Question

which of the following correctly shows the bond polarity? choose 1 answer: a δ+f−clδ− b δ+o−sδ− c δ+p−nδ− d δ+i−iδ−

Explanation:

Bond polarity is determined by the difference in electronegativity between the two atoms in the bond. The more electronegative atom has a partial negative charge ($\delta -$) and the less electronegative atom has a partial positive charge ($\delta +$). Electronegativity increases across a period and decreases down a group in the periodic table.

• For option A, F is more electronegative than Cl, so it should be $\delta -$ on F and $\delta +$ on Cl.
• For option B, O is more electronegative than S, so it should be $\delta -$ on O and $\delta +$ on S.
• For option C, N is more electronegative than P. So, the partial - positive charge ($\delta +$) will be on P and partial - negative charge ($\delta -$) will be on N, which is correctly shown.
• For option D, since both atoms are I, there is no electronegativity difference and the bond is non - polar.

Answer:

C. $\delta +\text{P}-\text{N}^{\delta -}$