elements are placed in the periodic table according to their electron configurations, [38] the periodic recurrences of which explain the trends in properties across the periodic table. [ 39 ] An electron can be thought of as inhabiting an atomic orbital , which characterizes the probability it can be found in any particular region around the atom.
The ionic radius is not a fixed property of a given ion, but varies with coordination number, spin state and other parameters. Nevertheless, ionic radius values are sufficiently transferable to allow periodic trends to be recognized. As with other types of atomic radius, ionic radii increase on descending a group.
Atomic radius of elements of the groups 2, 13 and 14, showing the "d-block contraction", especially for Ga and Ge. The d-block contraction (sometimes called scandide contraction [1]) is a term used in chemistry to describe the effect of having full d orbitals on the period 4 elements.
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Calculated atomic radii of period 2 elements in picometers. Period 2 is the first period in the periodic table from which periodic trends can be drawn. Period 1, which only contains two elements (hydrogen and helium), is too small to draw any conclusive trends from it, especially because the two elements behave nothing like other s-block elements.