If there is unequal sharing among electrons, which of the following
elements would the electrons be most attracted to? (Hint: Look at their locations on the periodic table.)
O tin (Sn)
O arsenic (As)
O sulfur (S)
O fluorine (F)

D. Fluorine.

Explanation:

For an atom to accept an electron, from another atom, it must have high electron affinity compared to the other elements.

Large atoms then to have high electron affinity compared to smaller atoms and most large atoms are non metals while elements with smaller atomic radius are metals. Tin(Sn), Arsenic(As) are metals and they have lower electrons affinity compared to Sulfur (S) and Fluorine (F).

Fluorine have a high electron affinity than Sulfur and hence has a larger atomic radius and can easily draw most of the electrons shared between the two atoms.

There's a trend to electron affinity and I.e it increases down the period and decreases down the group.

Most group (VII)A elements form electrovalent compounds due to their tendency to pull the shared electron towards them(high electron affinity) compared to Sulfur (a group VIA) element.

(75°f − 32) × 5/9 = 23.889°c