Q6P. - Organic Chemistry (Mcmurry)

Question

Make three-dimensional drawings of the following molecules, and predict whether each has a dipole moment. If you expect a dipole moment, show its direction.

$\left(\mathbf{a}\right){\mathbf{H}}_{\mathbf{2}}{\mathbf{CPCH}}_{\mathbf{2}}\left(\mathbf{b}\right){\mathbf{CHCl}}_{\mathbf{3}}\left(\mathbf{c}\right){\mathbf{CH}}_{\mathbf{2}}{\mathbf{Cl}}_{\mathbf{2}}\left(\mathbf{d}\right){\mathbf{H}}_{\mathbf{2}}{\mathbf{CPCCl}}_{\mathbf{2}}$

Step-by-Step Solution

Answer

Dipole moment

A dipole moment is defined as a measurement of the separation of the two opposite electrical charges. Dipole moments are a vector quantity. The magnitude is equal to charge multiplied by the distance between the charges and the direction is from negative charge to positive charge.

                                                                $\mathrm{\mu }=\mathrm{q}\times \mathrm{r}$

Where $\mathrm{\mu }$ is the dipole moment, q is the charge, and r is the distance between the charges.

Predicting the net dipole moment of a molecule by drawing its structure

For each bond identify the more electronegative element, and draw a arrow that points from the less electronegative element to the more electronegative element. Estimate the sum of the individual dipole moments to arrive at the dipole moment for the entire molecule.

A,b,c,d should not be included inside the image box