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Chapter 8: Problem 54

Give an example of an ionic compound where both the anion and the cation are isoelectronic with each of the following noble gases. a. \(\mathrm{Ne} \quad\) c. \(\mathrm{Kr}\) b. \(\mathrm{Ar} \quad\) d. \(\mathrm{Xe}\)

Short Answer

Expert verified
a. Neon (Ne): NaF (sodium fluoride) b. Argon (Ar): KCl (potassium chloride) c. Krypton (Kr): RbBr (rubidium bromide) d. Xenon (Xe): CsI (cesium iodide)

Step by step solution

01

Identify the electron configuration of the given noble gases

First, identify the electron configuration of each noble gas. The noble gases are in group 18 of the periodic table. Electron configurations are given as [previous noble gas] Ns^2 Np^6, where N is the period number. a. Neon (Ne): Ne has 10 electrons, and its electron configuration is 1s^2 2s^2 2p^6. b. Argon (Ar): Ar has 18 electrons, and its electron configuration is [Ne] 3s^2 3p^6. c. Krypton (Kr): Kr has 36 electrons, and its electron configuration is [Ar] 4s^2 3d^10 4p^6. d. Xenon (Xe): Xe has 54 electrons, and its electron configuration is [Kr] 5s^2 4d^10 5p^6.
02

Identify the ions isoelectronic with each noble gas

Next, we need to find ions that have the same number of electrons as the noble gases. We can do this by looking at the periodic table and by adding or removing electrons from adjacent elements. a. Neon (Ne): Ions isoelectronic with Ne (10 electrons) - Na^+ (11 - 1 = 10 electrons) - F^- (9 + 1 = 10 electrons) b. Argon (Ar): Ions isoelectronic with Ar (18 electrons) - K^+ (19 - 1 = 18 electrons) - Cl^- (17 + 1 = 18 electrons) c. Krypton (Kr): Ions isoelectronic with Kr (36 electrons) - Rb^+ (37 - 1 = 36 electrons) - Br^- (35 + 1 = 36 electrons) d. Xenon (Xe): Ions isoelectronic with Xe (54 electrons) - Cs^+ (55 - 1 = 54 electrons) - I^- (53 + 1 = 54 electrons)
03

Form the ionic compounds using the identified ions

Now that we know the ions isoelectronic with each noble gas, we can form ionic compounds using these ions. a. Neon (Ne): Ionic compound = Na^+ and F^- Compound: NaF (sodium fluoride) b. Argon (Ar): Ionic compound = K^+ and Cl^- Compound: KCl (potassium chloride) c. Krypton (Kr): Ionic compound = Rb^+ and Br^- Compound: RbBr (rubidium bromide) d. Xenon (Xe): Ionic compound = Cs^+ and I^- Compound: CsI (cesium iodide) So, the ionic compounds are NaF, KCl, RbBr, and CsI, where both the anions and cations are isoelectronic to Ne, Ar, Kr, and Xe, respectively.

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