11. Bonding & Molecular Structure

Which of the following is the most polar bond?

What is the percent ionic character of a 125 pm bond which has a bond dipole of 4.5 D?

Two dichloroethylene molecules with the same chemical formula 1C2H2Cl22, but different arrangements of atoms are shown. (b) Which form of dichloroethylene has a dipole moment of 2.39 D, and which has a dipole moment of 0.00 D?

(a) Does CS2 have a dipole moment? If so, in which direction does the net dipole point?

(b) It turns out that ozone, O3, has a small dipole moment. How is this possible, given that all the atoms are the same?

(c) Does the molecule BF2Cl have a dipole moment?

Match the following descriptions with the type of bond (ionic, nonpolar covalent, covalent). (a) One or more electrons are transferred from a metal to a nonmetal atom.

Which of the following bonds are polar? (a) C¬O, (b) Sl¬F, (c) N¬Cl, (d) C¬Cl. Which is the more electronegative atom in each polar bond?

Arrange the bonds in each of the following sets in order of increasing polarity: (c) C¬S, B¬F, N¬O.

Arrange the bonds in each of the following sets in order of increasing polarity: (b) O¬Cl, S¬Br, C¬P

(b) If you were to put HBr under very high pressure, so its bond length decreased significantly, would its dipole moment increase, decrease, or stay the same, if you assume that the effective charges on the atoms do not change?

(a) From the data in Table 8.2, calculate the effective charges on the Br atom of the HBr molecule in units of the electronic charge, e.

The iodine monobromide molecule, IBr, has a bond length of 249 pm and a dipole moment of 1.21 D. (a) Which atom of the molecule is expected to have a negative charge?

Which of the following substances contain bonds that are largely ionic? (a) HF (b) HI (c) PdCl2 (d) BBr3 (e) NaOH (f) CH3Li

Show the direction of polarity for each of the bonds in Problem 7.51 using the notation. (b) Si-Li or Si-Cl

Which of the substances CdBr2, P4, BrF3, MgO, NF3, BaCl2, POCl3, and LiBr contain bonds that are: (b) nonpolar covalent?

(b) What would you expect for the magnitude and direction of the bond dipoles in this series?

Which of the substances S8, CaCl2, SOCl2, NaF, CBr4, BrCl, LiF, and AsH3 contain bonds that are: (a) largely ionic? (b) nonpolar covalent? (c) polar covalent?

Determine if a bond between each pair of atoms would be pure covalent, polar covalent, or ionic. a. Br and Br b. C and Cl c. C and S d. Sr and O

Order the following compounds according to the increasing ionic character of their bonds: CCl4, BaCl2, TiCl3, ClO2.

Draw the Lewis structure for BrF with an arrow representing the dipole moment.

Consider the collection of nonmetallic elements: B, As, O, and I. (a) Which two would form the most polar single bond?

The substance chlorine monoxide, ClO(g), is important in atmospheric processes that lead to depletion of the ozone layer. The ClO molecule has an experimental dipole moment of 1.24 D, and the Cl¬O bond length is 160 pm. (b) Based on the electronegativities of the elements, which atom would you expect to have a partial negative charge in the ClO molecule?

(c) The measured dipole moment of BrCl is 0.57 D. If you assume the bond length in BrCl is the sum of the atomic radii, what are the partial charges on the atoms in BrCl using the experimental dipole moment?

(b) Using these partial charges and the atomic radii given in Figure 7.8, estimate the dipole moment of the molecule.

The O¬H bond lengths in the water molecule 1H2O2 are 96 pm, and the H¬O¬H angle is 104.5°. The dipole moment of the water molecule is 1.85 D. (b) Calculate the magnitude of the bond dipole of the O¬H bonds. (Note: You will need to use vector addition to do this.)

A polar covalent bond would form in which of the following pairs of atoms

Which bond would you expect to be the most polar?

For each bond, show the direction of polarity by selecting the correct partial charges.

Determine whether a bond between each pair of atoms would be pure covalent, polar covalent, or ionic.

Which of the following bonds would be the most polar without being considered ionic?

A polar covalent bond would form in which one of the following pairs of atoms?