What conclusion can be drawn from the statement that an element has high electron affinity, high electronegativity, and a high ionization energy?

A) The element is most likely from Group 1A or 2A and in period 1 or 2.

B) The element is most likely from Group 2A or 3A and in period 6 or 7.

C) The element is most likely from Group 4A or 5A and in period 4 or 5.

D) The element is most likely from Group 6A or 7A and in period 2 or 3.

D) The element is most likely from Group 6A or 7A and in period 2 or 3.

Explanation:

Electronegativity of an atom is the tendency of an atom to attract shared paired of electron to itself. Electronegativity increase across the period from left to right. The ability of an atom to attract electron to itself is electronegativity. Group 7A and 6A elements can easily attract atoms to itself so they are highly electronegative. The most electronegative element in the periodic table is fluorine. Group 6A and 7A is likely to have high electronegativity.

Electron affinity of an atom is the amount of energy release when an atom gains electron. Generally, when atom gains electron they become negatively charged. Group 6A and 7A elements have high electron affinity.

Ionization energy is the energy required to remove one or more electron from a neutral atom to form cations. ionization energy of group 7A and 6A are usually high because the energy required to remove these electron is usually very high. The elements in this groups usually gain electron easily so the energy to remove electron is very high.