Question

Use the symbol ${\mathit{\delta }}^{\mathbf{+}}$and ${\mathit{\delta }}^{\mathbf{+}}$to show the direction of polarity of the bond between carbon and oxygen.

$\mathit{C}{\mathit{H}}_{\mathbf{3}}\mathbf{-}\mathit{O}\mathit{H}$

Short answer

$H_3{C}^{\delta +}-O^{\delta -}H$

Step-by-step solution

Defining bond polarity

The distribution of positive and negative electrical charges over a bond is known as bond polarity. The bond polarity can be determined by comparing the difference in electronegativity between the atoms.

" width="9" height="19" role="math" style="max-width: none; vertical-align: -4px;" localid="1664883424373">Step2: Determining of role="math" localid="1664883414773" δ+ and δ+ over a bond.

The electronegativity of oxygen is 3.44 and that of carbon is 2.5. Out of two, oxygen being more electronegative develops a partial negative charge and carbon develops a partial positive charge. This separation in their charges makes them polar.

The direction of polarity is shown below.

The direction is always shown from positive to negative polarity. This is called the dipole moment