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Chapter 9: Problem 28

Draw the Lewis structure for each of the following molecules or ions, and predict their electron-domain and molecular geometries: (a) \(\mathrm{AsF}_{3},\) (b) \(\mathrm{CH}_{3}^{+},\) (c) \(\mathrm{BrF}_{3},\) (d) \(\mathrm{ClO}_{3}^{-},\) (e) \(\mathrm{XeF}_{2}\), (f) \(\mathrm{BrO}_{2}^{-}\).

Short Answer

Expert verified
(a) AsF3: Lewis structure has As as the central atom with three single bonds to F atoms and two lone pairs on As. Electron-domain geometry is trigonal bipyramidal, and molecular geometry is T-shaped. (b) CH3+: Lewis structure has C as the central atom with three single bonds to H atoms. Electron-domain geometry and molecular geometry are both trigonal planar. (c) BrF3: Lewis structure has Br as the central atom with three single bonds to F atoms and two lone pairs on Br. Electron-domain geometry is trigonal bipyramidal, and molecular geometry is T-shaped. (d) ClO3-: Lewis structure has Cl as the central atom with three single bonds to O atoms and one lone pair on Cl. Electron-domain geometry is tetrahedral, and molecular geometry is trigonal pyramidal. (e) XeF2: Lewis structure has Xe as the central atom with two single bonds to F atoms and three lone pairs on Xe. Electron-domain geometry is trigonal bipyramidal, and molecular geometry is linear. (f) BrO2-: Lewis structure has Br as the central atom with two single bonds to O atoms and one lone pair on Br. Electron-domain geometry is tetrahedral, and molecular geometry is trigonal pyramidal.

Step by step solution

01

(a) AsF3 Lewis structure, electron-domain and molecular geometry

1. Count valence electrons: As has 5 valence electrons and F has 7. There are 3 F atoms, so the total number of valence electrons is 5 + (3 × 7) = 26. 2. As the central atom is As, we will connect each F atom to As with single bonds. 3. As the octet rule requires 8 electrons, there are 8 × 4 = 32 needed for complete octets. We have 26, so we will put the remaining 6 electrons on the As atom as lone pairs. 4. The electron-domain geometry is trigonal bipyramidal, with three bonding pairs and two lone pairs in the equatorial positions. This results in a molecular geometry of T-shaped.
02

(b) CH3+ Lewis structure, electron-domain and molecular geometry

1. Count valence electrons: C has 4 valence electrons and H has 1. There are 3 H atoms and a positive charge, so the total number of valence electrons is 4 + (3 × 1) - 1 = 6. 2. C is the central atom. Connect each H atom to the central C atom with single bonds. 3. All atoms have their required number of electrons, no additional electrons are needed. 4. The electron-domain geometry is trigonal planar, as there are three bonding pairs and no lone pairs. This results in a molecular geometry of trigonal planar.
03

(c) BrF3 Lewis structure, electron-domain and molecular geometry

1. Count valence electrons: Br has 7 valence electrons and F has 7. There are 3 F atoms, so the total number of valence electrons is 7 + (3 × 7) = 28. 2. Br is the central atom. Connect each F atom to the central Br atom with single bonds. 3. We need 8 × 4 = 32 electrons for complete octets, and we have 28. We will put the remaining 4 electrons on the Br atom as lone pairs. 4. The electron-domain geometry is trigonal bipyramidal, with three bonding pairs and two lone pairs in the equatorial positions. This results in a molecular geometry of T-shaped.
04

(d) ClO3- Lewis structure, electron-domain and molecular geometry

1. Count valence electrons: Cl has 7 valence electrons and O has 6. There are 3 O atoms and a negative charge, so the total number of valence electrons is 7 + (3 × 6) + 1 = 26. 2. Cl is the central atom. Connect each O atom to the central Cl atom with single bonds. 3. We need 8 × 4 = 32 electrons for complete octets, and we have 26. We will distribute the remaining 6 electrons as lone pairs on O atoms. 4. The electron-domain geometry is tetrahedral, with three bonding pairs and one lone pair on the central atom. This results in a molecular geometry of trigonal pyramidal.
05

(e) XeF2 Lewis structure, electron-domain and molecular geometry

1. Count valence electrons: Xe has 8 valence electrons and F has 7. There are 2 F atoms, so the total number of valence electrons is 8 + (2 × 7) = 22. 2. Xe is the central atom. Connect each F atom to the central Xe atom with single bonds. 3. We need 8 × 3 = 24 electrons for complete octets, and we have 22. We will put the remaining 2 electrons on the Xe atom as lone pairs. 4. The electron-domain geometry is trigonal bipyramidal, with two bonding pairs and three lone pairs in the axial positions. This results in a molecular geometry of linear.
06

(f) BrO2- Lewis structure, electron-domain and molecular geometry

1. Count valence electrons: Br has 7 valence electrons and O has 6. There are 2 O atoms and a negative charge, so the total number of valence electrons is 7 + (2 × 6) + 1 = 20. 2. Br is the central atom. Connect each O atom to the central Br atom with single bonds. 3. We need 8 × 3 = 24 electrons for complete octets, and we have 20. We will distribute the remaining 4 electrons as lone pairs on O atoms. 4. The electron-domain geometry is tetrahedral, with three bonding pairs and one lone pair on the central atom. This results in a molecular geometry of trigonal pyramidal.

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Most popular questions from this chapter

The orbital diagram that follows presents the final step in the formation of hybrid orbitals by a silicon atom. What type of hybrid orbital is produced in this hybridization? [Section 9.5\(]\)

In ozone, \(\mathrm{O}_{3},\) the two oxygen atoms on the ends of the molecule are equivalent to one another. (a) What is the best choice of hybridization scheme for the atoms of ozone? (b) For one of the resonance forms of ozone, which of the orbitals are used to make bonds and which are used to hold nonbonding pairs of electrons? (c) Which of the orbitals can be used to delocalize the \(\pi\) electrons? (d) How many electrons are delocalized in the \(\pi\) system of ozone?

The molecule shown here is difluoromethane \(\left(\mathrm{CH}_{2} \mathrm{~F}_{2}\right),\) which is used as a refrigerant called R-32. (a) Based on the structure, how many electron domains surround the \(\mathrm{C}\) atom in this molecule? (b) Would the molecule have a nonzero dipole moment? (c) If the molecule is polar, in what direction will the overall dipole moment vector point in the molecule? [Sections 9.2 and 9.3\(]\)

What is the hybridization of the central atom in (a) \(\mathrm{SiCl}_{4}\), (b) HCN, (d) \(\mathrm{TeCl}_{2}\) (c) \(\mathrm{SO}_{3}\)

(a) Methane \(\left(\mathrm{CH}_{4}\right)\) and the perchlorate ion \(\left(\mathrm{ClO}_{4}^{-}\right)\) are both described as tetrahedral. What does this indicate about their bond angles? (b) The \(\mathrm{NH}_{3}\) molecule is trigonal pyramidal, while \(\mathrm{BF}_{3}\) is trigonal planar. Which of these molecules is flat?
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