Francium (Fr)
Cs (cesium) is most likely to donate one electron as it is classified as an alkali metal with a single valence electron in its outermost energy level.
Chlorine is a nonmetal. It is only one electron short of a noble gas electron configuration and is much more likely to abstract an electron from some other element than to donate one to some other element.
Elements in the 1st group have 1 valence electron. So they are likely to donate 1 electron to get more stable. potassium, rubidium and cesium are likely to donate 1 electron.
Oxygen is electron withdrawing because it is electronegative and tends to attract electrons towards itself in a chemical bond. This results in oxygen being less likely to donate electrons and more likely to withdraw them.
Chlorine is more likely to accept electrons than donate them due to its electronegativity. In its natural state, chlorine tends to gain one electron to achieve a stable electron configuration, forming a chloride ion.
Arsenic.
When it is stable. that is, all of it's electron shells are fully occupied.
The element with the atomic number 17, which is chlorine, would most likely have the Lewis dot symbol because it typically gains one electron to achieve a stable electron configuration.
The element is likely lithium (Li). Lithium has 3 electron energy levels (shells) and 3 valence electrons in its outermost energy level.
Helium (He) is the element that has a negative electron affinity. This means that it is less likely to gain an electron compared to other elements listed (Kr, O, Ca, and Mg) which have positive electron affinities.
To become more stable, fluorine is most likely to gain 1 electron and form F- ion.
The element with a valence electron configuration of ns2 np4 is sulfur (S). Since it needs to gain 2 electrons to achieve a stable electron configuration, it is most likely to form an ion with a charge of -2.