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?

A. The period 2 element would be more reactive because the attractive force of protons is stronger when there are fewer neutrons interfering.

B. 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.

C. The period 4 element would be more reactive because the attractive force of protons is stronger when there are more neutrons helping.

D. 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

Answer is: B. 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.

For example, fluorine (the period 2) is more reactive than bromine (the period 4).

Fluorine (F) is nonmetal with greatest electronegativity, which means it easily gain electrons.

Fluorine jas atomic number 9, which means it has 9 protons and 9 electrons. It gain one electron to form fluorine anion (F⁻) with stable electron configuration like closest noble gas neon (Ne) with 10 electrons.

Electron configuration of fluorine: ₉F 1s² 2s² 2p⁵.

Answer 2

Answer : Option B) 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 : The reactivity of the Periods decreases as we go from left to right across a period. The farther to the left and down the periodic chart we go, the easier it is for electrons to be donated or taken away, resulting in higher reactivities of the elements. The attractive force of the protons is found to be stronger when electrons are found to be attracted to a closer electron shell.