Arrange the following groups of atoms in order of their increasing atomic radius:

K,Rb,F,B,Be

I think its
F<B<Be<K<Rb

someone can you correct me pls

I think B<Be<<Rb

Look at www.webelements

To arrange the given groups of atoms in order of increasing atomic radius, you need to consider the periodic trend in atomic radius.

Atomic radius generally increases as you move down a group (vertical column) in the periodic table and decreases as you move across a period (horizontal row).

Let's analyze the given groups of atoms:

- F (Fluorine): Fluorine is located in Group 17 (or Group VIIA) of the periodic table. As we move up Group 17, the atomic radius decreases due to an increased attraction between the positively charged nucleus and the valence electrons. Therefore, F has the smallest atomic radius among the given elements.

- B (Boron): Boron is located in Group 13 (or Group IIIA) of the periodic table. As we move down Group 13, the atomic radius increases due to the addition of new energy levels. Boron has a slightly larger atomic radius than F.

- Be (Beryllium): Beryllium is located in Group 2 (or Group IIA) of the periodic table. Moving down the group, the atomic radius increases due to the addition of new energy levels. Be has a larger atomic radius than B.

- K (Potassium): Potassium is located in Group 1 (or Group IA) of the periodic table. Moving down the group, the atomic radius increases due to the addition of new energy levels. Therefore, K has a larger atomic radius than Be.

- Rb (Rubidium): Rubidium is located immediately below potassium in Group 1 (or Group IA) of the periodic table. Since rubidium is further down the group, it has a larger atomic radius than potassium.

Based on this analysis, the correct order from the smallest to the largest atomic radius is:

F < B < Be < K < Rb

Therefore, you were correct in your initial response.