Question

1. arrange the following elements in order from smallest ionization energy to largest ionization energy.

periodic table
smallest ionization energy → largest ionization energy
a b c
choices:
f br cl

Explanation:

Ionization energy is the energy required to remove an electron from an atom. In a group of the periodic table, ionization energy decreases as we move down the group. The elements \(F\), \(Cl\), and \(Br\) are in Group 17 (halogens). \(Br\) is below \(Cl\), and \(Cl\) is below \(F\). As we move down the group (from \(F\) to \(Cl\) to \(Br\)), the atomic size increases. With an increase in atomic size, the outermost electrons are less tightly held by the nucleus. So, it becomes easier to remove an electron (lower ionization energy) as we move down the group.

Answer:

A. \(Br\)
B. \(Cl\)
C. \(F\)