Question

nonmetals (reactivity trends) 1. arrange these nonmetals in order of most reactive to least reactive: fluorine (f), chlorine (cl), iodine (i), bromine (br). - why does fluorine react more strongly than iodine? - are they in the same group or the same period?

Explanation:

Step1: Recall non - metal reactivity trend

In the halogen group (Group 17 of the periodic table), reactivity decreases down the group.

Step2: Identify group and period

Fluorine (F), chlorine (Cl), bromine (Br), and iodine (I) are in the same group (Group 17) and different periods. Fluorine is in period 2, chlorine in period 3, bromine in period 4 and iodine in period 5.

Step3: Explain reactivity difference

Fluorine has the smallest atomic radius among them. Its outermost electrons are closer to the nucleus and have a stronger attraction to the nucleus. So, it can gain an electron more easily than iodine, which has a larger atomic radius and a weaker attraction for an additional electron.

Answer:

1. Order of reactivity from most to least reactive: Fluorine (F) > Chlorine (Cl) > Bromine (Br) > Iodine (I).

They are in the same group (Group 17, halogens). Fluorine reacts more strongly than iodine because fluorine has a smaller atomic radius and a stronger attraction for electrons due to its higher effective nuclear charge and fewer electron - shielding effects compared to iodine.