Which of the following chemical equations is connected to the definitions of (a) the first ionization energy of oxygen (i) O1g2 + e-¡O-1g2 (ii) O1g2¡O+1g2 + e- (iii) O1g2 + 2 e-¡O2-1g2 (iv) O1g2¡O2+1g2 + 2 e- (v) O+1g2¡O2+1g2 + e-

Key Concepts

Ionization Energy

Ionization energy is the energy required to remove an electron from an atom or ion in its gaseous state. The first ionization energy specifically refers to the energy needed to remove the outermost electron from a neutral atom, resulting in a positively charged ion. Understanding this concept is crucial for analyzing chemical equations that involve electron removal.

Oxygen's Electron Configuration

Oxygen has an atomic number of 8, with an electron configuration of 1s² 2s² 2p⁴. This configuration indicates that oxygen has six valence electrons, making it relatively electronegative and likely to gain or lose electrons during chemical reactions. Recognizing the electron configuration helps in predicting the behavior of oxygen in ionization processes.

Chemical Equations and Electron Transfer

Chemical equations represent the transformation of reactants into products, often involving the transfer of electrons. In the context of ionization, the equations illustrate how an atom loses electrons to form cations. Understanding how to interpret these equations is essential for identifying which equation corresponds to the first ionization energy of oxygen.