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-

Verified step by step guidance

insert step 1> Identify the definition of first ionization energy: it is the energy required to remove the outermost electron from a neutral atom in the gaseous state.

insert step 2> Look for the equation that represents the removal of one electron from a neutral oxygen atom (O) in the gaseous state.

insert step 3> Analyze each option: (i) represents the gain of an electron, (ii) represents the removal of one electron from a neutral oxygen atom, (iii) represents the gain of two electrons, (iv) represents the removal of two electrons, and (v) represents the removal of an electron from a positively charged ion.

insert step 4> Determine that option (ii) O(g) → O⁺(g) + e⁻ correctly represents the first ionization energy of oxygen.

insert step 5> Conclude that the correct chemical equation related to the first ionization energy of oxygen is option (ii).

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Video duration:

Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

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.

Recommended video:

Guided course

01:32

Balancing Chemical Equations

Related Practice

Textbook Question

Identify two ions that have the following ground-state electron configurations: (a) [Ar]

Textbook Question

Identify two ions that have the following ground-state electron configurations: (b) [Ar]3d⁵

Textbook Question

Identify two ions that have the following ground-state electron configurations: (c) [Kr]5s²4d¹⁰

Textbook Question

Hydrogen is an unusual element because it behaves in some ways like the alkali metal elements and in other ways like nonmetals. Its properties can be explained in part by its electron configuration and by the values for its ionization energy and electron affinity. (a) Explain why the electron affinity of hydrogen is much closer to the values for the alkali elements than for the halogens.

Textbook Question

The first ionization energy of the oxygen molecule is the energy required for the following process: O21g2¡O2 +1g2 + e- The energy needed for this process is 1175 kJ>mol, very similar to the first ionization energy of Xe. Would you expect O2 to react with F2? If so, suggest a product or products of this reaction.

views

Textbook Question

It is possible to define metallic character as we do in this book and base it on the reactivity of the element and the ease with which it loses electrons. Alternatively, one could measure how well electricity is conducted by each of the elements to determine how 'metallic' the elements are. On the basis of conductivity, there is not much of a trend in the periodic table: Silver is the most conductive metal, and manganese the least. Look up the first ionization energies of silver and manganese; which of these two elements would you call more metallic based on the way we define it in this book?