Question

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? 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

The reactivity of a nonmetal element in period 2 would be more violent than an element in period 4, as the size of the element and its ability to gain electrons would decrease as you go down the group in the table. Nonmetals want to form negative ions, as their weak valence shell allows them to gain electrons from other elements.

From the information gathered, the answer is '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'. 

Answer 2

Answer:

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.

Explanation:

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