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Chapter 8: Problem 48

What noble gas has the same election configuration as each of the ions in the following compounds? a. cesium sulfide b. strontium fluoride c. calcium nitride d. aluminum bromide

Short Answer

Expert verified
The noble gases with the same electron configuration as the ions in the given compounds are: a. Cesium sulfide: Xenon (Xe) and Argon (Ar) b. Strontium fluoride: Krypton (Kr) and Neon (Ne) c. Calcium nitride: Argon (Ar) and Neon (Ne) d. Aluminum bromide: Neon (Ne) and Krypton (Kr)

Step by step solution

01

a. Cesium sulfide

1. Determine the charges of the ions in the compound Cesium (Cs) is an alkali metal in group 1, so it has a +1 charge. Sulfur (S) is a non-metal in group 16, so it has a -2 charge. 2. Write the electron configuration of the ions Cesium ion (Cs⁺): Cesium has the electron configuration [Xe]6s1. Upon losing 1 electron, it becomes [Xe]. Sulfide ion (S²⁻): Sulfur has the electron configuration [Ne]3s²3p⁴. Upon gaining 2 electrons, it becomes [Ar]. Thus, the noble gas with the same electron configuration as the ions in cesium sulfide is Xenon (Xe) and Argon (Ar).
02

b. Strontium fluoride

1. Determine the charges of the ions in the compound Strontium (Sr) is an alkaline earth metal in group 2, so it has a +2 charge. Fluorine (F) is a halogen in group 17, so it has a -1 charge. 2. Write the electron configuration of the ions Strontium ion (Sr²⁺): Strontium has the electron configuration [Kr]5s². Upon losing 2 electrons, it becomes [Kr]. Fluoride ion (F⁻): Fluorine has the electron configuration [He]2s²2p⁵. Upon gaining 1 electron, it becomes [Ne]. Thus, the noble gas with the same electron configuration as the ions in strontium fluoride is Krypton (Kr) and Neon (Ne).
03

c. Calcium nitride

1. Determine the charges of the ions in the compound Calcium (Ca) is an alkaline earth metal in group 2, so it has a +2 charge. Nitrogen (N) is a non-metal in group 15, so it has a -3 charge. 2. Write the electron configuration of the ions Calcium ion (Ca²⁺): Calcium has the electron configuration [Ar]4s². Upon losing 2 electrons, it becomes [Ar]. Nitride ion (N³⁻): Nitrogen has the electron configuration [He]2s²2p³. Upon gaining 3 electrons, it becomes [Ne]. Thus, the noble gas with the same electron configuration as the ions in calcium nitride is Argon (Ar) and Neon (Ne).
04

d. Aluminum bromide

1. Determine the charges of the ions in the compound Aluminum (Al) is a metal in group 13, so it has a +3 charge. Bromine (Br) is a halogen in group 17, so it has a -1 charge. 2. Write the electron configuration of the ions Aluminum ion (Al³⁺): Aluminum has the electron configuration [Ne]3s²3p¹. Upon losing 3 electrons, it becomes [Ne]. Bromide ion (Br⁻): Bromine has the electron configuration [Ar]4s²3d¹₀4p⁵. Upon gaining 1 electron, it becomes [Kr]. Thus, the noble gas with the same electron configuration as the ions in aluminum bromide is Neon (Ne) and Krypton (Kr).

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Most popular questions from this chapter

Write Lewis structures and predict the molecular structures of the following. (See Exercises 111 and \(112 .\) ) a. \(\mathrm{OCl}_{2}, \mathrm{KrF}_{2}, \mathrm{BeH}_{2}, \mathrm{SO}_{2}\) b. \(\mathrm{SO}_{3}, \mathrm{NF}_{3}, \mathrm{IF}_{3}\) c. \(\mathrm{CF}_{4}, \mathrm{SeF}_{4}, \mathrm{KrF}_{4}\) d. \(\mathrm{IF}_{5}, \mathrm{AsF}_{5}\) Which of these compounds are polar?

Which of the following molecules have net dipole moments? For the molecules that are polar, indicate the polarity of each bond and the direction of the net dipole moment of the molecule. a. \(\mathrm{CH}_{2} \mathrm{Cl}_{2}, \mathrm{CHCl}_{3}, \mathrm{CCl}_{4}\) b. \(\mathrm{CO}_{2}, \mathrm{~N}_{2} \mathrm{O}\) c. \(\mathrm{PH}_{3}, \mathrm{NH}_{3}\)

Order the following species with respect to carbon-oxygen bond length (longest to shortest). $$ \mathrm{CO}, \quad \mathrm{CO}_{2}, \quad \mathrm{CO}_{3}^{2-}, \quad \mathrm{CH}_{3} \mathrm{OH} $$ What is the order from the weakest to the strongest carbonoxygen bond? \(\left(\mathrm{CH}_{3} \mathrm{OH}\right.\) exists as \(\mathrm{H}_{3} \mathrm{C}-\mathrm{OH}\).)

Arrange the atoms and/or ions in the following groups in order of decreasing size. a. \(\mathrm{O}, \mathrm{O}^{-}, \mathrm{O}^{2-}\) b. \(\mathrm{Fe}^{2+}, \mathrm{Ni}^{2+}, \mathrm{Zn}^{2+}\) c. \(\mathrm{Ca}^{2+}, \mathrm{K}^{+}, \mathrm{Cl}^{-}\)

Which compound in each of the following pairs of ionic substances has the most exothermic lattice energy? Justify your answers. a. \(\mathrm{LiF}, \mathrm{CsF}\) b. NaBr, NaI c. \(\mathrm{BaCl}_{2}, \mathrm{BaO}\) d. \(\mathrm{Na}_{2} \mathrm{SO}_{4}, \mathrm{CaSO}_{4}\) e. \(\mathrm{KF}, \mathrm{K}_{2} \mathrm{O}\) f. \(\mathrm{Li}_{2} \mathrm{O}, \mathrm{Na}_{2} \mathrm{~S}\)
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