Question

element electronegativity
h 2.2
n 3.0
f 4.0
cl 3.2
se 2.6
i 2.7
based on the information in the table, which of the following arranges the bonds in order of decreasing polarity?
choose 1 answer:
a cl - f > se - n > h - i
b cl - f > h - i > se - n
c h - i > se - n > cl - f
d se - n > h - i > cl - f

Explanation:

Step1: Recall polarity - electronegativity relation

Polarity of a bond is determined by the electronegativity difference between the two atoms in the bond. The greater the electronegativity difference, the more polar the bond.

Step2: Calculate electronegativity differences for Cl - F

For the Cl - F bond: Electronegativity of F = 4.0, electronegativity of Cl = 3.2. Difference $\Delta_1=4.0 - 3.2=0.8$.

Step3: Calculate electronegativity differences for Se - N

For the Se - N bond: Electronegativity of N = 3.0, electronegativity of Se = 2.6. Difference $\Delta_2=3.0 - 2.6 = 0.4$.

Step4: Calculate electronegativity differences for H - I

For the H - I bond: Electronegativity of I = 2.7, electronegativity of H = 2.2. Difference $\Delta_3=2.7 - 2.2=0.5$.

Step5: Compare the differences

Since $0.8>0.5 > 0.4$, the order of bond polarity is Cl - F > H - I > Se - N.

Answer:

B. Cl - F > H - I > Se - N