Question

Consider the following electronegativity values:
H = 2.1, Cl = 3.0, F = 4.0
Which molecule below would you expect to have the more polar bond?

a) HCl b) H2 c) HF d) Cl2 e) F2

Answer 1

Answer: option C. HF

Explanation: A polar bond is a covalent bond between two atoms where the electrons forming the bond are unequally distributed. Fluorine is more electronegative than hydrogen so the electrons in the bond are more closely associated with the fluorine atom than with the hydrogen atom.

Answer 2

Given the electronegativity values, the molecule with the most polar bond is d) HF.

The polarity of a bond depends on the difference in the electronegativities of the elements that form it. The higher the difference in their electronegativities, the more polar the bond.

Let's calculate the difference in the electronegativities for the following molecules.

a) HCl

$\Delta EN = |EN(H)- EN(Cl)| = |2.1-3.0| = 0.9$

b) H₂

$\Delta EN = |EN(H)- EN(H)| = |2.1-2.1| = 0.0$

c) HF

$\Delta EN = |EN(H)- EN(F)| = |2.1-4.0| = 1.9$

d) Cl₂

$\Delta EN = |EN(Cl)- EN(Cl)| = |3.0-3.0| = 0.0$

e) F₂

$\Delta EN = |EN(F)- EN(F)| = |4.0-4.0| = 0.0$

Given the electronegativity values, the molecule with the most polar bond is d) HF.

Learn more: https://brainly.com/question/24775418