Question

selected properties of antimony (sb) and iodine (i) are listed in the table below.

element	atomic radius (pm)	first ionization energy (kj/mol)	electron affinity (kj/mol)	electronegativity
i	140	1008	-295	?

which predictions can most likely be made?
sb has a lower ionization energy but a higher electronegativity than i.
sb has a lower ionization energy but a lower electronegativity than i.
sb has a higher ionization energy but a lower electronegativity than i.
sb has a lower ionization energy and a lower electronegativity than i.
sb has a higher ionization energy and a higher electronegativity than i.

Explanation:

Step1: Analyze ionization - energy trend

In the periodic table, as we move across a period from left - to - right, the first ionization energy generally increases. Antimony (Sb) is in Group 15 and Iodine (I) is in Group 17. Iodine is to the right of antimony in the same period. So, Sb has a lower first ionization energy than I.

Step2: Analyze electronegativity trend

Electronegativity also increases across a period from left - to - right. Since Iodine is to the right of antimony in the same period, Sb has a lower electronegativity than I.

Answer:

Sb has a lower ionization energy and a lower electronegativity than I.