The scatter plot below shows the first ionization energies and atomic radii of several of the second- and third-period elements of the periodic table: N at (1400,0.75); O at (1300,0.6); C at (1200,0.90); S at (1000,1.1); P at (1100,1.2); B at (800,1.2); Be at (900,1.4); Si at (750,1.5), Mg at (700,1.6); Al at (590,1.7); Li at (500,2.0); Na at (450,2.3); K at (410,2.7) Which conclusion can be drawn based on the information in this graph? As the electronegativity value for the elements increases, the atomic radius decreases. The electronegativity values and the atomic radii of these elements are directly proportional. As the electronegativity value of the elements increases, the atomic radius increases exponentially. No relationship appears to exist between the atomic radius and the first ionization energy of an element.