re - order each list in the table below, if necessary so that the atoms or ions in it are listed in\natoms…

re - order each list in the table below, if necessary so that the atoms or ions in it are listed in\natoms or ions in order\natoms or ions\nof decreasing size\natoms or ions\nb²⁺, b, be\nf, li, b\nbr⁻, f⁻, cl⁻

re - order each list in the table below, if necessary so that the atoms or ions in it are listed in\natoms or ions in order\natoms or ions\nof decreasing size\natoms or ions\nb²⁺, b, be\nf, li, b\nbr⁻, f⁻, cl⁻

Answer

Explanation:

Step1: Consider atomic/ionic radius trends

Atomic radius decreases across a period due to increasing nuclear charge. Cations are smaller than their parent atoms. Anions are larger than their parent atoms and ionic radius increases down a group.

Step2: Analyze B²⁺, B, Be

Beryllium (Be) and boron (B) are in the same period. B has a larger nuclear charge than Be but B²⁺ has lost 2 electrons. So the order is B > Be > B²⁺.

Step3: Analyze F, Li, B

Li, B, and F are in the same period. Atomic radius decreases across the period. So the order is Li > B > F.

Step4: Analyze Br⁻, F⁻, Cl⁻

These are halide anions. Ionic radius increases down the group. So the order is Br⁻ > Cl⁻ > F⁻.

Answer:

B, Be, B²⁺ Li, B, F Br⁻, Cl⁻, F⁻