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Chapter 3: Problem 63

Consider the following energy changes: Magnesium oxide exists as \(\mathrm{Mg}^{2+} \mathrm{O}^{2-}\) and not as \(\mathrm{Mg}^{+} \mathrm{O}^{-}\) Explain.

Short Answer

Expert verified
Magnesium oxide forms as \(\mathrm{Mg}^{2+} \mathrm{O}^{2-}\) rather than \(\mathrm{Mg}^{+} \mathrm{O}^{-}\) because both ions achieve greater stability by adopting noble gas configurations as required by the octet rule. In doing so, Magnesium loses two electrons to form \(\mathrm{Mg}^{2+}\), and Oxygen gains two electrons to form \(\mathrm{O}^{2-}\).

Step by step solution

01

Recall the electron configurations of Magnesium and Oxygen atoms

Start by recalling the electron configurations of Magnesium (Mg) and Oxygen (O). Magnesium has an atomic number of 12 and an electron configuration of \[1s^2 \ 2s^2 \ 2p^6 \ 3s^2.\] Oxygen has an atomic number of 8 and an electron configuration of \[1s^2 \ 2s^2 \ 2p^4.\]
02

Consider the ionization energies of Magnesium and Oxygen atoms

Ionization energy is the energy required to remove an electron from an atom or ion. Magnesium has two ionization energies, as it can lose one or two electrons from its outermost shell. - The first ionization energy of Magnesium corresponds to the energy required to remove the first 3s electron, forming \(\mathrm{Mg}^{+}\). - The second ionization energy of Magnesium corresponds to the energy required to remove the second 3s electron, forming \(\mathrm{Mg}^{2+}\). Since Oxygen needs to gain electrons to attain a stable configuration, it has electron affinity. - Oxygen can gain one electron to form \(\mathrm{O}^{-}\) or two electrons to form \(\mathrm{O}^{2-}\).
03

Recall the octet rule

The octet rule states that atoms tend to gain, lose, or share electrons to have a full outer shell containing eight electrons. - When Magnesium loses two electrons to form \(\mathrm{Mg}^{2+}\), it attains a stable noble gas configuration: \(1s^2 \ 2s^2 \ 2p^6\) - When Oxygen gains two electrons to form \(\mathrm{O}^{2-}\), it also attains a stable noble gas configuration: \(1s^2 \ 2s^2 \ 2p^6\)
04

Analyze the stability of ions

Comparing the stability of ions formed in the different cases: - Forming \(\mathrm{Mg}^{2+}\) and \(\mathrm{O}^{2-}\) leads both ions to have a stable noble gas configuration, which is highly stable and tends to occur in nature. - Forming \(\mathrm{Mg}^{+}\) and \(\mathrm{O}^{-}\), on the other hand, would result in incomplete electron configurations and would make both ions less stable.
05

Conclude

As a result of this analysis, we can conclude that Magnesium oxide forms as \(\mathrm{Mg}^{2+} \mathrm{O}^{2-}\) rather than \(\mathrm{Mg}^{+} \mathrm{O}^{-}\) due to the greater stability achieved by both ions when they adopt noble gas configurations by losing or gaining electrons as required by the octet rule.

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