* Electronegativity: Electronegativity is the ability of an atom to attract electrons in a bond. The higher the electronegativity, the stronger the pull on the shared electrons.

* Periodic Trends: Electronegativity increases as you move across a period (left to right) and decreases as you move down a group (top to bottom) on the periodic table.

Looking at the list:

* Chlorine (Cl), Fluorine (F), Bromine (Br), Iodine (I): These are all halogens and are located in the same group. Iodine is at the bottom of the group, meaning it has the lowest electronegativity. This means that in a bond, iodine will have the weakest pull on shared electrons, resulting in the largest partial negative charge.

* Carbon (C): Carbon is not a halogen and has a lower electronegativity than all the halogens.

Therefore, iodine will have the largest partial negative charge when compared to the other listed elements.