Looking at the same nonmetal group on the periodic table, how does the reactivity of an element in period 2 compare to the reactivity of an element in period 4?

Question

The period 2 element would be more reactive because the attractive force of protons is stronger when there are fewer neutrons interfering.
The period 2 element would be more reactive because the attractive force of protons is stronger when electrons are attracted to a closer electron shell.
The period 4 element would be more reactive because the attractive force of protons is stronger when there are more neutrons helping.
The period 4 element would be more reactive because the attractive force of protons is stronger when electrons are attracted to a farther electron shell.

Answer 1

To compare the reactivity of nonmetal elements in different periods of the periodic table, it's important to consider the general trends in reactivity as you go down a group.

For nonmetals, reactivity typically increases as you move up a group. For example, within the halogens (Group 17), fluorine (a period 2 element) is more reactive than iodine (a period 4 element). This is because the smaller atomic size of period 2 elements allows their valence electrons to be more strongly attracted to the nucleus.

So, when comparing a nonmetal from period 2 to one from period 4 in the same group, the period 2 element (like oxygen or nitrogen) will generally be more reactive than the period 4 element (like sulfur or phosphorus).

Considering your provided statements, the most fitting reasoning would be:

"The period 2 element would be more reactive because the attractive force of protons is stronger when electrons are attracted to a closer electron shell."

This reflects the idea that the closer proximity of the nucleus (due to a smaller atomic radius in period 2) results in a stronger attraction between the nucleus and the valence electrons, enhancing the reactivity of the element.