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Chapter 9: Problem 67

Of the noble gases, only \(\mathrm{Kr}, \mathrm{Xe},\) and \(\mathrm{Rn}\) are known to form a few compounds with \(\mathrm{O}\) and/or \(\mathrm{F}\). Write Lewis structures for the following molecules: (a) \(\mathrm{XeF}_{2},\) (b) \(\mathrm{XeF}_{4}\), (c) \(\mathrm{XeF}_{6}\), (d) \(\mathrm{XeOF}_{4}\), (e) \(\mathrm{XeO}_{2} \mathrm{~F}_{2}\). In each case Xe is the central atom.

Short Answer

Expert verified
The Lewis structures for the given molecules where in case of each molecule Xe is the central atom are: XeF2, Xe with 3 lone pairs surrounded by two F atoms, each with 3 lone pairs; XeF4, Xe in center with 2 lone pairs, surrounded by 4 F atoms; XeF6, Xe in center with 1 lone pair, surrounded by 6 F atoms; XeOF4, Xe in center with 1 lone pair, surrounded by 4 F atoms and 1 O atom; XeO2F2, Xe in center with 2 lone pairs, surrounded by 2 F atoms and 2 O atoms.

Step by step solution

01

Draw the Lewis structure for XeF2

For XeF2, there are a total of 8 (from Xe) + 7*2 (from two F atoms) = 22 valence electrons. To get a stable configuration, there are 3 lone pairs in Xe apart from the two F atoms. Hence, the Lewis structure for XeF2 will be: Xe with 3 lone pairs in its orbit, surrounded by two F atoms, each of which also has 3 lone pairs. Xe shares 1 pair with each F.
02

Draw the Lewis structure for XeF4

For XeF4, the total number of valence electrons is 36. Here, Xe has 2 lone pairs and it is surrounded by 4 F atoms. Each F atom has 3 lone pairs, and Xe shares 1 pair with each F atom. Thus, the Lewis structure for XeF4 has Xe at the center with 2 lone pairs, surrounded by 4 F atoms.
03

Draw the Lewis structure for XeF6

For XeF6, there are total 8+7*6=50 valence electrons. Xe has 1 lone pair and it is surrounded by 6 F atoms. Each F atom has 3 lone pairs, and Xe shares 1 pair with each F. Thus, the Lewis structure for XeF6 has Xe at the center with 1 lone pair, surrounded by 6 F atoms.
04

Draw the Lewis structure for XeOF4

For XeOF4, the total valence electrons are 8+6+7*4 = 40. Xe has 1 lone pair and is surrounded by 4 F atoms and 1 O atom. Each F atom has 3 lone pairs and O has 2 lone pairs. Xe shares 1 pair with each F and O atom. Hence, Lewis structure has Xe at the center with 1 lone pair, surrounded by 4 F atoms and 1 O atom.
05

Draw the Lewis structure for XeO2F2

For XeO2F2, total valence electrons = 8+6*2+7*2=34. Xe has 2 lone pairs and it is surrounded by 2 F atoms and 2 O atoms. Each F atom has 3 lone pairs and each O atom has 2 lone pairs. Xe shares 1 pair with each F and O atom. Thus, Lewis structure for XeO2F2 has Xe in center with 2 lone pairs, surrounded by 2 F atoms and 2 O atoms.

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Most popular questions from this chapter

Most organic acids can be represented as \(\mathrm{RCOOH}\) where \(\mathrm{COOH}\) is the carboxyl group and \(\mathrm{R}\) is the rest of the molecule. (For example, \(\mathrm{R}\) is \(\mathrm{CH}_{3}\) in acetic acid, \(\mathrm{CH}_{3} \mathrm{COOH} .\) ) (a) Draw a Lewis structure for the carboxyl group. (b) Upon ionization, the carboxyl group is converted to the carboxylate group, \(\mathrm{COO}^{-}\). Draw resonance structures for the carboxylate group.

Because fluorine has seven valence electrons \(\left(2 s^{2} 2 p^{5}\right),\) seven covalent bonds in principle could form around the atom. Such a compound might be \(\mathrm{FH}_{7}\) or \(\mathrm{FCl}_{7}\). These compounds have never been prepared. Why?

In 1999 an unusual cation containing only nitrogen \(\left(\mathrm{N}_{5}^{+}\right)\) was prepared. Draw three resonance structures of the ion, showing formal charges. (Hint: The \(\mathrm{N}\) atoms are joined in a linear fashion.)

Arrange the following bonds in order of increasing ionic character: carbon to hydrogen, fluorine to hydrogen, bromine to hydrogen, sodium to chlorine, potassium to fluorine, lithium to chlorine.

Methyl isocyanate \(\left(\mathrm{CH}_{3} \mathrm{NCO}\right)\) is used to make certain pesticides. In December \(1984,\) water leaked into a tank containing this substance at a chemical plant, producing a toxic cloud that killed thousands of people in Bhopal, India. Draw Lewis structures for \(\mathrm{CH}_{3} \mathrm{NCO},\) showing formal charges.
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