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Chapter 20: Problem 75

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 or ions that are isoelectronic with the given xenon compounds are: a. Xenon tetroxide (XeO4): Iodine trioxide ion (IO3^-) d. Xenon tetrafluoride (XeF4): Iodine tetrachloride ion (ICl4^-) b. Xenon trioxide (XeO3): Iodine dioxide ion (IO2^-) e. Xenon hexafluoride (XeF6): Iodine hexachloride ion (ICl6^2-) c. Xenon difluoride (XeF2): Iodine oxide ion (IO^-)

Step by step solution

01

1. Calculate total number of valence electrons for xenon compounds.

First, we need to find the total number of valence electrons for each xenon compound using the periodic table. a. Xenon tetroxide (XeO4): Xe = 8 valence electrons, O = 6 valence electrons Total valence electrons = 8 + 4*(6) = 32 d. Xenon tetrafluoride (XeF4): Xe = 8 valence electrons, F = 7 valence electrons Total valence electrons = 8 + 4*(7) = 36 b. Xenon trioxide (XeO3): Xe = 8 valence electrons, O = 6 valence electrons Total valence electrons = 8 + 3*(6) = 26 e. Xenon hexafluoride (XeF6): Xe = 8 valence electrons, F = 7 valence electrons Total valence electrons = 8 + 6*(7) = 50 c. Xenon difluoride (XeF2): Xe = 8 valence electrons, F = 7 valence electrons Total valence electrons = 8 + 2*(7) = 22
02

2. Find iodine compounds or ions that have the same total number of valence electrons.

Now, we will find the iodine compounds or ions that have the same total number of valence electrons as each xenon compound. a. For XeO4 (32 valence electrons), I = 7 valence electrons ICl3 has 32 valence electrons: 7 + 3*(7) = 28, so it is not isoelectronic with XeO4. IF3 has 32 valence electrons: 7 + 3*(7) = 28, so it is not isoelectronic with XeO4. IO3^- has 32 valence electrons: 7 + 3*(6) + 1 = 32, so it is isoelectronic with XeO4. d. For XeF4 (36 valence electrons), I = 7 valence electrons ICl4^- has 36 valence electrons: 7 + 4*(7) + 1 = 36, so it is isoelectronic with XeF4. b. For XeO3 (26 valence electrons), I = 7 valence electrons ICl^- has 26 valence electrons: 7 + 1*(7) + 1 = 15, so it is not isoelectronic with XeO3. IF^- has 26 valence electrons: 7 + 1*(7) + 1 = 15, so it is not isoelectronic with XeO3. IO2^- has 26 valence electrons: 7 + 2*(6) + 1 = 26, so it is isoelectronic with XeO3. e. For XeF6 (50 valence electrons), I = 7 valence electrons ICl6^2- has 50 valence electrons: 7 + 6*(7) + 2 = 50, so it is isoelectronic with XeF6. c. For XeF2 (22 valence electrons), I = 7 valence electrons ICl^- has 22 valence electrons: 7 + 1*(7) + 1 = 15, so it is not isoelectronic with XeF2. IF^- has 22 valence electrons: 7 + 1*(7) + 1 = 15, so it is not isoelectronic with XeF2. IO^- has 22 valence electrons: 7 + 1*(6) + 1 = 22, so it is isoelectronic with XeF2. To summarize: a. Xenon tetroxide (XeO4): Iodine trioxide ion (IO3^-) d. Xenon tetrafluoride (XeF4): Iodine tetrachloride ion (ICl4^-) b. Xenon trioxide (XeO3): Iodine dioxide ion (IO2^-) e. Xenon hexafluoride (XeF6): Iodine hexachloride ion (ICl6^2-) c. Xenon difluoride (XeF2): Iodine oxide ion (IO^-)

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