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Chapter 7: Q101E (page 405)

The molecule XF3 has a dipole moment. Is X boron or phosphorus?

Short Answer

Expert verified

The molecular structure of \({\rm{P}}{{\rm{F}}_{\rm{3}}}\)is not symmetrical and hence dipole does not cancels out.

Step by step solution

01

Concept Introduction

It is a measure of the system's overall polarity .The electric dipole moment gives the separation of positive and negative electrical charges inside a system.

02

Find lone pair and dipole moment

There are no lone pairs in\({\rm{B}}{{\rm{F}}_{\rm{3}}}\),however one lone pair is present in\({\rm{P}}{{\rm{F}}_{\rm{3}}}\).

Therefore, as a result, the molecular structure of \({\rm{P}}{{\rm{F}}_{\rm{3}}}\) is asymmetrical, and the dipole does not cancel out.

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Most popular questions from this chapter

Describe the molecular structure around the indicated atom or atoms:

  1. The sulfur atom in sulfuric acid, H2SO4 [ (HO)2 SO2]

  2. The chlorine atom in chloric acid, HClO3 [HOClO2]

  3. The oxygen atom in Hydrogen peroxide, HOOH

  4. The nitrogen atom in nitric acid, HNO3 [HONO2]

  5. The oxygen atom in OH group in nitric acid, HNO3 [HONO2]

  6. The central oxygen atom in the ozone molecule, O3

  7. Each of the carbon atoms in the propyne, CH3 CCH

  8. The carbon atom in Freon, CCl2 F2

  9. each of the carbon atoms in allene H2CCCH2

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.

What feature of a Lewis structure can be used to tell if a molecule鈥檚 (or ion鈥檚) electron-pair geometry and molecular structure will be identical?

Write the electron configuration for the monatomic ions formed from the following elements (which form the greatest concentration of monatomic ions in seawater): (a) \({\rm{Cl}}\) (b) \({\rm{Na}}\) (c) \({\rm{Mg}}\)(d) \({\rm{Ca}}\) (e) \({\rm{K}}\) (f) \({\rm{Br}}\) (g) \({\rm{Sr}}\) (h) \({\rm{F}}\).

In terms of the bonds present, explain why acetic acid, \(C{H_3}C{O_2}H\), contains two distinct types of carbon-oxygen bonds, whereas the acetate ion, formed by loss of a hydrogen ion from acetic acid, only contains one type of carbon-oxygen bond. The skeleton structures of these species are shown:
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