The successive ionization energies for a second-period element are given. What is the identity of the element? (LO 6.8) Ea1 = 1402 kJ/mol Ea2 = 2856 kJ/mol Ea3 = 4578 kJ/mol Ea4 = 7475 kJ/mol Ea5 = 9445 kJ/mol Ea6 = 53,266 kJ/mol Ea7 = 64,630 kJ/mol (a) Be (b) C (c) N (d) F

Ionization energy is the energy required to remove an electron from a gaseous atom or ion. It is a key factor in determining an element's reactivity and is influenced by the atomic structure, including the number of protons and the distance of electrons from the nucleus. Generally, ionization energy increases across a period due to increased nuclear charge and decreases down a group due to increased electron shielding.

The trends in ionization energies can provide insights into the identity of an element. As you move across a period from left to right, ionization energies typically increase due to greater effective nuclear charge. A significant jump in ionization energy, such as the one observed in the provided data, indicates the removal of an electron from a much more stable electron configuration, often suggesting the completion of an electron shell.

Electron configuration describes the distribution of electrons in an atom's orbitals. Understanding the electron configuration of an element helps predict its chemical behavior and reactivity. For the second-period elements, the configurations can be used to identify stability and the likelihood of losing electrons, which is crucial when analyzing the provided ionization energies and determining the element in question.