Question

comparing differences in period lorenzo is making a prediction. \i learned that nonmetals increase in reactivity when moving from left to right. so i predict that xenon will be more reactive than iodine.\ is lorenzo correct? if so, why? if not, explain his error.

Explanation:

1. Recall the reactivity trend of nonmetals in the periodic table: For nonmetals (excluding noble gases), reactivity generally increases from left to right across a period because they tend to gain electrons, and the effective nuclear charge increases, making it easier to attract electrons.
2. Identify the elements: Xenon (\(Xe\)) is a noble gas, and iodine (\(I\)) is a nonmetal (halogen). Noble gases have a full valence electron shell, making them extremely unreactive under normal conditions.
3. Analyze Lorenzo's error: He applied the nonmetal reactivity trend (left - to - right increase) to a noble gas. The trend of increasing reactivity for nonmetals across a period does not include noble gases, as noble gases are already stable with a full octet (or duplet for helium) and do not readily react. Iodine, being a halogen, is much more reactive than xenon because it needs one electron to complete its valence shell and is highly electronegative, while xenon has a full valence shell and little tendency to react.

Answer:

Lorenzo is not correct. The trend of nonmetals increasing in reactivity from left to right across a period does not apply to noble gases (like xenon). Noble gases have a full valence electron shell, making them extremely unreactive. Iodine (a halogen, non - noble - gas nonmetal) is more reactive than xenon because iodine needs to gain one electron to complete its valence shell and is highly electronegative, while xenon has a stable, full valence shell and has little tendency to react.