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

Question

Chemistry

Blake Huff

28 November, 23:33

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

+4

Answers (1)

Know the Answer?

Tyrese Fitzpatrick · 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.

Consider the following electronegativity values:H = 2.1, Cl = 3.0, F = 4.0Which molecule below would you expect to have the more polar bond?a) HCl b) H2 c) HF d) Cl2 e) F2

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