Question

part 2 (1 point) label the most polar bond in ch₃oh by dragging the δ⁺ (partial positive charge) and δ⁻ (partial negative charge) labels to the correct atoms of the bond. note that for each bond, only one of each atom is labelled, and not all atoms will have a label.

Explanation:

Step1: Recall electronegativity concept

Electronegativity is the ability of an atom to attract electrons in a covalent - bond. The greater the electronegativity difference between two atoms in a bond, the more polar the bond.

Step2: Identify electronegativities of atoms in CH₃OH

The electronegativities of C (carbon) is approximately 2.5, H (hydrogen) is approximately 2.1, and O (oxygen) is approximately 3.5.

Step3: Calculate electronegativity differences

• For C - H bond: $\Delta\chi=|2.5 - 2.1| = 0.4$.
• For C - O bond: $\Delta\chi=|3.5 - 2.5| = 1.0$.
• For O - H bond: $\Delta\chi=|3.5 - 2.1| = 1.4$.

The O - H bond has the largest electronegativity difference.

Step4: Assign partial charges

Oxygen is more electronegative than hydrogen. So, the oxygen atom in the O - H bond has a partial negative charge ($\delta^-$) and the hydrogen atom has a partial positive charge ($\delta^+$).

Answer:

$\delta^+$ on H atom of O - H bond, $\delta^-$ on O atom of O - H bond.