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Chapter 1: Problem 3

Species that have the same number of electrons are described as isoelectronic. What \(+2\) ion is isoelectronic with \(\mathrm{Na}^{+}\) ? What \(-2\) ion?

Short Answer

Expert verified
The +2 ion is ext{Mg}^{2+}, and the -2 ion is ext{O}^{2-}.

Step by step solution

01

Understanding isoelectronic species

Species that are isoelectronic have the same number of electrons. To find ions that are isoelectronic with a given ion, we need to determine the number of electrons in the given ion first.
02

Determine electrons in Na+

A neutral sodium atom ( ext{Na}) has 11 electrons. Since ext{Na}^{+} is a cation with a charge of +1, it loses one electron, resulting in a total of 10 electrons.
03

Finding a +2 ion with 10 electrons

We need to identify a neutral element with 12 electrons, which loses 2 electrons to become a +2 ion and ends up with 10 electrons. Magnesium ( ext{Mg}) is this element, so ext{Mg}^{2+} is isoelectronic with ext{Na}^{+}.
04

Finding a -2 ion with 10 electrons

We need to find a neutral element with 8 electrons, which gains 2 electrons to become a -2 ion and ends up with 10 electrons. Oxygen ( ext{O}) has 8 electrons, and when it gains 2 electrons, it forms ext{O}^{2-}, making it isoelectronic with ext{Na}^{+}.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Electron Configuration
Understanding electron configuration is key to comprehending how elements and their ions behave. Electron configuration describes how electrons are distributed in an atom's orbitals. Each element has a unique configuration.
For example, a neutral sodium atom has an electron configuration of 1s虏 2s虏 2p鈦� 3s鹿. This reflects its 11 electrons, filling the orbitals from lowest to highest energy. When sodium becomes an ion, it loses one electron. This changes its electron configuration to 1s虏 2s虏 2p鈦�, which mirrors that of neon, a noble gas.
Electron configurations help us determine how atoms gain, lose, or share electrons. They are crucial for identifying isoelectronic species.
Ionic Charge
Ionic charge refers to the electric charge an atom has when it becomes an ion. This happens when atoms either lose or gain electrons.
Atoms with less than four valence electrons typically lose them to form positive ions, or cations, with charges equal to the number of lost electrons. Conversely, atoms with more than four valence electrons typically gain electrons to form negative ions, or anions.
  • Cations have positive charges, denoted as "+" and an accompanying number indicating the magnitude of the charge.
  • Anions have negative charges, denoted as "-" along with a numeral.
This concept is essential to understanding isoelectronic species, as the charge determines the number of electrons. Isoelectronic ions with \({Na}^{+}\) include ions that have adjusted their electron count to match.
Sodium Ion
The sodium ion, denoted as \(\text{Na}^{+}\), is formed from a sodium atom, \(\text{Na}\), which typically has 11 electrons.
When sodium loses one electron to achieve a more stable electron configuration, it becomes positively charged with 10 electrons. This loss gives it the electron configuration of 1s虏 2s虏 2p鈦�, making it isoelectronic with neon.
Sodium ions are common in biological systems and play a crucial role in nerve function. Understanding the characteristics of \(\text{Na}^{+}\) provides insight into other isoelectronic species, as it helps identify which other ions have similar electron numbers and configuration.
Magnesium Ion
The magnesium ion, represented as \(\text{Mg}^{2+}\), is formed when a magnesium atom, with 12 electrons, loses two electrons.
This forms an ion with a charge of +2, resulting in an electron count of 10, which is isoelectronic with \(\text{Na}^{+}\) and neon.
Like other metals, magnesium readily forms cations, and its ion is prevalent in various compounds. Its energy level change provides the electron configuration 1s虏 2s虏 2p鈦�. The ion is essential in many biological processes, making understanding its properties crucial.
Oxygen Ion
Oxygen usually exists as a neutral atom with 8 electrons, indicated as \(\text{O}\). When it gains 2 electrons, it forms the oxide ion, \(\text{O}^{2-}\).
This change increases its electron number to 10, aligning its electron configuration with \(\text{Na}^{+}\) and \(\text{Mg}^{2+}\).
The oxide ion's electron configuration becomes 1s虏 2s虏 2p鈦�, matching that of neon.
Oxygen ions are important in chemical reactions, particularly in forming stable anionic compounds. Understanding \(\text{O}^{2-}\) helps in identifying isoelectronic species in various reactive environments.

