Question

use the following data to determine the least to most polar molecule
n-o h-f h-cl n-n

Explanation:

Step1: Recall Electronegativity Difference

Polarity depends on electronegativity difference ($\Delta EN$) between atoms. Larger $\Delta EN$ means more polar. For a bond $A - B$, $\Delta EN = |EN_A - EN_B|$.

Step2: Find Electronegativities (from Periodic Table)

• $N - N$: $EN_N = 3.0$ (approx). $\Delta EN = |3.0 - 3.0| = 0$ (non - polar, least polar).
• $N - O$: $EN_N = 3.0$, $EN_O = 3.5$. $\Delta EN = |3.0 - 3.5| = 0.5$.
• $H - Cl$: $EN_H = 2.1$, $EN_Cl = 3.0$. $\Delta EN = |2.1 - 3.0| = 0.9$.
• $H - F$: $EN_H = 2.1$, $EN_F = 4.0$. $\Delta EN = |2.1 - 4.0| = 1.9$ (most polar).

Step3: Order by $\Delta EN$ (Least to Most Polar)

Sort the bonds by increasing $\Delta EN$: $N - N$ (0) < $N - O$ (0.5) < $H - Cl$ (0.9) < $H - F$ (1.9).

Answer:

Least to most polar: $N - N$, $N - O$, $H - Cl$, $H - F$