In each of the following pairs of bonds, which bond is more polar? Show the direction of the dipole moment for the more polar bond.

(a) H–C or H–N

(b) O–C or Cl–N

(c) S–O or S–F

Strategy

Use the table of electronegativities in Figure 9.9 to determine the electronegativity difference. The more polar bond will be the one with the larger difference in electronegativity. The arrow points toward the more electronegative element and it’s length is related to the electronegativity difference.

Figure 9.9

Transcribed Image Text:

H 2.1 Li Be 1.0 1.5 2.0 Na Mg 0.9 Al Si P S Cl 1.2 1.5 1.8 2.1 2.5 3.0 A EES C N O F 2.5 3.0 3.5 4.0 K Ca Ga Ge As Se Br 0.8 1.0 1.8 1.8 2.0 2.4 2.8 Sn Sb 1.8 Rb Sr In 0.8 0.9 1.7 Cs Ba TI Pb 0.7 0.9 1.8 1.9 1.9 2.0 2.2 Po At Te I 2.5 1.9 2.1 H Figure 9.9 Electronegativities of representative elements. Li Na Be K Mg B Rb Al Ca Cs C с Sr Ga Si Ba N In Ge P Sn T1 S As F Sb Pb Cl Se Br Te Bi I Po At