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Most popular questions from this chapter

In each of the following pairs, determine whether the two represent resonance contributors of a single species or depict different substances. If two structures are not resonance contributors, explain why. (a) \(: \ddot{\mathrm{N}}-\mathrm{N} \equiv \mathrm{N}: \quad\) and \(\quad: \mathrm{N}=\mathrm{N}=\mathrm{N}\) : (c) \(: \ddot{\mathrm{N}}-\mathrm{N} \equiv \mathrm{N}: \quad\) and \(\quad: \ddot{\mathrm{N}}-\ddot{\mathrm{N}}-\ddot{\mathrm{N}}\) : (b) \(: \ddot{\mathrm{N}}-\mathrm{N} \equiv \mathrm{N}\) and \(: \ddot{\mathrm{N}}-\mathrm{N}=\ddot{\mathrm{N}}\) :

The compounds FCl and ICl have dipole moments \(\mu\) that are similar in magnitude \((0.9\) and \(0.7 \mathrm{D}\), respectively \()\) but opposite in direction. In one compound, chlorine is the positive end of the dipole; in the other it is the negative end. Specify the direction of the dipole moment in each compound, and explain your reasoning.

Which is the stronger base in each of the following pairs? (Note: This information will prove useful when you get to Chapter 9.) (a) Sodium ethoxide \(\left(\mathrm{NaOCH}_{2} \mathrm{CH}_{3}\right)\) or sodium amide \(\left(\mathrm{NaNH}_{2}\right)\) (b) Sodium acetylide \((\mathrm{NaC} \equiv \mathrm{CH})\) or sodium amide \(\left(\mathrm{NaNH}_{2}\right)\) (c) Sodium acetylide \((\mathrm{NaC} \equiv \mathrm{CH})\) or sodium ethoxide \(\left(\mathrm{NaOCH}_{2} \mathrm{CH}_{3}\right)\) Sample Solution (a) \(\mathrm{NaOCH}_{2} \mathrm{CH}_{3}\) contains the ions \(\mathrm{Na}^{+}\) and \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{O}^{-} . \mathrm{NaNH}_{2}\) contains the ions \(\mathrm{Na}^{+}\) and \(\mathrm{H}_{2} \mathrm{~N}^{-} . \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{O}^{-}\) is the conjugate base of ethanol; \(\mathrm{H}_{2} \mathrm{~N}^{-}\) is the conjugate base of ammonia. \(\begin{array}{lll}\text { Base } & \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{O}^{-} & \mathrm{H}_{2} \mathrm{~N}^{-} \\ \text {Conjugate acid } & \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH} & \mathrm{NH}_{3} \\ \mathrm{p} K_{\mathrm{a}} \text { of conjugate acid } & 16 & 36\end{array}\) The conjugate acid of \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{O}^{-}\) is stronger than the conjugate acid of \(\mathrm{H}_{2} \mathrm{~N}^{-}\). Therefore, \(\mathrm{H}_{2} \mathrm{~N}^{-}\) is a stronger base than \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{O}^{-}\).

Referring to the periodic table as needed, write electron configurations for all the elements in the third period. Sample Solution The third period begins with sodium and ends with argon. The atomic number \(Z\) of sodium is 11 , and so a sodium atom has 11 electrons. The maximum number of electrons in the 1s, \(2 \mathrm{~s}\), and \(2 \mathrm{p}\) orbitals is ten, and so the eleventh electron of sodium occupies a 3 s orbital. The electron configuration of sodium is \(1 s^{2} 2 s^{2} 2 p_{x}^{2} 2 p_{y}^{2} 2 p_{z}^{2} 3 s^{1}\).

Write structural formulas for all the constitutional isomers of (a) \(\mathrm{C}_{3} \mathrm{H}_{8}\) (b) \(\mathrm{C}_{3} \mathrm{H}_{6}\) (c) \(\mathrm{C}_{3} \mathrm{H}_{4}\)
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