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You can download a PDF version of the table for printing. Atomic radius decreases as you move across a period from left to right and decreases as you move up a group from bottom to top. Thus, helium is the smallest element, and francium is the largest. This is due to trends in the periodic table, and the effective nuclear charge that holds the valence electrons close to the nucleus. As can be seen in the figures below, the atomic radius increases from top to bottom in a group, and decreases from left to right across a period. Each atom is shown relative to the largest atom, cesium. Atomic radii vary in a predictable way across the periodic table. Which explains the change in ionization energy that occurs between removing the first and second electrons from an atom? Sr Electronegativities of the elements Be, Mg, Ca, and Sr follow a specific trend within their group. This special periodic table shows the relative size of atoms of periodic table elements based on atomic radius data. Which predictions can most likely be madeabout ionization/electronegativity? energy needed to remove an electron from an atom or ion in the gas phase Which best describes ionization energy? The ionization energy increases because the ratio of the protons to electrons increases. Element Atomic radius First ionization energy Na Al Rb Ar Sb has a lower ionization energy and a lower electronegativity than I. Ar Which element would most likely have an electron affinity measuring closest to zero?
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