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Chapter 7: Q94E (page 403)

Predict the electron pair geometry and the molecular structure of each of the following ions:

  1. \({{\rm{H}}_{\rm{3}}}{{\rm{O}}^{\rm{ + }}}\,\)
  2. \({\rm{PC}}{{\rm{l}}_{\rm{4}}}{\rm{ - }}\)
  3. \({\rm{SnC}}{{\rm{l}}_{\rm{3}}}^{\rm{ - }}\)
  4. \({\rm{BrC}}{{\rm{l}}_{\rm{4}}}^{\rm{ - }}\)
  5. \({\rm{IC}}{{\rm{l}}_{\rm{3}}}\)
  6. \({\rm{Xe}}{{\rm{F}}_{\rm{4}}}\)
  7. \({\rm{S}}{{\rm{F}}_{\rm{2}}}\)

Short Answer

Expert verified

Electron-pair geometry considers the placement of all electrons. Molecular structure considers only the bonding-pair geometry.

Step by step solution

01

Concept Introduction

The three-dimensional arrangement of atoms in a molecule is predicted by the VSEPR theory. It states that valence electrons will adopt an electron-pair shape that reduces repulsions between high-electrons-density locations (bonds and/or lone pairs).

02

Find the electron pair geometry and the molecular structure

Therefore, the arrangement of all electrons is taken into account in electron-pair geometry. Only the bonding-pair geometry is taken into account in molecular structure.

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Most popular questions from this chapter

A molecule with the formula\({\rm{A}}{{\rm{B}}_{\rm{3}}}\), in which A and B represent different atoms, could have one of three different shapes. Sketch and name the three different shapes that this molecule might have. Give an example of a molecule or ion that has each shape.

Sodium nitrite, which has been used to preserve bacon and other meats, is an ionic compound. Write the resonance forms of the nitrite ion, \({\rm{NO}}_{\rm{2}}^{\rm{ - }}\).

Predict the electron pair geometry and the molecular structure of each of the following:

  1. \({\rm{IO}}{{\rm{F}}_{\rm{5}}}\)(I is the central atom)
  2. \({\rm{POC}}{{\rm{l}}_{\rm{3}}}\)(P is the central atom)
  3. \({\rm{C}}{{\rm{l}}_{\rm{2}}}{\rm{SeO}}\)(Se is the central atom)
  4. \({\rm{ClS}}{{\rm{O}}^{\rm{ + }}}\)(S is the central atom)
  5. \({{\rm{F}}_{\rm{2}}}{\rm{SO}}\)(S is the central atom)
  6. \({\rm{N}}{{\rm{O}}_{\rm{2}}}^{\rm{ - }}\)
  7. \({\rm{SiO}}_{\rm{4}}^{{\rm{4 - }}}\)

Which of these molecules and ions contain polar bonds? Which of these molecules and ions have dipole moments?

  1. \({{\rm{H}}_{\rm{3}}}{{\rm{O}}^{\rm{ + }}}\)
  2. \({\rm{PC}}{{\rm{l}}_{\rm{4}}}^{\rm{ - }}\)
  3. \({\rm{SnCl}}_{\rm{3}}^{\rm{ - }}\)
  4. \({\rm{BrCl}}_{\rm{4}}^{\rm{ - }}\)
  5. \({\rm{IC}}{{\rm{l}}_{\rm{3}}}\)
  6. \({\rm{Xe}}{{\rm{F}}_{\rm{4}}}\)
  7. \({\rm{S}}{{\rm{F}}_{\rm{2}}}\)

Use the simulation (http://openstaxcollege.org/l/16MolecPolarity) to perform the following exercises for a real molecule. You may need to rotate the molecules in three dimensions to see certain dipoles. (a) Sketch the bond dipoles and molecular dipole (if any) for O3. Explain your observations. (b) Look at the bond dipoles for NH3. Use these dipoles to predict whether N or H is more electronegative. (c) Predict whether there should be a molecular dipole for NH3 and, if so, in which direction it will point. Check the molecular dipole box to test your hypothesis.
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