The electron pair in a h-f bond could be
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.

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.