The electron pair in a H-F bond could be considered___.

a) closer to H because hydrogen has a larger radius and thus exerts greater control over the shared electron pair.

b) closer to F because fluorine has a higher electronegativity than hydrogen.

c) closer to H because hydrogen has a lower electronegativity than fluorine.

d) an inadequate model since the bond is ionic.

Question

Tatiana Santos

Chemistry

22 October, 04:10

The electron pair in a H-F bond could be considered___.

a) closer to H because hydrogen has a larger radius and thus exerts greater control over the shared electron pair.

b) closer to F because fluorine has a higher electronegativity than hydrogen.

c) closer to H because hydrogen has a lower electronegativity than fluorine.

d) an inadequate model since the bond is ionic.

+3

Answers (1)

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Tristan Tanner · Answer 1

Answer: b) closer to F because fluorine has a higher electronegativity than hydrogen.

Explanation:

Electronegativity is defined as the property of an element to attract a shared pair of electron towards itself.

A polar covalent bond is defined as the bond which is formed when there is a difference of electronegativities between the atoms.

Non-polar covalent bond is defined as the bond which is formed when there is no difference of electronegativities between the atoms.

electronegativity of flourine = 3.98

electronegativity of hydrogen = 2.1

As electronegativity of flourine is greater than that of electronegativity of hydrogen, the electron pair lie towards flourine, thus creating a partial negative charge on flourine and a partial positive charge on hydrogen.