Question

Which of the following molecules would one expect to have a non-polar covalent bond?
a. HCI
b. F2
c. HF
d CIF

Answer 1

b. F₂ have a polar covalent bond

Explanation:

The type of bond depends on the difference of the electronegativity of the two elements.

if the electronegativity difference is under 0.4 the bond is non-polar covalent

if the electronegativity difference is between 0.4 and 1.7 the bond is polar covalent

if the electronegativity difference is greater 1.7 the bond is ionic

a. HCl

electronegativity of Cl - electronegativity of H = 3 - 2.2 = 0.8, so the bond is polar covalent

b. F₂

electronegativity of F - electronegativity of F = 4 - 4 = 0 , so the bond is non-polar covalent

c. HF

electronegativity of F - electronegativity of H = 4 - 2.2 = 1.8, in this case because non-metals are involved in the bond we consider this to be a polar covalent bond.

d. ClF

electronegativity of F - electronegativity of Cl = 4 - 3 = 1, so the bond is polar covalent

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Answer 2

A covalent bond is the sharing of electron pairs between the atoms of the elements in a compound. Fluorine $(\rm F_{2})$ will have a non-polar covalent bond.

What is non-polar covalent bond?

A non-polar covalent bond is the sharing of the electrons equally between the two atoms of the molecules, while polar is the sharing of the electrons unequally between the atoms.

The electronegativity of the element also plays role in the polarity and non-polarity of the atom or the molecule. The electronegativity difference below 0.4 results in non-polar bonds while between 0.4 and 1.7 results in polar bonds.

The electronegativity difference of the fluorine is zero while that of the hydrochloric acid, hydrogen fluoride and chlorine monofluoride is 0.8, 1.8 and 1 respectively.

Therefore, option b. $\rm F_{2}$ will have a non-polar covalent bond.

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