Chemists often relate electronegativity (EN), first-ionization energy (IE1), and electron affinity (EA) to rationalize chemical reactivity.
(a) Construct a conceptual diagram (for example, a flow chart or network diagram) that visually relates EN, IE1, and EA to one another through their common dependence on effective nuclear charge (Zeff) and atomic radius. Your diagram should explicitly indicate whether each relationship is direct or inverse.
(b) Using your diagram, explain why elements with high electronegativity values generally also have large magnitudes of electron affinity (more exothermic) and high IE1 values.
(c) Consider the elements sulfur (S) and chlorine (Cl). Using the relationships in your diagram, predict which element’s gaseous atoms more readily accept an additional electron and provide a quantitative or qualitative justification.
(d) Despite the general correlations, aluminum (Al) has a first-ionization energy that is slightly lower than that of magnesium (Mg). Use your diagram and electron-configuration arguments to justify this deviation from the trend.
a. Part (a)
b. Part (b)
c. Part (c)
d. Part (d)