Which of the following compounds would you expect to have a dipole moment? If the molecule has a dipole moment, specify its direction.
(a) BF3
(b) H2O
(c) CH4
(d) CH3Cl
(e) CH2O
(f) HCN
Sample Solution (a) Boron trifluoride is planar with 120° bond angles. Although each boron-fluorine bond is polar, their combined effects cancel and the molecule has no dipole moment.
We need at least 10 more requests to produce the solution.
0 / 10 have requested this problem solution
The more requests, the faster the answer.