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Chapter 20: Problem 67

The xenon halides and oxides are isoelectronic with many other compounds and ions containing halogens. Give a molecule or ion in which iodine is the central atom that is isoelectronic with each of the following. a. xenon tetroxide d. xenon tetrafluoride b. xenon trioxide e. xenon hexafluoride c. xenon difluoride

Short Answer

Expert verified
The iodine-containing molecules and ions isoelectronic with the given xenon compounds are: a. XeO₄ - IO₄⁻ d. XeF₄ - IF₄⁻ b. XeO₃ - IO₃⁻ e. XeF₆ - IF₆⁻ c. XeF₂ - IF₂⁻

Step by step solution

01

Determine the electron count in XeO₄

Xe has 54 electrons, and O has 8 electrons. Since there are 4 O atoms, we have: Electron count = 54 + (4 × 8) = 54 + 32 = 86 electrons
02

Find an iodine-containing molecule or ion with 86 electrons

Iodine (I) has 53 electrons. To reach 86 electrons, we need 33 more electrons. Divide 33 by 8 (number of electrons in O) = 4.125. Thus, we need 4 oxygen atoms and 1 extra electron: Iodine molecule/ion = IO₄⁻ The iodine-containing species that are isoelectronic with XeO₄ are IO₄⁻. d. Xenon tetrafluoride: XeF₄
03

Determine the electron count in XeF₄

Xe has 54 electrons, and F has 9 electrons. Since there are 4 F atoms, we have: Electron count = 54 + (4 × 9) = 54 + 36 = 90 electrons
04

Find an iodine-containing molecule or ion with 90 electrons

Iodine (I) has 53 electrons. To reach 90 electrons, we need 37 more electrons. Divide 37 by 9 (number of electrons in F) = 4.11. Thus, we need 4 fluorine atoms and 1 extra electron: Iodine molecule/ion = IF₄⁻ The iodine-containing species that are isoelectronic with XeF₄ are IF₄⁻. b. Xenon trioxide: XeO₃
05

Determine the electron count in XeO₃

Xe has 54 electrons, and O has 8 electrons. Since there are 3 O atoms, we have: Electron count = 54 + (3 × 8) = 54 + 24 = 78 electrons
06

Find an iodine-containing molecule/ion with 78 electrons

Iodine (I) has 53 electrons. To reach 78 electrons, we need 25 more electrons. Divide 25 by 8 (number of electrons in O) = 3.125. Thus, we need 3 oxygen atoms and 1 extra electron: Iodine molecule/ion = IO₃⁻ The iodine-containing species that are isoelectronic with XeO₃ are IO₃⁻. e. Xenon hexafluoride: XeF₆
07

Determine the electron count in XeF₆

Xe has 54 electrons, and F has 9 electrons. Since there are 6 F atoms, we have: Electron count = 54 + (6 × 9) = 54 + 54 = 108 electrons
08

Find an iodine-containing molecule or ion with 108 electrons

Iodine (I) has 53 electrons. To reach 108 electrons, we need 55 more electrons. Divide 55 by 9 (number of electrons in F) = 6.11. Thus, we need 6 fluorine atoms and 1 extra electron: Iodine molecule/ion = IF₆⁻ The iodine-containing species that are isoelectronic with XeF₆ are IF₆⁻. c. Xenon difluoride: XeF₂
09

Determine the electron count in XeF₂

Xe has 54 electrons, and F has 9 electrons. Since there are 2 F atoms, we have: Electron count = 54 + (2 × 9) = 54 + 18 = 72 electrons
10

Find an iodine-containing molecule/ion with 72 electrons

Iodine (I) has 53 electrons. To reach 72 electrons, we need 19 more electrons. Divide 19 by 9 (number of electrons in F) = 2.11. Thus, we need 2 fluorine atoms and 1 extra electron: Iodine molecule/ion = IF₂⁻ The iodine-containing species that are isoelectronic with XeF₂ are IF₂⁻. In summary, the iodine-containing molecules and ions isoelectronic with the given xenon compounds are: a. XeO₄ - IO₄⁻ d. XeF₄ - IF₄⁻ b. XeO₃ - IO₃⁻ e. XeF₆ - IF₆⁻ c. XeF₂ - IF₂⁻

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