Chapter 4: Problem 92

Write electron configurations for \(\mathrm{O}, \mathrm{O}^{2+}\), and \(\mathrm{O}^{2-}\). Which form would you expect to find in most compounds of oxygen? Why?

Short Answer

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The electron configurations for oxygen (O), oxygen cation (O²⁺), and oxygen anion (O²⁻) are: - O: 1s^2 2s^2 2p^4 - O²⁺: 1s^2 2s^2 2p^2 - O²⁻: 1s^2 2s^2 2p^6 The most common form of oxygen in compounds is the anion, O²⁻, because gaining 2 electrons results in a stable, full outer electron shell (2p^6), resembling the noble gas neon. This stability enables O²⁻ to readily form chemical bonds with other elements through ionic bonding.

Step by step solution

Identify the atomic number of oxygen

The atomic number of oxygen is 8, which means it has 8 protons and 8 electrons in its neutral form.

Write the electron configuration for the neutral oxygen atom (O)

To write the electron configuration for O, we will follow the Aufbau principle and the Pauli exclusion principle, filling in orbitals from lower to higher energy levels: 1s^2 2s^2 2p^4 We have filled the 1s, 2s, and 2p orbitals so that the sum of electrons is 8, the total number of electrons in a neutral oxygen atom.

Write the electron configuration for the oxygen cation with a 2+ charge (O²⁺)

For O²⁺, we need to remove two electrons from the electron configuration of the neutral oxygen atom. To do this, we will remove the electrons from the highest energy orbital, which is the 2p orbital. Oxygen cation (O²⁺) electron configuration: 1s^2 2s^2 2p^2

Write the electron configuration for the oxygen anion with a 2- charge (O²⁻)

For O²⁻, we need to add two electrons to the electron configuration of the neutral oxygen atom. We will add the electrons to the highest energy orbital that is not yet full, which is the 2p orbital. Oxygen anion (O²⁻) electron configuration: 1s^2 2s^2 2p^6

Identify the most common form for oxygen in compounds and explain why

The most common form of oxygen in compounds is the anion, O²⁻. This is because when oxygen gains 2 electrons, it becomes more stable, having a full outer electron shell (2p^6). In this configuration, the oxygen anion has the stable electron configuration of a noble gas – neon, which allows it to readily form chemical bonds with other elements in a process called ionic bonding.

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Write electron configurations for \(\mathrm{O}, \mathrm{O}^{2+}\), and \(\mathrm{O}^{2-}\). Which form would you expect to find in most compounds of oxygen? Why?

Short Answer

Step by step solution

Identify the atomic number of oxygen

Write the electron configuration for the neutral oxygen atom (O)

Write the electron configuration for the oxygen cation with a 2+ charge (O²⁺)

Write the electron configuration for the oxygen anion with a 2- charge (O²⁻)

Identify the most common form for oxygen in compounds and explain why

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